Finish transfer of all pyro chemicals

- Template pdf: finetune for rendering non-print style
- Set correct order for chapters

.gitignore

@@ -1,2 +1,3 @@
 build/
 *.log
+*.DS_Store

Makefile

@@ -41,6 +41,7 @@ DOCX_ARGS = --standalone --reference-doc templates/docx.docx
 EPUB_ARGS = --template templates/epub.html --epub-cover-image $(COVER_IMAGE)
 HTML_ARGS = --template templates/html.html --standalone --to html5
 PDF_ARGS = --template templates/pdf.latex --pdf-engine xelatex
+TEX_ARGS = --template templates/pdf.latex --pdf-engine xelatex
 
 # Per-format file dependencies
 
@@ -49,6 +50,7 @@ DOCX_DEPENDENCIES = $(BASE_DEPENDENCIES)
 EPUB_DEPENDENCIES = $(BASE_DEPENDENCIES)
 HTML_DEPENDENCIES = $(BASE_DEPENDENCIES)
 PDF_DEPENDENCIES = $(BASE_DEPENDENCIES)
+TEX_DEPENDENCIES = $(BASE_DEPENDENCIES)
 
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 # Basic actions
@@ -77,6 +79,9 @@ html:	$(BUILD)/html/$(OUTPUT_FILENAME).html
 .PHONY: pdf
 pdf:	$(BUILD)/pdf/$(OUTPUT_FILENAME).pdf
 
+.PHONY: tex 
+tex:	$(BUILD)/tex/$(OUTPUT_FILENAME).tex
+
 .PHONY: docx
 docx:	$(BUILD)/docx/$(OUTPUT_FILENAME).docx
 
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 	$(CONTENT) | $(CONTENT_FILTERS) | $(PANDOC_COMMAND) $(ARGS) $(PDF_ARGS) -o $@
 	@echo "$@ was built"
 
+$(BUILD)/tex/$(OUTPUT_FILENAME).tex:	$(TEX_DEPENDENCIES)
+	mkdir -p $(BUILD)/tex
+	$(CONTENT) | $(CONTENT_FILTERS) | $(PANDOC_COMMAND) $(ARGS) $(TEX_ARGS) -o $@
+	@echo "$@ was built"
+
 $(BUILD)/docx/$(OUTPUT_FILENAME).docx:	$(DOCX_DEPENDENCIES)
 	mkdir -p $(BUILD)/docx
 	$(CONTENT) | $(CONTENT_FILTERS) | $(PANDOC_COMMAND) $(ARGS) $(DOCX_ARGS) -o $@

README.md

@@ -1,3 +1,3 @@
-# Pyrotechnics Revived eBook 
-
+# 21st century Pyrotechny
+ 
 Pyrotechics information preservation project in eBook format

chapters/1000-suppliers.md

@@ -1,28 +0,0 @@
-# Suppliers
-
-* [Lortone ball mills](https://lortone.com/)
-
-## United States (US)
-
-* [CannonFuse.com](https://cannonfuse.com/)
-* [Pyroworks US](https://pyroworks.us/)
-* [Skylighter](https://www.skylighter.com/)
-
-## Europe (EU)
-
-**Spain (ES)**
-
-* [Nitroparis](https://nitroparis.com/)
-
-**Germany (DE)**
-
-* [Pyro-Tools.eu](https://pyro-tools.eu/)
-
-**The Netherlands (NL)**
-
-
-
-**United Kingdom (UK)**
-
-* [Cooperman435](https://www.cooperman435.co.uk/)
-* [Potterycrafts](https://www.potterycrafts.co.uk/)

chapters/99-0-chemicals.md

@@ -1,5 +1,10 @@
 # Chemicals
 
-A chemical substance is a form of matter having constant chemical composition and characteristic properties. Some references add that chemical substance cannot be separated into its constituent elements by physical separation methods, i.e., without breaking chemical bonds. Chemical substances can be simple substances, chemical compounds, or alloys.
+A chemical substance is a form of matter having constant chemical composition
+and characteristic properties. Some references add that chemical substance
+cannot be separated into its constituent elements by physical separation
+methods, i.e., without breaking chemical bonds. Chemical substances can be
+simple substances, chemical compounds, or alloys.
 
-In pyrotechnics specific chemicals are used for different effects, and some as helpers during manufacturing like solvents and binders.
+In pyrotechnics specific chemicals are used for creating different effects.
+Some are used as helpers during manufacturing like solvents and binders.

chapters/99-1-chemical-acetone.md

@@ -0,0 +1,30 @@
+## Acetone
+
+**Formula**
+
+$C3H6O$
+
+**Pyrotechnics use**
+
+Solvent
+
+**Description**
+
+Acetone is a very volatile flammable liquid that is commonly used as a solvent.
+Nitrocellulose, parlon and red gum dissolve very well in acetone. The solution
+of nitrocellulose is called nitrocellulose lacquer. Working with acetone can be
+difficult as compositions dry out very quickly. The evaporation of the acetone
+also causes cooling of composition, sometimes even below 0° C. This can result
+in condensation of water.
+
+**Sources**
+
+Acetone can usually be bought at any paint store. Making acetone at home is
+very impractical and unnecessary as it can be bought just about anywhere at low
+cost.
+
+**Hazards**
+
+Acetone is very volatile and flammable. Acetone vapour is heavier than air and
+spreads over the ground. Only work with acetone outside or in a well ventilated
+area.

chapters/99-1-chemical-aluminium.md

@@ -0,0 +1,106 @@
+## Aluminium
+
+**Formula**
+
+$Al$
+
+**Pyrotechnic use**
+
+Fuel
+
+**Synonyms**
+
+Aluminium metal
+
+**Description**
+
+Aluminium powder is one of the most often used fuels in pyrotechnics. A wide
+range of effects are possible with different types of powder, with differences
+in particle size, shape and impurities. The finest powders (e.g., German Dark
+and XD-30) can be 'airfloat', and are commonly used in flash compostions. Fine
+aluminium is also used in small percentages in some hobby-rocket fuels. Courser
+powders are generally used for sparkling effects. With these larger particle
+types, many effects--such as flitter, glitter, firefly and snowball--can be
+achieved.
+
+**Sources**
+
+Aluminium powder is sometimes sold as a pigment in (art) paint stores. This
+powder, known as 'aluminium bronze', is a flaky powder with a stearin coating.
+It is quite expensive but readily available and a source for small quantities.
+Aluminium grit and turnings can sometimes be found in machine shops were
+aluminium is processed. If fine enough this can be used as is, but it can also
+be ball milled into flakes. These flakes are quite reactive as they have a
+large surface area and can be used for several effects. Sanding aluminium
+chunks can also make aluminium powder. I've heard of people building a machine
+to do this, and the results can be quite good depending on the sanding paper
+used and the set-up. Another source of usable aluminium powder is to burn
+tetra-paks, and then powder the resultant aluminium residue in a ball mill.
+Aluminium powder can also be found inside an Etch A Sketch. In Boating stores,
+it can be found as a two component epoxy for protection of boat hulls against
+UV radiation, mesh size is questionable.
+
+**Dark (Pyro) Aluminium type**
+
+It is a very fine powder and dark grey in colour. Nominal mesh size is 200 but
+it contains particles of 2µ. There is a wide variety of uses for dark
+aluminium, for example: flash powders, star compositons, fountains, waterfalls,
+torches, flares, etc. For all this purposes it is generally used as a fuel.
+Many powders sold as "dark" aren´t really dark aluminium but the atomized type
+(often 63µ) and although the color of the former may vary it has to be dark
+grey and not light grey or even whitish grey (some of the best dark aluminium
+comes from Eckart Germany and this powder is nearly black in color = German
+Dark). Under the microscope it´s possible to identify atomized and dark powders
+quite well: the former are spherical in shape while the latter are irregular
+and angular. Dark alu is generally the most expensive of all the alu powders.
+
+**Atomatized Aluminium powder type**
+
+Atomized Aluminuim is increasingly used in fireworks although there are only
+limited uses for it (this is because spherical or spindle shaped particles are
+more difficult to ignite than a flake). In practice no material coarser than
+120 mesh can be used and commercial atomized powders are generally 300+ mesh
+and light grey to grey in colour. It is needed for glitter effects and other
+special stars, to give an example only.
+
+**Flake Aluminium type**
+
+There are mainly three different types of flake alu (all silver in colour). The
+first is "bronze" also known as paint grade aluminium. This fluffy powder is
+used for making paint and the particle size is very fine (sometimes less than
+2µ). Paint aluminium generally contains grease or stearine (the content varies
+from one to four percent by weight) which decreases its reactivity.
+Nevertheless aluminium bronze is easily obtained from an artist supply and
+produces quite good silver effects. It can be used wherever "bright" aluminium
+is mentioned in a composition. Generally it´s a dirty business to work with
+fatty aluminium. It only passes the mesh when accompanied by another material.
+The second flake aluminium is the real "bright" or "brilliant" powder we can
+subsitute with bronze for most purposes. Bright alu usually passes 120 mesh
+(nominal mesh Flake Aluminiumsize 120-200) and like "bronze" is very fluffy and
+leafing mass. The main difference to the latter is that brilliant powders
+contain less grease/stearine (0,5% by weight max) or are coated with another
+material which means that they aren´t as fatty to handle as bronze grades. They
+are used as a fuel for many purposes and to obtain silver effects. The third
+flake grade is called "flitter" which means flake powders of a larger mesh size
+than bright aluminium. It is sold as "fine", "middle" and "coarse"
+flake/flitter. Some people think that using flitter larger mesh variations are
+allowed. Sometimes this might be true but corresponding to the correct mesh
+size often makes the critical difference. As a rule of thumb fine flitter is:
+80-120 mesh, middle flitter is: 30-80 mesh and coarse flitter (=coarse flake)
+is 10-30 mesh.
+
+Aluminium Particle Types: <PICTURE>
+
+**Hazards**
+
+Aluminium is a neurotoxin that alters the function of the blood-brain barrier.
+Additionally small particles that are airborne act as tiny razors when they
+come in contact with lung or eye tissue, and a dust mask and goggles should be
+worn at all times when working with aluminium powder. Mixtures containing
+nitrates and aluminium powder are prone to heating up spontaneously and may
+ignite, especially when wet. This is caused by the reduction of the nitrate by
+aluminium, forming amides. These very basic compounds react further with
+aluminium powder in a very exothermic reaction that can cause spontaneous
+ignition. An ammonia smell is often produced in this reaction. Adding 1 to 2%
+boric acid to compositions containing nitrates and aluminium is common practice
+and will often prevent spontaneous ignition.

chapters/99-1-chemical-ammonium-chloride.md

@@ -0,0 +1,44 @@
+## Ammonium chloride
+
+**Formula**
+
+$NH4Cl$
+
+**Pyrotechnic use**
+
+Smoke colorant
+
+**Synonyms**
+
+Zalmiak
+
+**Description**
+
+Ammonium chloride is used in smoke compositions.
+When heated ammonium chloride decomposes to $HCl$ and $NH3$, both gasses. These recombine in the air to give a smoke consisting of fine particles of ammonium chloride.
+
+**Sources**
+
+Ammonium chloride solution is easily prepared by neutralising ammonia
+solution with hydrochloric acid. It is advised to use a slight excess of
+ammonia. That is to make sure no remaining acid will be present in the ammonium
+chloride obtained on evaporation and crystallisation. Otherwise traces of the
+acid solution may be enclosed in the crystals, possibly leading to spontaneous
+ignition of mixtures made with it.
+
+**Hazards**
+
+Ammonium chloride based smoke is irritating to the eyes and lungs as
+it contains some remaining HCl and NH3. Ammonium chloride itself is not
+poisonous and is even used in some type of candy. But as with all fine powders
+a dust mask must be worn, and since ammonium chloride is irritating to the skin
+and damaging to the eyes, gloves and goggles are important. According to
+Shimizu, ammonium chloride forms an exception to the rule that ammonium
+compounds should not be mixed with chlorates. Due to the lower solubility of
+potassium chlorate (compared to ammonium chlorate) no ammonium chlorate should form. Use these mixtures with great caution (or avoid
+them) since it seems inevitable that small amounts of ammonium chlorate will
+still form. The lower solubility of potassium chlorate will make it the -main-
+product in a double decomposition reaction but not the -only- product. It is
+strongly advised not to mix with metal powders, specifically copper, because it
+will become extremely corrosive. Toxicity: Oral rat LD50 : 1650 mg/kg
+Investigated as a mutagen.

chapters/99-1-chemical-ammonium-dichromate.md

@@ -0,0 +1,25 @@
+## Ammonium dichromate
+
+**Formula**
+
+$(NH4)2Cr2O7$
+
+**Pyrotechnic use**
+
+Reducer? TBD
+
+**Synonyms**
+
+Ammonium Pyrochromate
+
+**Description**
+
+Ammonium dichromate is sometimes used to suppress the reaction of magnesium in an ammonium perchlorate-type composition. In this case it is better than potassium dichromate, which is normally used for this purpose.
+
+**Hazards**
+
+Ammonium dichromate is one of the most hazardous pyro chemicals.
+
+It is explosive as a standalone and listed T+ because of it´s nature as a potential carcinogene.
+
+It is absorbed through the skin, and is corrosive. Maximum safety measures necessary!!!

chapters/99-1-chemical-ammonium-nitrate.md

@@ -0,0 +1,45 @@
+## Ammonium nitrate
+
+**Formula**
+
+$NH4NO3$
+
+**Pyrotechnic use**
+
+Oxidiser
+
+**Synonyms**
+
+ammonia nitre
+
+**Description**
+
+Ammonium nitrate is an oxidiser. It is very hygroscopic and therefore not used
+very often in fireworks. It finds some use in composite propellants, but
+performance is not as good as perchlorate-based propellants.
+
+**Sources**
+
+Ammonium nitrate solution can be prepared by neutralising ammonia solution with
+nitric acid. It is advised to use a slight excess of ammonia. That is to make
+sure no remaining acid will be present in the ammonium nitrate obtained on
+evaporation and crystallisation. Otherwise traces of the acid solution may be
+enclosed in the crystals, possibly leading to spontaneous ignition of mixtures
+made with it. Large quantities of ammonium nitrate can also be cheaply bought
+as fertilizer. ammonium nitrate can be extracted from ferilizer with water
+leaving the ammonium sulfate(solid) behind. Ammonium nitrate can also be found
+as the active agent in instant cold packs.
+
+**Hazards**
+
+Large masses of ammonium nitrate have been known to explode on some occasions
+although it is very insensitive. Smaller quantities are less likely to
+detonate. The risk of detonation increases when ammonium nitrate is molten or
+mixed with fuels such as metal powders or organic substances. Ammonium nitrate
+should never be mixed with chlorates as this may result in ammonium chlorate
+formation, possibly leading to spontaneous ignition. Mixtures of metal powders
+and ammonium nitrate are likely to heat up spontaneously and may ignite,
+especially when moist. This can sometimes be prevented by the addition of small
+amounts of boric acid (1 to 2%), but in general it is better to avoid these
+mixtures at all. The hygroscopic nature of ammonium nitrates makes this problem
+worse (also see aluminium). Toxicity: Oral rat LD50: 2217 mg/kg

chapters/99-1-chemical-ammonium-perchlorate.md

@@ -0,0 +1,25 @@
+## Ammonium perchlorate
+
+**Formula**
+
+$NH4ClO4$
+
+**Pyrotechnic use**
+
+Oxidiser
+
+**Synonyms**
+
+Perchloric acid ammonium salt
+
+**Description**
+
+Ammonium perchlorate is an oxidiser used in a large number of compositions. Very impressive colour compositions can be made with it, but their burn rate is often too low for use in star compositions. For lance work and torches slow burning is an advantage and it is therefore commonly used in these items. Ammonium perchlorate is also used in composite rocket propellants, including the propellants used in the solid propellant boosters used for the space shuttle. The decomposition products of ammonium perchlorate are all gasses that are very beneficial for rocket propellants.
+
+**Sources**
+
+Ammonium perchlorate is usually bought from chemical suppliers or from dedicated pyro suppliers. Fine ammonium perchlorate powder is a regulated substance in most countries and cannot easily be bought or transported. Since it is such a useful chemical in pyrotechnics it can be worth the time and effort to try to prepare it at home. This can be done by first making sodium perchlorate followed by double decomposition with ammonium chloride (other ammonium compounds can be used). The preparation of sodium perchlorate is most easily accomplished by electrolysis. Chemical Destruction of any chlorates present in the sodium perchlorate must be performed BEFORE Ammonium Chloride is added as Ammonium Chlorate is very unstable. Amateur production of Ammonium Perchlorate via electrolysis is dangerous and not recommended.
+
+**Hazards**
+
+Ammonium perchlorate can detonate by itself, although it is not very sensitive. Larger amounts and mixtures of ammonium perchlorate with metal powders or organic substances are more likely to detonate. Harmful if swallowed, inhaled or absorbed through the skin. Toxicity: ORL-RAT LD50 4200 mg kg SCU-RAT LD50 1600 mg kg

chapters/99-1-chemical-anthracene.md

@@ -0,0 +1,25 @@
+## Anthracene
+
+**Formula**
+ 
+$C14H10$
+
+**Pyrotechnic use**
+
+Smoke compositions
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Blue or - if impure - green crystals gained by the distillation of coal tar. Anthracene is used in oxygen-negative compositions together with potassium perchlorate for black smoke production. It was excessively used in German smoke grenades during the second world war.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+TBD

chapters/99-1-chemical-antimony-trisulfide.md

@@ -0,0 +1,27 @@
+## Antimony trisulfide
+
+**Formula**
+ 
+$Sb2S3$
+
+**Pyrotechnic use**
+
+Fuel in glitter compositions, fountain compositions and flash powder.
+
+**Synonyms**
+ 
+Stibnite, Antimonite, Antimony sulfide/sulphide, Antimony (III) sulfide/sulphide
+
+**Description**
+ 
+Antimony trisulfide is a green powder. It is a fuel used in various white star compositions of the potassium perchlorate-base. It is sometimes used in glitter compositions, fountain compositions and [flash powder](Flash_powder.html "Flash powder"), however it is used less and less for flash powder as it is very poisonous and can usually be replaced by sulphur or completely omitted. Flash compositions containing antimony trisulfide are very sensitive to friction, shock, and static electricity.
+
+**Sources** 
+
+Antimony trisulfide is sometimes sold as a pigment in (art) paint stores, but it is not commonly found these days due to it's toxicity. It can be made at home by fusing a [stoichiometric](Stoichiometric.html "Stoichiometric") mixture of [antimony metal](Antimony_metal.html "Antimony metal") and [sulfur](Sulfur.html "Sulfur"). This is a _very dangerous_ operation since lethally toxic fumes will form, and it should only be performed with proper safety precautions taken.
+
+**Hazards**
+
+Xn, Xi
+
+Antimony trisulfide should never be used in any mixture containing chlorates, or else spontaneous ignition may occur. Mixtures with antimony trisulfide and perchlorates are very sensitive to friction and shock, and extra caution should be exercised when handling these mixtures. These mixtures are best avoided entirely. Wear proper protective clothing, including a dust mask and gloves, when working with compositions containing antimony trisulfide as it is very poisonous, and toxic to the kindnys and liver. Toxicity: ORAL (LD50): Acute: 7000 mg/kg [Rat] IPR-MUS LD50: 209 mg/kg. Most Antimony trisulphide that has been mined will contain a small Arsenic impurity which can contribute to toxicity depending on levels. At levels above 0.5% the material is classified as hazardous for shipping by air (IATA regulations 2010).

chapters/99-1-chemical-antimony.md

@@ -0,0 +1,31 @@
+## Antimony
+
+**Formula**
+ 
+$Sb$
+
+**Pyrotechnic use**
+
+Fuel, Ball-mill media alloy.
+
+**Synonyms**
+ 
+Antimony metal powder, Stibium, Antimony black, Regulus of antimony
+
+**Description**
+
+Milled antimony is a dark grey powder of 200+ mesh, but generally Sb can be bought as heavy, large size silver crystals that look and feel like pyrite. The powder is used for white fires (in lances etc.), to assure ignition (with Al) and as an important ingredient in glitter compositions although they do not necessarily employ antimony. Moreover antimony can be used to harden lead (employed e.g. for casting ball-mill media).
+
+**Sources** 
+
+TBD
+
+**Hazards**
+
+T, N, Xn, Xi
+
+Antimony in powdered form is harmful. Do not ingest. Prevent inhaling and contact with eyes and skin. Use proper safety equipments such as latex gloves, goggles and a dust mask or respirator. Toxic to aquatic organisms, may cause long-term adverse effects in the aquatic environment. Do not dispose of in the environment.
+
+[http://www.firebird.bc.ca/documents/MSDS/MSDSAntimony.pdf](www.firebird.bc.ca/documents/MSDS/MSDSAntimony.pdf "www.firebird.bc.ca/documents/MSDS/MSDSAntimony.pdf")
+
+[http://www.espimetals.com/msds's/antimony.pdf](www.espimetals.com/msds%27s/antimony.html "www.espimetals.com/msds's/antimony.pdf")

chapters/99-1-chemical-ascorbic-acid.md

@@ -0,0 +1,25 @@
+## Ascorbic acid
+
+**Formula**
+ 
+$C6H8O6$
+
+**Pyrotechnic use**
+
+Fuel for the composition Golden Powder, a black powder substitute.
+
+**Synonyms**
+ 
+Vitamin C
+
+**Description**
+ 
+Ascorbic acid is an organic acid. Its appearance is white to light yellow crystals or powder. It is water soluble. In pyrotechnics it is primarily used as a fuel for the composition [Golden Powder](Golden_Powder.html "Golden Powder"), a black powder substitute.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+None, as it can be used as a food supplement.

chapters/99-1-chemical-barium-carbonate.md

@@ -0,0 +1,27 @@
+## Barium carbonate
+
+**Formula**
+ 
+$BaCO3$
+
+**Pyrotechnic use**
+
+Green and white colorant
+
+**Synonyms**
+ 
+Barium mono-carbonate, Carbonic acid barium salt
+
+**Description**
+ 
+Barium carbonate is used both in white and green color compositions. When chlorine donors are present in a composition a green color will result from the formation of BaCl+ in the flame. Without chlorine donors BaO will be formed which emits white light. Barium carbonate is convenient to use in chlorate based color compositions since it will neutralise residual acid which reduces the risk of spontaneous ignition.
+
+**Sources** 
+
+Barium carbonate is cheaply available in kilogram quantities from ceramic supply shops. However, this material is often contaminated with small amounts of barium sulfide that are left over from the production process. Therefore, ceramics grade barium carbonate should never be used in mixtures incompatible with sulphides such as chlorate based mixtures. Barium carbonate is not easily made at home.
+
+**Hazards**
+
+Xn, Xi
+
+Most barium compounds are very poisonous, especially the more soluble barium compounds such as the chlorate and nitrate. A dust mask should be worn at all times when working with barium carbonate. Unlike its soluble cousins which can be easily washed from the hands with lots of water the carbonate is not so easily removed and care to remove the powder from under finger nails is important before eating etc. Barium carbonate is soluble in stomach acid, and therefore a poison by ingestion.

chapters/99-1-chemical-barium-chlorate.md

@@ -0,0 +1,27 @@
+## Barium chlorate
+
+**Formula**
+ 
+$BaClO3$
+
+**Pyrotechnic use**
+
+Oxidiser and green colorant
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Barium chlorate is used as an oxidiser in green color compositions and can produce intense greens. Fierce burning and high color purity compositions can be made with it.
+
+**Sources** 
+
+Barium chlorate is usually purchased from chemical suppliers or from dedicated pyro suppliers. It can be made at home from sodium chlorate and barium chloride by double decomposition however purifying the product by recrystallising can be a lot of work because all traces of the sodium must be removed so as to not interfere with pure green colors. Barium chlorate can also be prepared from barium chloride by electrolysis in a process analogous to that used for preparing sodium chlorate.
+
+**Hazards**
+
+Xi, O
+
+Barium chlorate is poisonous and a dust mask should be worn at all times when handling it. Barium chlorate should never be mixed with sulfur or sulfides or allowed to come in contact with mixtures containing sulfur or sulfides since this could result in spontaneous ignition. Sulfur reacts with water and air to form small amounts of sulfuric acid. Sulfuric acid and chlorates react producing ClO2, an explosive gas that will ignite many organic materials on contact. Mixtures made with barium chlorate are often especially sensitive to friction and shock (even more so than potassium chlorate based mixtures) and should be handled with extra care.

chapters/99-1-chemical-barium-nitrate.md

@@ -0,0 +1,29 @@
+## Barium nitrate
+
+**Formula**
+
+$Ba(NO3)2$
+
+**Pyrotechnics use**
+
+Oxidizer
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Barium nitrate is used as an oxidizer in both white and green color compositions. When chlorine donors are present in a composition a green color will result from the formation of BaCl+ in the flame. Without chlorine donors BaO will be formed which emits bright white light. Barium nitrate is seldom used as the sole oxidizer in green color compositions. It is usually combined with perchlorate's to improve the color and increase the burning rate.
+
+**Sources** 
+
+Barium nitrate may be prepared from nitric acid or ammonium nitrate and barium carbonate, which is available from ceramic supply stores. It can also be made from sodium nitrate and barium chloride by double decomposition and recrystallizing for purity. It should be done outside with an electric hotplate and stainless steel ware. Garden hose at the ready and nothing left outside for the kids to handle. Wash any spills into the ground with the hose until below the surface. Spread some ammonium sulphate fertilizer over and water some more. This will convert soluble barium salts to insoluble barium sulphate, which is harmless. Neutralize all waste solution with enough ammonium sulphate until white clouds of powder is no longer seen in the clear liquid then it is safe to dump onto ground.
+
+**Hazards**
+
+T, O, Xn, Xi
+
+Barium nitrate is poisonous. May be fatal if swallowed! A dust mask should be worn at all times when handling it. Mixtures of metal powders and barium nitrate sometimes heat up spontaneously and may ignite, especially when moist. This can usually be prevented by the addition of small amounts of boric acid (1 to 2%). It is advisable to avoid using water to bind such compositions. Red gum or shellac with alcohol or nitrocellulose lacquer are preferred binder and solvents (also see aluminium).
+
+Causes irritation to the respiratory tract. Symptoms may include coughing, shortness of breath. Systemic poisoning may occur with symptoms similar to those of ingestion. If ingested it may cause tightness of the muscles of the face and neck, vomiting, diarrhea, abdominal pain, muscular tremors, anxiety, weakness, labored breathing, cardiac irregularity, convulsions, and death from cardiac and respiratory failure. Estimated lethal dose lies between 1 to 15 grams. Death may occur within hours or up to a few days. May cause kidney damage. Causes irritation to skin. Symptoms include redness, itching, and pain. If it comes into contact with eyes it causes irritation, redness, and pain.

chapters/99-1-chemical-barium-sulfate.md

@@ -0,0 +1,27 @@
+## Barium sulfate
+
+**Formula**
+ 
+$BaSO4$
+
+**Pyrotechnic use**
+
+High temperature oxidizer.
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Barium sulfate is used as a high temperature oxidizer in some green and white compositions, as well as being the oxidiser in the flash phase of some strobe compositions. It is also used as an additive in many firefly star compositions. Barium nitrate is more common in green pyrotechnic formulas, as it is a more amiable oxidizer and produces a superior colour.
+
+**Sources** 
+
+Barium sulfate may be precipitated from a solution of a soluble barium salt, such as barium nitrate or chloride, and a sulfate. Magnesium sulfate and Potassium sulfate are both cheaply available as fertilizer and are convenient to use. Magnesium sulfate can be found at pharmacies and grocery stores under its common name as Epsom salt. The precipitated barium sulfate is a very fine powder which may be rinsed by repeated washings with hot water, settling and decanting. A final washing in the filter with acetone or ethanol will allow it to dry quickly, but is not a necessary step. Do not use sulfuric acid to precipitate barium sulfate as this may result in the inclusion of acid droplets in the precipitated particles which can lead to spontaneous ignition in chlorate compositions. There is some debate active regarding the safety of using sulfates in combination with chlorates regardless off acid contamination.
+
+**Hazards**
+
+Xi
+
+Unlike many other barium compounds, barium sulfate is not very poisonous due to its low solubility in water. Indeed it is ingested in significant quantity regularly as a part of some medical procedures.

chapters/99-1-chemical-bentonite-clay.md

@@ -0,0 +1,23 @@
+## Bentonite clay
+
+**Formula**
+ 
+$(Na,Ca)0.33(Al,Mg)2Si4O10(OH)2·(H2O)n$
+
+**Synonyms**
+ 
+Bentonite Clay, Gumbrin, Akajo, Aquagel (gold), Asama, Askangel, Baroco, Yellow stone, Western bond, Natural gel, and many others...
+
+**Description**
+ 
+Bentonite is a white solid, mostly in dust or pellet form. It is generally used for nozzles, since it doesn't disintegrate quickly like cardboard or other products. Bentonite clay is a very important in making fireworks.
+
+**Sources** 
+
+Bentonite is easy to obtain. Pottery stores sells it, but a cheaper alternative is "Clumping Kitty Litter," which is often Bentonite clay, and can be found in most supermarkets. One of the best brands to use is "Fresh Step," which (unlike many other types of clumping kitty litters) does not erode or crumble easily. In Australia ,rural store , Unimin "activegel" 20k bag used to seal leaking dam.
+
+**Hazards**
+
+Xi
+
+Bentonite, in dust form, is suspected to be carcinogenic. Wear a dust mask or respirator when working with bentonite.

chapters/99-1-chemical-bismuth-subcarbonate.md

@@ -0,0 +1,23 @@
+## Bismuth subcarbonate
+
+**Formula**
+ 
+$(BiO)2CO3$
+
+**Synonyms**
+ 
+Bismuth oxycarbonate, Basic bismuth carbonate
+
+**Description**
+ 
+Bismuth subcarbonate is a fine white to yellow-white powder used mainly in Crackling microstars (Dragon eggs) as a substitution for Poisonous Lead tetraoxide and expensive Bismuth trioxide
+
+**Sources** 
+
+Bismuth subcarbonate can be purchased from Pyrotechnic suppliers.
+
+**Hazards**
+
+Xi
+
+Bismuth subcarbonate is not particularly hazardous. However it is a skin, eye and respiratory system irritant. Wear gloves, dust mask, protection glasses, and do not ingest. Large ingested amounts can cause systemic bismuth poisoning with symptoms of headache, skin rashes, kidney damage, and rarely mild jaundice.

chapters/99-1-chemical-bismuth-yellow.md

@@ -0,0 +1,23 @@
+## Bismuth yellow
+
+**Formula**
+ 
+$Bi2O3$
+
+**Synonyms**
+ 
+Bismuth(III)oxide
+
+**Description**
+ 
+It is used in crackling stars (Dragon's eggs) as a non-toxic substitute for toxic lead compounds. For this purpose it is mixed with magnalium and copper oxide.
+
+**Sources** 
+
+Bismuth yellow can be found at various Pyro supplies. The major defect is the comparatively high price of bismuth.
+
+**Hazards**
+ 
+Xi
+
+Harmful by inhalation, in contact with skin and if swallowed. Wear suitable protective clothing when working with Bismuth yellow, such as dust mask and latex gloves.

chapters/99-1-chemical-boric-acid.md

@@ -0,0 +1,23 @@
+## Boric acid
+
+**Formula**
+ 
+$H3BO3$
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Boric acid is a white powder which is used as an additive to compositions containing aluminium and a nitrate. The metal powder can reduce the nitrate to an amide, which will react with the metal powder in a very exothermic reaction that can lead to spontaneous ignition of the composition. This process is often accompanied by a smell of ammonia and is most likely to occur with wet compositions. Addition of a few percent boric acid can often prevent this reaction from taking place since it neutralizes the very basic amides forming ammonia and a borate. It is also advisable to avoid using a water-soluble binder for these compositions. Using red gum or shellac with alcohol or nitrocellulose lacquer is safer. Boric acid is hygroscopic. The use of boric acid with magnesium or magnalium is not advised, as it actively attacks and corrodes these metals.
+
+**Sources** 
+
+Boric acid is cheaply and in kilogram quantities available from ceramic supply shops. It is also sold in many drug stores at a somewhat higher price, but since only small quantities are needed the price is not really important. It is also sold in Homecenters as an effective insecticide for roachs (it may list the contents as orthoboric acid). 99% pure boric acid is available as "Roach away" in walmart.
+
+**Hazards**
+ 
+C
+
+Boric acid is really poisonous, and should be cleaned up very well after using.

chapters/99-1-chemical-calcium-carbonate.md

@@ -0,0 +1,27 @@
+## Calcium carbonate
+
+**Formula**
+ 
+$CaCO3$
+
+**Pyrotechnic use**
+
+Colorant
+
+**Synonyms**
+ 
+Precipitated chalk, Limestone, Calcite, Carbonic acid calcium salt.
+
+**Description**
+ 
+Colorless powder. It slowly reacts with NH4ClO4 in presence of moisture. Calcium carbonate is often used in toy fireworks as a cheap substitute for strontium salts, but the flame is reddish orange and not so beautiful as e.g. with SrCO3.
+
+**Sources** 
+
+A cheap source is the ceramics supply. Price is about $3/kg for the technical grade. you can also get it easely by powdering clean egg shells.
+
+**Hazards**
+ 
+Xi
+
+Dust may cause irritation to eyes, skin or respiratory system. Wear gloves, protection goggles and dust mask when manipulating fine powder.

chapters/99-1-chemical-calcium-nitrate.md

@@ -0,0 +1,23 @@
+## Calcium nitrate
+
+**Formula**
+ 
+$Ca(NO3)2$
+
+**Synonyms**
+ 
+Norwegian saltpeter
+
+**Description**
+ 
+Calcium nitrate is the calcium salt of nitric acid. It's extremly hygroscopic, much more than Sodium nitrate. Because of that it's not used much in pyrotechnics.
+
+**Sources** 
+
+Calcium nitrate is used as a fertiliser.
+
+**Hazards**
+ 
+O
+
+Calcium nitrate is an oxidiser, store separate from fuels and acids.

chapters/99-1-chemical-calcium-sulfate.md

@@ -0,0 +1,22 @@
+## Calcium sulfate
+
+**Formula**
+ 
+$CaSO4.x H2O$ where x= ~0.5 or 2
+
+**Synonyms**
+ 
+1. Hemihydrate = Plaster of Paris, Crystacal, Densite, Gypsum hemihydrate, Tiger stone
+2. Dihydrate = Gypsum, Alabaster
+
+**Description**
+ 
+The hemihydrate (x=~0.5) is commonly known as plaster of Paris. The dihydrate (x=2) occurs as a mineral known as gypsum. Calcium sulfate can be used as a high temperature oxidizer in orange color compositions. Excellent strobe compositions can be made with it.
+
+**Sources** 
+
+Plaster can be used as is in strobe and exotic flash compositions, but is better to remove the water which is easily accomplished by heating. Plaster of Paris can be bought at hardware vendors and is often sold in hobby shops.
+
+**Hazards**
+ 
+Calcium sulfate dihydrate may act as an eye or respiratory irritant. Wear safety glasses and dust mask.

chapters/99-1-chemical-charcoal.md

@@ -0,0 +1,23 @@
+## Charcoal
+
+**Formula**
+ 
+Mixture with variable composition, generally of empirical formula $C8H4O$ 
+
+**Synonyms**
+ 
+Alcohol, Undenatured Alcohol, Ethyl Alcohol, Dehydrated Alcohol, Spiritus
+
+**Description**
+ 
+Charcoal finds widespread use in pyrotechnics. Many types of charcoal exist, each with its own properties. It is a complex organic substance containing moisture, ash, carbon, hydrogen, oxygen and a variety of volatiles. All of these elements have a vital use in fireworks. Charcoal made from willow or grapevine is considered great for black powder, while hardwood charcoals e.g. pine charcoal are commonly used for spark effects. The particle size and the process used to make the charcoal also play an important role in the quality of the charcoal for a specific purpose. Very fine charcoal floats in air and is therefore sometimes referred to as 'airfloat'.
+
+**Sources** 
+
+Barbeque briquettes are mixed with clay and are not suitable for making black powder. Charcoal can be purchased from supermarkets, BBQ supply stores and directly from online pyrotechnic chemical suppliers. Charcoal can easily be prepared at home.
+
+**Hazards**
+ 
+Xi
+
+Fine charcoal dust is easily breathed in, and a dust mask should be worn when working with it. Freshly prepared charcoal can be pyrophoric even when not powdered and it must be allowed to stand for a day at least before it is used in any compositions.

chapters/99-1-chemical-chloroform.md

@@ -0,0 +1,25 @@
+## Chloroform
+
+**Formula**
+ 
+$CHCl3$
+
+**Pyrotechnic use**
+
+Non-polar solvent
+
+**Synonyms**
+ 
+trichloromethane, methyl trichloride
+
+**Description**
+ 
+Chloroform is often used as a non-polar solvent. It is also used an anaesthetic, however it has a higher toxicity as well as being an environmental hazard. It is more commonly found in refrigerants in today's usage. And has a molar mass of 119.38g/mol. It has a melting point of -63.5°C, a boiling point of 61.2°C, and a density of 1.48g/cm^3, liquid. It's solubility in water is 0.8g/100mL at 20°C making it insoluble in water. It's flash-point is specified as non-flammable. It is a common solvent since it's usually nonreactive and miscible with most organic liquids where it may be volatile.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+Xn Xi, Carcinogen

chapters/99-1-chemical-chlorowax.md

@@ -0,0 +1,25 @@
+## Chlorowax
+
+**Formula**
+ 
+TBD
+
+**Pyrotechnic use**
+
+Chlorine donor
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Chlorowax is a type of chlorinated paraffin resin, in the form of a cream colored powder. It is used as a chlorine donor (contains 70% chlorine). Chlorinated paraffins are used as secondary plasticizers for polyvinyl chloride (PVC). Chlorinated paraffins are also used as extreme pressure additives in metal-machining fluids or as metal-working lubricants or cutting oils because of their viscous nature, compatibility with oils, and property of releasing hydrochloric acid at elevated temperatures. They are added to paints, coatings and sealants to improve resistance to water and chemicals, which is most suitable when they are used in marine paints, as coatings for industrial flooring, vessels and swimming pools and as road marking paints. Solvents are xylene, acetone and alcohol.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+Unknown

chapters/99-1-chemical-clay.md

@@ -0,0 +1,21 @@
+## Clay
+
+**Formula**
+ 
+Mixture with variable composition
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Different types of clay are used for nozzles, plugs or filler. Of all the types of clay in use bentonite and kaolin are probably the most common. Ground kitty litter is a cheap alternative and works well. Clay is a very important in making fireworks.
+
+**Sources** 
+
+As mentioned, kitty litter can be a cheap source of clay. A cheap variety of non-clumping kitty litter can be ground (mortar and pestle or ball mill) and sieved to obtain a fine powder which is easily pressed into a compact pellet. Bentonite and kaolin clay are also available from ceramic supply stores.
+
+**Hazards**
+ 
+Clay is not particularly toxic or dangerous, but bentonite has shown to case cancer in animals but the evidence is unclear.

chapters/99-1-chemical-cmc.md

@@ -0,0 +1,25 @@
+## CMC
+
+**Formula**
+ 
+$[C6H7O2(OH) x (OCH2COONa)y]n$
+
+**Pyrotechnic use**
+
+Binder
+
+**Synonyms**
+ 
+Sodium carboxymethyl cellulose, CMC sodium salt, Sodium cellulose carboxymethyl ether, Cellulose gum, Cellulose glycolic acid sodium salt, Sodium cellulose glycolate
+
+**Description**
+ 
+An off-white fine powder, readily soluble in water. Can be used as a thickening agent and/or binder, likewise dextrin. CMC is commonly used as an abbreviation for Sodium Carboxy-Methyl Cellulose
+
+**Sources** 
+
+Hardware stores, as wallpaper adhesive.
+
+**Hazards**
+ 
+Fire hazard (dust), mild eye irritation, respiratory tract irritation, skin irritation/allergic dermatitis, non-toxic if ingested small amounts, do not induce vomiting.

chapters/99-1-chemical-colophonium.md

@@ -0,0 +1,27 @@
+## Colophonium
+
+**Formula**
+ 
+Mixture of compounds, mainly abietic acid, $C20O2H30$
+
+**Pyrotechnic use**
+
+Binder, fuel-binder.
+
+**Synonyms**
+ 
+Colophony resin, wood resin, pine resin
+
+**Description**
+ 
+Colophonium is an alcohol soluble resin which is sometimes used as a binder and as a fuel-binder combination . As such it is not used very often since it is expensive and doesn't have much adhesion capacity. Shimizu discerns two different types of colophony. One type is called wood resin and strongly smells of wood or somewhat like an aetheric oil. This is the common resin. Another type he names "combustion agent bl" in some of his books and this is sold as a natural phenolic resin called Vinsol, available at some pyro suppliers.
+
+**Sources** 
+
+Artist paint stores often sell colophonium. It is also used by violin players, for the treatment of wooden floors and in the paper industry.
+
+**Hazards**
+ 
+Xi
+
+Colophonium is not particularly toxic or dangerous.

chapters/99-1-chemical-copal-gum.md

@@ -0,0 +1,25 @@
+## Copal gum
+
+**Formula**
+ 
+Mixture of compounds
+
+**Pyrotechnic use**
+
+Alcohol soluble binder
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+An expensive yellowish-brown resin collected from Copal trees in East Indonesia. It is most likely an obsolete binder\auxiliary fuel that was previous used by the Chinese or Indonesians. Copal gum is soluble in alcohol.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+Copal gum is a non-carcinogenic material that is slightly flammable at high temperatures and has a health hazard rating of one.

chapters/99-1-chemical-copper-acetate.md

@@ -0,0 +1,31 @@
+## Copper acetate
+
+**Formula**
+ 
+$Cu(CH,3COO)2$
+
+**Pyrotechnic use**
+
+Blue colorant
+
+**Synonyms**
+ 
+Cupric acetate
+
+**Description**
+ 
+It has recently been used in some blue star formulas as a replacement for Paris green. Although it is sometimes said that the color is equally good, this remains doubtful since the acetate does not contain arsenic, which is essential in mediating the chlorine transfer to the copper.
+
+**Sources** 
+
+Simple synthesis
+
+Method 1: Cu(CH,3COO)2 can be produced by the reaction between Copper (II) oxide (CuO),Copper carbonate (basic) (CuCO3), and/or Copper hydroxide (Cu(OH)2) and Acetic acid (vinegar works). Evaporate to obtain crystals. These will be contaminated with Acetic acid, so dissolve and recrystallize them in distilled water to obtain purer product.
+
+Method 2: Dissolve copper metal in a warm Acetic acid by adding hydrogen peroxide or bubbling air through the solution. Evaporate to obtain crystals. These will be contaminated with Acetic acid, so dissolve and recrystallize them in distilled water to obtain purer product.
+
+Method 3: Dissolve Calcium carbonate in Acetic acid to form Calcium acetate. Add this slowly to a Copper sulfate solution to precipitate insoluble Calcium sulfate, leaving Copper acetate in solution. Filter and, if you want crystals, dry.
+
+**Hazards**
+ 
+TBD

chapters/99-1-chemical-copper-acetoarsenite.md

@@ -0,0 +1,25 @@
+## Copper acetoarenite
+
+**Formula**
+ 
+$Cu3As2O3Cu(C2H3O2)2$
+
+**Pyrotechnic use**
+
+Blue colorant
+
+**Synonyms**
+ 
+Paris Green
+
+**Description**
+ 
+Copper acetoarsenite is a green powder which is used in blue color compositions. It can produce great blues but it is also very poisonous and is used less and less for that reason. Today alternatives are available that will produce deep blues with less poisonous and cheaper compounds.
+
+**Sources** 
+
+Copper acetoarsenite was used in the past as a pigment known as emerald green, kings green or vienna green. Nowadays it is no longer used and it is very hard to find a paint supplier that still has it. It can be prepared at home but extreme caution must be excercised since arsenic compounds are very poisonous. The following preparation originates from Shimizu: "300 g of copper sulphate is dissolved in 1000 ml water, to which 250 g of glacial acetic acid is added; This solution is named 'A'. Then 200 g of sodium carbonate and 200 g of arsenious acid (comment: note that this is an aqueous solution of arsenic-III-oxide, which is a strong poison) are added to 1000 ml water and boiled to form a solution, this is named 'B'. B is added little by little to A with constant stirring. Carbon dioxide gas is generated with active bubbling. When all the solution B has been added, it is boiled for about 30 minutes, when copper acetoarsenite appears gradually as green particles in the solution. The mother liquor is removed by vacuum filtration, and then green substance, copper acetoarsenite, is washed with water untill the sulphate ion dissapears; it is then dried. The yield is about 180 g."
+
+**Hazards**
+ 
+Copper acetoarsenite is very poisonous and should only be handled wearing a dust mask. Smoke from compositions containing this compound should not be inhaled. It is best to avoid the use of this compound altogether as several safer alternatives have become available in the past decades.

chapters/99-1-chemical-copper-benzoate.md

@@ -0,0 +1,25 @@
+## Copper benzoate
+
+**Formula**
+ 
+$Cu(C6H5COO)2$
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Copper benzoate is a fuel which is used in some blue color compositions. It is not used very often as it is more expensive than most alternatives.
+
+**Sources** 
+
+Some specialised chemical vendors supply the material. Alternatively it can be manufactured without great difficulty via two different routes. In one, Benzoic acid and Copper carbonate are boiled in water until the reaction is complete. In the the other route, described in the following synthesis tutorial, the material is obtained from a solution of sodium or potassium benzoate and a soluble copper salt. When these solutions are added together a green precipitate of copper benzoate forms. This is filtered, thoroughly rinsed with hot water and left to dry.
+
+**Synthesis**
+
+TBD
+
+**Hazards**
+ 
+Copper benzoate is poisonous and should be handled wearing a dust mask

chapters/99-1-chemical-copper-carbonate.md

@@ -0,0 +1,28 @@
+## Copper carbonate
+
+**Formula**
+ 
+$CuCO3.Cu(OH)2$
+
+**Synonyms**
+ 
+Malachite
+
+**Description**
+ 
+A beautiful light blue to deeper blue powder, which sometimes is used as a pigment. Used as a blue flame colorant in low temperature class compositions of the potassium (per)chlorate base or in compositons of the ammonium perchlorate base. The resulting blue is weaker than that using Paris green or CuSO4.
+
+**Sources** 
+
+Pyro suppliers, ceramic supply store (used for glazing, ceramic grade copper carbonate sometimes might contain acidic impurities left from production and should therefore be tested).
+
+**Synthesis**
+
+Method 1: Dissolve a soluble copper compound (Copper acetate, Copper (II) chloride, or Copper sulfate for example) in as little distilled water as possible. Make a seperate solution of Sodium carbonate or Sodium bicarbonate in as little distilled water as possible. Mix these two solutions slowly and Copper carbonate will precipitate out. (if you are using Sodium bicarbonate there will be a lot of fizzing) Filter, wash with distilled water, and allow to dry without heating it. (sunlight is OK)
+
+Method 2: Add Copper hydroxide to Carbonic acid (tonic water) and Copper carbonate will precipitate out. Filter, wash with distilled water, and allow to dry without heating it. (sunlight is OK)
+**Hazards**
+ 
+Xn
+
+TBD

chapters/99-1-chemical-copper-chromite.md

@@ -0,0 +1,21 @@
+## Copper chromite
+
+**Formula**
+ 
+$CuCr2O4$
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Copper chromite is employed as a catalyst is certain rocket propellants. It is typically added in 1 to 5% quantities to whistle or composite rocket fuels which increases the burn rate. A range of other catalysts exist which can often be substituted for copper chromite. Examples are Iron oxide (red) and Manganese dioxide.
+
+**Sources** 
+
+Copper chromite is very hard to make or obtain other than from dedicated pyro chemicals suppliers.
+
+**Hazards**
+ 
+Copper chromite is poisonous and should be handled wearing a dust mask.

chapters/99-1-chemical-copper-i-chloride.md

@@ -0,0 +1,29 @@
+## Copper (I) chloride
+
+**Formula**
+ 
+$CuCl$
+
+**Synonyms**
+ 
+Cuprous Chloride, Cuprous monochloride, Nantokite
+
+**Description**
+ 
+CuCl is a white or green powder, the green color comes from oxidized impurities. It is insoluble in water, but soluble in hydrochloric acid. It is almost never used in pyrotechnics.
+
+**Sources** 
+
+TBD
+
+**Synthesis**
+
+Method 1: Boil an aqueous solution of Copper (II) chloride together with powdered or granulated copper metal. The copper (I) chloride will form in the water as a green powder. Filter it and dry.
+
+Method 2: Make a solution of Copper sulfate. Then add Sodium chloride and Potassium metabisulfite. When the reaction is finished you will see white Copper (I) chloride on the bottom of container. Then decant the supernatent solution to leave Copper (I) chloride. Wash it with Ethanol (water works well too) two or three times to obtain a purer product.
+
+Method 3: Pure white Copper (I) chloride can be produced from red Copper (I) oxide (Cu2O)and a stochiometric quantity of Hydrochloric acid. This method also produces soluble Copper (II) chloride (CuCl2). Too much Hydrochloric acid will convert the CuCl to CuCl2. The two chlorides, if done well, can be separated by simple decantation. Wash with water then dry.
+
+**Hazards**
+ 
+Xn, N

chapters/99-1-chemical-copper-ii-chloride.md

@@ -0,0 +1,33 @@
+## Copper (II) chloride
+
+**Formula**
+ 
+$CuCl2$
+
+**Pyrotechnic use**
+
+Blue colorant
+
+**Synonyms**
+ 
+Cupric Chloride,Copper Chloride, Campfire Blue
+
+**Description**
+ 
+Not to be mistaken with Copper-I-oxide, copper II chloride is a yellow-brown solid which slowly absorbs moisture to form a blue-green dihydrate. It is used as a color producing agent in some blue star compositions. It is also employed to achieve a blue fire in campfires by soaking wood chips in a water/copper chloride solution and throwing them in the fire. Another way is to sprinkle the powder into the flame. The boilling temperature of CuCl2 is very low thus it can create great blue fire at low temperature.
+
+**Sources** 
+
+TBD
+
+**Synthesis**
+
+Method 1: CuCl2 can be produced by the reaction between Copper (II) oxide (CuO),Copper carbonate (basic) (CuCO3), and/or Copper hydroxide (Cu(OH)2) and Hydrochloric acid. (Do not dilute the acid after dissolving otherwise Copper (I) Chloride will precipitate out) Evaporate to obtain crystals. These will be contaminated with HCl, so dissolve and recrystallize them in distilled water to obtain purer product.
+
+Method 2: Dissolve copper metal in a warm 15% Hydrochloric acid by adding hydrogen peroxide or bubbling air through the solution. Evaporate to obtain crystals. These will be contaminated with HCl, so dissolve and recrystallize them in distilled water to obtain purer product.
+
+Method 3 (Note: I have not tried this method. It will undoubtably be tricky to get right, but hopefully faster than the Method 2): Dissolve copper metal in FeCl3. Once as much copper as possible will dissolve, decant the solution. Evaporate this until light greenish blue CuCl2 crystals form, but not lime green FeCl2 crystals. These will be contaminated with FeCl2, so dissolve and recrystallize them in distilled water to obtain purer product.
+
+**Hazards**
+ 
+The gases produced from the burning of CuCl2 should be avoided. The compound itself is not very poisonous but careful handling is advisable.

chapters/99-1-chemical-copper-ii-oxide.md

@@ -0,0 +1,29 @@
+## Copper (II) oxide
+
+**Formula**
+ 
+$CuO$
+
+**Synonyms**
+ 
+Cupric oxide, black copper oxide
+
+**Description**
+ 
+Copper oxide is a black powder employed in blue color compositions in combination with chlorine donors. It is also used in high temperature thermite mixtures. (like crackling microstars) Cupric oxide is used in the ceramic industry for imparting blue, green or red tints in glasses, glazes and enamels. It is occasionally employed for incorporation in mineral supplements for insuring against an insufficiency of copper in the diet of animals. Among its other uses is the preparation of copper ammonium hydroxide solutions for the rayon industry.
+
+**Sources** 
+
+Copper(II)oxide is usually available from ceramic supply stores.
+
+**Synthesis**
+
+Method 1: Add a solution of sodium or potassium hydroxide to a hot solution of a soluble copper(II) compound (Copper sulfate or Copper (II) chloride for example). This will yield a blue gel-like precipitate of Copper hydroxide. Then bring the solution to a boil. The precipitate will turn black and powdery. Boil for a minute or two to complete the reaction and allow the black copper (II) oxide precipitate to settle. Then decant the liquid. Add some boiling hot water to the precipitate, stir and allow to settle again. Then decant and repeat 5 more times. This will remove all soluble impurities from the copper(II)oxide. Then the precipitate is filtered and allowed to dry.
+
+Method 2: Electrolysis of a oxidizing solution like chlorate solution yield copper (II) oxide as long as enough chlorate is present. The chlorate, sadly, convert back to chloride in this process. The result salt can be decanted and washed 3-4 times for purity. Other oxidizing soluble salts like bleach (Sodium hypochlorite) can be used. Once the oxidizing substance is depleted, the electrolysis will form Copper (I) oxide (Cu2O) which can be turned into Copper (II) oxide by roasting it in air.
+
+Method 3: Heat dry Copper hydroxide to 185oC, wet Copper hydroxide to 80oC, or Copper carbonate (basic) to 290oC.
+
+**Hazards**
+ 
+Copper(II)oxide is harmful and should be handled wearing a dust mask.Copper(II) oxide is an irritant. It also can cause damage to the endocrine and central nervous system. Contact to the eyes can cause irritation and damage to the corneas, and potentially can cause conjunctivitis. Contact to the skin can cause irritation and discoloration. Ingesting cupric oxide can lead to central nervous system depression, liver and kidney damage, gastrointestinal damage, circulatory system failure or damage to the vascular system. Inhalation can lead to damage to the lungs and septum. Inhalation of fumes of cupric oxide can lead to a disease called metal-fume fever, which has symptoms similar to influenza. Prolonged exposure to cupric oxide can lead to dermatitis, and can cause a toxic build-up of copper in people with Wilson's disease. Handling copper(II) oxide should be done in well ventilated area, and care should be taken to avoid contact with the skin or eyes. After handling, one should wash thoroughly.

chapters/99-1-chemical-copper-oxychloride.md

@@ -0,0 +1,32 @@
+## Copper oxychloride
+
+**Formula**
+ 
+$[3CuO.CuCl2•3.5H2O]$
+
+**Pyrotechnic use**
+
+Blue colorant
+
+**Synonyms**
+ 
+Copper(II)oxychloride, tricopper chloride trihydroxide, copper chloride oxide hydrate
+
+**Description**
+ 
+Copper oxychloride is a green powder used as blue color agent, is a basic copper chloride and is usually manufactured either by the action of hydrochloric acid on copper metal or by the air oxidation of cuprous chloride suspensions. It has a number of applications, by far the most important being as an agricultural fungicide, for which purpose it is extensively employed in formulated form as dusts, wettable powders and pastes.
+
+**Sources** 
+
+Pyro suppliers such as Skylighter.
+
+**Synthesis**
+
+Copper oxychloride can be produce easily at home from metallic copper. First, the electrolysis of copper anode in KCl/NaCl solution, will yield copper I oxide (red). The oxide is washed to remove alkali ion by repeated decantations. Then hydrochloric acid is mixed with the washed oxide in a very stochiometric quantity. Not enough is best and easier but yield impure end product. The solution is then bubbled through with air to convert CuCl to Oxychloride and CuCl2 following this reaction:
+
+6 CuCl + 3/2 O2 + 3 H2O → 2 Cu3Cl2(OH)4 + CuCl2
+This process can take more than 2 day with an aquarium pump. Be sure to recover and boil down CuCl2 produce too.
+
+**Hazards**
+ 
+Harmful if swallowed or inhaled. Overexposure can lead to nausea, diarrhea, gastrointestinal distress, headaches, weakness, and possible liver and kidney damage. May cause irritation of eyes, nasal passages, throat and skin.

chapters/99-1-chemical-copper-sulfate.md

@@ -0,0 +1,36 @@
+## Copper sulfate
+
+**Formula**
+ 
+$CuSO4.5H2O$
+
+**Synonyms**
+ 
+Copper sulfate, cupric sulfate, blue vitriol, bluestone, Chalcanthite
+
+**Description**
+ 
+Copper(II) sulfate is the chemical compound with the formula CuSO4. This salt exists as a series of compounds that differ in their degree of hydration. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate, the most commonly encountered salt, is bright blue. It is used as a blue flame colorant in ammonium perchlorate based compositions where it sometimes substitutes the more expensive Paris green. The resulting blue color is almost as good as with the latter. It is not easily scattered and not anywhere near as toxic. Small amounts of copper sulfate are contained even in mineral waters. Copper sulfate can be used as a minor oxidizer and in combination with finely powdered Mg can be used as a pressure sensitive composition due to the waters of hydration (this is very unstable though). Copper sulfate is not good for colored flash experimentation,though.
+
+**Sources** 
+
+Pyro suppliers, paint stores, drugstore (in Europe at least it can be bought to keep your pool clean, works great for that purpose) is also available as a copper patina for stained glass. (must be evaporated as it is in a solution) may also be available as a fungicide for gardens depending upon the demographic in your area.
+
+**Synthesis**
+
+Copper sulfate can be produced by the use of a "piranha" solution.
+
+H2SO4+H2O2+Cu--->CuSO4x5H2O
+
+  
+Copper sulfate can also be synthesized by electrolysis of a solution of sulfuric acid with a copper anode, which forms H2 gas at the cathode and CuSO4 by the following reaction.
+
+Cu(s)+2H+(aq)--->Cu2+(aq)+H2 (g)
+
+The sulfate from the sulfuric acid is unchanged by this reaction, giving an end product of a solution of CuSO4. This must be done with an excess of sulfuric acid, since when the acid is depleted this will begin to form a mixture of Cu(OH)2 and CuO.
+
+**Hazards**
+
+N, Xn, Xi
+
+Due to its acidic nature it must not be used together with chlorates or phosphorus. Nonetheless it can be used with perchlorates or nitrates. Copper sulfate is toxic and used in lakes to kill sea weed.

chapters/99-1-chemical-copper.md

@@ -0,0 +1,25 @@
+## Copper
+
+**Formula**
+ 
+$Cu$
+
+**Pyrotechnic use**
+
+Fuel
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+ 
+Copper powder is a rusty orange colored fine powder which was used not so long ago in the manufacture of stars to achieve a green and blue colors. Atomized powder is particularly well suited to the strobe applications. It is no longer used today as it is replaced with chemicals like barium and copper oxides.
+
+**Sources** 
+
+Copper powder can be purchased through craft or ceramic stores.
+
+**Hazards**
+ 
+The metal, when powdered, is a fire hazard. At concentrations higher than 1 mg/L, copper can stain clothes and items washed in water.

chapters/99-1-chemical-cryolite.md

@@ -0,0 +1,25 @@
+## Cryolite
+
+**Formula**
+ 
+$Na3(AlF6)$
+
+**Synonyms**
+ 
+Sodium Aluminum Fluoride, Sodium fluoaluminate
+
+**Description**
+ 
+Used as a non-hygroscopic yellow colouring agent in some star compositions.
+
+**Sources** 
+
+Pyrotechnic supplies, such as skylighter.
+
+**Hazards**
+
+T, N
+
+_Acute_: Poison by ingestion. Large doses of overexposure cause severe nausea, vomiting, diarrhea, abdominal burning and cramp-like pains. Contact with skin and eyes may cause irritation. Inhalation can cause irritation to mucous membranes and respiratory tracts. 
+
+_Chronic_: May cause fluorosis, which is a condition affecting the bones and teeth.

chapters/99-1-chemical-dechlorane.md

@@ -0,0 +1,24 @@
+## Dechlorane
+
+**Formula**
+
+$C10Cl12$
+
+**Pyrotechnics use**
+
+Chlorine donor
+
+**Synonyms**
+
+Mirex
+
+**Description**
+
+Sold under the name Mirex, was used as a insecticide until banned. It can be used as an exotic Chlorine donor, which while effective, has been banned in fireworks by many authorities due to the toxicity.
+
+**Sources** 
+
+
+**Hazards**
+ 
+Prolonged and repeated exposure to Mirex can result in damage to the liver and it can enter the body via inhalation, ingestion, and absorption via skin. Any contact should be avoided and appropriate safety precautions should be taken.

chapters/99-1-chemical-dextrin.md

@@ -0,0 +1,26 @@
+## Dextrin
+
+**Formula**
+
+Mixture of polysaccharides.
+
+**Pyrotechnics use**
+
+Binder (water soluble)
+
+**Synonyms**
+
+ TBD
+
+**Description**
+
+Dextrin is one of the most commonly used binders in pyrotechnics as it is very cheap and readily available. It is water-soluble and can produce rock hard stars. Its cohesive power is weaker than that of SGRS anyway. Dextrin should not be used in a very damp climate as the stars tend to get wet rather than non-dextrin stars. Western pyrotechnics uses dextrin rather than SGRS, while the former is not popular in Japan and China.
+
+**Sources** 
+
+Dextrin is easily prepared from starch. Potato and cornstarch will both work fine. The starch is spread out on a sheet in a layer about 1 cm thick and placed in the oven. The oven is then heated to 220°C (400°F) for several hours. The dextrin will turn slightly yellowish brown. One way to check if all the starch has been converted is to dissolve a small sample in boiling hot water and add a drop of KI3 solution (Lugol's iodine solution). A blue colour indicates presence of starch, which means the conversion hasn't completed yet. KI3 solution is conveniently prepared by dissolving a crystal of elemental iodine in a potassium iodide solution.
+
+**Hazards**
+
+Dextrin is not particularly toxic or dangerous.
+

chapters/99-1-chemical-dextrose.md

@@ -0,0 +1,25 @@
+## Dextrose
+
+**Formula**
+
+$C6H12O6$
+
+**Pyrotechnics use**
+
+Fuel
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+In pyrotechnics, Dextrose is primarily used as a fuel in Candy propellant. It does not caramelize as readily as Sucrose, and it is somewhat less hygroscopic. It can be utilized as its monohydrate or it can be desiccated into it's anhydrous form. See Nakka's rocketry page for more information.
+
+**Sources** 
+
+Dextrose is available as weightlifting dietary supplement.
+
+**Hazards**
+ 
+Dextrose is not particularly toxic or dangerous.

chapters/99-1-chemical-ethanol.md

@@ -4,6 +4,10 @@
  
 $C2H5OH$
 
+**Pyrotechnics use**
+
+Solvent
+
 **Synonyms**
  
 Alcohol, Undenatured Alcohol, Ethyl Alcohol, Dehydrated Alcohol, Spiritus
@@ -18,4 +22,4 @@ Chemically pure ethanol can be quite expensive due to increased tax, unless it i
 
 **Hazards**
  
-Ethanol is flammable and volatile. Ethanol vapour is heavier than air and spreads over the ground. Provide adequate ventilation when working with ethanol.
+Ethanol is flammable and volatile. Ethanol vapour is heavier than air and spreads over the ground. Provide adequate ventilation when working with ethanol.

chapters/99-1-chemical-ferro-silicon.md

@@ -0,0 +1,25 @@
+## Ferro-silicon
+
+**Formula**
+
+Sometimes written $FeSi$
+
+**Pyrotechnics use**
+
+TBD
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Alloy of iron and silicon. Comes as a powder with a black grey metallic lustre. Reacts with and dissolves in alkali solution generating hydrogen gas. Shows no reaction with acids. Mainly used as fuel in red thermite (high temperature ignition composition), where the heat of combustion generally increases with the Si content. Commercial standards discern 6 classes of the material, of which class one shows the highest Si-content (88-93%) and is therefore recommended for fireworks use. Differences between classes are quite large: e.g. class 3 shows only about 45% of Si.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+TBD

chapters/99-1-chemical-ferro-titanium.md

@@ -0,0 +1,26 @@
+## Ferro-titanium
+
+**Formula**
+ 
+Fe-Ti (60%-40%)
+
+**Pyrotechnics use**
+
+Spark effect
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+
+An alloy of iron and titanium. Granular, silvery powder. Gives yellow-white sparks. Used in fountain, or palm-tree comet-type star compositions.
+
+**Sources** 
+
+Pyrotechnic supplies, such as skylighter.
+
+**Hazards**
+
+See iron and titanium.
+

chapters/99-1-chemical-glass.md

@@ -0,0 +1,24 @@
+## Glass
+
+**Formula**
+ 
+
+**Pyrotechnics use**
+
+Striker composition ingredient
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+It finds only little use in pyrotechnics, where it is generally contained in striker compositions (to provide initial energy caused by friction). Glass powder is an important ingredient in safety matches.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+Glass powder, or dust, is an irritant to the lungs and eyes. The same precautions for asbestos apply. Glass powder in the lungs will cause scaring and silicosis, an incurable and painful affliction. Respirator and eyes goggles required.

chapters/99-1-chemical-graphite.md

@@ -0,0 +1,25 @@
+## Graphite
+
+**Formula**
+
+$C$
+
+**Pyrotechnics use**
+
+TBD
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Graphite is a black and shiny powder or rods. Used for glazing black powder grains to give it a better flow, or as dry lubricant for different tools. Also used to opacify rocket fuel grains. The opacifier accelerates the rate of surface burning and prevents infrared energy from penetrating the propellant grain and causing it to explode.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+TBD

chapters/99-1-chemical-guanidine-nitrate.md

@@ -0,0 +1,27 @@
+## Guanidine nitrate
+
+**Formula**
+
+$NH:C(NH2)2.HNO3$
+
+**Pyrotechnics use**
+
+Oxidizer
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+
+White crystals. It is quite stable against shock and friction and not hygroscopic. It is used in some strobe compositions where it is decomposed by copper salts or other compounds acting as catalysts. Some smoke formulas employ guanidine nitrate. It also found use in toy rocket fuels such as JETEX and may be found in some explosives. It is quite attractive because it has a high gas output, low flame temperature, and non-toxic combustion products.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+
+O, Xn
+ 
+

chapters/99-1-chemical-gum-arabic.md

@@ -0,0 +1,27 @@
+## Gum arabic
+
+**Formula**
+
+Mixture of compounds
+
+**Pyrotechnics use**
+
+Binder
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+This gum resin, also known as Acacia gum, is obtained mainly from acacia wood and is produced in Many hot dry areas of the world, mainly Sudan, the rest of the Horn of Africa, Southern Arabia, and India. The resin occurs in colourless, yellowish or brown pieces, and is largely protein based. Gum Arabic is soluble in water and alcohol, or a mix of the two. Gum Arabic solutions tend to ferment during storage and become acidic. Therefore they are generally consumed within one day after manufacture while old adhesives are discarded for safety reasons. It is usual to employ the gum with gunpowder type compositions only, and is generally thought to be the best adhesive for Black match and Quick match manufacture.
+
+In strength of binding, Gum Arabic is superior to most other binders. Stars made with three to five per cent Gum Arabic are suitable for hard flash breaks.
+
+**Sources** 
+
+Gum Arabic may be bought in artistic painting supply stores alongside other binders like Red gum. It can also be obtained from stores that supply conservators - like shellac or red gum, it is sometimes used to seal wood surfaces. Gum Arabic is most commonly used in gummy sweets and soft drinks, though extraction from a can of coke is a process that the author does not think would be effective, and has never heard of being attempted.
+
+**Hazards**
+
+Gum Arabic is not particularly dangerous or toxic under normal conditions, but Gum Arabic solutions tend to ferment during storage, and become acidic. Therefore, they are generally consumed within one day after manufacture while old adhesives are discarded for safety reasons. Due to this, Gum Arabic is not to be used with compositions containing chlorates, under any circumstance.

chapters/99-1-chemical-hexachlorobenzene.md

@@ -0,0 +1,26 @@
+## Hexachlorobenzene
+
+**Formula**
+
+$C6Cl6$
+
+**Pyrotechnics use**
+
+Chlorine donor
+
+**Synonyms**
+ 
+HCB
+
+**Description**
+
+Hexachlorobenzene (HCB) has been used as a powerful chlorine donor in colour compositions. It is soluble in diethyl ether, benzene, ethanol and chloroform. It can not serve as a binder.
+
+**Sources** 
+
+The use of HCB must be avoided.
+
+**Hazards**
+
+HCB is very toxic to aquatic organisms and it may cause long term adverse effects in the aquatic environment. Hexachlorobenzene has a half life in the soil of between 3 and 6 years. Biomagnification up the food chain does occur.
+

chapters/99-1-chemical-hexachloroethane.md

@@ -0,0 +1,27 @@
+## Hexachloroethane
+
+**Formula**
+
+$C2Cl6$
+
+**Pyrotechnics use**
+
+Chlorine donor, Smoke compositions
+
+**Synonyms**
+
+Carbon hexachloride
+
+**Description**
+
+It is a colourless material that slowly sublimes at room temperature producing a special odour. Carbon hexachloride would be a strong chlorine donor (about 90% chlorine) but due to its volatility it is not often used to enhance the flame of colored stars or flares. Together with zinc powder, Al or Mg it finds some use in white smokes though which are sealed in a tin case where volatility is no problem. The material on the market is larger grains from 3-5mm and these should be crushed to pass 20 mesh before use in smoke compositions. Both material and compositions containing HCE must be kept sealed after mixing.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+Xn, N
+
+Note that HCE is listed as a contact poison, which can enter the body through inhalation, food or skin contact! Take the necessary precautions (breathing mask, gloves). The volatile gases can lead to absence!

chapters/99-1-chemical-hexamine.md

@@ -0,0 +1,24 @@
+## Hexamine
+
+**Formula**
+ 
+$(CH2)6N4$
+
+**Pyrotechnics use**
+
+Fuel
+
+**Synonyms**
+
+Hexamethylenetetramine, Urotropine
+
+**Description**
+
+Crystals of hexamine burn with a yellow flame and the material has been used in small indoor fireworks employing magnesium and lithium salts. In contrast to metaldehyde formerly used for this purpose it does not produce poisonous formaldehyde when lighted indoors. Lancaster states that "hexamine would be quite useful as a fuel, but does not appear to have found much application, possibly because of the cost." (Fireworks PaP p.111) Some armys employ ESBIT fuel to allow the soldiers to cook their meals while in field. Hexamine is the main ingredient. Soluble in water.
+
+**Sources** 
+
+
+**Hazards**
+ 
+F, Xn

chapters/99-1-chemical-hydrochloric-acid.md

@@ -0,0 +1,27 @@
+## Hydrochloric acid
+
+**Formula**
+
+$HCl$
+
+**Pyrotechnics use**
+
+None
+
+**Synonyms**
+
+Hydrogen chloride, muriatic acid
+
+**Description**
+
+HCl is a gas which when dissolved in water is an acid by dissociation producing H3O+ and Cl-. It can be used in the synthesis of Ammonium chloride or other chloride salts. Is a strong halogenating compound, and one of the strongest acids that normal people can aquire.
+
+**Sources** 
+
+Hydrochloric acid is available in hardware stores and paint shops in litre quantities to a reasonable price, it is used as a concrete cleaner as it chlorinates the calcium carbonate into water soluble Calcium Chloride and hydrogen gas.
+
+**Hazards**
+ 
+Hydrochloric acid is an irritant in low concentrations, but becomes more corrosive in concentrations above 25%. In solutions with high concentrations, some of the hydrogen ions and chlorine ions, which are separated while dissolved, combine and rise out of the solution as a gas. This gas almost immediately dissolves in the water in the air, and appears as a white mist. This mist is corrosive to the skin and unhealthy to breathe in. If the air is very dry, it will come out as a gas but not be visible as mist, this is still dangerous though as it turns back to acid as soon as it gets in contact with the water in your body.
+
+A well ventilated workshop and a chemical resistant labcoat is recommended for the use of HCl(a) as the gas fuming off will replace the hydroxyl groups of cellulose (cotton, that means clothing) with chlorine causing degradation and further fuming of HCl off the clothing contaminated. It must be noted that if clothing is contaminated with HCl you must not wash it as it will dissolve the clothes in the wash.

chapters/99-1-chemical-iron-oxide-black.md

@@ -0,0 +1,26 @@
+## Iron oxide (black)
+
+**Formula**
+ 
+$Fe3O4$
+
+**Pyrotechnics use**
+
+Oxidizer (high temperature)
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+
+Black Iron Oxide is a black powder. It is sometimes used in thermite however thermite produced using black iron oxide is less powerful than thermite that uses red iron oxide. It is also a catalyst and can be used in R-Candy. It is magnetic.
+
+**Sources** 
+
+
+**Hazards**
+
+It is a skin and eye irritant and gloves and eye protection should be warn when handling.
+ 
+

chapters/99-1-chemical-iron-oxide-red.md

@@ -0,0 +1,25 @@
+## Iron oxide (red)
+
+**Formula**
+
+$Fe2O3$
+
+**Pyrotechnics use**
+
+Catalyst
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Red iron oxide is used as a catalyst in composite and whistling rocket propellant and Candy rocket propellant formulations. It is also added to some glitter formulations and used for thermite, a mixture that produces enormous amounts of heat, forming molten iron. Due to it's catalytic properties it is also added to primes, and even coloured star compositions to increase their ignitability and burn rate.
+
+**Sources** 
+
+Common rust is not iron oxide. It is a mixture of oxides and hydroxides. A cheap source for red iron oxide is the ceramics supply shop. It is also bought as cement color in hardware stores for about $5.00 a pound.
+
+**Hazards**
+ 
+Red iron oxide is not particularly toxic or dangerous. It does however stain surfaces and textiles.

chapters/99-1-chemical-iron.md

@@ -0,0 +1,26 @@
+## Iron
+
+**Formula**
+
+$Fe$
+
+**Pyrotechnics use**
+
+Yellow spark effect
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Iron powder is used for spark effects, mainly in fountains and sparklers. It produces golden yellow branching sparks. Not every iron alloy will work equally well. Iron alloys with a high carbon content generally work best. Stainless steel will produce hardly any sparks.
+
+**Sources** 
+
+Iron turnings can often be had for free from places were iron is used for construction. Drilling, sawing etc produces a powder with wide range of particles. This powder is treated with mineral oil to remove oil and grease, sieved, and then coated with linseed oil.
+
+**Hazards**
+
+Iron particulates of micron-submicron size are pyrophoric (may spontaneously ignite on contact with air). Care should be exercised with this particularly reactive form of iron. Iron needs to be protected before use in pyrotechnic compositions. Otherwise it will corrode and render the composition useless or even dangerous. Iron containing compositions are generally best kept dry and not bound with water soluble binders. Iron can be coated with linseed or tung oil. The latter was used in ancient China (and may still be used today). Linseed is very convenient to use and easy to obtain. Blackpowder-like compositions (ie Charcoal/sulfur/saltpeter based) with added metal, such as they are often used in fountains, are more sensitive than the composition without added metal. Extra caution, especially when pressing or ramming, should be excersised.
+

chapters/99-1-chemical-isopropyl-alcohol.md

@@ -0,0 +1,27 @@
+## Isopropyl alcohol
+
+**Formula**
+ 
+$CH3CHOHCH3$
+
+**Pyrotechnics use**
+
+Solvent
+
+**Synonyms**
+ 
+IPA, 2-propanol, isopropanol
+
+**Description**
+
+Isopropyl alcohol is a common name for propan-2-ol, a colourless, flammable chemical compound with a strong odor. Isopropanol is the main ingredient in rubbing alcohol and is used as a disinfectant, and is a common solvent. In pyrotechnics it is commonly mixed with water. The isopropanol alcohol reduces the surface tension in a mixture and makes the water actually "wetter". This increases the absorption rate much faster than it would with just plain water.
+
+**Sources** 
+
+It can be easily bought from supermarkets, pharmacies, and chemists in the form of isopropanol rubbing alcohol.
+
+**Hazards**
+
+Isopropyl alcohol is flammable. It should be kept away from heat and open flame. Isopropyl alcohol is oxidized by the liver into acetone. Symptoms of isopropyl alcohol poisoning include flushing, headache, dizziness, CNS depression, nausea, vomiting, anaesthesia, and coma. Use in well-ventilated areas and use protective gloves while using. Poisoning can occur from ingestion, inhalation, or absorption.
+ 
+

chapters/99-1-chemical-lactose.md

@@ -0,0 +1,25 @@
+## Lactose
+
+**Formula**
+
+$C12H22O11.H2O$
+
+**Pyrotechnics use**
+
+Fuel
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Lactose is extensively used as a combustion agent in colored smoke compositions containing organic dyes. Sometimes it finds use also as a fuel in blue color compositions, where cool burning is required.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+Lactose is not particularly toxic or dangerous.

chapters/99-1-chemical-lampblack.md

@@ -0,0 +1,28 @@
+## Lampblack
+
+**Formula**
+
+Mixture of carbon 
+
+**Pyrotechnics use**
+
+Streamer spark effect
+
+**Synonyms**
+
+Pine black, oil black, pine soot
+
+**Description**
+
+Lampblack is obtained by the incomplete burning of pine wood and the resulting very fine powder usually passes 350 mesh. The work with it is known for its extreme dirtyness. Due to its fineness it easily spreads into every mixture, even at small amounts. It might be used as a component of BP and the force of the resulting powder is large. Small amounts of lampblack are included in various compositions to enhance ignitability and effect. Lampblack is one of the main components of flower pots and moreover contributes to the Senko Hanabi effect. Some of the best and longest lasting (japanese quality) golden streamer stars can be manufactured with it. Lampblack is not easily damped and therefore it is advisable to add a small amount of alcohol (reduces surface tension) to make moistening easier. The major defect is its high price.
+
+It must be noted that lampblack adheres to the mesh and consequently can´t be sieved on its own. Nonetheless it passes the mesh well when accompanied by other materials used for the same composition. In this case it spreads quite well into every mixture and therefore small amounts of lampblack are employed in various star compositions for ease of ignition.
+
+**Sources** 
+
+Pyro suppliers only
+
+**Hazards**
+
+Do not breathe as it is a suspected carcinogen.
+

chapters/99-1-chemical-lead-tetraoxide.md

@@ -0,0 +1,26 @@
+## Lead tetraoxide
+
+**Formula**
+ 
+$Pb3O4$
+
+**Pyrotechnics use**
+
+**Synonyms**
+ 
+Lead minium, Minium, Triplumbic tetroxide, Red lead, Lead tetroxide
+
+**Description**
+
+Lead tetraoxide is primarly used to make crackling microstars. The composition is very sensitive, explosive and poisonous. It is in fact one of the most dangerous compounds used commonly in modern pyrotechnics. Alternative crackling mixtures e.g. based on bismuth trioxide exist (which is less poisonous), but the high price of bismuth trioxide generally restricts its use. Together with ferro-silicon minium is the original "red thermite".
+
+**Sources** 
+
+Lead tetraoxide may be prepared from a solution of lead nitrate and sodium hydroxide. Note that the procedure involves extremely corrosive and poisonous chemicals and should only be attempted by those who have access to (and know how to use) the right equipment and can handle the waste properly. Prepare a concentrated solution of sodium hydroxide by dissolving 300 grams of sodium hydroxide in water. The solution will heat up during this. To prevent it from boiling suddenly add only small portions at a time. When all has dissolved, allow it to cool down to room temperature. Dissolve 50 grams of lead nitrate in 200 ml of water, and slowly add the sodium hydroxide solution to this solution while stirring continuesly. A white precipitate will form first, which will turn orange when all sodium hydroxide solution has been added. Stir this solution well for another hour, and then allow the lead tetraoxide to settle. Carefully decant the supernatant, add boiling hot water to the residue, stir, allow to settle and decant again. Repeat this 5 more times. Then filter and rinse the lead tetraoxide in the filter several times with hot water.
+
+**Hazards**
+
+T, N
+
+Lead tetraoxide, like most lead compounds, is extremely poisonous. Lead is an accumulative neurotoxin and extreme care should be taken to prevent direct contact. Lead tetraoxide may be absorbed by inhalation and ingestion. Wear a respirator, gloves, and protective clothing.
+

chapters/99-1-chemical-linseed-oil.md

@@ -0,0 +1,26 @@
+## Linseed oil
+
+**Formula**
+
+TBD
+
+**Pyrotechnics use**
+
+Metal powder coating
+
+**Synonyms**
+ 
+Flax seed oil
+
+**Description**
+
+Linseed oil is made from the seed of the flax plant. Available in many forms: Brown, boiled, raw and refined. It is used to coat various metal powders or filings you want to keep from oxidizing or reacting with other chemicals. The coating preserves the metal with a varnish coating. Adding some solvent will help distribute the oil and ensure complete coating. You must screen your metals while drying, otherwise it will turn into hard clumps. The cheapest form (usually boiled) is suitable for fireworks.
+
+**Sources** 
+
+Linseed oil products are available at paint and hardware stores.
+
+**Hazards**
+
+Rags dampened with boiled linseed oil are a fire hazard, because they provide a large surface area for oxidation of the oil. The oxidation is an exothermic reaction which thermal runaway accelerates as the rags get hotter. Such rags should be washed, soaked with water or incinerated to avoid unexpected spontaneous combustion.
+

chapters/99-1-chemical-magnalium.md

@@ -0,0 +1,31 @@
+## Magnesium
+
+**Formula**
+
+Alloy of magnesium and aluminum, usually 50:50. Sometimes written: $MgAl$
+
+**Pyrotechnics use**
+
+Fuel
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Magnalium is a very brittle alloy of magnesium and aluminum. Some common uses are in for spark effects, in strobing compositions and in crackling stars. Lancaster gives some typical mesh sizes for different uses: Magnalium used for strobe stars, for spark effects or to enhance other stars has to be finer than 120 mesh, while for use in crackling microstars it has to be something between 30 and 50 mesh. The coarser type is generally harder to find commercially. Magnalium can also be substituted into most mixtures that aluminium finds use in. These include; thermite and flashpowder. Again, avoid unstable combinations, and remember that MgAl is very reactive.
+
+**Sources** 
+
+The best sources for magnesium are sacrificial anodes. These find use in water cylinders, and general rust prevention. Aluminum is found easily as scrap which can be melted down. Magnalium can be made at home, but it is best to become familiar with molten metals, so prior experience with aluminum(or other foundry work)is recommended. Plan well and prepare yourself for working with molten metals that may ignite if you plan to make it at home. If the metal ignites expect it to burn very brightly and hot. Explosions will not occur if you restrict production batches to under 600g, and if common sense is used. Do it outside and away from anything flammable. If it ignites, pour sand or dirt onto it. However, if it is overly large, it might be best to let it burn out. Never use water. A sand/dirt bed around the smelting area is a cheap and wise precaution, as molten MgAl will burn through asphalt and damage concrete. Don't look directly into the burning metal as it may damage your eyes. Start by melting aluminum in a steel can(baked bean size is preferrable).
+
+The molten metal should be covered with a blanket of inert gas. In this case neither nitrogen nor carbon dioxide will function as an inert gas. It is not best to get a cylinder of argon gas at a welding supply store, as it wont be needed whatever way you look at it. It will be useless unless blanketing the MgAl inside the can(it will blow away on the ground)and it isnt cheap for the canister, or argon. You can use sulfur or charcoal, but these are usually not needed unless it starts burning out of control(which is shouldnt, because the oxide layer is generally thick, and there is scarcely enough oxygen in the can to allow further burning). Sulfur will make you MgAl smell like rotten eggs, along with causing a nasty flare up the first time it is applied. One pinch is all that is needed. The best choice is to keep powdered charcoal at hand, and to fashion a reusable lid for the can to stop oxygen getting in. The bottom of a larger can is useful for this, and can easily be reused.
+
+Using an electric furnace for the melting is very convenient and allows good control over the temperature. Alternatively, a cheap charcoal chimeny or charcoal furnace with a steel can in it will work too(a can is best, as you can peel it away from the ingot when done, using tinsnips). Be careful if using a aluminum furnace, as having the can hotter than orange can cause cracks in the can, allowing molten MgAl to pour into the coals(once it has started leaking, you have little hope in stopping it, so take it out and place it into a pail of sand. Regulating the air flow on the charcoal is the best solution. To the molten aluminum, magnesium is added in solid form. The melt should be stirred from time to time. When all the magnesium has melted,the can is removed and the melt is allowed to solidify.
+
+Once out of the furnace it is wise to sprinkle a layer of powdered charcoal on top of the melt to act as an inert blanket to stop oxygen meeting the melt. When cool, it is then easily crushed up in smaller chunks with an heavy hammer. These chunks are ground in a blender or coffee grinder. It can also be ball milled into a fine powder using steel media but this can be dangerous since the metal powder can become pyrophoric(if ball milled for overly long). Ceramic alumina media comes in handy here, as it does not spark.
+
+**Hazards**
+ 
+Magnalium dust is harmful and a dust mask should be worn when handling fine dust. Mixtures containing nitrates or ammonium perchlorate and magnalium sometimes heat up and may ignite spontaneously, especially when moist. Coating magnalium with linseed oil will prevent reaction with nitrates, but this treatment does not protect the magnalium from ammonium perchlorate. Only treating the magnalium with potassium dichromate will prevent this reaction. This is done by boiling the magnalium in a 5% potassium dichromate solution. Adding fine potassium dichromate powder to such compositions may also help. Take note that military flash bangs use Ammonium perchlorate and magnesium mixtures, but making these is only to be attempted by experienced pyrotechnicians.

chapters/99-1-chemical-magnesium.md

@@ -0,0 +1,27 @@
+## Magnesium
+
+**Formula**
+
+$Mg$
+
+**Pyrotechnics use**
+
+Fuel
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+
+Magnesium powder is used in a wide variety of compositions, both for spark effects and 'normal' fuel purposes. Relatively coarse magnesium is used for spark effects. In flares and some bright colored star compositions it functions as a normal fuel. It is superior to aluminum in color compositions since MgCl2 and MgO are more easily vaporised than the corresponding aluminum compounds. This reduces the amount of black-body radiation and improves the color purity.
+
+**Sources** 
+
+Magnesium powder is available from dedicated pyro suppliers. Making magnesium at home is very difficult. Magnesium can be bought in boating supply stores. It is used to prevent corrosion of a ships hull. For that purpose it is welded to the hull. The lower position of magnesium in the electrochemical series will make the magnesium corrode before the steel will. Making such a block of magnesium into a fine powder will not be easy. Filing or cutting and ball milling may be tried. Ball milling of metals can be dangerous however since the metal can become pyrophoric. However, if a person is to drill a lot of holes and collect the shavings, these may be ball milled quite easily.
+
+**Hazards**
+
+F
+
+Magnesium dust is harmful and a dust mask should be worn when handling fine dust. Mixtures containing nitrates, chlorates or perchlorates and magnesium sometimes heat up and may ignite spontaneously, especially when moist. Coating magnesium with linseed oil will prevent reaction with most oxidizers, but this treatment does not protect the magnesium from ammonium perchlorate. Only treating the magnesium with potassium dichromate will prevent this reaction. This is done by boiling the magnesium in a 5% potassium dichromate solution. The magnesium will turn brown when this is done. Adding fine potassium dichromate powder to such compositions may also help.

chapters/99-1-chemical-manganese-dioxide.md

@@ -0,0 +1,25 @@
+## Manganese dioxide
+
+**Formula**
+
+$MnO2$
+
+**Pyrotechnics use**
+
+Catalyst
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Manganese dioxide can be used as a catalyst in composite and whistling rocket propellant formulations. A thermite-like mixture can also be made with it. The manganese dioxide thermite burns more slowly than the iron oxide based mixture with a bright white glow.
+
+**Sources** 
+
+Mangese dioxide can be obtained from old batteries or from the ceramics supply store. The mangese dioxide in batteries is mixed with several other compounds from which it must be separated. An easy, though messy way to do this is as follows: Find a couple of depleted carbon-zinc batteries. Only carbon-zinc type batteries will do. Do not use other types such as rechargable or lithium based batteries. These, especially the rechargable ones, contain extremely dangerous and/or poisonous compounds such as cadmium, mercury and metallic lithium. Carbon-zinc batteries may contain small amounts of mercury as well, especially the older types, so precautions should be taken to prevent skin and eye contact and to prevent breathing or swallowing of dust. So: wear your dust mask, glasses, gloves and old clothing. Then carefully take the battery apart. You'll find a greyish white (zinc oxide) or metallic coating (zinc metal) inside, depending on wheter the battery is empty or not. This surrounds a black, sometimes wet, mass. This black stuff contains among other things the mangese dioxide. Peel the coating off and save the black mass. There is also a black rod inside attached to the anode. This is a graphite rod and can be saved for chlorate (and maybe perchlorate) preparations. We'll assume you use 2 batteries from here on. (if not, adjust amounts accordingly). Place the black mass in 200 ml of 30% hydrochloric acid. The manganese dioxide will slowly dissolve, giving off chlorine gas. Chlorine gas is dangerous: it attacks the lungs and is poisonous. Do this outside or better yet: in a fume hood if you have one. Allow the manganese dioxide several days to dissolve. The solution is then filtered which should yield a clear solution of manganese(III)chloride. In a separate container dissolve 200 grams of sodium hydroxide in a liter of bleach. Add the manganese(III)chloride solution slowly to the bleach/sodium hydroxide solution. This results in a brown precipitate of manganese dioxide which is filtered, rinsed several times with boiling hot water and dried.
+
+**Hazards**
+ 
+Mangese dioxide is poisonous and leaves brown stains on glassware etc. The stains can be removed with dilute hydrochloric acid (of course, only when the stained object is not attacked by it).

chapters/99-1-chemical-mercury-chloride.md

@@ -0,0 +1,27 @@
+## Mercury chloride
+
+**Formula**
+
+$Hg2Cl2$
+
+**Pyrotechnics use**
+
+Chlorine donor
+
+**Synonyms**
+
+Calomel, Mercurous chloride.
+
+**Description**
+
+Mercury(I)chloride is a dense yellowish-white solid that was once used as a chlorine donor for enriching colour, but owing to it's high toxicity and relatively low chlorine content (15%) when compared to the likes of polyvinyl chloride and parlon, it hasn't been widely used in around 40 years.
+
+**Sources** 
+
+TBD
+
+**Hazards**
+ 
+Xn
+
+Mercury(I)chloride is toxic and precautions should be taken to minimise exposure by any route.

chapters/99-1-chemical-methanol.md

@@ -0,0 +1,25 @@
+## Methanol
+
+**Formula**
+
+$CH3OH$
+
+**Pyrotechnics use**
+
+Solvent
+
+**Synonyms**
+
+Wood alcohol, methyl alcohol, hydroxymethane, carbinol
+
+**Description**
+
+Methanol is used as a solvent, much in the same way ethanol is used. Red gum and shellac, two common binders both dissolve in methanol. Methanol/water mixtures are also often used since the methanol increases the 'wetness' of the water (it reduces the surface tension of the water) and reduces the solubility of common oxidisers.
+
+**Sources** 
+
+Methanol is often more cheaply and easily available than ethanol because it is toxic and no extra taxes are charged for it. It finds use in a certain type of camping stove and can often be bought in camping supply stores.
+
+**Hazards**
+ 
+Methanol is flammable, volatile and toxic. Methanol vapour is heavier than air and spreads over the ground. Provide adequate ventilation when working with methanol

chapters/99-1-chemical-methyl-ethyl-ketone.md

@@ -0,0 +1,27 @@
+## Methyl ethyl ketone (MEK)
+
+**Formula**
+
+$C4H8O$
+
+**Pyrotechnics use**
+
+Solvent
+
+**Synonyms**
+
+M.E.K. 
+
+**Description**
+
+MEK (methyl ethyl ketone), also known as butanone, is a manufactured organic chemical. It is a colorless liquid with a sharp, sweet odor. Like Acetone, MEK is a ketone, and has many similarities. It dissolves many substances, and is used as a solvent for gums, resins, cellulose acetate and Nitrocellulose. MEK is listed as a Table II precursor under the United Nations Convention Against Illicit Traffic in Narcotic Drugs and Psychotropic Substances.
+
+**Sources** 
+
+
+**Hazards**
+
+F, Xi
+
+MEK is very volatile and flammable. MEK vapour is heavier than air, and spreads over the ground. Only work with MEK outside or in a well ventilated area. The known health effects to people from exposure to MEK are slight irritation of the nose, throat, skin, and eyes. There are no known cases of any humans dying from breathing MEK alone. Other than minor irritation, it's basically harmless.
+

chapters/99-1-chemical-methylene-chloride.md

@@ -0,0 +1,25 @@
+## Methylene chloride
+
+**Formula**
+
+$CH2Cl2$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+
+Dichloromethane, DCM, Methylene dichloride, Solmethine, Narkotil, Solaesthin
+
+**Description**
+
+Methylene chloride is a solvent that is used for parlon, saran, and paint thinning etc. They are also used to solvent-bond plastic aerial shell halves.
+
+**Sources** 
+
+Methylene chloride can easily be purchased from paint and hardward stores. It can not be made at home.
+
+**Hazards**
+
+Methylene chloride also know as dichloromethane is the least toxic of the simple chlorohydrocarbons, but it is not without its health risks as its high volatility makes it an acute inhalational hazard. Dichloromethane is also metabolized by the body to carbon monoxide potentially leading to carbon monoxide poisoning. Prolonged skin contact can result in the dichloromethane dissolving some of the fatty tissues in skin, resulting in skin irritation or chemical burns. It may be carcinogenic, as it has been linked to cancer of the lungs, liver, and pancreas in laboratory animals. Dichloromethane is a mutagen and crosses the placenta, causing fetal toxicity in women who are exposed to it during pregnancy. In animal experiments it was fetotoxic at doses that were maternally toxic but no teratogenic effects were seen.
+

chapters/99-1-chemical-naphthalene.md

@@ -0,0 +1,26 @@
+## Naphtalene
+
+**Formula**
+
+$C10H8$
+
+**Pyrotechnics use**
+
+Black smoke
+
+**Synonyms**
+
+Naphthalin(e), White tar, camphor tar, Albocarbon
+
+**Description**
+
+It is a white compound with a tar-like odour. It often comes as plate-like crystals. Melts at 80 deg.C. and is insoluble in water. Main pyrotechnical use is for production of black smokes (similar to anthracene). Used as an insecticide (therefore it can be found in moth balls).
+
+**Sources** 
+
+
+**Hazards**
+
+May cause irritation. Toxic by inhalation or ingestion. Possible carcinogen.
+ 
+

chapters/99-1-chemical-nitric-acid.md

@@ -0,0 +1,25 @@
+## Nitric acid
+
+**Formula**
+
+$HNO3$
+
+**Pyrotechnics use**
+
+Synthesis of nitrate compounds
+
+**Synonyms**
+ 
+TBD
+
+**Description**
+
+Nitric acid is not used in pyrotechnic compositions but it can be used to prepare a variety of useful nitrates from carbonates, hydroxides, oxides or free elements. It is used in the explosives industry in the preparation of a lot of commonly used explosives (eg TNT, RDX, PETN, nitrocellulose). Most high explosives have no use in fireworks, though nitrocellulose is used in some fireworks compositions as an acetone soluble binder.
+
+**Sources** 
+
+It is possible to prepare nitric acid in several ways. It can also be bought at some drug stores. It is sold at professional gardening suppliers and at welding shops (it is used to passivate stainless steel after welding). One way to prepare it is by distilling a mixture of sulfuric acid and sodium nitrate. This process is dangerous and requires some equipment. This method is probably too dangerous for the average amateur pyro. Another possible method is by precipitating barium sulfate from a barium nitrate solution by adding sulfuric acid. What remains is a nitric acid solution. It should be possible to prepare quite concentrated solutions by using concentrated sulfuric acid and a saturated (not hot!) barium nitrate solution. It is important that the sulfuric acid is added to the barium nitrate solution and not the other way around. The mixing of the liquids will produce heat and if the barium nitrate solution is added to the sulfuric acid it could cause sudden boiling and splatting. Therefore, add the sulfuric acid slowly to the barium nitrate while constantly stirring. Allow the mixture to cool from time to time if it gets too hot. A white precipitate of barium sulfate should form. The mixture is then filtered through a sintered glass filter to obtain clear solution of nitric acid. Another method would consist of equal amounts of sulfuric acid and potassium nitrate heated a retort. The retort is heated until the solution starts bubbling, and the nitric acid evaporates. The acid then condenses in the neck of the retort, and drips out the end into a separate flask that is submerged in chilled water. After the reaction is complete, the resulting nitric acid is around 80-95% pure. This process yields red fuming nitric acid, which you'll see fumes coming out of the flask when the lid is removed. A byproduct of this reaction is potassium hydrogen sulfate (KHSO4), which appears as a white crystalline mass at the bottom of the retort.
+
+**Hazards**
+ 
+Nitric acid is corrosive. The fumes are dangerous to the lungs, eyes and skin. Skin will be stained yellow upon contact. Avoid all contact with both liquid and fumes. Wear eye and skin protection (lab apron, gloves, safety glasses, etc). In some reactions (especially those with metals) a brown gas will develop: nitrogen dioxide. It is very toxic, corrosive and will attack your lungs badly. Only work with nitric acid with adequate ventilation and proper protective clothing. Don't use any solutions more concentrated than 60%. Don't try to prepare high explosives at home and don't allow any organic material to contact nitric acid accidentially because that may result in the formation of dangerously explosive and/or sensitive materials.

chapters/99-1-chemical-nitrocellulose.md

@@ -0,0 +1,25 @@
+## Nitrocellulose
+
+**Formula**
+
+[C6H7(NO3)3O5]n Nitrated cellulose, prepared from various natural fibers.
+
+**Pyrotechnics use**
+
+Binder
+
+**Synonyms**
+ 
+Cellulose nitrate, Flash paper, Gun cotton
+
+**Description**
+
+Nitrocellulose is used as a binder in pyrotechnic compositions. It is also used in some items without any other oxidizers or fuels. In other fields of pyrotechnics than fireworks it is widely used as a propellant, sometimes mixed with nitroglycerin and other materials (so called double- or triple base propellants).
+
+**Sources** 
+
+Nitrocellulose is sold in gun shops to those with the proper licenses in some countries. Nitrocellulose is the main compound in smokeless gunpowder. Double and triple base powders seem to be most common though. A less nitrated but usable form of cellulose, called celluloid, is also used in some household items: ping-pong balls (see Nitrocellulose lacquer). This may be a source for small amounts. Celluloid is also used for film but that is getting a little scarce these days with digital cameras taking over the market. It is probably too expensive for pyro uses anyway. Finally, it is possible to make nitrocellulose at home. The procedure is too lengthy to describe well here, but it involves treating cellulose (preferably cotton or paper) with a mixture of sulfuric acid, nitric acid and water. The product is then washed extensively and stabilized. Properly stabilizing the product at home may be difficult and commercial nitrocellulose is preferred for that reason.
+
+**Hazards**
+ 
+

chapters/99-1-chemical-orpiment.md

@@ -0,0 +1,21 @@
+## Orpiment
+
+**Formula**
+ 
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Orpiment is a very poisonus and extremly carcinogen Arsenicsulfide with yellow to gold colour. The Alchemists tried to make gold from it in the 13 centry. It is used for colour efects in Pyrotechnics and smoke mix,
+
+**Sources** 
+
+
+**Hazards**
+ 
+

chapters/99-1-chemical-paraffin-oil.md

@@ -0,0 +1,21 @@
+## Paraffin oil
+
+**Formula**
+ 
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Paraffin oil is sometimes used as an additive (about 1%) in colored fires to make pressing easier and to offer moisture protection e.g. in compositions containing large amounts of strontium nitrate. It also reduces the sensitivity of the composition.
+
+**Sources** 
+
+
+**Hazards**
+ 
+

chapters/99-1-chemical-parlon.md

@@ -0,0 +1,26 @@
+## Parlon
+
+**Formula**
+
+$(C4H6Cl2)n$
+
+**Pyrotechnics use**
+
+Chlorine donor and binder
+
+**Synonyms**
+
+Chlorinated rubber, chlorub, pergut
+
+**Description**
+
+Parlon is a acetone-soluble polymer that is used as a chlorine donor and binder. It is a good example of one of the new chemicals that has become available in the past few decades for use in compositions.
+
+**Sources** 
+
+Parlon seems to be available from dedicated pyro suppliers only.
+
+**Hazards**
+
+Parlon is not particularly dangerous.
+

chapters/99-1-chemical-petroleum-jelly.md

@@ -0,0 +1,23 @@
+## Petroleum jelly
+
+**Formula**
+ 
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+
+Paraffin jelly, mineral jelly, Vasoline/Vaseline, petrolatum, soft paraffin.
+
+**Description**
+
+A semi-solid mixture of hydrocarbons used mainly for Whistle rocket mix. Clear to white solid. Used to desensitize, waterproof and bind various compositions.
+
+**Sources** 
+
+Vasoline or other petroleum jellys are found in most supermarkets or drug stores.
+
+**Hazards**
+ 
+May cause eye, skin or digestive irritation. Material presents a low health hazard in normal use.

chapters/99-1-chemical-polyvinyl-chloride.md

@@ -0,0 +1,27 @@
+## Polyvinyl chloride
+
+**Formula**
+ 
+$[C2H3Cl]n$
+
+**Pyrotechnics use**
+
+Chlorine donor
+
+**Synonyms**
+
+PVC
+
+**Description**
+
+Like parlon and saran, PVC is a polymeric chlorine donor and fuel. It can be used in the form of a fine powder or as a solution in tetrahydrofuran (THF). It is sometimes used as a binder, but it is very brittle. Small amounts of plasticiser (dioctyl phtalate is common) may be added to improve the mechanical properties.
+
+**Sources** 
+
+As an alternative to the PVC powder available from chemical suppliers and dedicated pyro suppliers, PVC glue may also be used. It is usually sold in hardware stores and comes in two varieties: gelling or gap-filling and normal. Both are essentially a concentrated solution of PVC. I have no experience with the gelling variety, but the normal variety can succesfully be used in compositions. The gelling variety may be better suited for pyro purposes since it seems it contains more PVC. Another possibility is to use 'Sculpy' or 'Fimo' clay. These modelling clays consist of PVC with a large amount of plasticiser. The plasticiser may affect the color of a composition negatively, but reasonable results can still be obtained with it. It can simply be kneaded into a composition with some effort. This type of clay is usually hardened by heating it in an oven, but do not be tempted to do this with pyrotechnic mixtures as they may ignite.
+
+**Hazards**
+
+PVC itself is not particularly dangerous or toxic. Dioctyl phtalate is a suspected carcinogen however and THF is a very flamable and volatile liquid.
+ 
+

chapters/99-1-chemical-potassium-benzoate.md

@@ -0,0 +1,23 @@
+## Potassium Benzoate
+
+**Formula**
+
+$KC7H5O2$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Potassium benzoate is commonly used in whistle compositions. It is a white powder
+
+**Sources** 
+
+Potassium benzoate can be prepared from benzoic acid and potassium carbonate or hydroxide. Benzoic acid is not very soluble, but both potassium carbonate and hydroxide are. Dissolve 140.2g potassium carbonate or 56.1g potassium hydroxide in 250 ml water, and add 146g benzoic acid. Bring the mixture to a boil. If potassium carbonate is used, CO2 gas will evolve. Continue boiling untill all benzoic acid has dissolved, occasionally adding some water to make up for what has evaporated. When all benzoic acid has dissolved, continue boiling untill the first crystals of potassium benzoate are observed (ie the saturation point has been reached). Then allow the solution to cool to room temperature. Potassium benzoate will crystalise in needle shaped crystals. Filter, and rinse the crystals twice with ice-cold water. The crystals may be dried in an oven at 100 deg C.
+
+**Hazards**
+ 
+Potassium benzoate is not particularly dangerous.

chapters/99-1-chemical-potassium-carbonate.md

@@ -0,0 +1,19 @@
+## Potassium Carbonate
+
+**Formula**
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+
+**Sources** 
+
+
+**Hazards**
+ 
+

chapters/99-1-chemical-potassium-chlorate.md

@@ -0,0 +1,23 @@
+## Potassium Chlorate
+
+**Formula**
+
+$KClO3$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Potassium chlorate is a very common oxidiser in pyrotechnics, even though it has some treacherous properties and other oxidisers would sometimes be safer to use. Part of the reason of its popularity in commercial pyrotechnics is that it is cheap and easily available. The large scale production of this compound made the first quality colored fireworks possible, about a century ago. Potassium chlorate is a stronger oxidiser than potassium perchlorate. In some special cases it can be used safely instead of potassium perchlorate. The only use in display fireworks where Potassium Chlorate has no suitable alternative is as an oxidiser in the production of coloured smoke.
+
+**Sources** 
+
+Potassium chlorate can be prepared at home. For this purpose, sodium chlorate is prepared first by electrolysis. It may also be obtained as a herbicide in some countries (France, for example) Then, by double decomposition with potassium chloride, potassium chlorate is prepared from this solution. The product is recrystallised, dried and powdered. Other means of manufacturing Potassium chlorate include boiling a mixture of calcium hypochlorite and potassium chloride, and filtering while boiling. The crystals will form upon cooling. This reaction also produces calcium chloride which can be scraped off the top of the solution.
+
+**Hazards**
+ 
+Potassium chlorate is toxic, and breathing protection should be worn when handling fine powder. Compositions made with potassium chlorate tend to be more sensitive than those based on nitrates and perchlorates and should therefore be handled accordingly. Potassium chlorate, or any chlorate for that matter, should never be used in combination with Ammonium perchlorate or most other Ammonium compounds.Additionally, it is widely considered incompatible with sulfur and sulfides. Mixtures containing both are very sensitive and may spontaneously ignite. In general, when using chlorates great care should be taken to avoid contamination of other compositions or tools. Also read the general safety page for more information on this problem.

chapters/99-1-chemical-potassium-chloride.md

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+## Potassium Chloride
+
+**Formula**
+ 
+$KCl$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+
+Potassium mono-chloride, chloride of potassium
+
+**Description**
+
+Potassium chloride is not directly used in pyrotechnics, but can be used to make other pyrotechnic chemicals such as Potassium perchlorate and Potassium chlorate. It is used to turn NaClO4 into KClO4 and NaCl (see Preparing perchlorates). it is also used to increase smoke density in very small amounts; mainly to potassium chlorate based smoke compositions.
+
+**Sources** 
+
+Potassium chloride is sometimes used as a water softener salt, instead of NaCl (check the label). It can be bought at hardware stores and grocery stores.
+
+**Hazards**
+
+KCl is not particularly toxic or dangerous.
+

chapters/99-1-chemical-potassium-dichromate.md

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+## Potassium Dichromate
+
+**Formula**
+
+$K2Cr2O7$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Potassium dichromate is a bright orange crystalline subststance that is used to treat magnesium powder. The treatment makes magnesium more resistant to spontaneous reactions that could result in lower reliability of the mixture or spontaneous ignition.
+
+**Sources** 
+
+
+**Hazards**
+
+T+, N, O, Carc.
+
+Potassium dichromate is toxic, corrosive and a carcinogen. It should be handled with extreme care and proper protective clothing.
+

chapters/99-1-chemical-potassium-nitrate.md

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+## Potassium Nitrate
+
+**Formula**
+ 
+$KNO3$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+
+Saltpeter/Saltpetre, Nitrate of potash, Niter/Nitre, KN
+
+**Description**
+
+Potassium nitrate is probably the most extensively employed oxidizer in pyrotechnics. It used for a wide variety of applications, the most important of which is probably in the manufacture of black powder. Potassium nitrate is a white powder or long needle-like crystals. Potassium nitrate is a very important and common oxidizer.
+
+**Sources** 
+
+Potassium nitrate is used as fertilizer. As such it can be bought cheaply and in large quantities. Another possible source for potassium nitrate is 'stump remover', though this is somewhat more expensive. Alternatively, potassium nitrate can be prepared from other chemicals. For example from nitric acid and potassium carbonate or hydroxide (acid-base reaction), or sodium nitrate and potassium chloride (fractional crystallization). Another source of KNO3 is in butcheries (meat stores). They use KNO3 to treat some meats like biltong. At all times, make sure the product is free of acid since this makes the risk of accidental ignition much greater.
+
+The average Joe can synthesize potassium nitrate is by dissolving 40 grams of ammonium nitrate (found in instant cold packs) and 37 grams of potassium chloride (as a sodium chloride salt alternative) in 100mL of water. If the ammonium nitrate is found in the form of prills (or small spheres), it should be dissolved then filtered using a coffee filter. Once the two chemicals are mixed, they need to be heated. Do not boil. As the solution is heating, try to dissolve as much potassium chloride as possible. When done heating, stick it in the refrigerator. What is happening in terms of chemistry is a double displacement reaction is taking place between the potassium chloride and ammonium nitrate producing potassium nitrate and ammonium chloride: KCl + NH4NO3 → KNO3 + NH4Cl. As the solution cools, the potassium nitrate crystallizes out and leaves ammonium chloride in the solution. Simply remove the crystals and your left with fairly pure KNO3. See external links for video.
+
+Ace Hardware sells pure potassium nitrate as high yield stump remover.
+
+**Hazards**
+
+O, Carc.
+
+Potassium nitrate is not particularly dangerous or toxic in small amounts. Ingesting potassium nitrate in larger amounts, however, has been linked to cancer, especially in small children. It is suspected that it is metabolized into the known carcinogen Potassium nitrite (KNO2).

chapters/99-1-chemical-potassium-perchlorate.md

@@ -0,0 +1,26 @@
+## Potassium Perchlorate
+
+**Formula**
+
+$KClO4$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Potassium perchlorate is a very common oxidiser in pyrotechnics. Composition based on perchlorates tend to be less sensitive than those based on chlorates, and perchlorates can be used with sulfur and sulfides. For these reasons potassium perchlorate is much preferred above chlorates. Drawback is its slightly higher price.
+
+**Sources** 
+
+Potassium perchlorate can be prepared at home. For this purpose, sodium perchlorate is prepared first by electrolysis. Then, by double displacement with potassium chloride, potassium perchlorate is prepared from this solution. The product is recrystallised, dried and powdered.
+
+**Hazards**
+
+O, Xn
+
+Potassium perchlorate is toxic, and breathing protection should be worn when handling fine powder, Potassium Perchlorate can be absorbed through the skin!
+

chapters/99-1-chemical-potassium-permanganate.md

@@ -0,0 +1,25 @@
+## Potassium Permanganate
+
+**Formula**
+ 
+$KMnO4$
+
+**Pyrotechnics use**
+
+Oxidizer
+
+**Synonyms**
+
+TBD
+
+**Description**
+
+Potassium permanganate is not commonly used in pyrotechnics. Compositions based on permanganates are more sensitive than those based on nitrates and other common oxidizers. It should not be mixed with sulfur. Additionally, it does stain everything it comes in contact with. While it is not incompatible with sulfur in the same way that Chlorates are, it is incompatable with many common organic chemicals, and contamination from such ordinary substances as paper, food or soil could cause extreme sensitivity, especially in the presence of water or high humidity. Though it may be relatively unstable, if used properly, it can be a very useful oxidizer
+
+**Sources** 
+
+Difficult. KMnO4 can be used to produce illicit substances. Consequently, the DEA has restricted its use and sale by classifying it as a List I controlled precursor. Potassium permanganate is listed as a Table I precursor under the United Nations Convention Against Illicit Traffic in Narcotic Drugs and Psychotropic Substances. This makes it very difficult to find in California.
+
+**Hazards**
+ 
+Potassium permanganate is toxic, and breathing protection should be worn when handling fine powder. Also gloves and protective clothing should be warn due to its staining ability. It is also friction sensitive, so extreme care should be taken when mixing it. Do not grind or mill it. When potassium permanganate is mixed with organic materials it may spontaneously ignite. Accidental introduction of this substance into Sulfuric acid results in formation of ozone and extremely unstable Manganese(VII)oxide which violently reacts with most organic substances including many common plastics, paper, wood, and dry skin. It also is explosive by itself.

chapters/99-1-chemical-realgar.md

@@ -0,0 +1,25 @@
+## Realgar
+
+**Formula**
+
+$As2S2$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+Arsenic disulphide, Red arsenic, commonly known as Realgar. The name comes from the Arabic "rahj al-gahr", meaning powder of the mine. It's formula is variously quoted as AsS or As4S4. Yellow arsenic is the trisulfide (As2S3) and is known as Orpiment from the Latin "Auripigmentum" meaning yellow pigment.
+
+**Description**
+
+Powdered realgar is orange-red in colour and produced by sublimation of arsenopyrite or crushing the native red crystals. The latter method is employed on the ore coming mainly from China and the States of Utah, Wyoming etc. (and maybe this practice is a nightmare for everyone who collects minerals). Red arsenic is toxic of course and both toxicity and price practically preclude its use in present fireworks. Realgar in this respect suffers much the same fate as Paris Green. Generally mixtures employing realgar are sensitive to both shock and friction but sensitivity varies with different oxidizers. Many old-fashioned formulas included realgar as a component in various star compositions, for producing yellow smokes and noise units (together with potassium chlorate). While the small modern sound units are generally produced using the oxides of lead, copper or bismuth, it´s sometimes difficult to find replacements for star-making (e.g. Antimony trisulfide for some applications).
+
+**Sources** 
+
+Realgar is very hard to get and/or generally very expensive. I once managed to find a commercial source but the price for one kilo exceeded $1000 (no I did not buy the stuff). Nowadays realgar can only be found in some painting supplies for the mentioned price.
+
+**Hazards**
+
+Realgar can very easily cause cancer. In the long run it's more poisonous than white arsenic!
+

chapters/99-1-chemical-red-gum.md

@@ -0,0 +1,24 @@
+## Red Gum
+
+**Formula**
+
+Mixture of compounds.
+
+**Pyrotechnics use**
+
+Organic fuel and binder
+
+**Synonyms**
+ 
+
+**Description**
+
+Red gum, or accaroid resin, is one of the most widely used organic fuels in modern pyrotechnics and is particularly effective with Potassium perchlorate. It is made from the excretions of Grass Trees (Xanthorrhoea Genus), native to Australia. Most of the worlds product originates from Kangaroo Island, South Australia. Historically a different resin by the same name has been sold, which was extracted from waste products of the Eucalyptus timber industry. Red gum is soluble in many conventional solvents; alcohols, ethers, and ketones. Ethanol, methanol, acetone, isopropanol and butanone are commonly used in pyrotechnic preperation. It also has use as a binder.
+
+**Sources** 
+
+Red gum may be bought in artistic painting supply stores. It can also be obtained from stores that supply conservators - like shellac, red gum is sometimes used to seal wood surfaces.
+
+**Hazards**
+ 
+Red gum is not particularly dangerous or toxic.

chapters/99-1-chemical-red-phosphorus.md

@@ -0,0 +1,27 @@
+## Red Phosphorus
+
+**Formula**
+
+$P$
+ 
+**Pyrotechnics use**
+
+Friction compositions
+
+**Synonyms**
+
+Red amorphous phosphorus, Violet phosphorus, Hittorf's phosphorus
+
+**Description**
+
+Red phosphorus is a more stable and less reactive version of phosphorus. White phosphorus would ignite at about 40o C while the red version only catches fire in the air at temperatures above 240o C. In pyrotechnics, phosphorus is used in compositions that ignite through friction and in mixtures that burn very brightly, such as Armstrong's mixture.
+
+**Sources** 
+
+Red phosphorus may be formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight. There is also a method to obtain it by dissolving the strike plates taken off matchbook covers in acetone. It may also be sanded off the matchbook strike plates, but may result in paper contamination.
+
+**Hazards**
+ 
+N, F
+
+Although it does not ignite spontaneously like white phosphorus, red phosphorus is a flammable solid and is readily combustible. It may be ignited by an ignition source, heat, friction, static electrical spark, oxidizing agents (such as Potassium nitrate, Potassium chlorate, Potassium perchlorate, etc.), or physical impact. If it comes into contact with oxidants (e.g., chlorine, fluorine, or bromine), red phosphorus may burn spontaneously or explode. At normal temperature and humidity, red phosphorus reacts slowly with water vapour and Oxygen in the air to form phosphine gas, which is extremely toxic!

chapters/99-1-chemical-saran.md

@@ -0,0 +1,24 @@
+## Saran
+
+**Formula**
+
+Saran Resin, PVDC, Polyvinylidene chloride , Chlorinated polymer.
+
+**Pyrotechnics use**
+
+Chlorine donor and fuel
+
+**Synonyms**
+ 
+
+**Description**
+
+Saran is used as a chlorine donor and fuel much in the same way as parlon and PVC are. It can also serve as a binder, in which case acetone is a suitable solvent. It is known a superior chlorine donor due to its high chlorine content and superior burning characteristics.
+
+**Sources** 
+
+Saran seems to be available from chemical suppliers and dedicated pyro suppliers only.
+
+**Hazards**
+ 
+Saran is not particularly dangerous or toxic.

chapters/99-1-chemical-sawdust.md

@@ -0,0 +1,25 @@
+## Sawdust
+
+**Formula**
+ 
+
+**Pyrotechnics use**
+
+Smoke compositions and primes.
+
+**Synonyms**
+ 
+Wood meal.
+
+**Description**
+
+Sawdust comes from the cutting, sawing or sanding of wood, leaving small particles behind. Once collected, these particles are considered sawdust. Sawdust has several uses in pyrotechnics. Sawdust is used in certain smoke mixes as well as primes. The most common use for sawdust is in the form of wood meal, which is used in Veline's superprime.
+
+The most useful types of sawdust are of soft woods like pine and willow. It's relatively easy to produce sawdust or even wood meal by using a belt sander or any other type of sanding tool, even by hand. However, the latter will take quite a while to produce an amount that is useable.
+
+**Sources** 
+
+
+**Hazards**
+ 
+

chapters/99-1-chemical-shellac.md

@@ -0,0 +1,24 @@
+## Shellac
+
+**Formula**
+ 
+Mixture of compounds of average elemental composition C16H26O4
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Shellac has been in use as a binder and fuel for many centuries, but has been gradually replaced by Red gum. However, it is still sometimes claimed that shellac is a superior fuel for use in coloured compositions. It is a somewhat brittle but strong resin that dissolves in ethanol and acetone, albeit slowly.
+
+**Sources** 
+
+Shellac is available from artistic painting or woodworking supply stores. They usually have several varieties, of which 'orange shellac' works well. Some hardware stores also carry it under the name "white shellac".
+
+**Hazards**
+
+Shellac is not particularly dangerous or toxic. However it may be dissolved in methanol which is poisonous.
+

chapters/99-1-chemical-silicon.md

@@ -0,0 +1,23 @@
+## Silicon
+
+**Formula**
+
+$Si$
+
+**Pyrotechnics use**
+
+Hot prime compositons
+
+**Synonyms**
+ 
+
+**Description**
+
+The material used in fireworks is a dark grey powder called "fuzed" silicon and usually passes 240 mesh showing about 5% of impurity. It is mainly used for hot primes in combination with potassium nitrate or gunpowder, forming ignition compositions for special devices such as waterfalls with high Al content, or stars which are likely to blow blind. Once ignited, such primes produce a hot molten glass droplets and assure ignition of the main effect. They produce quite high temperatures, for the melting point of Si is 1420 deg C.
+
+**Sources** 
+
+
+**Hazards**
+ 
+

chapters/99-1-chemical-sodium-benzoate.md

@@ -0,0 +1,24 @@
+## Sodium Benzoate
+
+**Formula**
+
+$NaC6H5CO2$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Sodium benzoate is a white solid that is used as a fuel. It's most common use is in whistle mix, a mixture of potassium perchlorate and either sodium- or potassium benzoate.
+
+**Sources** 
+
+Sodium benzoate can be made from sodium carbonate (soda) or sodium hydroxide and benzoic acid which is often more easily available than it's salts. Benzoic acid is only sparingly soluble in water. Dissolve either 425 g hydrated sodium carbonate (common household soda) or 30 g sodium hydroxide in water. Add 100 g of benzoic acid and boil the solution. The benzoic acid will slowly dissolve. During boiling, occasionally add water to make up for what has evaporated. If sodium carbonate was used, carbon dioxide gas will evolve. After all the benzoic acid has dissolved, continue boiling allowing the water to evaporate untill crystallisation begins. Then stop heating and allow the solution to cool slowly to room temperature. Needle-shaped crystals of sodium benzoate will form upon cooling. Cool the solution further to 0 deg C, filtrate and rinse the crystals with ice-cold water. Purify the product by recrystallisation from water.
+
+**Hazards**
+
+Sodium benzoate is not particularly dangerous or toxic.
+

chapters/99-1-chemical-sodium-bicarbonate.md

@@ -0,0 +1,25 @@
+## Sodium BiCarbonate
+
+**Formula**
+
+$NaHCO3$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+Baking soda, cooking soda, bicarb soda, sodium hydrogencarbonate, or bicarbonate of soda
+
+**Description**
+
+Sodium bicarbonate is a white solid that is crystalline but often appears as a fine powder. Sodium bicarbonate is used as baking soda to lower the acidity of foods and give dough a darker color when cooked. Sodium bicarbonate is also widely used for a deodorizer and as a cleaning agent used for scrubbing and toothpaste. In pyrotechnics, sodium bicarbonate is used for some yellow compositions, as a delay agent in glitters, and as a burn rate modifier.
+
+**Sources** 
+
+It is sold in many shops for baking, as baking soda or bicarbonate of soda. It can also be used to make Na2CO3 very easily by heating it above 70 degrees Celsius (~160 degrees Fahrenheit).
+
+**Hazards**
+
+There is very little to no hazard when in contact with baking soda. As long as not to much is consumed it's harmless.
+

chapters/99-1-chemical-sodium-chlorate.md

@@ -0,0 +1,23 @@
+## Sodium Chlorate
+
+**Formula**
+
+$NaClO3$
+
+**Pyrotechnics use**
+
+
+**Synonyms**
+ 
+
+**Description**
+
+Sodium chlorate is hardly ever used in pyrotechnics, since it is very hygroscopic. It finds occasional use in composite rocket propellants. It is however very useful as a starting point in the preparation of several other (less hygroscopic) chlorates for which reason it is included here.
+
+**Sources** 
+
+Sodium chlorate can be prepared at home. It involves electrolysing a sodium chloride solution under certain circumstances. A description of the process, cell and anode design, etc. for home produciton may be found in the chlorate and perchlorate section of this page. In some countries, France for example, sodium chlorate may be obtained as a herbicide.
+
+**Hazards**
+
+Sodium chlorate is toxic, and breathing protection should be worn when handling fine powder. Compositions made with sodium chlorate tend to be more sensitive than those based on nitrates and perchlorates and should therefore be handled accordingly. Sodium chlorate, or any chlorate for that matter, should never be used in combination with sulfur and sulfides. Mixtures containing both are very sensitive and may spontaneously ignite. In general, when using chlorates great care should be taken to avoid contamination of other compositions or tools. Acidic solutions containing chlorates generate a very poisonous and explosive gas, ClO2.