Finish transfer of all pyro chemicals
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## Gum arabic
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**Formula**
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Mixture of compounds
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**Pyrotechnics use**
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Binder
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**Synonyms**
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TBD
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**Description**
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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.
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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.
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**Sources**
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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.
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**Hazards**
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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.
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## Hexachlorobenzene
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**Formula**
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$C6Cl6$
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**Pyrotechnics use**
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Chlorine donor
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**Synonyms**
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HCB
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**Description**
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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.
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**Sources**
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The use of HCB must be avoided.
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**Hazards**
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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.
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## Hexachloroethane
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**Formula**
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$C2Cl6$
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**Pyrotechnics use**
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Chlorine donor, Smoke compositions
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**Synonyms**
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Carbon hexachloride
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**Description**
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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.
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**Sources**
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TBD
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**Hazards**
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Xn, N
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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!
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**Formula**
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$(CH2)6N4$
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**Pyrotechnics use**
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Fuel
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**Synonyms**
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Hexamethylenetetramine, Urotropine
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**Description**
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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.
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**Sources**
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**Hazards**
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F, Xn
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## Hydrochloric acid
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**Formula**
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$HCl$
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**Pyrotechnics use**
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None
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**Synonyms**
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Hydrogen chloride, muriatic acid
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**Description**
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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.
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**Sources**
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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.
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**Hazards**
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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.
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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.
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## Iron oxide black
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## Iron oxide (black)
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**Formula**
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$Fe3O4$
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**Pyrotechnics use**
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Oxidizer (high temperature)
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**Synonyms**
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TBD
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**Description**
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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.
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**Sources**
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**Hazards**
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It is a skin and eye irritant and gloves and eye protection should be warn when handling.
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## Iron oxide red
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## Iron oxide (red)
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**Formula**
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$Fe2O3$
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**Pyrotechnics use**
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Catalyst
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**Synonyms**
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TBD
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**Description**
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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.
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**Sources**
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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 $5.00 a pound.
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**Hazards**
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Red iron oxide is not particularly toxic or dangerous. It does however stain surfaces and textiles.
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## Iron
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**Formula**
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$Fe$
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**Pyrotechnics use**
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Yellow spark effect
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**Synonyms**
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TBD
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**Description**
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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.
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**Sources**
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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.
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**Hazards**
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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.
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**Formula**
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$CH3CHOHCH3$
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**Pyrotechnics use**
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Solvent
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**Synonyms**
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IPA
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IPA, 2-propanol, isopropanol
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**Description**
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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.
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**Sources**
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It can be easily bought from supermarkets, pharmacies, and chemists in the form of isopropanol rubbing alcohol.
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**Hazards**
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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.
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## Lactose
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**Formula**
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$C12H22O11.H2O$
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**Pyrotechnics use**
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Fuel
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**Synonyms**
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TBD
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**Description**
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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.
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**Sources**
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TBD
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**Hazards**
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Lactose is not particularly toxic or dangerous.
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## Lampblack
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**Formula**
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Mixture of carbon
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**Pyrotechnics use**
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Streamer spark effect
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**Synonyms**
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Pine black, oil black, pine soot
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**Description**
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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.
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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.
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**Sources**
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Pyro suppliers only
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**Hazards**
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Do not breathe as it is a suspected carcinogen.
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**Formula**
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$Pb3O4$
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**Pyrotechnics use**
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**Synonyms**
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Lead minium, Minium, Triplumbic tetroxide, Red lead, Lead tetroxide
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**Description**
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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".
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**Sources**
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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.
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**Hazards**
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T, N
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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.
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## Linseed oil
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**Formula**
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TBD
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**Pyrotechnics use**
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Metal powder coating
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**Synonyms**
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Flax seed oil
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**Description**
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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.
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**Sources**
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Linseed oil products are available at paint and hardware stores.
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**Hazards**
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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.
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## Magnesium
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**Formula**
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Alloy of magnesium and aluminum, usually 50:50. Sometimes written: $MgAl$
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**Pyrotechnics use**
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Fuel
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**Synonyms**
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TBD
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**Description**
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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.
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**Sources**
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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).
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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.
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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.
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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.
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**Hazards**
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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.
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## Magnesium
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**Formula**
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$Mg$
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**Pyrotechnics use**
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Fuel
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**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.
|
||||
|
|
|
|||
|
|
@ -1,20 +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).
|
||||
|
|
@ -1,20 +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.
|
||||
|
|
|
|||
|
|
@ -1,20 +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
|
||||
|
|
|
|||
|
|
@ -1,10 +1,12 @@
|
|||
## Methyl ethyl ketone
|
||||
## Methyl ethyl ketone (MEK)
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$C4H8O$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Solvent
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
|
@ -12,10 +14,14 @@ 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.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +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.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +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.
|
||||
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +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.
|
||||
|
|
@ -1,19 +1,24 @@
|
|||
## 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**
|
||||
|
||||
|
|
|
|||
|
|
@ -11,6 +11,7 @@
|
|||
|
||||
**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**
|
||||
|
||||
|
|
|
|||
|
|
@ -11,6 +11,7 @@
|
|||
|
||||
**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**
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +0,0 @@
|
|||
## Paris green
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
**Description**
|
||||
|
||||
|
||||
**Sources**
|
||||
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
|
|
@ -1,20 +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.
|
||||
|
||||
|
|
|
|||
|
|
@ -7,14 +7,17 @@
|
|||
|
||||
|
||||
**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.
|
||||
|
|
|
|||
|
|
@ -2,9 +2,11 @@
|
|||
|
||||
**Formula**
|
||||
|
||||
$[C2H3Cl]n$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Chlorine donor
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
|
@ -12,10 +14,14 @@ 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.
|
||||
|
||||
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Potassium Benzoate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$KC7H5O2$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,12 @@
|
|||
|
||||
**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.
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Potassium Chlorate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$KClO3$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,12 @@
|
|||
|
||||
**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.
|
||||
|
|
|
|||
|
|
@ -2,19 +2,24 @@
|
|||
|
||||
**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.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Potassium Dichromate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$K2Cr2O7$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,14 @@
|
|||
|
||||
**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.
|
||||
|
||||
|
|
|
|||
|
|
@ -2,19 +2,29 @@
|
|||
|
||||
**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).
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Potassium Perchlorate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$KClO4$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,15 @@
|
|||
|
||||
**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!
|
||||
|
||||
|
|
|
|||
|
|
@ -2,19 +2,24 @@
|
|||
|
||||
**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.
|
||||
|
|
@ -1,20 +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!
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +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.
|
||||
|
|
|
|||
|
|
@ -1,20 +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!
|
||||
|
|
|
|||
|
|
@ -1,20 +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.
|
||||
|
|
|
|||
|
|
@ -5,12 +5,17 @@
|
|||
|
||||
**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**
|
||||
|
||||
|
|
|
|||
|
|
@ -2,6 +2,7 @@
|
|||
|
||||
**Formula**
|
||||
|
||||
Mixture of compounds of average elemental composition C16H26O4
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,13 @@
|
|||
|
||||
**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.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,16 +1,19 @@
|
|||
## 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**
|
||||
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Sodium Benzoate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$NaC6H5CO2$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,13 @@
|
|||
|
||||
**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.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +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.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Sodium Chlorate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$NaClO3$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,12 @@
|
|||
|
||||
**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.
|
||||
|
|
@ -1,20 +1,26 @@
|
|||
## Sodium Chloride
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$NaCl$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Delay agent
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
Common salt, halite, table salt,
|
||||
|
||||
**Description**
|
||||
|
||||
Sodium chloride is used in pyrotechnics as delay agent in a few glitter formulas, but besides that, it is hardly ever used, since it is very hygroscopic. It is white or colourless solid in the form of crystals or powder.
|
||||
|
||||
**Sources**
|
||||
|
||||
Sodium chloride can be purchased almost anywhere.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
If inhaled it may cause mild irritation to the respiratory tract. Ingestion in very large can cause vomiting, diarrhoea, and prostration. Dehydration and congestion occur in most internal organs. Hypertonic salt solutions can produce violent inflammatory reactions in the gastrointestinal tract. Skin Contact may irritate damaged skin; absorption can occur with effects similar to those via ingestion. Eye Contact causes irritation, redness, and pain.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +1,25 @@
|
|||
## Sodium Nitrate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$NaNO3$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Oxidizer
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
**Description**
|
||||
|
||||
Sodium nitrate finds occasional use as an oxidiser in flare and tracer compositions because of the high efficiency of light emission that can be obtained with it, but its high hygroscopic nature limits its use. Sodium nitrate can be used to prepare potassium nitrate, a much less hygroscopic and more often used oxidiser.
|
||||
|
||||
**Sources**
|
||||
|
||||
Sodium nitrate is sold as a food preservative, 95% pure sodium nitrate is also available as a fertilizer. In the Netherlands this fertilizer is sold under the name 'chilisalpeter'. If required, it can be easily purified by recrystallisation.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Sodium nitrate is not healthy to eat, but careful use as always with chemicals make it not dangerous to work with. Since it's very hygroscopic it can cause dangerous mixes with Aluminium or Magnesium.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +1,25 @@
|
|||
## Sodium Oxalate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$Na2C2O4$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Yellow/golden color compositions and delay agent in glitter compositions.
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
Disodium oxalate
|
||||
|
||||
**Description**
|
||||
|
||||
Sodium oxalate is mainly used for making yellow to golden colors in composition. It is also used for delay agent in some glitter compositions.
|
||||
|
||||
**Sources**
|
||||
|
||||
Various pyro supplies. Sodium oxalate can also be made at home using oxalic acid and a sodium salt.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Sodium oxalate is harmful by skin contact, ingestion and inhalation. Use proper safety gear when working with sodium oxalate, such as latex gloves, goggles and a dust mask.
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Sodium Perchlorate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$NaClO4$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,12 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Sodium perchlorate is hardly ever used in pyrotechnics, since it is very hygroscopic. It finds occasional use in composite rocket propellants. It is however very usefull as a starting point in the preparation of several other (less hygroscopic) perchlorates for which reason it is included here.
|
||||
|
||||
**Sources**
|
||||
|
||||
Sodium perchlorate can be prepared at home. It involves electrolysing a sodium chloride solution under certain circumstances.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Sodium perchlorate is toxic, and breathing protection should be worn when handling fine powder.
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Sodium Silicate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$Na2SiO3$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,12 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Sodium silicate, also known as water glass or liquid glass, available in liquid and solid (prill) form, is used for passive fire protection.
|
||||
|
||||
**Sources**
|
||||
|
||||
It can be bought from online pyrotechnic stores and ceramic supply shops. It can be bought in either liquid form or a dry powder. When dry it is mixed with water and a small amount is placed around pass fire holes and exhaust holes (see hummer).
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Sodium silicate is corrosive and may cause health problems with over exposure. It is best to avoid eye and skin contact and vapour or mist inhalation.
|
||||
|
|
|
|||
|
|
@ -13,10 +13,18 @@ SGRS
|
|||
|
||||
**Description**
|
||||
|
||||
Soluble glutinous rice starch more commonly referred to as 'SGRS' is a binder used by the Japanese star makers. SGRS is used as a water-soluble binder in many of Takeo Shimizu's formulas. This is not just because SGRS is more easily obtained in Japan than cornstarch derivatives like dextrin. SGRS does indeed have superior binding characteristics than dextrin, and somewhat less of it can be used than dextrin in most formulas.
|
||||
|
||||
**Sources**
|
||||
|
||||
Soluble glutinous rice starch can be hard to come by, but can be made at home:
|
||||
|
||||
"Glutinous rice is polished and soaked in cold water for a week. This is then steamed in a steam basket and pounded into a cohesive mass. The mass is stretched into a thin plate like a squashed cake, which is parched at a suitable temperature. The parched cake is ground into a fine powder. The powder is somewhat brownish, but has a large cohesion power and is perfectly gelatinized in combination with water. This is the most useful binding agent for firework stars." - Shimizu
|
||||
|
||||
I have recently made some SRGS: soak rice in cold water for a week, steam for an hour, dry out in oven. Powder in coffee grinder. All worked fine but seemed a lot of effort and time consuming. Second attempt: put dry rice in coffee grinder mixed resulting flour with water, brought to boil and simmered for 15 minutes, stiring continously. Transfered resulting 'glue' to low oven to brown. Put dry mixture in coffee grinder to produce identical SRGS in just over two hours.
|
||||
|
||||
The warm mix of the rice flour reminded me of wallpaper paste. I have now made some stars with 'Polycel' powder and another lot with a propietry 'boiled flour' wallpaper paste. Using the quantities of these wallpaper pastes as given for SRGS I have got a series of identical stars. However wallpaper adhesive is in fact CMC (Sodium carboxymethyl cellulose).
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Soluble glutinous rice starch is not particularly toxic or dangerous.
|
||||
|
|
@ -1,7 +1,8 @@
|
|||
## Sorbitol
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$C6H14O6$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,6 +12,7 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Sorbitol is a low melting point sugar alcohol and has many different uses. In pyrotechnics it is used with potassium nitrate as a rocket propellant. Its main advantage over other sugars such as glucose is its lower melting temperature and the fact that it can not caramelise like other sugars
|
||||
|
||||
**Sources**
|
||||
|
||||
|
|
|
|||
|
|
@ -2,19 +2,23 @@
|
|||
|
||||
**Formula**
|
||||
|
||||
$C3H5(C18H35O2)3$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
Stearic acid
|
||||
|
||||
**Description**
|
||||
|
||||
Stearin is used in conjunction with Aluminum flakes to help in the grinding process in making Dark Aluminum powder. It is also used in some fountain composition, which calls for stearin powder. Stearin is a glyceryl ester of stearic acid, derived from animal fats created as a by-product of processing beef. It is used as tallow in the manufacture of candles and soap.
|
||||
|
||||
**Sources**
|
||||
|
||||
It can be bought as a candles in many shops. Purified (white) animal fat like pig is in most part made of stearic acid and is a good substitute for most application
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Evaporated stearin like all fat is slightly toxic for the lung
|
||||
|
|
|
|||
|
|
@ -1,20 +1,24 @@
|
|||
## Steel (Iron)
|
||||
## Steel
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
Alloy metal with Iron: $Fe$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Yellow sparkle effect
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
Alloy steel, galvanized steel, carbon steel, and sometimes wrought iron (a mild steel).
|
||||
|
||||
**Description**
|
||||
|
||||
Steel is a solid grayish-brown alloy of iron with either carbon, manganese, tungsten, or vanadium. These additional substances harden the iron through smelting and combining, but they also make the final product (steel) more brittle. Most steel contains a very large list of trace elements, with most having contents under 1 percent. Sulfur is a common trace element, so steel may be dangerous in extremely sulfur sensitive compounds. Steel is the most common metal used in modern industrial building, but there are stronger, lighter, but more expensive alternatives. Due to the main element in steel being iron, steel retains a strong ferromagnetic property.
|
||||
|
||||
**Sources**
|
||||
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Steel is not particularly dangerous, even in the powdered form. Ingestion of steel powder is dangerous, but supposedly not fatal. Steel is inflammable without an external oxidizer, but it does propose a dust explosion hazard if floating in the air.
|
||||
|
|
@ -1,7 +1,8 @@
|
|||
## Strontium Carbonate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$SrCO3$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,13 @@
|
|||
|
||||
**Description**
|
||||
|
||||
White to pale pink powder. Strontium carbonate is used in combination with chlorine donors to produce red colors. It also acts as an acid neutraliser, for which reason it is prefered in chlorate based compositions (which may spontaneously ignite when traces of acid are present).
|
||||
|
||||
**Sources**
|
||||
|
||||
Strontium carbonate is cheaply available in kilogram quantities from ceramic supply shops. However, this material is often contaminated with small amounts of strontium sulfide which are left over from the production process. Therefore, ceramics grade strontium carbonate should never be used in mixtures incompatible with sulfides such as chlorate based mixtures. Strontium carbonate is not easily made at home.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Strontium carbonate is not particularly dangerous or toxic.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +1,26 @@
|
|||
## Strontium Nitrate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$Sr(NO3)2$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
Strontium dinitrate
|
||||
|
||||
**Description**
|
||||
|
||||
Strontium nitrate is an oxidizer commonly employed in red color compositions in combination with chlorine donors. Strontium nitrate tends to absorb water.
|
||||
|
||||
**Sources**
|
||||
|
||||
Strontium nitrate may be prepared from nitric acid or ammonium nitrate and strontium carbonate, which is available from ceramic supply stores. Use an excess of strontium carbonate to ensure complete neutralization of acid and recrystallise the product from a slightly alkaline solution to prevent the inclusion of acid solvent droplets in the crystals.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
O, Xn
|
||||
|
||||
All Strontium salts are irritating and damaging to the eyes so goggles and gloves should be worn when working with strontium salts. Before using any new chemical, or even buying it you should get a full MSDS on it (shown at bottom of page.) Toxicity: Oral rat LD50: 2750 mg/kg.
|
||||
|
|
@ -1,7 +1,8 @@
|
|||
## Sodium Oxalate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$SrC2O4.H2O$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,14 @@
|
|||
|
||||
**Description**
|
||||
|
||||
A fine white, insoluble powder made by precipitation. The water content may be a drawback. It is sometimes used to obtain red colours (even if more expensive than the carbonate) and in some glitter formulas together with gunpowder and Al. Do not use in chlorate mixtures and keep it away from acids.
|
||||
|
||||
**Sources**
|
||||
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Xn
|
||||
|
||||
Strontium oxalate is harmful by skin contact, inhalation and ingestion as it is a salt of oxalic (ethanedioic) acid, it can cause renal failure and may even prove to be fatal if ingested.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Strontium Sulfate
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$SrSO4$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,12 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Strontium sulfate is used as a high-temperature oxidiser in some metal based red color compositions, and is particularly important in Ammonium perchlorate based red strobes.
|
||||
|
||||
**Sources**
|
||||
|
||||
Strontium sulfate may be precipitated from a solution of a soluble strontium salt, such as strontium nitrate or chloride, and a sulfate. Magnesium and potassium sulfate are both cheaply available as fertilizer and are convenient to use. The precipitated strontium 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. Do not use sulfuric acid to precipitate strontium sulfate as this may result in the inclusion of acid droplets in the precipitated particles which can lead to spontaneous ignition of some mixtures.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Strontium sulfate is not particularly dangerous or toxic.
|
||||
|
|
|
|||
|
|
@ -1,21 +1,26 @@
|
|||
## Sucrose
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$C12H22O11$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Fuel
|
||||
|
||||
**Synonyms**
|
||||
|
||||
Sugar
|
||||
White table sugar
|
||||
|
||||
**Description**
|
||||
|
||||
Sucrose (also known as ordinary table sugar) is a colorless crystalline solid that is used as a fuel for some compositions. It's most commonly used in smoke mix and in Candy propellant.
|
||||
|
||||
**Sources**
|
||||
|
||||
It very cheaply available in large amounts in supermarkets. When you have a choice, it is best to use 'pure icing sugar'. This is finely powdered, and contains no contaminants or binders. Beware of buying 'icing mix' which contains around 20% binder
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Sucrose is not particularly hazardous or dangerous.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Sulfur
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$S$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,13 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Sulfur has always been used extensively in pyrotechnics. It serves as a fuel, and reduces the ignition temperature of mixtures. It also tends to increase the burning rate and friction or shock sensitivity of most mixtures.
|
||||
|
||||
**Sources**
|
||||
|
||||
Sulfur is available from agricultural supply stores where it is sold as a fungicide under the name 'dusting sulfur'. It is a fine powder mixed with a few percent of calcium carbonate. The calcium carbonate may disturb delicate color compositions, but for most purposes dusting sulfur works well. If a purer form of sulfur is required, sulfur may also be obtained from drug stores sometimes. However, these often sell 'flowers of sulfur', which has been purified by sublimation and which contains some acid. This needs to be neutralized before use as it could cause spontaneous ignition. To do this, allow 100g of this sulfur to soak in a liter of water/household ammonia (1:5). Stir well occasionally and measure the pH. It should still be alkaline after two days, after which time the sulfur may be filtered and washed with hot water to remove the ammonia. Check the pH of the washing water while filtering. After it has become neutral, flush the water away with ethanol and allow the sulfur to dry. Mix the dry powder with 2% magnesium carbonate to neutralize any acid that may be formed in reactions with the atmosphere.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Sulfur can increase the sensitivity of some mixtures, especially those based on chlorate or perchlorate oxidizers. Mixtures of chlorates and sulfur are also known to ignite spontaneously and should therefore be avoided at all times (also read the safety section). Mixtures of perchlorates and sulfur are less likely to ignite spontaneously but are still very sensitive and need to be treated with extreme caution. Burning sulfur produces sulfur dioxide gas, inhalation of which should be avoided because it is extremely poisonous. Sulfur is a very important chemical in pyrotechnics.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +1,25 @@
|
|||
## Sulfuric Acid
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$H2SO4$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Synthesis of some compounds
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
**Description**
|
||||
|
||||
Sulfuric acid itself finds no use in pyrotechnics, but it can be used in the preparation of an number of useful compounds for which reason it is included here. Sulfuric acid can also be used to ignite chlorates or chlorate containing mixtures, although in practical pyrotechnics this is not actually useful.
|
||||
|
||||
**Sources**
|
||||
|
||||
Sulfuric acid has many sources. It can be bought at many laboratory supply stores and web sites. The major drawback to ordering on the web is that there will be a hazmat fee for larger quantities and higher concentrations. An alternative is ordering Sodium bisulfate which is some what cheap and doesn't require hazmat shipping. Then using it in solution where it will have a pH of 1.4 in a 1 molar solution and will behave like Sulfuric acid. Other sources are liquid lead acid battery's, humidifier cleaner, and drain opener. Sulfuric acid can also be made at home but it will be in an unusable low concentration and small amount and not needed to be explained here.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Sulfuric acid and its fumes are extremely corrosive. Wear proper protective clothing (gloves, apron and a face shield are minimal) and provide adequate ventilation when working with it. Reactions with metals often produce flammable hydrogen gas (hydrogen). The presence of acid can cause spontaneous reactions in many pyrotechnic mixtures and should at all times be avoided. When working with sulfuric acid, have no chemicals or compositions nearby to prevent contamination. Make sure all traces of acid in chemicals produced with sulfuric acid are removed if they are to be used in pyrotechnics compositions.
|
||||
|
||||
|
|
|
|||
|
|
@ -1,11 +1,12 @@
|
|||
## Tetrahydrofuran (THF)
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$(CH2)4O$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Solvent?
|
||||
Solvent for PVC
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
|
@ -13,10 +14,11 @@ THF
|
|||
|
||||
**Description**
|
||||
|
||||
A colorless, water-miscible organic liquid. It is a highly polar solvent and is used mainly to dissolve PVC
|
||||
|
||||
**Sources**
|
||||
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
THF is a highly flammable and care should be taken to keep sources of ignition. When handling latex gloves should not be used as THF will dissolve them. Gloves made from polyacrylonitrile should be used, such as common kitchen Marigolds for the amateur chemist.
|
||||
|
|
|
|||
|
|
@ -1,21 +1,24 @@
|
|||
## Titanium
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$Ti$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Metal fuel
|
||||
Metallic fuel for white sparks
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
**Description**
|
||||
|
||||
Metallic titanium is used in pyrotechnics to produce bright white sparks of a superior quality. The particle size and shape of the titanium will affect the colour and duration of the sparks, with smaller mesh producing smaller and shorter-lasting sparks. The effect of a titanium-fountain is superior to all effects that can be obtained with aluminium or magnalium for that purpose.
|
||||
|
||||
**Sources**
|
||||
|
||||
Titanium powder is commonly sold by dedicated pyrotechnic suppliers, and some metal suppliers. Titanium shavings and curls are sometimes available from places where titanium metal is worked. These are often contaminated with oil which can be removed by washings with white gas or acetone. Titanium curls can be heated in an oven to make them more brittle, which facilitates crushing them into a powder. Ball milling of titanium to very fine powders can be made pyrophoric and due to the hardness of the material it is likely to cause excessive damage to the Barrel and Media.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
While it will not react with any pyrotechnic chemicals, Titanium can spark if hit with other metals (especially steel) or against itself. Black powder like compositions containing titanium, such as often used in fountains, are notably more sensitive than mixtures without titanium.
|
||||
|
|
|
|||
|
|
@ -2,6 +2,7 @@
|
|||
|
||||
**Formula**
|
||||
|
||||
Sodium alumino sulfosilicate
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,15 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Ultramarine is a blue pigment consisting primarily of a double silicate of aluminium and sodium with some sulfides or sulfates, and occurring in nature as a proximate component of lapis lazuli. It was traditionally used for cave drawings and eventually pigments in art and other areas. In pyrotechnics, it is used as a fuel that burns bright yellow in color, but is rarely used anymore thanks to the development of such materials as sodium oxalate and cryolite. These newer materials are cheaper and easier to obtain, and therefore are more frequently used.
|
||||
|
||||
**Sources**
|
||||
|
||||
Sold as Blue Pigment 29, Ultramarine, and Sodium alumino sulfosilicate from chemical suppliers, crafting, and ceramic stores.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Xi
|
||||
|
||||
Slight irritant. Carcinogenicity unknown.
|
||||
|
||||
|
|
|
|||
|
|
@ -2,18 +2,24 @@
|
|||
|
||||
**Formula**
|
||||
|
||||
$H2O$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Solvent
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
**Description**
|
||||
|
||||
Simple enough, this is H2O. Found in any household, water can be taken straight from the tap for most purposes, including drinking. Just be sure not to drink after mixing with one of our harmful pyrotechnic compounds. Ingesting firework materials is probably best avoided altogether, though absorption through firework smoke sniffing is habitual for many firework lovers.
|
||||
|
||||
Water, in pyrotechnics, is used to knead stars while binding, to make paste for making tubes and pasting shells, to make slurries of compositions for various purposes(eg. black match), and to make granulated BP.
|
||||
|
||||
**Sources**
|
||||
|
||||
Everywhere
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
|
|
|||
|
|
@ -1,19 +0,0 @@
|
|||
## Wood Meal
|
||||
**Formula**
|
||||
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
**Description**
|
||||
|
||||
|
||||
**Sources**
|
||||
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
|
|
@ -1,7 +1,8 @@
|
|||
## Xanthan Gum
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$(C35H49O29)n$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,9 +12,11 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Xanthan gum is a polysaccharide used as a food additive and rheology modifier (Davidson ch. 24). It is produced by a process involving fermentation of glucose or sucrose by the Xanthomonas campestris bacterium. Xanthan gum burns relatively hot, especially when mixed with nitrates. It is used in some stars as a fuel and to regulate the burn rate. Xanthan gum must be used sparingly due to the fact that it will create molten slag in nozzles (dross), and it will become molten on the out side of stars, preventing them from burning properly, reversing the positive effects the gum adds. Xanthan gum is typically used in stars that spark or glitter such as Penny stars, and will brighten the sparks but shorten their life.
|
||||
|
||||
**Sources**
|
||||
|
||||
Xanthan gum can be bought at a grocery store.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
|
|
|||
|
|
@ -1,19 +1,24 @@
|
|||
## Xylene
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$C8H10$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
Solvent
|
||||
|
||||
**Synonyms**
|
||||
|
||||
Xylol
|
||||
|
||||
**Description**
|
||||
|
||||
Xylene 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**
|
||||
|
||||
Xylene can easily be purchased from paint and hardware stores. It can not be made at home.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
|
|
|||
|
|
@ -1,20 +0,0 @@
|
|||
## Xylol
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
||||
**Synonyms**
|
||||
|
||||
|
||||
**Description**
|
||||
|
||||
|
||||
**Sources**
|
||||
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
|
|
@ -1,20 +1,25 @@
|
|||
## Zinc Oxide
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$ZnO$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
White smoke
|
||||
|
||||
**Synonyms**
|
||||
|
||||
Zinc white, Calamine
|
||||
|
||||
**Description**
|
||||
|
||||
Zinc oxide is used to produce white smoke.
|
||||
|
||||
**Sources**
|
||||
|
||||
Zinc oxide is usually available as a white pigment called 'zinc white' in artistic paint stores. It can also be prepared by igniting a piece of zinc sheet.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Zinc oxide is not particularly toxic or dangerous.
|
||||
|
|
|
|||
|
|
@ -1,7 +1,8 @@
|
|||
## Zinc
|
||||
|
||||
**Formula**
|
||||
|
||||
|
||||
$Zn$
|
||||
|
||||
**Pyrotechnics use**
|
||||
|
||||
|
|
@ -11,10 +12,12 @@
|
|||
|
||||
**Description**
|
||||
|
||||
Metallic zinc is used in rocket propellants, for spark effects and in white smoke compositions. Zinc powder is quite heavy and zinc-based stars often require heavier lift or burst charges to propel them.
|
||||
|
||||
**Sources**
|
||||
|
||||
Zinc powder is used in paints for the protection of steel. Spray cans containing an suspension of zinc powder are commonly sold in hardware stores. The zinc powder may be extracted by emptying the spray can in a large container, allowing the powder to settle, decanting the solvent and paints and repeated washing with paint thinner or acetone. However this is an expensive way to obtain zinc powder when high purity is available commercially at about $3 per pound in 50 pound drums. Unfortunately it cakes to rock hard masses in a few years on storage and requires ball milling every year to keep it usable.
|
||||
|
||||
**Hazards**
|
||||
|
||||
|
||||
Zinc powder in presence of nitrates can spontaneously heat up when wet.
|
||||
|
|
|
|||
|
|
@ -17,6 +17,7 @@
|
|||
* [HOBBY CHEMICAL SUPPLY](https://hobbychemicalsupply.com/shop)
|
||||
* https://fireworkchemicals.com/
|
||||
* https://www.greatlakesmortarracks.us/
|
||||
* https://pyro-aluminum.com/
|
||||
|
||||
## Russia (RU)
|
||||
|
||||
|
|
|
|||
Loading…
Reference in New Issue