"hazardous waste. The Environmental Protection Agency (EPA) lists barium chlorate as hazardous. Barium chlorate Barium chlorate, Ba(ClO), is a white crystalline solid, the barium salt of chloric acid. It is an irritant and toxic, as are all soluble barium compounds. It is sometimes used in pyrotechnics to produce a green color. It also finds use in the production of chloric acid. Barium chlorate can be produced through a double replacement reaction between solutions of barium chloride and sodium chlorate: On concentrating and chilling the resulting mixture, barium chlorate precipitates. This is perhaps the most common preparation, exploiting the lower solubility"
"barium chromate but instead contain some small sulfur content as well. The different crystals contain a range of sulfur impurities ranging from the more pure dark crystals, Ba(Cr, S)O, to the less pure light crystals, Ba(Cr, S)O. Hashemite was found to be an isostructural chromate analog of baryte, BaSO. It can be synthesized by reacting barium hydroxide or barium chloride with potassium chromate. Barium chromate Barium chromate, named barium tetraoxochromate(VI) by the IUPAC, is a yellow sand like powder with the formula BaCrO. It is a known oxidizing agent and produces a green flame when heated, a result of the"
"Barium chromate Barium chromate, named barium tetraoxochromate(VI) by the IUPAC, is a yellow sand like powder with the formula BaCrO. It is a known oxidizing agent and produces a green flame when heated, a result of the barium ions. The first naturally occurring barium chromate was found in the country of Jordan. The brown crystals found perched on host rocks were named hashemite in honor of the Hashemite Kingdom of Jordan. The hashemite crystals range in color from light yellowish-brown to a darker greenish-brown and are usually less than 1mm in length. The hashemite crystals are not composed of pure"
"as an oxidizer, chemical reactions involving the dissociated elements of the perchlorate—potassium and chlorine ions—create barium compounds which emit green light (especially BaCl). The potassium compounds formed by this reaction emit mostly near-infrared light, and so they do not affect the color of the star in a significant way. This reaction occurs at temperatures exceeding 2500 °C (4500 °F), at which the ions in KCl dissociate into free K and Cl. Alternatively, SrCO can be added to the candle to produce a red or pink star, but, because it does not oxidize, more oxidizers and fuels must be added to"
"However, due to the instability of all chlorates to sulfur, acids, and ammonium ions, chlorates have been banned from use in class C fireworks in the United States. Therefore, more and more firework producers have begun to use more stable compound such as barium nitrate and barium carbonate. Barium chlorate is toxic to humans and can also harm the environment. It is very harmful to aquatic organisms if it is leached into bodies of water. Chemical spills of this compound, although not common, can harm entire ecosystems and should be prevented. It is necessary to dispose of this compound as"
"is not used for this purpose in fireworks due to the overwhelming yellow color of sodium. Boric acid is used to color methanol flames a transparent green. Borax is very soluble in ethylene glycol, moderately soluble in diethylene glycol and methanol, slightly soluble in acetone. It is poorly soluble in cold water, but its solubility increases significantly with temperature. The English word ""borax"" is Latinized: the Middle English form was ""boras"", from Old French ""boras, bourras"". That may have been from medieval Latin ""baurach"" (another English spelling), ""borac(-/um/em), borax"", along with Spanish ""borrax"" (> ""borraj"") and Italian ""borrace"", in the"
"Barium chloride Barium chloride is the inorganic compound with the formula BaCl. It is one of the most common water-soluble salts of barium. Like most other barium salts, it is white, toxic, and imparts a yellow-green coloration to a flame. It is also hygroscopic, converting first to the dihydrate BaCl(HO). It has limited use in the laboratory and industry. BaCl crystallizes in two forms (polymorphs). One form has the cubic fluorite (CaF) structure and the other the orthorhombic cotunnite (PbCl) structure. Both polymorphs accommodate the preference of the large Ba ion for coordination numbers greater than six. The coordination of"
"color-emitting atom in the salt is also released and reacts chemically with excess oxygen providing the source of the colored flame. In NATO standard ammunition (including US), the oxidizer salt is usually a mixture of strontium compounds (nitrate, peroxide, etc.) and the metallic fuel is magnesium. Burning strontium yields a bright red light. Russian and Chinese tracer ammunition generates green light using barium salts. An oxidizer and metallic fuel alone, however, do not make a practical pyrotechnic for the purposes of producing colored light. The reaction is too energetic, consuming all materials in one big flash of white lightwhite light"
"Its toxicity limits its applicability. Barium chloride, along with other water-soluble barium salts, is highly toxic. Sodium sulfate and magnesium sulfate are potential antidotes because they form barium sulfate BaSO, which is relatively non-toxic because of its insolubility. Barium chloride Barium chloride is the inorganic compound with the formula BaCl. It is one of the most common water-soluble salts of barium. Like most other barium salts, it is white, toxic, and imparts a yellow-green coloration to a flame. It is also hygroscopic, converting first to the dihydrate BaCl(HO). It has limited use in the laboratory and industry. BaCl crystallizes in"
"Strontium chloride Strontium chloride (SrCl) is a salt of strontium and chloride. It is a typical salt, forming neutral aqueous solutions. Like all compounds of Sr, this salt emits a bright red colour in a flame; in fact it is used as a source of redness in fireworks. Its chemical properties are intermediate between those for barium chloride, which is more toxic, and calcium chloride. Strontium chloride can be prepared by treating strontium hydroxide or strontium carbonate with hydrochloric acid: Crystallization from cold aqueous solution gives the hexahydrate, SrCl·6HO. Dehydration of this salt occurs in stages, commencing above . Full"
"the necessary confinement. Otherwise such mixtures simply deflagrate with an intense purple flame characteristic of potassium. Flash compositions used in firecrackers usually consist of a mixture of aluminium powder and potassium perchlorate. This mixture, sometimes called flash powder, is also used in ground and air fireworks. As an oxidizer, potassium perchlorate can be used safely in the presence of sulfur, whereas potassium chlorate cannot. The greater reactivity of chlorate is typical – perchlorates are kinetically poorer oxidants. Chlorate produces chloric acid, which is highly unstable and can lead to premature ignition of the composition. Correspondingly, perchloric acid is quite stable."
"of chlorine, and the reaction to monochlorides, may actually impair their color purity or intensity. At high temperatures, the atoms will ionize. The emission spectra of ions are different than of neutral atoms; the ions may emit in undesired spectral ranges. For example, Ba emits in blue wavelengths. Ionization can be suppressed by addition of an easier-to-ionize metal with weak visible emission of its own, e.g. potassium; the potassium atoms then act as electron donors, neutralizing the barium ions. The color blue is notoriously difficult to produce in fireworks, as the copper compounds need to be heated at a specific"
"off with saying that fireworks ""come from a range of different colours, all of which are due to the excited states of different metal atoms"". He decided to take a salt that contains a metal, opting to use table salt, because it's sodium chloride. The flame was blue, but it became an orange colour, because ""all of the sodium atoms in there are getting really, really excited"". He tried a copper one, which made the flame a green colour. He said fireworks work on the same principle as a match. It is a chemical reaction called ""combustion"". He lit the"
"Barium perchlorate Barium perchlorate is a powerful oxidizing agent, with the formula Ba(ClO). It is used in the pyrotechnic industry. Barium perchlorate decomposes at 505 °C. Gallucci and Gerkin (1988) analyzed the structure of the hydrate isomer Barium Perclorate Trihydrate (Ba(ClO)•3HO) by X-ray crystallography. The barium ions are coordinated by six water oxygen atoms at 2.919Å and six perchlorate oxygens at 3.026Å in a distorted icosahedral arrangement. The perchlorate fails by a narrow margin to have regular tetrahedral geometry, and has an average Cl-O bond length of 1.433Å. The space-group assignment of the structure was resolved, with the centrosymmetric assignment"
"being the characteristic output of magnesium-oxide (MgO), for example. Therefore, in the case of using strontium nitrate and magnesium, to produce a red colored flame that is not over-powered by the white light from the burning fuel, a chlorine donor is provided in the pyrotechnic mixture, so that strontium chloride can also form in the flame, cooling it so that the white light of MgO is greatly reduced. Cooling the flame in this manner also lengthens the reaction rate so that the mixture has an appreciable burn time. Polyvinyl chloride (PVC) is a typical organic fuel in colored light for"
"Barium oxide Barium oxide, BaO, is a white hygroscopic non-flammable compound. It has a cubic structure and is used in cathode ray tubes, crown glass, and catalysts. It is harmful to human skin and if swallowed in large quantity causes irritation. Excessive quantities of barium oxide may lead to death. It is prepared by heating barium carbonate with coke, carbon black or tar or by thermal decomposition of barium nitrate. Barium oxide is used as a coating for hot cathodes, for example, those in cathode ray tubes. It replaced lead(II) oxide in the production of certain kinds of glass such"
"four water ligands and benzoate. Copper benzoate Copper benzoate is the chemical compound with the formula Cu(CHCO). This coordination complex is derived from the cupric ion and the conjugate base of benzoic acid. Because copper emits blue in a flame, this salt has found some use as a source of blue light in fireworks. In laboratory, copper benzoate can be made by combining aqueous solutions of potassium benzoate with copper sulfate. Copper benzoate precipitates as a pale blue solid: The primary use of this compound is in production of blue flame in fireworks. Copper benzoate made from sodium benzoate for"
"Mercury(I) bromide Mercury(I) bromide or mercurous bromide is the chemical compound composed of mercury and bromine with the formula HgBr. It changes color from white to yellow when heated and fluoresces a salmon color when exposed to ultraviolet light. It has applications in acousto-optical devices. A very rare mineral form is called kuzminite, Hg(Br,Cl). Mercury(I) bromide is prepared by the oxidation of elemental mercury with elemental bromine or by adding sodium bromide to a solution of mercury(I) nitrate. It decomposes to mercury(II) bromide and elemental mercury. In common with other Hg(I) (mercurous) compounds which contain linear X-Hg-Hg-X units, HgBr contains"
"Erbium(III) chloride Erbium(III) chloride, is a violet solid with the formula ErCl. It is used in the preparation of erbium metal. It is also found as a pink crystalline hexahydrate, CAS number [10025-75-9]. It has the interesting property that the pink colour is much more intense under the light from a fluorescent lamp, as may be seen from the picture. Anhydrous erbium(III) chloride is formed from the hexahydrate by heating under a strongly chlorinating atmosphere, such as chlorine or hydrogen chloride; otherwise erbium oxide chloride, ErOCl, is formed. An alternative preparation is to react the readily available ErO with excess"
"Copper benzoate Copper benzoate is the chemical compound with the formula Cu(CHCO). This coordination complex is derived from the cupric ion and the conjugate base of benzoic acid. Because copper emits blue in a flame, this salt has found some use as a source of blue light in fireworks. In laboratory, copper benzoate can be made by combining aqueous solutions of potassium benzoate with copper sulfate. Copper benzoate precipitates as a pale blue solid: The primary use of this compound is in production of blue flame in fireworks. Copper benzoate made from sodium benzoate for use in fireworks may result"
"Environmentally-friendly red light flare An environmentally-friendly red-light flare was a pyrotechnic (firework) flare which used lithium-based formulations that emitted red light. A flare is used for signaling, illumination, or defensive countermeasures in civilian or military applications. It is based on a non-hygroscopic (not absorbing air) dilithium nitrogen-rich salt that served as an oxidizer and red colorant. The U.S. Army Research Laboratory and the Ludwig Maximilian Institution were credited as the research facilities for developing this product announced in January 2018. As of 2018, this is the first documented red-light flare compound that is based on lithium and does not contain"
"hydrochloric acid, releasing chlorine. The irreversible reaction of digesting barium chromate with a solution of sodium ferrate forms barium ferrate, and the color of the solution is changed from red to yellow due to the sodium chromate that is also formed. Alkaline sulfates decompose barium ferrate that has not been dried, forming barium sulfate, ferric hydroxide and oxygen gas. Barium ferrate, therefore, appears to be one of the most insoluble salts known. Barium ferrate Barium ferrate is the chemical compound of formula BaFeO. This is a rare compound containing iron in the +6 oxidation state. The ferrate(VI) ion has two"
"Strontium nitrate Strontium nitrate is an inorganic compound made of the elements strontium and nitrogen with the formula Sr(NO). This colorless solid is used as a red colorant and oxidizer in pyrotechnics. Strontium nitrate is typically generated by the reaction of nitric acid on strontium carbonate. Like many other strontium salts, strontium nitrate is used to produce a rich red flame in fireworks and road flares. The oxidizing properties of this salt are advantageous in such applications. Strontium nitrate can aid in eliminating and lessening skin irritations. When mixed with glycolic acid, strontium nitrate reduces the sensation of skin irritation"
"in both oxidation and reduction atmospheres. However, in the presence of magnesium, cobalt can become purple, pink or reddish blue depending on whether it was fired in oxidation (yields purple) or reduction. Cobalt is also commonly used in black glazes and in washes as decorative medium. Common saturation percentages for low saturation range from (.25 to .5%) and in high saturation from (1 to 2%). ""Chrome is a rather versatile and fickle colorant,"" (Chappell). Chrome oxide (CrO) is commonly used for achieving greens. However, in the presence of zinc, chrome can produce brown. Glazes with tin oxide present will often"
"as optical crown glass. While lead oxide raised the refractive index, it also raised the dispersive power, which barium oxide does not alter. Barium oxide also has use as an ethoxylation catalyst in the reaction of ethylene oxide and alcohols, which takes place between 150 and 200 °C. It is also a source of pure oxygen through heat fluctuation. It readily oxidises to BaO by formation of a peroxide ion. The complete peroxidation of BaO to BaO occurs at moderate temperatures but the increased entropy of the O molecule at high temperatures means that BaO decomposes to O and BaO"
"blush to pink if fumed with chrome or if chrome is present in the glaze with the tin, often intense pinks occur. If fired above cone 6, chrome will fume and become a gas in the kiln. Common saturation percentages for chrome at low saturation range from (.25 to .5%) and at higher percentages from (1 to 2%). Chrome is a refractory. Iron is commonly used as a colorant in its red iron oxide form as (FeO). Red iron oxide is commonly used to produce earthy reds and browns. It is the metal responsible for making earthenwares red. Iron is"
"all the pellets are the same. Uranium oxide (urania) was used to color glass and ceramics prior to World War II, and until the applications of radioactivity were discovered this was its main use. In 1958 the military in both the USA and Europe allowed its commercial use again as depleted uranium, and its use began again on a more limited scale. Urania-based ceramic glazes are dark green or black when fired in a reduction or when UO is used; more commonly it is used in oxidation to produce bright yellow, orange and red glazes. Orange-colored Fiestaware is a well-known"
"actinium hydroxide and thorium hydroxide: these three adjacent hydroxides may be separated by precipitating them with ammonia. Radium chloride (RaCl) is a colorless, luminous compound. It becomes yellow after some time due to self-damage by the alpha radiation given off by radium when it decays. Small amounts of barium impurities give the compound a rose color. It is soluble in water, though less so than barium chloride, and its solubility decreases with increasing concentration of hydrochloric acid. Crystallization from aqueous solution gives the dihydrate RaCl·2HO, isomorphous with its barium analog. Radium bromide (RaBr) is also a colorless, luminous compound. In"
"Chrome yellow Chrome yellow is lead(II) chromate (PbCrO). It occurs naturally as the mineral crocoite but the mineral itself was never used as a pigment for paint. After the French chemist Louis Vauquelin discovered the new element chromium in 1797 lead chromate was synthesized in the laboratory and its use as a pigment began in the second decade of the nineteenth century. Chrome yellow had been commonly produced by mixing solutions of lead nitrate and potassium chromate and filtering off the lead chromate precipitate. Because the pigment tends to react with hydrogen sulfide and darken on exposure to air over"
"Pyridinium chlorochromate Pyridinium chlorochromate (PCC) is a yellow-orange salt with the formula [CHNH][CrOCl]. It is a reagent in organic synthesis used primarily for oxidation of alcohols to form carbonyls. A variety of related compounds are known with similar reactivity. Although no longer widely used, PCC offers the advantage of the selective oxidation of alcohols to aldehydes or ketones, whereas many other reagents are less selective. PCC consists of a pyridinium cation, [CHNH], and a tetrahedral chlorochromate anion, [CrOCl]. Related salts are also known, such as 1-butylpyridinium chlorochromate, [CHN(CH)][CrOCl] and potassium chlorochromate. PCC is commercially available. Discovered by accident, the reagent"
"stars—usually just called stars—which produce intense light when ignited. Stars contain five basic types of ingredients. Some of the more common color-producing compounds are tabulated here. The color of a compound in a firework will be the same as its color in a flame test (shown at right). Not all compounds that produce a colored flame are appropriate for coloring fireworks, however. Ideal colorants will produce a pure, intense color when present in moderate concentration. The brightest stars, often called Mag Stars, are fueled by aluminium. Magnesium is rarely used in the fireworks industry due to its lack of ability"
"search for substitutes for chromium or at least a change to less toxic chromium(III) compounds. The mineral crocoite (which is also lead chromate PbCrO) was used as a yellow pigment shortly after its discovery. After a synthesis method became available starting from the more abundant chromite, chrome yellow was, together with cadmium yellow, one of the most used yellow pigments. The pigment does not photodegrade, but it tends to darken due to the formation of chromium(III) oxide. It has a strong color, and was used for school buses in the United States and for the Postal Service (for example, the"
"are altered, allowing them to combine with the iron in the blood, whilst the carbonate reacts with the haemoglobin to produce a solid. After heating the resulting solid to an ash, filtering and diluting, Diesbach added green vitriol (iron sulphate) to create a complex ion: ferric ferrocyanide. Finally, adding spirit of salt (hydrochloric acid) draws out a brilliant colour: Prussian blue. Ever since seeing fireworks as a child, another German chemist, Justus von Liebig, had become obsessed with trying to better understand the elements by creating explosive combinations. Specifically, he was interested in the explosive compound silver fulminate. In 1825"