Lead bromate chlorate

Impact sensitivities of mixtures of red phosphorus with various oxidants were determined in a direct drop-ball method, which indicated higher sensitivities than those determined with an indirect striker mechanism. Mixtures with silver chlorate were most sensitive, those with bromates, chlorates and chlorites were extremely sensitive, and mixtures with sodium peroxide and potassium superoxide were more sensitive than those with barium, calcium, magnesium, strontium or zinc peroxides. Mixtures with perchlorates or iodates had sensitivities comparable to those of unmixed explosives, such as lead azide, 3,5-dinitrobenzenediazonium-2-oxide etc. 

Lead acetate-lead bromate, 1540 Lead(II) chlorite, 4102 Mercury(II) bromate, 0270 Potassium bromate, 0255 Potassium chlorate, 4017 Potassium periodate, 4620 Silver bromate, 0007... 

Lead Aceto-Bromate A29"L Lead Aceto-Chlorate A29"L... 

Indications. A blue colour indicates the presence of an oxidising agent such as bromate, chlorate, chromate, dichromate, iodate, lead (IV), manganese (III, IV, VII), nitrate, nitrite, permanganate, or vanadate. 

Lead Aceto-Bromate A29"L Lead Aceto-Chlorate A29 L Lead Aceto Perchlorate A29"L Lead Aceto-Sodium Perchlorate A29-L Lead Acetylide A76-R Lead Azide (Lead Diazide) (LA) Aj45 to A556... 

Lead Aceto-Bromate A29 L Lead Aceto-Chlorate A29 L... 

COPPER (7440-50-8) Cu The powder forms the friction-, heat-, or shock-sensitive explosive detonator, copper acetylide, with acetylene gas acetylenic compounds and ethylene oxides. The powder forms explosive materials with azides (e.g., sodium azide forms potentially explosive copper azide). Finely divided material forms friction-, heat-, or shock-sensitive explosive with powdered divided bromates, chlorates, and iodates of barimn, calcimn, magnesium, potassium, sodium, or zinc. Violent reaction, possibly explosive, when finely dispersed powder comes in contact with strong oxidizers ammonium nitrate alkynes, bromine vapor, calcium carbide, chlorine, ethylene oxide, hydrazine mononitrate, hydrogen peroxide, hydrogen sulfide, finely divided bromates, iodine, lead azide, potassium peroxide, sodium peroxide (incandescence), sulfuric acid. Incompatible with acids, anhydrous ammonia chemically active metals such as potassium, sodium, magnesium, and zinc, zirconium, strong bases. 

LEAD SULFIDE (1314-87-0) PbS Noncombustible solid. Reacts violentiy with iodine monochloride, hydrogen peroxide. Incompatible with bromates, chlorates, hydrazinium nitrate, iodates, mercurous chloride, silver azide, zinc(II) nitrate, hexahydrate. 

Chlorates and bromates feature the expected pyramidal ions X03 with angles close to the tetrahedral (106-107°). With iodates the interatomic angles at iodine are rather less (97-105°) and there are three short I-O distances (177-190 pm) and three somewhat longer distances (251-300 pm) leading to distorted perovskite structures (p. 963) with pseudo-sixfold coordination of iodine and piezoelectric properties (p. 58). In Sr(I03)2.H20 the coordination number of iodine rises to 7 and this increases still further to 8 (square antiprism) in Ce(I03)4 and Zr(I03)4. 

Hydroxylamine is a powerful reducant, particularly when anhydrous, and if exposed to air on a fibrous extended surface (filter paper) it rapidly heats by aerobic oxidation. It explodes in contact with air above 70°C [1]. Barium peroxide will ignite aqueous hydroxylamine, while the solid ignites in dry contact with barium oxide, barium peroxide, lead dioxide and potassium permanganate, but with chlorates, bromates and perchlorates only when moistened with sulfuric acid. Contact of the anhydrous base with potassium dichromate or sodium dichromate is violently explosive, but less so with ammonium dichromate or chromium trioxide. Ignition occurs in gaseous chlorine, and vigorous oxidation occurs with hypochlorites. 

Lead dioxide Lead perchlorate Lithium chlorate Lithium hypochlorite Lithium perchlorate Lithium peroxide Magnesium bromate Magnesium chlorate Magnesium perchlorate Magnesium peroxide Manganese dioxide Mercurous chlorate Mono-(trichloro)-tetra-(mono-potassium dichloro)-penta-s-triazinetrione... 

Hydrofluoric acid like water is an associated liquid, and even the gas, as we shall soon see, is associated. It has the power of uniting with fluorides. It also seems to be an ionizing solvent for a soln. of potassium fluoride in liquid hydrogen fluoride is an excellent conductor it also possesses marked solvent powers. According to E. C. Franklin,7 the liquid readily dissolves potassium fluoride, ehloride, and sulphate sodium fluoride, bromide, nitrate, chlorate, and bromate acetamide and urea. The solvent action is not so marked with barium fluoride, cupric chloride, and silver cyanide while calcium and lead fluorides copper sulphate and nitrate ferric chloride, mercuric oxide, and magnesium metal, are virtually insoluble in this menstruum. Glass also is not affected by the liquid if moisture be absent. The liquid scarcely acts on most of the metals or non-metals at ordinary temp., though it does act on the alkali metals at ordinary temp., much the same as does water, with the simultaneous production of flame. 

The violence of the explosion is feebler with iodates than it is with chlorates or bromates. The chlorates transform lead oxide to the dioxide manganese oxide in fused alkalies to manganates etc. Ammonium iodate explodes when heated alone. Chloric, bromic, and iodic acids with their salts are energetic oxidizing agents. 

Heating samples of this or the corresponding chlorine compounds, leads to explosions if contaminated with caesium bromate or chlorate, which are byproducts of the syntheses. 

Lead chromate Sulfur Lead(II) chlorite Non-metals Phosphorus(III) oxide Potassium bromate Non-metals Potassium chlorate Charcoal, etc., or Non-metals Potassium chlorite Sulfur Potassium perchlorate Sulfur Potassium permanganate Non-metals Silver bromate Sulfur compounds Silver chlorite Hydrochloric acid, etc. 

Oxygen may also be obtaiued by heating the chlorates of other metals, notably barium,1 calcium,2 strontium,3 lead,4 and silver,5 or by decomposition of metallic bromates and iodates.6... 

IV.21 IODATES, IO3 Solubility The iodates of the alkali metals are soluble in water those of the other metals are sparingly soluble and, in general, less soluble than the corresponding chlorates and bromates. Some solubilities in g -1 at 20° are lead iodate 0 03 (25°), silver iodate 0-06, barium iodate O 22, calcium iodate 3-7, potassium iodate 81-3, and sodium iodate 90 0. Iodic acid is a crystalline solid, and has a solubility of 2,330 g t 1 at 20°. 

Mercury(II) nitrate solution white precipitate of mercury(II) iodate (difference from chlorate and bromate). Lead acetate solution similarly gives a precipitate of lead iodate. Mercury(II) chloride solution, which is practically un-ionized (as mercuric chloride is covalent) gives no precipitate. 

---