Alkali metals calcium

Copper(II) sulfate Cumene hydroperoxide Cyanides Cyclohexanol Cyclohexanone Decaborane-14 Diazomethane 1,1-Dichloroethylene Dimethylformamide Hydroxylamine, magnesium Acids (inorganic or organic) Acids, water or steam, fluorine, magnesium, nitric acid and nitrates, nitrites Oxidants Hydrogen peroxide, nitric acid Dimethyl sulfoxide, ethers, halocarbons Alkali metals, calcium sulfate Air, chlorotrifluoroethylene, ozone, perchloryl fluoride Halocarbons, inorganic and organic nitrates, bromine, chromium(VI) oxide, aluminum trimethyl, phosphorus trioxide... 

Chromates are usually yellow or red in colour, and, except those of ammonium, the alkali metals, calcium, strontium, and magnesium, are practically insoluble in w ater. They are obtained by oxidation of chromites, by fusion of chromium sesquioxide with the appropriate base in presence of air or of an oxidising agent by oxidation of chromium salts in solution or by double decomposition. Normal, di-, and tri-clrromates, etc., are derived from one and the same acid oxide KaCrOj behaves like an alkali torvards CrOg, since it is quantitatively converted into dichromate. A large number of complex double chromates are known. 

AMILMERCAPTANO (Spanish) (110-66-7) Forms explosive mixture with air (flash point 65°F/18°C). Ignites on contact with concentrated nitric acid. Contact with water, steam, or acids produces toxic and flammable vapors. Incompatible with oxidizers, reducing agents, alkali metals, calcium hypochlorite. 

Alkali metals, calcium hypochlorite, halogens, oxidizers... 

Incompatibilities and Reactivities Alkali metals, calcium oxide... 

In the third step of the analysis, 1 ml of dilute ammonia is added upon which the precipitate dissolves. And in the final step of analysis 1 ml of ammonium carbonate solution R is added. This must not give a precipitate. This alkaline media will dissolve the sodium methoxyphenylacetic acid salt, but reveal if the precipitate was of one of the earth alkali metals calcium, strontium, or barium, since these ions form insoluble hydroxides and carbonates at high pH. Also salts of heavy metals are revealed in this way ... 

The metals commonly employed in these reductions include the alkali metals, calcium, zinc, magnesium, tin and iron. The alkali metals are often used in solution in liquid ammonia or as suspensions in inert solvents such as ether or toluene, frequently with addition of an alcohol or water to act as a proton source. Many reductions are also effected by direct addition of sodium, or particularly, zinc or tin to a solution of the compound being reduced in a hydroxylic solvent, such as ethanol, acetic acid or an aqueous mineral acid. 

Major Hazards Powerful allergen with high acute toxicity extremely unstable may explode on contact with alkali metals, calcium sulfate (Drierite), or rough edges such as those found on ground glass. 

Beall G.H., "Alkali Metal, Calcium Fluorosilicate Glass-Ceramic Article," U.S. Pat. No. 4 386 162,1983. 

The group 2A elements, called the alkaline earth metals, are also fairly reactive, although not quite as reactive as the alkali metals. Calcium, for example, reacts fairly vigorously when dropped into water but does not explode as dramatically as sodium. Other alkaline earth metals include magnesium (a conunon low-density structural metal), stfontium, and barium. 

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