Cadmium bromide

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Cadmium bromide
Cadmium bromide
Identifiers
CAS number 7789-42-6 YesY
13464-92-1 (tetrahydrate)
PubChem 24609
ChemSpider 23011 YesY
UNII 7726AXS0WH YesY
RTECS number EU9935000
Jmol-3D images Image 1
Properties
Molecular formula CdBr2
Molar mass 272.22 g/mol
Appearance white to pale yellow crystalline solid
Density 5.192 g/cm3, solid
Melting point 568 °C (1,054 °F; 841 K)
Boiling point 844 °C (1,551 °F; 1,117 K)
Solubility in water 56.3 g/100 mL (0 °C)
98.8 g/100 mL (20 °C)
160 g/100 mL (100 °C)
Solubility soluble in alcohol, ether, acetone and liquid ammonia.
Structure
Crystal structure Rhombohedral, hr9, SpaceGroup = R-3m, No. 166
Hazards
EU Index 048-001-00-5
EU classification Harmful (Xn)
Dangerous for the environment (N)
R-phrases R20/21/22, R50/53
S-phrases (S2), S60, S61
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
LD50 225 mg/kg, oral (rat)
Related compounds
Other anions Cadmium chloride,
Cadmium iodide
Other cations Zinc bromide,
Calcium bromide,
Magnesium bromide
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Cadmium bromide is a cream-coloured crystalline ionic cadmium salt of hydrobromic acid that is soluble in water. It is very toxic, along with other cadmium compounds.

Uses[edit]

It is used in the manufacturing of photographic film, engraving and lithography.

Preparation[edit]

Cadmium bromide is prepared by heating cadmium with bromine vapor. Also the compound can be prepared by the treatment of dry cadmium acetate with glacial acetic acid and acetyl bromide. Alternatively, it can be obtained by dissolving cadmium or cadmium oxide in hydrobromic acid and evaporating the solution to dryness under helium in an inert atmosphere.[1]

References[edit]

  1. ^ Patnaik, P. (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.