Cadmium bromide

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Cadmium bromide
Cadmium bromide
IUPAC name
Cadmium(II) bromide
Other names
Cadmium dibromide
3D model (JSmol)
ECHA InfoCard 100.029.241
RTECS number EU9935000
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)
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.
-87.3·10−6 cm3/mol
Rhombohedral, hr9, SpaceGroup = R-3m, No. 166
Harmful (Xn)
Dangerous for the environment (N)
R-phrases (outdated) R20/21/22, R50/53
S-phrases (outdated) (S2), S60, S61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
Lethal dose or concentration (LD, LC):
225 mg/kg, oral (rat)
US health exposure limits (NIOSH):
PEL (Permissible)
[1910.1027] TWA 0.005 mg/m3 (as Cd)[1]
REL (Recommended)
IDLH (Immediate danger)
Ca [9 mg/m3 (as Cd)][1]
Related compounds
Other anions
Cadmium chloride,
Cadmium iodide
Other cations
Zinc bromide,
Calcium bromide,
Magnesium bromide
Except where otherwise noted, 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.


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


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.[2]


  1. ^ a b c "NIOSH Pocket Guide to Chemical Hazards #0087". National Institute for Occupational Safety and Health (NIOSH). 
  2. ^ Patnaik, P. (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.