|Molar mass||366.22 g/mol|
|Appearance||white to pale yellow crystals|
|Density||5.640 g/cm3, solid|
|Melting point||387 °C (729 °F; 660 K)|
|Boiling point||742 °C (1,368 °F; 1,015 K)|
|787 g/L (0 °C)
847 g/L (20 °C)
1250 g/L (100 °C)
|Solubility||soluble in ethanol, acetone, ether and ammonia|
|Trigonal, hP3, space group P3m1, No. 164|
|EU classification||T Xn N|
|R-phrases||R23/25, R33, R68, R50/53|
|S-phrases||(S2), S22, S45, S60, S61|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is: / ?)(|
Cadmium iodide is prepared by the addition of cadmium metal, or its oxide, hydroxide or carbonate to hydroiodic acid.
Also, the compound can be made by heating cadmium with iodine.
In cadmium iodide the iodide anions form a hexagonal close packed arrangement while the cadmium cations fill all of the octahedral sites in alternate layers. The resultant structure consists of a layered lattice. This same basic structure is found in many other salts and minerals. Cadmium iodide is mostly ionically bonded but with partial covalent character.
Cadmium iodide's crystal structure is the prototype on which the crystal structures many other compounds can be considered to be based. Compounds with any of the following characteristics tend to adopt the CdI2 structure:
- Iodides of moderately polarising cations; bromides and chlorides of strongly polarising cations
- Hydroxides of dications, i.e. compounds with the general formula M(OH)2
- Sulfides, selenides and tellurides (chalcogenides) of tetracations, i.e. compounds with the general formula MX2, where X = S, Se, Te
Compounds with the CdI2 crystal structure
Chlorides and bromides
Hydroxides of M2+
Chalcogenides of M4+