Chlorate

Chlorate
Structure and bonding in the chlorate ion
The chlorate ion
Names
Other names
Chlorate(V)
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
1491
UNII
UN number 1461
  • InChI=1S/ClHO3/c2-1(3)4/h(H,2,3,4)/p-1
    Key: XTEGARKTQYYJKE-UHFFFAOYSA-M
  • O=Cl(=O)[O-]
Properties
ClO3
Molar mass 83.4512
Structure
Trigonal pyramidal
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
oxidation agent
Related compounds
Other anions
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Chlorate is the common name of the ClO
3
anion, whose chlorine atom is in the +5 oxidation state. The term can also refer to chemical compounds containing this anion, with chlorates being the salts of chloric acid. Other oxyanions of chlorine can be named "chlorate" followed by a Roman numeral in parentheses denoting the oxidation state of chlorine: e.g., the ClO
4
ion commonly called perchlorate can also be called chlorate(VII).

As predicted by valence shell electron pair repulsion theory, chlorate anions have trigonal pyramidal structures.

Chlorates are powerful oxidizers and should be kept away from organics or easily oxidized materials. Mixtures of chlorate salts with virtually any combustible material (sugar, sawdust, charcoal, organic solvents, metals, etc.) will readily deflagrate. Chlorates were once widely used in pyrotechnics for this reason, though their use has fallen due to their instability. Most pyrotechnic applications that formerly used chlorates now use the more stable perchlorates instead.