Chlorate

Chlorate

Names
Other names Chlorate(V)
Identifiers
CAS Number	14866-68-3
3D model (JSmol)	Interactive image
ChEBI	CHEBI:49709 ion CHEBI:23109 class of salts
ChemSpider	94578
Gmelin Reference	1491
PubChem CID	104770
UNII	08Z8093742
UN number	1461
CompTox Dashboard (EPA)	DTXSID3073137
InChI InChI=1S/ClHO3/c2-1(3)4/h(H,2,3,4)/p-1 Key: XTEGARKTQYYJKE-UHFFFAOYSA-M
SMILES O=Cl(=O)[O-]
Properties
Chemical formula	ClO3−
Molar mass	83.4512
Structure
Molecular shape	Trigonal pyramidal
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	oxidation agent
Related compounds
Other anions	bromate iodate
Related compounds	chloride hypochlorite chlorite perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

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.