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How are the chlorate and chlorite ions different from each other? How are they similar to the sulfate and sulfite ions?
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Differences
- Formulas: chlorate = ClO3^-; chlorite = ClO2^- (chlorate has one more oxygen).
- Oxidation state of Cl: +5 in ClO3^- (chlorate) vs +3 in ClO2^- (chlorite).
- Charge: both chlorate and chlorite are singly charged anions (−1).
- Geometry: ClO3^- is commonly described as trigonal-pyramidal (three bonding O plus one lone pair on Cl in resonance-averaged structures); ClO2^- is bent (two bonding O and more lone-pair character).
- Acids: chloric acid HClO3 vs chlorous acid HClO2.
Similarities to sulfate/sulfite
- Same naming pattern: “-ate” means the oxyanion with more oxygens, “-ite” has one fewer oxygen (e.g. sulfate SO4^2- vs sulfite SO3^2-).
- Both are families of oxyanions (central atom + oxygen); their negative charge is delocalized by resonance over the oxygens.
- Each pair has corresponding oxyacids (HClO3/HClO2 and H2SO4/H2SO3).
- In each pair the central atom has a higher oxidation state in the “-ate” ion than in the “-ite” ion (Cl +5 vs +3; S +6 vs +4).
Key difference between the two families: the halogen oxyanions (chlorate/chlorite) carry −1 charge, whereas the chalcogen oxyanions (sulfate/sulfite) carry −2, because Cl is from group 17 while S is from group 16.
- Formulas: chlorate = ClO3^-; chlorite = ClO2^- (chlorate has one more oxygen).
- Oxidation state of Cl: +5 in ClO3^- (chlorate) vs +3 in ClO2^- (chlorite).
- Charge: both chlorate and chlorite are singly charged anions (−1).
- Geometry: ClO3^- is commonly described as trigonal-pyramidal (three bonding O plus one lone pair on Cl in resonance-averaged structures); ClO2^- is bent (two bonding O and more lone-pair character).
- Acids: chloric acid HClO3 vs chlorous acid HClO2.
Similarities to sulfate/sulfite
- Same naming pattern: “-ate” means the oxyanion with more oxygens, “-ite” has one fewer oxygen (e.g. sulfate SO4^2- vs sulfite SO3^2-).
- Both are families of oxyanions (central atom + oxygen); their negative charge is delocalized by resonance over the oxygens.
- Each pair has corresponding oxyacids (HClO3/HClO2 and H2SO4/H2SO3).
- In each pair the central atom has a higher oxidation state in the “-ate” ion than in the “-ite” ion (Cl +5 vs +3; S +6 vs +4).
Key difference between the two families: the halogen oxyanions (chlorate/chlorite) carry −1 charge, whereas the chalcogen oxyanions (sulfate/sulfite) carry −2, because Cl is from group 17 while S is from group 16.
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