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How are the chlorate and chlorite ions different from each other? How are they sim

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Answered by GPT-5 mini AI
Short answer first:
- Chlorate = ClO3^-; chlorite = ClO2^-.
- Chlorate has one more oxygen and a higher chlorine oxidation state (+5) than chlorite (+3).
- Both are oxyanions of chlorine, carry a single negative charge, and are oxidizing species, but chlorate is generally the stronger oxidizer.

Details and comparison

Similarities
- Both are chlorine oxyanions with overall charge −1.
- Both have resonance-stabilized Cl–O bonding and place most negative charge on oxygen atoms.
- Both are conjugate bases of oxyacids (chlorite ← HClO2, chlorate ← HClO3) and form salts such as NaClO2 (sodium chlorite) and NaClO3 (sodium chlorate).
- Both can act as oxidizing agents.

Differences
- Formula: chlorite = ClO2^- ; chlorate = ClO3^-.
- Oxidation state of Cl: chlorite +3, chlorate +5.
- Geometry: chlorite has three electron domains (two O atoms + one lone pair) → bent molecular shape; chlorate has four electron domains (three O atoms + one lone pair) → trigonal pyramidal molecular shape.
- Bond orders (from resonance): average Cl–O bond order ≈ 1.5 in chlorite, ≈ 1.33 in chlorate.
- Acidity: chlorous acid (HClO2) is a weak acid (pKa ≈ 1.96); chloric acid (HClO3) is a strong acid (largely dissociated).
- Reactivity: chlorate (higher oxidation state) is usually a stronger oxidizer; chlorite is also a good oxidizer but less so and is often used to generate chlorine dioxide.

Naming tip: the “-ite” ion has one fewer oxygen than the corresponding “-ate” ion (chlorite < chlorate).