What are the oxidation numbers of the chlorine and oxygen atoms in the perchlorate ion (ClO4–)?

Oxygen: –2

Chlorine: +7

Question

What are the oxidation numbers of the chlorine and oxygen atoms in the perchlorate ion (ClO4–)?

Oxygen: –2

Chlorine: +7

BlackTom AI · Accepted Answer

The perchlorate ion ClO4– consists of one chlorine atom bonded to four oxygen atoms, with an overall charge of −1. 
First, assign the common oxidation state to oxygen in most oxides: each oxygen is typically −2. With four oxygens, the total from oxygen is 4 × (−2) = −8. 
Let x be the oxidation state of chlorine. The sum of oxidation states in the ion must equal the overall charge, so x + (−8) = −1. Solving gives x = +7 for chlorine. 
Thus, each oxygen is in the −2 oxidation state, and chlorine is in the +7 oxidation state in ClO4–. 
This aligns with standard rules for oxidation states in oxyanions, where chlorine can exhibit high oxidation states (up to +7) in highly oxidized species like perchlorate. 
Note on the provided options: since the question states Oxygen: −2 and Chlorine: +7 as the chosen pair, this corresponds to the correct balancing of the charge on ClO4–. Any alternative pair would violate either the known oxidation state of oxygen in most compounds or the overall charge balance of the ion.

CHEM 110 Section 3 (PM) SP25 Pre-Lecture Quiz 38 C15-3-4

What are the oxidation numbers of the chlorine and oxygen atoms in the perchlorate ion (ClO4–)? Oxygen: –2 Chlorine: +7

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