Consider the perchlorate (ClO 4 ) ion. (a) Assign oxidation states to all of the atoms

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Consider the perchlorate (ClO₄^–) ion.

(a) Assign oxidation states to all of the atoms in perchlorate.

(b) Explain why the chlorine atom in perchlorate does not follow the halide rule.

(d) Would it be possible to have an even higher oxidation state for the Cl atom in some other compound? Explain.

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Introductory Chemistry Atoms First

ISBN: 9780321927118

5th Edition

Authors: Steve Russo And Michael Silver

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Question Posted: Dec 05, 2023 05:08 AM

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Consider the perchlorate (ClO 4 ) ion. (a) Assign oxidation states to all of the atoms

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a In the perchlorate ion ClO4 the oxidation state of chlorine is 7 This is the highest oxidation sta...View the full answer

Introductory Chemistry Atoms First

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