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Assign an oxidation state to each element in each reaction and use the change in

Chapter 16, Problem 57P

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QUESTION:

What is the oxidation state of S in each ion?

(a) \(\mathrm{SO}_4{ }^{2-}\)

(b) \(\mathrm{SO}_3{ }^{2-}\)

(c) \(\mathrm{HSO}_3{ }^{-}\)

(d) \(\mathrm{HSO}_4^{-}\)

Questions & Answers

QUESTION:

What is the oxidation state of S in each ion?

(a) \(\mathrm{SO}_4{ }^{2-}\)

(b) \(\mathrm{SO}_3{ }^{2-}\)

(c) \(\mathrm{HSO}_3{ }^{-}\)

(d) \(\mathrm{HSO}_4^{-}\)

ANSWER:

Step 1 of 5

The following rules should be followed to calculate the oxidation number of an element in the compound.

1) The oxidation number of the atoms in any free, uncombined element, is zero

2) The sum of the oxidation numbers of all atoms in a compound is zero

3) The sum of the oxidation numbers of all atoms in an ion is equal to the charge of the ion

4) The oxidation number of fluorine in all its compounds is

5) The oxidation number of other halogens in their compounds is usually

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