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Chapter 17: Problem 46

Determine the oxidation number of each atom in \(\mathrm{PO}_{4}^{3-} .\)

Short Answer

Expert verified
The oxidation number of Phosphorus (P) in \(\mathrm{PO}_{4}^{3-}\) is +5 and that of Oxygen (O) is -2.

Step by step solution

01

Identifying Oxygen Oxidation State

In most compounds, the oxidation state of oxygen is -2. So for four oxygen atoms the cumulative oxidation state is -2 * 4 = -8.
02

Determining Phosphorus Oxidation State

The overall charge of \( \mathrm{PO}_{4}^{3-} \) is -3 and the sum of oxidation numbers in this ion should be equal to this charge, so the oxidation number for Phosphorus must make the sum of the oxidation numbers equal to -3. If we let the oxidation number of Phosphorus be x, the equation becomes: x + (-8) = -3. Solving for x gives x = +5.
03

Final Oxidation Numbers

So, the oxidation number of Phosphorus (P) is +5 and that of Oxygen (O) is -2.

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