2 Answers

Emk · Answer 1 · 2018-12-05T03:17:07+0000

Final answer:

The oxidation state of phosphorus in the phosphate ion ((PO₃³⁻) is +3, which is determined by the known oxidation state of oxygen and the overall charge of the ion.

Step-by-step explanation:

To determine the oxidation state of phosphorus in the phosphate ion (PO₃³⁻), we can use the known oxidation state of oxygen and the overall charge of the ion. Oxygen typically has an oxidation state of −2. Since there are three oxygen atoms, their total contribution is −6. The overall charge of the ion is −3, which means phosphorus must balance this with an oxidation state that, when added to the contribution from oxygen, equals the overall charge.

The equation representing this balance is:

x (oxidation state of P) + 3(−2) = −3

Solving for x yields:

x = −3 + 6

x = +3

Therefore, the oxidation state of phosphorus in PO₃³⁻ is +3.

Zermingore · Answer 2 · 2018-12-07T21:12:11+0000

Express the oxidation state numerically (e.g., +1).

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Ions

In an ion, the sum of the oxidation states is equal to the overall ionic charge. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In OH−, for example, the oxygen atom has an oxidation state of −2 and the hydrogen atom has an oxidation state of +1, for a total of (−2)+(+1)=−1.