Oxidation state on
as in the nitrate ion
: +5.
Explanation
The sum of oxidation states on all atoms in an ion should be the same as the charge of the ion.
The oxidation state of nitrogen N tends to vary. However, the oxidation state of oxygen O is -2 in most cases, with the following exceptions:
Oxidation state of O in
![\text{O}_2](/tpl/images/0487/1109/c4be0.png)
: 0.Oxidation state of O in
![\text{H}_2\text{O}_2](/tpl/images/0487/1109/5039e.png)
and other peroxides: -1.The oxidation state of O will be positive when it is bonded to fluorine F.
To find the oxidation state on N, consider the atoms in a nitrate ion:
There are three O atoms in each nitrate ion, as seen in the subscript "3".There's only one N atom in each nitrate ion.
The oxidation state of each O atom is expected to be -2. There are three O atoms in each nitrate ion. The oxidation state of the three atoms will add up to
.
The oxidation state of the N atom needs to be found. Charge on the nitrate ion is -1. Thus
![\begin{array}{ccc}\text{oxidation state on all atoms in the ion}&= &\text{charge of the ion}\\(\text{oxidation state on N}) + 3 \times (-2) &=& -1\end{array}](/tpl/images/0487/1109/4d68d.png)
.
Therefore, the oxidation state of the nitrogen N atom in the nitrate ion
is +5.