To determine the oxidation state of the
individual nitrogen atom in NH4OH, certain rules on oxidation numbers must be
followed. Here are the relevant rules that will be useful.
1. The sum
of the oxidation numbers of all the atoms for a neutral compound is zero.
2. The
oxidation number of H is +1 when combined with more electronegative elements.
In this case, N and O are more electronegative than H.
3. The
oxidation number of O is typically -2 in compounds.
It should also be noted that the number of atoms of an
element present on the compound must be multiplied to its oxidation number. Thus,
we have the following equation:
(Oxidation no. of N) + 5(Oxidation no. of H) + (Oxidation no.
of O) = 0
(Oxidation no. of N) + 5(1) + (-2) = 0
(Oxidation no. of N) = -3
Thus, the oxidation state/number of N in NH4OH is -3.
