- Hydrogen (H) typically has an oxidation number of +1 in most compounds, except in metal hydrides where it can be -1. In this case, let's assign it +1.
- Oxygen (O) usually has an oxidation number of -2 in compounds.
- Phosphorus (P) is the central atom, so its oxidation number is variable and needs to be determined.
Using the following formula, we can calculate the oxidation number of P:
\(Charge\ of\ the\ molecule = \sum (Oxidation\ numbers\ of\ individual\ atoms\times their\ respective\ counts) \)
The charge of H3PO2 is 0 since it is a neutral molecule.
Plugging in the assigned oxidation numbers:
\( 0 = (3 \times +1) + (2 \times -2) + (1 \times Oxidation\ number\ of\ P) \)
Simplifying the equation:
\( 0 = +3 -4 + Oxidation\ number\ of\ P \)
\( Oxidation\ number\ of\ P = +4 -3 = +1\)
Therefore, the oxidation number of phosphorus in H3PO2 is +1.
