What is the valence of phosphorus (P) in the compound P4O10?

In the compound P4O10, each phosphorus atom has a valence of +5. This can be understood by analyzing the overall oxidation states of the elements involved in the compound.

Oxygen typically has an oxidation state of -2. Since there are 10 oxygen atoms in P4O10, they collectively contribute a total oxidation state of -20 (10 x -2). To maintain charge neutrality in the compound, the total oxidation state contributed by the four phosphorus atoms must be +20.

We can determine the oxidation state of phosphorus by dividing the total oxidation state needed (+20) by the number of phosphorus atoms (4). This calculation yields an individual oxidation state of +5 for each phosphorus atom:

[ \text{Total oxidation state of P} = +20 ]

[ \text{Number of P atoms} = 4 ]

[ \text{Oxidation state of P} = \frac{+20}{4} = +5 ]

Therefore, the valence of phosphorus in P4O10 is +5, indicating that each phosphorus atom is donating five electrons or holding a significant positive charge relative to neutral atoms. This reflects phosphorus’s ability to form strong covalent bonds with oxygen in this molecular compound