Question

Phosphorus cannot form $P{H}_5$ with its outer electronic configuration as $3s^{2}3p^3$ because:

• A. Phosphorus can not show + 5 oxidation state
• B. $P{H}_5$ is not a stable compound
• C. ${\Delta }_a$H value of dihydrogen and ${\Delta }_{eg}H$ value of hydrogen do not favor higher oxidation state of phosphorus
• D. Phosphorus is not very reactive

Answer 1

Answer: (C)

${\Delta }_a$H value of dihydrogen and ${\Delta }_{eg}H$ value of hydrogen do not favor higher oxidation state of phosphorus

Since higher oxidation state of $P$ is not favoured by high ${\Delta }_{a}H$ of dihydrogen and ${\Delta }_{eg}H$ of hydrogen,\ $P$ does not foe\rm $P{H}_5$ through it exhibits $+3$ and $+5$ oxidation states.

Therefore the correct Answer is option (C)