Question

Strong reducing behaviour of $H_{3}P{O}_2$ is due to :

• A. low oxidation state of phosphorus
• B. presence of two - OH groups and one P-H bond
• C. presence of one - OH group and two P-H bonds
• D. high electron gain enthalpy of phosphorus

Answer 1

The correct option is C presence of one - OH group and two P-H bonds

The oxidation state of Phosphorous in $H_{3}P{O}_2$ is $+1$ which is the lowest oxidation state of phosphorous. So phosphorous can oxidize to higher oxidation states and acts as good reducing agent.

Hence option A is correct.