In the reaction P4+3OH-+3H2O →3H2PO2-+PH3, phosphorus is undergoing

The oxidation state of elemental phosphorus (P4) is zero. Whereas the oxidation state of phosphorus in 3H2PO2- is +1 and oxidation state of phosphorus in PH3 is -3. The conversion of oxidation state from 0 to +1 is oxidation, conversion of oxidation state from 0 to -3 is reduction. The reaction in which both oxidation and reduction takes place is called a disproportionation reaction.

In the reaction P4+3OH-+3H2O →3H2PO2-+PH3, phosphorus is undergoing

The oxidation state of elemental phosphorus (P4) is zero. Whereas the oxidation state of phosphorus in 3H2PO2- is +1 and oxidation state of phosphorus in PH3 is -3. The conversion of oxidation state from 0 to +1 is oxidation, conversion of oxidation state from 0 to -3 is reduction. The reaction in which both oxidation and reduction takes place is called a disproportionation reaction.

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In the reaction $P_{4} + 3 {OH}^{-} + 3 H_{2} O \to 3 H_{2} P {O_{2}}^{-} + {PH}_{3}$ , phosphorus is undergoing

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Reduction

Hydrolysis

Oxidation

Disproportionation

answer is C.

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Detailed Solution

The oxidation state of elemental phosphorus ( $P_{4}$ ) is zero. Whereas the oxidation state of phosphorus in $3 H_{2} P {O_{2}}^{-}$ is $+ 1$ and oxidation state of phosphorus in ${PH}_{3}$ is $- 3$ . The conversion of oxidation state from $0$ to $+ 1$ is oxidation, conversion of oxidation state from $0$ to $- 3$ is reduction. The reaction in which both oxidation and reduction takes place is called a disproportionation reaction.