Question

Strong reducing behaviour of H₃PO₂ 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

Strong reducing behavior of H₃PO₂ is due to

(c) presence of one — OH group and two P — H bonds

Explanation:

• Hypophosphorous Acid ($H_3PO_2$) is an oxyacid of phosphor and is a strong reducing agent.

• Phosphorous can have a varying oxidation state from -3 to +5 of which Phosphorous oxyacids may have oxidation states from +1 to +5. Lower oxidation states signify its ability to be oxidized to a higher state and thus resulting in a reducing behavior.  

• The oxidation number of P in $H_3PO_2$ is +1.

• $H_3PO_2$ has one hydroxyl (OH) group and two P - H bonds as given in the figure below. (P - H bonds = 2 ; P - OH bonds = 1.)

• Increased number of P - H bonds show increased tendency to release hydrogen (H+) ions; exhibiting a reducing nature.

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Question 8.17 Consider the reactions:

(a) H3PO2(aq) + 4 AgNO3(aq) + 2 H2O(l)→H3PO4(aq) + 4Ag(s) + 4HNO3(aq)

(b) H3PO2(aq) + 2CuSO4(aq) + 2 H2O(l)→H3PO4(aq) + 2Cu(s) + H2SO4(aq)

(c) C6H5CHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq)→C6H5COO–(aq) + 2Ag(s) + 4NH3 (aq) + 2 H2O(l)

(d) C6H5CHO(l) + 2Cu2+(aq) + 5OH–(aq)→No change observed.

What inference do you draw about the behaviour of Ag+ and Cu2+ from these reactions?

Class XI Redox Reactions Page 273