Chemistry, asked by YashSingh5123, 9 months ago

Strong reducing behaviour of H₃PO₂ is due to [2015 RS]
(a) presence of one –OH group and two P–H bonds
(b) high electron gain enthalpy of phosphorus
(c) high oxidation state of phosphorus
(d) presence of two –OH groups and one P–H bond.

Answers

Answered by ElegantSplendor
28

Answer:

Strong reducing behaviour of H₃PO₂ is due to [2015 RS]

(a) presence of one –OH group and two P–H bonds

(b) high electron gain enthalpy of phosphorus

(c) high oxidation state of phosphorus

(d) presence of two –OH groups and one P–H bond.

Answered by brokendreams
0

Presence of one –OH group and two P–H bonds is the correct option.

Explanation:

  • Phosphorous is a group 15 element.
  • It has 5 valance electrons.
  • So the structure of H₃PO₂ has two PH bonds, one P-OH bond and one P O bond.
  • Phosphorous is significantly electronegative.
  • The addition of oxygen makes it even more electronegative and pulls the electron cloud.
  • So phosphorous can easily leave the hydrogens from PH bond.
  • So, it is highly reducing in nature.

For more information about reducing nature of H₃PO₂,

https://brainly.in/question/1629676

Orthophosphoric acid is non reducing whereas hypophosphorous acid is a strong reducing agent explain and justify the above statement with suitable example

https://brainly.in/question/7920162

H₃PO₂ and H₃PO₃ act as good reducing agents while H₃PO₄ does not. Discuss.

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