Question

The strong reducing property of hypophosphorous acid due to

• A. two P-H bond
• B. Its concentration
• C. presence of phophorus in its highest oxydation state
• D. The positive valency of phophorus

Answer 1

The Correct Option is A

Hypo phosphorous acid \((H_3PO_2)\) contains two \(P-H\) bonds, which are relatively weak compared to other chemical bonds. These \(P-H\) bonds can easily break, releasing hydrogen (H₂) gas and generating phosphorous-containing species with lower oxidation states.
The breaking of \(P-H\) bonds allows hypo phosphorous acid to donate electrons and act as a reducing agent in chemical reactions. The released hydrogen atoms can react with oxidizing agents, effectively reducing them. This property of hypo phosphorous acid makes it a strong reducing agent.
Therefore, option (A) the presence of two \(P-H\) bonds is responsible for the strong reducing property of hypo phosphorous acid.

Answer 2

Correct answer: two P–H bond 

Hypophosphorous acid (H₃PO₂) has the structure:

H–P(=O)(OH)–H

It contains two P–H bonds, and these are the source of its strong reducing property. These P–H bonds can donate electrons during redox reactions, allowing hypophosphorous acid to act as a powerful reducing agent.

Answer 3

The strong reducing property of hypophosphorous acid (H₃PO₂) is primarily due to the presence of two P-H bonds.

Explanation:

• Hypophosphorous acid has the following structure: H₂P(O)OH. It contains two hydrogen atoms directly bonded to the phosphorus atom (P-H bonds) and one hydroxyl group (P-OH bond).
• The P-H bonds are relatively easily broken, and the hydrogen atoms can be released as hydride ions (H^-), which are strong reducing agents. The phosphorus atom is oxidized in the process.
• The other factors are less significant:
  • The concentration of the acid can affect the *rate* of reduction, but it's the presence of the P-H bonds that makes it a reducing agent in the first place.
  • Phosphorus in hypophosphorous acid is in the +1 oxidation state, which is *not* its highest oxidation state (which is +5). A species in a low oxidation state is more likely to be a reducing agent.
  • The positive valency of phosphorus itself doesn't directly explain the reducing property.

Therefore, the correct answer is:

Two P-H bonds