Good reducing nature of H3PO2 is attributed to the presence of
Refer theory
The reducing nature of hypophosphorous acid (H3PO2) is due to the presence of P–H bonds in its structure. Let's understand why:
Step 1: Structure of H3PO2
Hypophosphorous acid has the molecular formula H3PO2. Its structure is:
More precisely, it has:
Step 2: Why P–H bonds cause reducing behavior?
The P–H bonds are relatively weak and can be easily broken. When H3PO2 acts as a reducing agent, it donates hydrogen atoms from these P–H bonds. The phosphorus atom gets oxidized while reducing another species.
Step 3: Comparison with other oxyacids
Phosphorous acid (H3PO3) has one P–H bond and is a weaker reducing agent. Orthophosphoric acid (H3PO4) has no P–H bonds and shows no reducing behavior. This confirms that the reducing nature increases with more P–H bonds.
Final Answer: The good reducing nature of H3PO2 is attributed to the presence of two P–H bonds.
Oxyacids of Phosphorus: Phosphorus forms several oxyacids with different oxidation states and properties. The reducing power depends on the number of P–H bonds present in the molecule.
Redox Chemistry: Understanding how compounds act as reducing agents by losing electrons or hydrogen atoms is fundamental to redox reactions.
While there isn't a specific formula, the key concept is:
Reducing strength ∝ Number of P–H bonds
H3PO2 (2 P–H) > H3PO3 (1 P–H) > H3PO4 (0 P–H) in reducing power
Amongst the following, the total number of compounds soluble in aqueous NaOH is
Identify the binary mixture(s) that can be separated into individual compounds, by differential extraction, as shown in the given scheme.
