Predict product(s) in the following reaction, `P_(4)+OH^(-)to `product(s)

Options

A. `PH_(3)`
B. `PO_(4)^(3-)`
C. `H_(2)PO_(2)^(-)`
D. `PO_(2)^(-)`

Answer

To predict the products of the reaction between white phosphorus (P₄) and hydroxide ions (OH⁻), we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are:
- White phosphorus (P₄)
- Hydroxide ions (OH⁻)

### Step 2: Understand the Nature of White Phosphorus
White phosphorus (P₄) is a highly reactive allotrope of phosphorus. It can react with bases such as sodium hydroxide (NaOH) in the presence of water.

### Step 3: Write the Balanced Reaction
When white phosphorus reacts with hydroxide ions and water, the products formed are:
- Sodium hypophosphite (NaH₂PO₂)
- Phosphine gas (PH₃)

The balanced chemical equation for this reaction can be written as:
\[ P_4 + 3 NaOH + 3 H_2O \rightarrow 3 NaH_2PO_2 + PH_3 \]

### Step 4: Identify the Products
From the balanced equation, we can identify the products:
1. Sodium hypophosphite (NaH₂PO₂)
2. Phosphine gas (PH₃)

### Step 5: Conclusion
Thus, the products of the reaction between P₄ and OH⁻ are:
- Phosphine gas (PH₃)
- Sodium hypophosphite (H₂PO₂⁻)

### Final Answer
The correct products are:
- A: Phosphine gas (PH₃)
- C: Sodium hypophosphite (H₂PO₂⁻)