Which one of the following elements does not form the compound `M_(4)O_(10)`.(M = element of group V)?

Options

A. P
B. Sb
C. As
D. Bi

Answer

To solve the question of which element from group V does not form the compound \( M_4O_{10} \), we can follow these steps:

### Step 1: Identify the elements in Group V
Group V elements include Nitrogen (N), Phosphorus (P), Arsenic (As), Antimony (Sb), and Bismuth (Bi).

### Step 2: Write the general formula for the oxides
The general formula given is \( M_4O_{10} \). We will substitute each element from Group V into this formula to check if the compound can exist.

### Step 3: Substitute each element into the formula
1. **For Phosphorus (P)**:
- Substitute \( M \) with \( P \): \( P_4O_{10} \)
- The oxidation state of phosphorus in this compound can be calculated as follows:
\[ 4x + 10(-2) = 0 \implies 4x - 20 = 0 \implies x = +5 \]
- Thus, \( P_4O_{10} \) exists.

2. **For Arsenic (As)**:
- Substitute \( M \) with \( As \): \( As_4O_{10} \)
- The oxidation state of arsenic can be calculated similarly:
\[ 4x + 10(-2) = 0 \implies 4x - 20 = 0 \implies x = +5 \]
- Thus, \( As_4O_{10} \) exists.

3. **For Antimony (Sb)**:
- Substitute \( M \) with \( Sb \): \( Sb_4O_{10} \)
- The oxidation state of antimony can be calculated:
\[ 4x + 10(-2) = 0 \implies 4x - 20 = 0 \implies x = +5 \]
- Thus, \( Sb_4O_{10} \) exists.

4. **For Bismuth (Bi)**:
- Substitute \( M \) with \( Bi \): \( Bi_4O_{10} \)
- The oxidation state of bismuth can be calculated:
\[ 4x + 10(-2) = 0 \implies 4x - 20 = 0 \implies x = +5 \]
- However, bismuth does not commonly exhibit a +5 oxidation state due to the inert pair effect. It primarily exists in the +3 oxidation state.

### Step 4: Conclusion
Since \( Bi_4O_{10} \) does not exist due to bismuth's inability to form a +5 oxidation state, the answer to the question is **Bismuth (Bi)**.