In which compound, the oxidation state of phosphorus is +4

Options

A. `P_(4)O_(11)`
B. `P_(4)O_(8)`
C. `P_(4)O_(6)`
D. `H_(3)PO_(4)`

Explanation

To determine in which compound the oxidation state of phosphorus is +4, we can analyze each compound systematically.

### Step-by-Step Solution:

1. **Identify the Compounds**: The compounds we need to analyze are P4O11, P4O8, P4O6, and H3PO4.

2. **Calculate Oxidation State for Each Compound**:

- **For P4O11**:
- Let the oxidation state of phosphorus be \( X \).
- The equation based on the oxidation states is:
\[ 4X + 11(-2) = 0 \]
- Simplifying gives:
\[ 4X - 22 = 0 \implies 4X = 22 \implies X = \frac{22}{4} = 5.5 \]
- So, the oxidation state of phosphorus in P4O11 is +5.5.

- **For P4O8**:
- Again, let the oxidation state of phosphorus be \( X \).
- The equation is:
\[ 4X + 8(-2) = 0 \]
- Simplifying gives:
\[ 4X - 16 = 0 \implies 4X = 16 \implies X = \frac{16}{4} = 4 \]
- Thus, the oxidation state of phosphorus in P4O8 is +4.

- **For P4O6**:
- Let the oxidation state of phosphorus be \( X \).
- The equation is:
\[ 4X + 6(-2) = 0 \]
- Simplifying gives:
\[ 4X - 12 = 0 \implies 4X = 12 \implies X = \frac{12}{4} = 3 \]
- Therefore, the oxidation state of phosphorus in P4O6 is +3.

- **For H3PO4**:
- Let the oxidation state of phosphorus be \( X \).
- The equation is:
\[ 3(+1) + X + 4(-2) = 0 \]
- Simplifying gives:
\[ 3 + X - 8 = 0 \implies X - 5 = 0 \implies X = 5 \]
- Hence, the oxidation state of phosphorus in H3PO4 is +5.

3. **Conclusion**: After analyzing all compounds, we find that the oxidation state of phosphorus is +4 in the compound **P4O8**.

### Final Answer:
The compound in which the oxidation state of phosphorus is +4 is **P4O8**.