Oxidation states of P in `H_(4)P_(2)O_(5),H_(4)P_(2)O_(6),H_(4)P_(2)O_(7)` respectively are

Options

A. `+3, +5, +4`
B. `+5, +3, +4`
C. `+5, +4, +3`
D. `+3, +4, +5`

Answer

To determine the oxidation states of phosphorus in the compounds \( H_4P_2O_5 \), \( H_4P_2O_6 \), and \( H_4P_2O_7 \), we can follow these steps:

### Step 1: Determine the oxidation state of phosphorus in \( H_4P_2O_5 \)

1. **Assign variables**: Let the oxidation state of phosphorus be \( x \).
2. **Set up the equation**: The total charge of the molecule is zero. The contribution from hydrogen (4 atoms) is \( 4(+1) = +4 \) and from oxygen (5 atoms) is \( 5(-2) = -10 \).
3. **Write the equation**:
\[ 2x + 4 - 10 = 0 \]
4. **Simplify the equation**:
\[ 2x - 6 = 0 \implies 2x = 6 \implies x = +3 \]
5. **Conclusion**: The oxidation state of phosphorus in \( H_4P_2O_5 \) is \( +3 \).

### Step 2: Determine the oxidation state of phosphorus in \( H_4P_2O_6 \)

1. **Assign variables**: Let the oxidation state of phosphorus be \( x \).
2. **Set up the equation**: The contribution from hydrogen (4 atoms) is \( 4(+1) = +4 \) and from oxygen (6 atoms) is \( 6(-2) = -12 \).
3. **Write the equation**:
\[ 2x + 4 - 12 = 0 \]
4. **Simplify the equation**:
\[ 2x - 8 = 0 \implies 2x = 8 \implies x = +4 \]
5. **Conclusion**: The oxidation state of phosphorus in \( H_4P_2O_6 \) is \( +4 \).

### Step 3: Determine the oxidation state of phosphorus in \( H_4P_2O_7 \)

1. **Assign variables**: Let the oxidation state of phosphorus be \( x \).
2. **Set up the equation**: The contribution from hydrogen (4 atoms) is \( 4(+1) = +4 \) and from oxygen (7 atoms) is \( 7(-2) = -14 \).
3. **Write the equation**:
\[ 2x + 4 - 14 = 0 \]
4. **Simplify the equation**:
\[ 2x - 10 = 0 \implies 2x = 10 \implies x = +5 \]
5. **Conclusion**: The oxidation state of phosphorus in \( H_4P_2O_7 \) is \( +5 \).

### Final Answer

The oxidation states of phosphorus in \( H_4P_2O_5 \), \( H_4P_2O_6 \), and \( H_4P_2O_7 \) are \( +3 \), \( +4 \), and \( +5 \) respectively.