Which of the following compound is most acidic?

Options

A. `Cl_(2)O_(7)`
B. `P_(4)O_(10)`
C. `SO_(3)`
D. `B_(2)O_(3)`

Explanation

To determine which of the given compounds is the most acidic, we will analyze the oxidation states of the central atoms in each compound. The general rule is that a higher oxidation state of the central atom correlates with a greater acidic character.

### Step-by-step Solution:

1. **Identify the Compounds**: The compounds given are Cl2O7, P4O10, SO3, and B2O3.

2. **Calculate the Oxidation State of the Central Atom**:
- **For Cl2O7**:
- Let the oxidation state of Cl be \( x \).
- The equation for the compound is: \( 2x + 7(-2) = 0 \) (since there are 7 oxygen atoms each with an oxidation state of -2).
- Solving this:
\[ 2x - 14 = 0 \implies 2x = 14 \implies x = 7 \]
- The oxidation state of Cl in Cl2O7 is +7.

- **For P4O10**:
- Let the oxidation state of P be \( x \).
- The equation is: \( 4x + 10(-2) = 0 \).
- Solving this:
\[ 4x - 20 = 0 \implies 4x = 20 \implies x = 5 \]
- The oxidation state of P in P4O10 is +5.

- **For SO3**:
- Let the oxidation state of S be \( x \).
- The equation is: \( x + 3(-2) = 0 \).
- Solving this:
\[ x - 6 = 0 \implies x = 6 \]
- The oxidation state of S in SO3 is +6.

- **For B2O3**:
- Let the oxidation state of B be \( x \).
- The equation is: \( 2x + 3(-2) = 0 \).
- Solving this:
\[ 2x - 6 = 0 \implies 2x = 6 \implies x = 3 \]
- The oxidation state of B in B2O3 is +3.

3. **Compare the Oxidation States**:
- Cl in Cl2O7: +7
- P in P4O10: +5
- S in SO3: +6
- B in B2O3: +3

4. **Determine the Most Acidic Compound**:
- According to the rule, the compound with the highest oxidation state of the central atom will be the most acidic.
- Cl2O7 has the highest oxidation state (+7) compared to the others.

5. **Conclusion**:
- Therefore, Cl2O7 is the most acidic compound among the given options.

### Final Answer:
**Cl2O7 is the most acidic compound.**