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 trend is that as the oxidation state of a non-metal increases, the acidity of its oxide also increases. Here are the steps to solve the problem:

### Step-by-Step Solution:

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

2. **Calculate the Oxidation State of Chlorine in Cl2O7**:
- Let the oxidation state of Cl be \( X \).
- The equation will be: \( 2X + 7(-2) = 0 \) (since there are 7 oxygen atoms).
- Simplifying gives: \( 2X - 14 = 0 \) → \( 2X = 14 \) → \( X = +7 \).

3. **Calculate the Oxidation State of Phosphorus in P4O10**:
- Let the oxidation state of P be \( Y \).
- The equation will be: \( 4Y + 10(-2) = 0 \).
- Simplifying gives: \( 4Y - 20 = 0 \) → \( 4Y = 20 \) → \( Y = +5 \).

4. **Calculate the Oxidation State of Sulfur in SO3**:
- Let the oxidation state of S be \( Z \).
- The equation will be: \( Z + 3(-2) = 0 \).
- Simplifying gives: \( Z - 6 = 0 \) → \( Z = +6 \).

5. **Calculate the Oxidation State of Boron in B2O3**:
- Let the oxidation state of B be \( W \).
- The equation will be: \( 2W + 3(-2) = 0 \).
- Simplifying gives: \( 2W - 6 = 0 \) → \( 2W = 6 \) → \( W = +3 \).

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

7. **Determine Acidity Based on Oxidation States**:
- The higher the oxidation state of the non-metal, the more acidic the oxide.
- From the calculated oxidation states, Cl2O7 has the highest oxidation state of +7.

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

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