The correct order of increasing acidic nature of `SO_(2), SiO_(2), P_(2)O_(3) and Al_(2)O_(3)` is

Options

A. `SO_(2) lt P_(2)O_(3) lt SiO_(2) lt Al_(2)O_(3)`
B. `Al_(2)O_(3) lt SiO_(2) lt SO_(2) lt P_(2)O_(3)`
C. `Al_(2)O_(3) lt SiO_(2) lt P_(2)O_(3) lt SO_(2)`
D. `SiO_(2) lt SO_(2) lt Al_(2)O_(3) lt P_(2)O_(3)`

Answer

To determine the correct order of increasing acidic nature of the oxides \( SO_2, SiO_2, P_2O_3, \) and \( Al_2O_3 \), we need to analyze the acidic strength based on the properties of the central atoms in these oxides.

### Step-by-Step Solution:

1. **Understanding Acidic Nature**:
Acidic nature of oxides is determined by how easily they can donate protons (H⁺ ions). The ability to donate protons is influenced by the positive charge on the central atom and its electronegativity.

**Hint**: Remember that higher positive charge and higher electronegativity generally lead to stronger acids.

2. **Determine the Oxidation States**:
- For \( SO_2 \): Sulfur has an oxidation state of +4.
- For \( SiO_2 \): Silicon has an oxidation state of +4.
- For \( P_2O_3 \): Each phosphorus has an oxidation state of +3 (total +6 for two phosphorus).
- For \( Al_2O_3 \): Each aluminum has an oxidation state of +3 (total +6 for two aluminum).

**Hint**: Calculate the oxidation states of the central atoms to understand their charge.

3. **Comparing Positive Charges**:
- \( SO_2 \) and \( SiO_2 \) both have a +4 charge.
- \( P_2O_3 \) has a +3 charge.
- \( Al_2O_3 \) has a +3 charge as well.

**Hint**: Higher oxidation states typically correlate with stronger acidic properties.

4. **Electronegativity Consideration**:
- The electronegativity order is: \( S > P > Si > Al \).
- Sulfur (in \( SO_2 \)) is the most electronegative, followed by phosphorus (in \( P_2O_3 \)), then silicon (in \( SiO_2 \)), and finally aluminum (in \( Al_2O_3 \)).

**Hint**: Higher electronegativity means a stronger ability to attract electrons, which can enhance acidic character.

5. **Ranking the Acidity**:
- \( Al_2O_3 \) has the lowest acidic nature due to the lowest charge and electronegativity.
- \( P_2O_3 \) follows next with a +3 charge and moderate electronegativity.
- \( SiO_2 \) has a +4 charge but lower electronegativity than sulfur.
- \( SO_2 \) has the highest acidic nature due to its +4 charge and high electronegativity.

6. **Final Order**:
The correct order of increasing acidic nature is:
\[ Al_2O_3 < P_2O_3 < SiO_2 < SO_2 \]

### Conclusion:
Therefore, the correct order of increasing acidic nature of \( SO_2, SiO_2, P_2O_3, \) and \( Al_2O_3 \) is:
\[ Al_2O_3 < P_2O_3 < SiO_2 < SO_2 \]