The correct order of acidic strength is :

To determine the acidic strength order of the given oxides (Cl₂O₇, SO₃, and P₄O₁₀), we analyze their oxidation states and electronegativities. Here's a detailed explanation:

Step 1: Identifying the Oxidation States

• Cl₂O₇: The oxidation state of chlorine (Cl) is +7.
• SO₃: The oxidation state of sulfur (S) is +6.
• P₄O₁₀: The oxidation state of phosphorus (P) is +5.

By calculating these oxidation states, we establish a basis for comparing the acidic strength order.

Step 2: Comparing Oxidation States

The acidic strength order of oxides depends heavily on the oxidation state of the central atom. Higher oxidation states correlate with stronger acids because they increase the atom's ability to stabilize the negative charge on its conjugate base.

• Chlorine in Cl₂O₇ has the highest oxidation state of +7.
• Sulfur in SO₃ follows with an oxidation state of +6.
• Phosphorus in P₄O₁₀ has the lowest oxidation state of +5.

Thus, based on oxidation states, the acidic strength order is:

Cl₂O₇ > SO₃ > P₄O₁₀

Step 3: Considering Electronegativity

Electronegativity also influences the acidic strength order. More electronegative central atoms draw electron density towards themselves, stabilizing the conjugate base and enhancing acidity.

• Chlorine is more electronegative than sulfur and phosphorus, supporting its position as the strongest acid.
• Sulfur's electronegativity is greater than that of phosphorus, making SO₃ stronger than P₄O₁₀.

Final Conclusion

Taking into account both oxidation states and electronegativity, the acidic strength order of the given oxides is:

Cl₂O₇ > SO₃ > P₄O₁₀

This order reflects the impact of higher oxidation states and electronegativity on acid strength.