Question:
Arrange the following oxides in correct order of their acidic character:
\[
I: N_2O_3, \quad II: P_2O_3, \quad III: N_2O_5, \quad IV: As_2O_3
\]
Arrange the following oxides in correct order of their acidic character:
\[ I: N_2O_3, \quad II: P_2O_3, \quad III: N_2O_5, \quad IV: As_2O_3 \]
\[ I: N_2O_3, \quad II: P_2O_3, \quad III: N_2O_5, \quad IV: As_2O_3 \]
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Oxides of non-metals with higher oxidation states are more acidic; acid strength decreases down a group.
Updated On: Jun 26, 2026
- I > III > II > IV
- III > I > II > IV
- IV > II > I > III
- III > I > IV > II
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The Correct Option is B
Solution and Explanation
Step 1: Recall acidic oxide trends.
Acidic character increases with electronegativity and oxidation state of the central atom.
Step 2: Analyze each oxide.
- III. N\(_2\)O\(_5\) → N in +5 oxidation → most acidic
- I. N\(_2\)O\(_3\) → N in +3 oxidation → moderately acidic
- II. P\(_2\)O\(_3\) → P in +3 oxidation → weaker acid than N\(_2\)O\(_3\)
- IV. As\(_2\)O\(_3\) → As in +3 oxidation → least acidic
Step 3: Arrange in decreasing order.
Acidic order: III > I > II > IV
Step 4: Conclusion.
\[ \boxed{\text{III \gt I \gt II \gt IV}} \]
Acidic character increases with electronegativity and oxidation state of the central atom.
Step 2: Analyze each oxide.
- III. N\(_2\)O\(_5\) → N in +5 oxidation → most acidic
- I. N\(_2\)O\(_3\) → N in +3 oxidation → moderately acidic
- II. P\(_2\)O\(_3\) → P in +3 oxidation → weaker acid than N\(_2\)O\(_3\)
- IV. As\(_2\)O\(_3\) → As in +3 oxidation → least acidic
Step 3: Arrange in decreasing order.
Acidic order: III > I > II > IV
Step 4: Conclusion.
\[ \boxed{\text{III \gt I \gt II \gt IV}} \]
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