Question:
Statement I: The bond angle order in \( OF_2, H_2O, OCl_2 \) is \( OF_2<H_2O<OCl_2 \)
Statement II: \( SiF_4, SnF_4, \) and \( PbF_4 \) are all ionic compounds.
Statement I: The bond angle order in \( OF_2, H_2O, OCl_2 \) is \( OF_2<H_2O<OCl_2 \)
Statement II: \( SiF_4, SnF_4, \) and \( PbF_4 \) are all ionic compounds.
Statement II: \( SiF_4, SnF_4, \) and \( PbF_4 \) are all ionic compounds.
Show Hint
When comparing bond angles in molecules with similar structures, consider the number of lone pairs and electronegativity. For covalent compounds like \( SiF_4 \), \( SnF_4 \), and \( PbF_4 \), remember that these compounds are not ionic, despite being composed of halogens.
Updated On: Apr 7, 2026
- Both Statement I and Statement II are correct
- Statement I is incorrect but Statement II is correct
- Statement I is correct but Statement II is incorrect
- Both Statement I and Statement II are incorrect
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The Correct Option is C
Solution and Explanation
Step 1: Analyzing Statement I.
- \( OF_2 \) has a bent shape with a bond angle of around \( 103^\circ \), which is less than the bond angle in \( H_2O \).
- \( H_2O \) has a bond angle of \( 104.5^\circ \) due to the two lone pairs of electrons on oxygen.
- \( OCl_2 \) also has a bent shape, but the bond angle is slightly less than \( H_2O \), around \( 111^\circ \).
Thus, the bond angle order is \( OF_2<H_2O<OCl_2 \). Statement I is correct.
Step 2: Analyzing Statement II.
- \( SiF_4 \), \( SnF_4 \), and \( PbF_4 \) are covalent compounds, not ionic compounds. They are all covalent network compounds where the central atom is covalently bonded to fluorine atoms.
- Therefore, Statement II is incorrect because these compounds are covalent, not ionic.
Step 3: Conclusion.
Since Statement I is correct but Statement II is incorrect, the correct answer is option (C).
Final Answer: (C) Statement I is correct but Statement II is incorrect
- \( OF_2 \) has a bent shape with a bond angle of around \( 103^\circ \), which is less than the bond angle in \( H_2O \).
- \( H_2O \) has a bond angle of \( 104.5^\circ \) due to the two lone pairs of electrons on oxygen.
- \( OCl_2 \) also has a bent shape, but the bond angle is slightly less than \( H_2O \), around \( 111^\circ \).
Thus, the bond angle order is \( OF_2<H_2O<OCl_2 \). Statement I is correct.
Step 2: Analyzing Statement II.
- \( SiF_4 \), \( SnF_4 \), and \( PbF_4 \) are covalent compounds, not ionic compounds. They are all covalent network compounds where the central atom is covalently bonded to fluorine atoms.
- Therefore, Statement II is incorrect because these compounds are covalent, not ionic.
Step 3: Conclusion.
Since Statement I is correct but Statement II is incorrect, the correct answer is option (C).
Final Answer: (C) Statement I is correct but Statement II is incorrect
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