Question:
Which of the following has a planar structure with two lone pairs?
Which of the following has a planar structure with two lone pairs?
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For molecules like XeF\(_4\), lone pairs affect the molecular geometry and can result in unique shapes such as square planar.
Updated On: Apr 18, 2026
- XeF\(_4\)
- NiF\(_4\)
- SF\(_4\)
- SF\(_6\)
- XeF\(_4\)
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the structure.
XeF\(_4\) has a square planar structure due to the presence of two lone pairs of electrons on the central xenon atom. This gives a total of four bonds, forming a square planar geometry.
Step 2: Analyzing the options.
- (A) XeF\(_4\) has a square planar structure with two lone pairs on the xenon atom.
- (B) NiF\(_4\) has a tetrahedral structure, not planar, with no lone pairs on the central atom.
- (C) SF\(_4\) has a seesaw structure with one lone pair.
- (D) SF\(_6\) has an octahedral structure with no lone pairs.
Step 3: Conclusion.
The correct answer is (A), as XeF\(_4\) has a square planar structure with two lone pairs.
XeF\(_4\) has a square planar structure due to the presence of two lone pairs of electrons on the central xenon atom. This gives a total of four bonds, forming a square planar geometry.
Step 2: Analyzing the options.
- (A) XeF\(_4\) has a square planar structure with two lone pairs on the xenon atom.
- (B) NiF\(_4\) has a tetrahedral structure, not planar, with no lone pairs on the central atom.
- (C) SF\(_4\) has a seesaw structure with one lone pair.
- (D) SF\(_6\) has an octahedral structure with no lone pairs.
Step 3: Conclusion.
The correct answer is (A), as XeF\(_4\) has a square planar structure with two lone pairs.
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