Question

The correct statement(s) for XeF\(_2\) is(are)

• A. Its bonding is best explained by classical 2-centered-2-electron bonds
• B. Its bonding is best explained by a non-classical 3-centered-4-electron bond
• C. It contains nine lone pairs of electrons
• D. Its point group is \(D_{\infty h}\)

Hint:

Hypervalent AX\(_2\) species like XeF\(_2\) are classic examples of 3c–4e bonding; remember the linear geometry (AX\(_2\)E\(_3\)) and \(D_{\infty h}\) symmetry.

Answer 1

The Correct Option is B, C, D

Step 1: Bonding model.
XeF\(_2\) is linear with an \(AX_2E_3\) arrangement about Xe. The two Xe–F bonds are best described by 3-center–4-electron (3c–4e) bonding over the F–Xe–F framework, not by two independent 2c–2e bonds. Thus (B) is true, (A) is false.
Step 2: Lone-pair count.
Each F has three lone pairs (\(2\times3=6\)), and Xe has three lone pairs in the equatorial positions of a trigonal bipyramidal electron geometry. Total \(=6+3=\mathbf{9}\) lone pairs \(\Rightarrow\) (C) true.
Step 3: Symmetry.
A linear, centrosymmetric F–Xe–F molecule has point group \(\mathbf{D_{\infty h}}\). Hence (D) is true.