Question

Which of the following overlapping is not present in XeO₃ molecule?

• A. ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{x}}$
• B. ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{y}}$
• C. ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{z}}$
• D. ${\mathrm{sp}}^3+\mathrm{s}$

Answer 1

The correct option is D

${\mathrm{sp}}^3+\mathrm{s}$

Explanation for correct option

(D) ${\mathrm{sp}}^3+\mathrm{s}$

${\mathrm{sp}}^3+\mathrm{s}$ does not take part in the hybridization of ${\mathrm{XeO}}_3$.

Ground state of electronic configuration $\mathrm{Xe}=\left[\mathrm{Kr}\right]4{\mathrm{d}}^{10}5{\mathrm{s}}^{2}5{\mathrm{p}}^6$

Excited state of electronic configuration $\mathrm{Xe}=\left[\mathrm{Kr}\right]4{\mathrm{d}}^{10}5{\mathrm{s}}^{2}5{\mathrm{p}}^{3}5{\mathrm{d}}^3$

The electronic configuration of Oxygen = $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^4$

From the hybridization of ${\mathrm{XeO}}_3$, it is clear that the Oxygen atom form bond with Xe like ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{x}}$, ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{y}}$ and ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{z}}$ but never form ${\mathrm{sp}}^3+\mathrm{s}$.

Explanation for incorrect options

Since, ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{x}}$, ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{y}}$, and ${\mathrm{sp}}^3+{\mathrm{p}}_{\mathrm{z}}$ are involved in the overlapping of XeO₃ molecule. Therefore, options (A), (B) and (C) are incorrect.

Thus, the correct option is (D) ${\mathrm{sp}}^3+\mathrm{s}$.