Concept: Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds. The type of hybridization can be determined by calculating the steric number (SN), which is the sum of the number of sigma bonds and the number of lone pairs around the central atom.

Why (C) is correct:

1. Determine the central atom and its valence electrons: In ${\mathrm{XeF}}_2$, Xenon (Xe) is the central atom. Xe is a noble gas and has 8 valence electrons.

2. Determine the number of sigma bonds: There are two fluorine (F) atoms bonded to Xe, forming two sigma bonds.

3. Determine the number of lone pairs: Each fluorine atom forms one single bond, using one electron from Xe. So, 2 electrons are used in bonding. The remaining electrons on Xe are $8-2=6$. These 6 electrons form $6/2=3$ lone pairs.

4. Calculate the steric number (SN): $\text{SN}=\text{Number of sigma bonds}+\text{Number of lone pairs}=2+3=5$.

5. Determine the hybridization: A steric number of 5 corresponds to $s{p}^{3}d$ hybridization.

Option Analysis:

• A) $s{p}^3$: This corresponds to a steric number of 4 (e.g., ${\mathrm{CH}}_4$). Incorrect.
• B) $s{p}^3{d}^3$: This corresponds to a steric number of 7 (e.g., ${\mathrm{IF}}_7$). Incorrect.
• C) $s{p}^{3}d$: This corresponds to a steric number of 5 (e.g., ${\mathrm{PCl}}_5$, ${\mathrm{XeF}}_2$). Correct.
• D) $s{p}^3{d}^2$: This corresponds to a steric number of 6 (e.g., ${\mathrm{SF}}_6$). Incorrect.

Correct Answer: (C)