Question

Bond angle is the highest in the molecule: A $\mathrm{XeO}{4}$ B $\mathrm{XeF}{4}$ C $\mathrm{XeO}{3}$ D $\mathrm{XeF}{2}$

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Answer

To determine which of the given molecules has the highest bond angle, we must first analyze the hybridization and molecular structure of each compound.

Analysis:

  1. $$ \mathrm{XeO}_{4} $$

    • Hybridization: $$ sp^3 $$
    • Structure: Tetrahedral
    • Bond Angle: $$ 109^\circ 28' $$
  2. $$ \mathrm{XeF}_{4} $$

    • Hybridization: $$ sp^3d^2 $$
    • Structure: Square planar
    • Bond Angle: $$ 90^\circ $$
  3. $$ \mathrm{XeO}_{3} $$

    • Hybridization: $$ sp^3 $$
    • Structure: Pyramidal
    • Bond Angle: Slightly greater than $$ 109^\circ 28' $$
  4. $$ \mathrm{XeF}_{2} $$

    • Hybridization: $$ sp^3d $$
    • Structure: Linear
    • Bond Angle: $$ 180^\circ $$

Conclusion:

Among the given molecules, $$ \mathrm{XeF}_{2} $$ has the highest bond angle of $$ 180^\circ $$ due to its linear structure.

Final Answer: D


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