Which of the following has the smallest bond angles? A. CO2 B. SO2 C. SO3 D. SO42- E. XeF4
The Correct Answer and Explanation is:
The correct answer is E. XeF4 (Xenon tetrafluoride).
Explanation:
The bond angle in a molecule depends on its molecular geometry, which is influenced by the number of bonding and non-bonding electron pairs around the central atom. This is described by the VSEPR (Valence Shell Electron Pair Repulsion) theory.
Let’s go through each option:
- CO2 (Carbon dioxide):
- CO2 has a linear geometry with two double bonds around the central carbon atom.
- The bond angle is 180°.
- SO2 (Sulfur dioxide):
- SO2 has a bent molecular geometry (due to one lone pair on the sulfur).
- The bond angle is approximately 120°, which is less than that of CO2.
- SO3 (Sulfur trioxide):
- SO3 has a trigonal planar geometry with no lone pairs on the sulfur.
- The bond angle is 120°.
- SO42- (Sulfate ion):
- SO42- has a tetrahedral geometry with four bonds around the sulfur atom.
- The bond angle is 109.5°.
- XeF4 (Xenon tetrafluoride):
- XeF4 has a square planar geometry, which is the result of 4 bonding pairs and 2 lone pairs around the xenon atom.
- Due to the lone pairs, the bond angles are 90° and 180°, which are significantly smaller compared to the others listed.
Conclusion:
Out of all these molecules, XeF4 has the smallest bond angles (90°), resulting from its square planar geometry and lone pairs on the central xenon atom.
