When 's' character of hybridized orbitals decreases the bond angle:
Correct answer: A. Decreases.
- A. Decreases.
- B. Increases.
- C. Becomes zero.
- D. Does not change.
Explanation
The correct answer is that the bond angle decreases. Hybrid orbitals with higher 's' character (e.g., sp) have larger bond angles (180°) compared to those with more 'p' character (e.g., sp3 with 109.5°). As 's' character decreases, the proportion of 'p' character increases, leading to smaller bond angles. Options B, C, and D are incorrect because they either misunderstand the relationship between 's' character and bond angles or suggest impossible outcomes.
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Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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