With the increase of which one of the following factors bond energy of a molecule decreases:
Correct answer: D. Number of lone pairs
- A. Electronegativity difference
- B. Bond order
- C. S-character
- D. Number of lone pairs
Explanation
Lone pairs are non-bonding electron pairs present on an atom. They can exert repulsive forces on the electrons involved in neighboring bonds, leading to bond weakening. The repulsion caused by lone pairs can distort the bond angles and disrupt the effective overlap of orbitals, ultimately lowering the bond energy. As a result, an increase in the number of lone pairs around a bond decreases the bond energy.
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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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