Bond length of O-O in lewis structure of given structure is:
Correct answer: C. Average of single and double bond
- A. Equal to single bond
- B. Equal to double bond
- C. Average of single and double bond
- D. Cannot be determined
Explanation
In molecules with delocalized electrons, such as benzene, the electrons are shared across multiple atoms, resulting in resonance structures. This delocalization causes all bonds to have an intermediate bond order (e.g. 1.5 in benzene) rather than distinct single or double bonds.
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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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