Which one of the following bonds has the highest bond energy?
Correct answer: C. N ≡ N
- A. C-C
- B. C ≡ C
- C. N ≡ N
- D. H-F
Explanation
Strength of bonds increases as the number of electron pairs in the bonds increase. Nitrogen and Carbon are in the same period however Nitrogen comes after Carbon, meaning that the size of nitrogen is less than that of carbon, having atoms closer to each other, thus requiring more energy to break N-N triple bond ( which is 941kJ/mole ) as compared to C-C triple bond ( which is 839 kJ/mole ).
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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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