1
Question
Explain why Cl-Cl bond is stronger than F-F bond?
Open in App
Solution
bond energy (in kJ/mol)
F-F:158
Cl-Cl: 244
Hence, in order of decreasing bond strength:
Cl-Cl => => (F-F) =>
Fluorine is an anomaly.
Bond strength decreases from chlorine to iodine as down the group, the atomic size becomes larger and thus the valence electron orbitals become more diffused, causing the overlap of orbitals to become less effective. Therefore the halogen-halogen bond becomes weaker.
Fluorine is an exception due to its extremely small size. The F-F bond length is so short that the lone pairs of electrons on the fluorine atoms repel each other and weakens the F-F bond.
bond energy (in kJ/mol)
F-F:158
Cl-Cl: 244
Hence, in order of decreasing bond strength:
Cl-Cl => => (F-F) =>
Fluorine is an anomaly.
Bond strength decreases from chlorine to iodine as down the group, the atomic size becomes larger and thus the valence electron orbitals become more diffused, causing the overlap of orbitals to become less effective. Therefore the halogen-halogen bond becomes weaker.
Fluorine is an exception due to its extremely small size. The F-F bond length is so short that the lone pairs of electrons on the fluorine atoms repel each other and weakens the F-F bond.
Suggest Corrections
7
Similar questions
Join BYJU'S Learning Program
Explore more
Join BYJU'S Learning Program
