CH3Cl < CH3F < CH3Br < CH3I
CH3Cl > CH3F > CH3Br > CH3I
CH3F > CH3Cl > CH3Br > CH3I
CH3F < CH3Cl < CH3Br < CH3I
In methyl halides, the bond dipole moment μbond is given by μbond = δ·r, where δ is the charge separation (proportional to electronegativity difference) and r is the bond length. Electronegativity trend: F > Cl > Br > I,
so δCH3–F > δCH3–Cl > δCH3–Br > δCH3–I.
Bond-length trend: rCH3–F < rCH3–Cl < rCH3–Br < rCH3–I.
Since the increase in bond length from F to Cl slightly overcomes the decrease in δ, CH3Cl has a marginally higher dipole moment than CH3F. Beyond Cl, both δ and r changes lead to decreasing μ.
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