Explain bromine is less electronegative than chlorine

Reference no: EM13187462

Here is it, Bromine is less electronegative than chlorine, yet methyl bromide and methyl chloride have very similar dipole moments. Why?

Assume the electron distribution would go more towards the methyl group as the bond is larger and larger, resulting in a higher dipole moment for the Chlorine. I'm super confused with this concept.

Reference no: EM13187462

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