Multiple Choice
Which of the following bonds would have the largest dipole moment?
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11. Bonding & Molecular Structure
Dipole Moment
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In the C–Br bond, which atom carries the partial negative charge (δ–) due to the dipole moment?
A
Carbon (C)
B
Bromine (Br)
C
Neither atom
D
Both atoms equally
Verified step by step guidance1
Understand that a dipole moment in a bond arises due to the difference in electronegativity between the two atoms involved.
Recall that the atom with the higher electronegativity attracts the bonding electrons more strongly, acquiring a partial negative charge (δ–).
Look up or recall the electronegativity values: Carbon (C) has an electronegativity of about 2.55, while Bromine (Br) has an electronegativity of about 2.96 on the Pauling scale.
Since Bromine has a higher electronegativity than Carbon, it will pull the shared electrons closer to itself, resulting in Bromine carrying the partial negative charge (δ–).
Therefore, in the C–Br bond, Bromine (Br) carries the partial negative charge due to the dipole moment.
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