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For each pair of molecules below, which molecule has the greater dipole moment?
(a) O_3 or SO_2
(b) HBr or HCl
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11. Bonding & Molecular Structure
Dipole Moment
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Which of the following pairs of atoms forms the most polar bond?
A
C and H
B
N and O
C
S and O
D
H and F
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Understand that bond polarity depends on the difference in electronegativity between the two atoms forming the bond. The greater the difference, the more polar the bond is.
Recall the approximate electronegativity values of the atoms involved: H (~2.1), C (~2.5), N (~3.0), O (~3.5), S (~2.5), and F (~4.0).
Calculate the electronegativity difference for each pair: for example, for C and H, subtract the electronegativities: |2.5 - 2.1| = 0.4.
Compare the differences for all pairs: C-H, N-O, S-O, and H-F. The pair with the largest difference will form the most polar bond.
Identify that H and F have the largest electronegativity difference (|4.0 - 2.1| = 1.9), which explains why the H-F bond is the most polar among the options.
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