Multiple Choice
In the C–Br bond, which atom carries the partial negative charge (δ–) due to the dipole moment?
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11. Bonding & Molecular Structure
Dipole Moment
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Which of the following bonds would be the most polar without being considered ionic?
A
N–O
B
H–F
C
C–H
D
S–Cl
Verified step by step guidance1
Step 1: Understand the concept of bond polarity. Bond polarity arises from the difference in electronegativity between two atoms bonded together. The greater the difference, the more polar the bond is.
Step 2: Recall the electronegativity values of the atoms involved: Hydrogen (H) ~2.1, Fluorine (F) ~4.0, Nitrogen (N) ~3.0, Oxygen (O) ~3.5, Carbon (C) ~2.5, Sulfur (S) ~2.5, Chlorine (Cl) ~3.0.
Step 3: Calculate or estimate the electronegativity differences for each bond: N–O, H–F, C–H, and S–Cl. The bond with the largest difference will be the most polar.
Step 4: Consider the ionic character threshold. Bonds with very large electronegativity differences (usually above ~1.7) tend to be ionic. Identify which bonds have differences below this threshold to exclude ionic bonds.
Step 5: Compare the differences and select the bond with the highest polarity that is still covalent (not ionic). This will be the most polar bond without being considered ionic.
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