Electronegativity Chemistry Example 3

Follow the full solution, then compare it with the other examples linked below.

Example 3

easy
Which bond is more polar: H–Cl or H–Br? (EN values: H = 2.1, Cl = 3.0, Br = 2.8)

Solution

  1. 1
    H–Cl: ΔEN=∣3.0−2.1∣=0.9\Delta\text{EN} = |3.0 - 2.1| = 0.9. H–Br: ΔEN=∣2.8−2.1∣=0.7\Delta\text{EN} = |2.8 - 2.1| = 0.7.
  2. 2
    H–Cl has a larger electronegativity difference, so it is more polar.

Answer

H–Cl is more polar\text{H–Cl is more polar}
Greater electronegativity differences lead to greater bond polarity.

About Electronegativity

A dimensionless measure of how strongly an atom attracts the shared electrons in a covalent bond toward itself, quantified on the Pauling scale from 0.7.

Learn more about Electronegativity →

More Electronegativity Examples

Example 1 easy

Arrange the following elements in order of increasing electronegativity: Na, Cl, F, O.

Example 2 medium

In the molecule HF, the electronegativity of H is 2.1 and F is 4.0. Describe the bond polarity and i

Example 4 medium

Which bond is more polar, C–H or O–H? Use these electronegativity values: C = 2.5, H = 2.1, O = 3.5.

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