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Electronegativity Difference and Bond Type

Calculate electronegativity difference between two elements, estimate ionic character percentage, and classify the bond type using Pauling scale values.

Pauling electronegativity. H=2.20, O=3.44, N=3.04, C=2.55, Na=0.93, Cl=3.16, F=3.98, S=2.58.
Pauling electronegativity of the second element.

Results

Electronegativity Difference1.24
Ionic Character31.9%
Bond Classification2 (1=Nonpolar Covalent, 2=Polar Covalent, 3=Ionic)

📖What is it?

Electronegativity is a measure of how strongly an atom attracts shared electrons in a bond. The Pauling scale (0.7 to 3.98) is the most common. The difference in electronegativity (Delta EN) between two bonded atoms determines the bond type: nonpolar covalent (<0.5), polar covalent (0.5-1.7), or ionic (>1.7).

🎯How to use

Enter the Pauling electronegativity values for both elements. The more electronegative element carries a partial negative charge (delta-). Common values: F=3.98, O=3.44, N=3.04, Cl=3.16, C=2.55, H=2.20, Na=0.93, K=0.82.

💡Example scenario

H-O bond: |2.20 - 3.44| = 1.24 -> polar covalent, 26% ionic character. Na-Cl bond: |0.93 - 3.16| = 2.23 -> ionic, 70% ionic character. C-H bond: |2.55 - 2.20| = 0.35 -> nonpolar covalent, 3% ionic character.

🏆Pro tip

Pauling's original threshold for ionic vs covalent is Delta EN > 1.7, but modern chemistry recognizes this as a continuum. Ionic character percentage uses the Pauling equation: % ionic = (1 - e^(-0.25 * Delta_EN^2)) x 100. Polyatomic molecules have bond polarity and molecular polarity (dipole moment) which can cancel in symmetric molecules like CO2.