Enter atom pairs to calculate their electronegativity difference and classify bond polarity. Uses Pauling electronegativity values to determine if bonds are nonpolar, slightly polar, polar covalent, or largely ionic.
Enter pairs of atoms to calculate their electronegativity difference and determine bond polarity. You can also test your own classification against the computed result.
Using Pauling electronegativity values to classify bonds from nonpolar to ionic.
Classification Thresholds:
For learning and homework practice only; not for professional chemical analysis or safety decisions.
Electronegativity is a measure of how strongly an atom attracts electrons in a chemical bond. The difference in electronegativity between two bonded atoms determines the polarity of the bond:
The Pauling scale is the most widely used electronegativity scale:
| ΔEN Range | Bond Type | Electron Sharing | Examples |
|---|---|---|---|
| < 0.4 | Nonpolar covalent | Nearly equal sharing | H–H, C–C, C–H |
| 0.4 – 1.0 | Slightly polar | Unequal but mostly shared | C–N, S–H |
| 1.0 – 2.0 | Polar covalent | Significant charge separation | H–Cl, C–O, O–H |
| ≥ 2.0 | Largely ionic | Electron transfer | Na–Cl, K–F, Ca–O |
Note: These thresholds are approximate guidelines. Different textbooks may use slightly different values.
F = 3.98
O = 3.44
N = 3.04
Cl = 3.16
C = 2.55
S = 2.58
H = 2.20
P = 2.19
Na = 0.93
K = 0.82
Ca = 1.00
Mg = 1.31
In a polar bond:
The dipole arrow points from δ+ toward δ− (toward Cl)
Determined solely by ΔEN between two atoms. A single bond is polar if electrons are not shared equally.
Depends on bond polarities AND molecular geometry. Symmetric molecules can be nonpolar even with polar bonds (e.g., CO2, CCl4).
Educational Use Only
This tool provides a simplified educational model for understanding bond polarity. Real bond character depends on many additional factors including oxidation state, hybridization, and molecular environment. Do not use for safety assessments, chemical engineering, or professional applications.
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