Is Chloroform (CHCl₃) Polar or Nonpolar?
Is Chloroform (CHCl₃) polar or nonpolar?
Chloroform has three C–Cl bonds (ΔEN = 0.61) and one C–H bond (ΔEN = 0.35). Unlike CCl₄, the substitution is asymmetric (3 Cl + 1 H), so the dipoles do not cancel.
| Formula | CHCl₃ |
| Polarity | Polar |
| Molecular Geometry | Tetrahedral |
| C–Cl Bond | ΔEN = 0.61 (polar) |
| C–H Bond | ΔEN = 0.35 (weakly polar) |
| Net Dipole | Yes |
Bond Dipoles
The three C–Cl bonds each have ΔEN = 0.61, and the C–H bond has ΔEN = 0.35. The Cl side of the molecule has more electron density than the H side.
Molecular Shape & Dipole Cancellation
Chloroform is tetrahedral at carbon, but the four substituents are not identical (3 Cl + 1 H). Compare to CCl₄ where all four are the same - that's what makes the difference.
Net Dipole Moment
The three C–Cl dipoles partially reinforce each other, pointing toward the Cl-heavy side. The net dipole points from H toward the three Cl atoms.
See bond dipoles, partial charges, and net dipole moments on interactive 3D molecules.
Visualize Chloroform's Polarity in 3DRelated Topics
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