Carbon tetrachloride, or CCl₄, is one of the most commonly tested molecules in IB Chemistry when students learn about polarity, molecular geometry, and electronegativity. Although each C–Cl bond is polar, the molecule itself is nonpolar — an idea that often confuses learners until they fully grasp molecular symmetry. This guide provides the IB-aligned explanation you need for exams and improves your understanding of bonding and structure across the course.
Quick Start Checklist
CCl₄ is nonpolar because:
- It has a tetrahedral shape.
- All four C–Cl bond dipoles cancel due to symmetry.
- The molecule has no net dipole moment.
- Polarity depends on both bond polarity and molecular geometry.
Understanding molecular behavior like this is essential for predicting physical properties and interpreting diagrams in Paper 1 and Paper 2. Strengthen these foundational skills with RevisionDojo’s chemistry-focused study tools:
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Why C–Cl Bonds Are Polar
Chlorine is more electronegative than carbon.
This means each C–Cl bond has a bond dipole pointing toward the chlorine atom.
Electronegativity difference:
- Carbon ≈ 2.5
- Chlorine ≈ 3.0
The difference is enough to create polar covalent bonds, but the polarity of individual bonds does not automatically determine the polarity of the entire molecule.
