BRAINCAKEMolecules with Multiple Bonds
Double Bonds with two bonding pairs (linear):
oxygen O=O carbon dioxide O=C=O carbon disulfide S=C=S
Triple Bonds with three bonding pairs (linear):
carbon monoxide C≡O cyanide ion C≡N- nitrogen N≡N
In electron pair repulsion theory, a double or triple bond counts as one region of electron density (one bonding area), because all of its electrons lie between the same two atoms. So it is the number of bonding areas and lone pairs, not the number of electron pairs, that decides the shape.
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Key terms in this lesson
- electron pair repulsion theory
- Electron pairs around a central atom arrange themselves as far apart as possible to minimise repulsion, deciding molecular shape.
- lone pair
- A pair of outer shell electrons on an atom that is not involved in bonding.
More in Discrete Molecules
- Displayed Formulae
- Dative Covalent Bonds
- Electron Pair Repulsion Theory
- The Shapes of Molecules
- Bond Angles
- Shape and Polarity
- Polyatomic Ions
- London Forces
All 25 lessons in Discrete Molecules · All Edexcel AS-level Chemistry topics