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One bonding pair (linear):
carbon monoxide C≡O HF cyanide ion C≡N- oxygen O=OTwo bonding pairs (linear):
BeI2 carbon dioxide O=C=O carbon disulfide S=C=STwo bonding pairs and one or two lone pairs (non-linear or bent):
H2O SO2 NO2

Three bonding pairs(trigonal planar):
BCl3 BF3 AlCl3 H2C=O CO32- NO3- SO3Three bonding pairs one lone pair (trigonal pyramidal):
NH3 H3O+Four bonding pairs (tetrahedral):
NH4+ CH4 SO42- SiH4 CH3OH PO43-Electron pair repulsion theory fails for transition metal compounds.

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Specification: OCR Chemistry A (H032), AS-level, 2.2.2 Bonding and structure. Topic: Shapes and Intermolecular Forces.

Key terms in this lesson

Ion
A positively or negatively charged atom or group of atoms, formed by the loss or gain of electrons.
Lone pair
A pair of outer-shell electrons that is not involved in bonding.
Electron pair repulsion theory
The theory that electron pairs around a central atom arrange themselves as far apart as possible to minimise repulsion, determining the shape of a molecule or ion.

More in Shapes and Intermolecular Forces

All 13 lessons in Shapes and Intermolecular Forces · All OCR AS-level Chemistry topics