The electron pair repulsion theory can be used to predict the shape and bond angles of covalent molecules and polyatomic ions.
The shape of a molecule depends on the number of electron pairs.
A lone pair of electrons is slightly closer to the central atom and therefore takes up more space than a bonded pair of electrons. As a result, repulsion from a lone pair is stronger than from a bonding pair. For each lone pair, the bond angle decreases by about 2.5°Double and triple bonds are treated as a single bonding region.
Electron pairs repel each other so they are arranged as far apart as possible. This minimises repulsion and holds the molecule in a particular shape.
The shape of a molecule depends on the number of electron pairs.
A lone pair of electrons is slightly closer to the central atom and therefore takes up more space than a bonded pair of electrons. As a result, repulsion from a lone pair is stronger than from a bonding pair. For each lone pair, the bond angle decreases by about 2.5°Double and triple bonds are treated as a single bonding region.