IB Chemistry home > Syllabus 2016 > Structure and bonding > 2, 3 and 4 electron domain molecules

Syllabus ref: 4.3

In the previous section we looked at how the electrons organise themselves around an atom to minimise repulsions. Now, by using the Lewis structures, we can predict the shapes of molecules and ions.

Two electron domain systems

Two electron domains (charge centres) always adopt a linear orientation to minimise repulsion between the negative charges.

In beryllium chloride the beryllium atom has only two electron domains.

It uses both of them to bond the two chlorine atoms.

  • Electronic shape = linear
  • Molecular shape = linear
  • Bond angle = 180º

top

Three electron domain systems

When the central atom has three electron domains the electronic shape adopted is trigonal planar. The actual shape of the molecule depends on the number of attached atoms.

The boron trifluoride molecule has the central boron atom with three regions of electron density (electron domains).

These adopt a trigonal planar orientation.

  • All three electron domains are used to bond fluorine atoms.
  • The molecular shape is trigonal planar.
  • F-B-F bond angle = 120º.

Three electron domains, but only two attached atoms produces an angular molecule

The sulfur dioxide molecule has the central sulfur atom with three electron domains.

These adopt a trigonal planar orientation.

Only two out of the three electron domains are used to bond oxygen atoms.

The molecular shape is angular.

O-S-O bond angle = 119º. The deviation from the expected bond angle of 120º is due to slightly different degrees of repulsion between the sulfur-oxygen bonding electrons and the lone pair on the sulfur atom.


top

Four electron domain systems

Molecules with four electron domains are very common, as four pairs of electrons make up a full octet of electrons. The domains adopt a tetrahedral orientation, but the molecular shape depends on the number of atoms or groups attached to the central atom.

Number of attached atoms or groups Molecular shape
4 tetrahedral
3 trigonal pyramidal
2 angular (bent)

The bond angles that are finally produced depends on the inter-electron repulsion between the bonding pairs of electrons and the non-bonding, or lone pairs. This is best understood using some examples.

The methane molecule - VSEPR


top