The lone pair of electrons occupies a relatively large volume, since they are held by only one atom. Hence, the molecular shape of #'SO'_2# is bent and is represented as In determining the molecular shape, we consider only the positions of the atoms, not the lone pairs. The molecular shape of #'SO'_2# is not trigonal planar.

The electron pair geometry of #'SO'_2# is trigonal planar. The central atom, #'S'#, has three groups bonded to it, two oxygen atoms and a lone pair. #'AX'_2'E'# - two bond pairs and one lone pair The shape of the molecule is trigonal planar.Īll the atoms are in the same plane, and the #'F-B-F'# bond angles are all 120°. Minimizing the repulsion causes the #'F'# atoms to form an equilateral triangle about the #'B'# atom, as shown below. The #'B'# atom has three bond pairs in its outer shell. The shape of the molecule is linear, and the #'Cl-Be-Cl'# bond angle is 180°. Repulsion between these two pairs causes the atoms to be as far apart as possible. The central #'Be'# atom has two bond pairs in its outer shell (SN = 2). The Lewis dot structure for #'BeCl'_2# is Lone pairs repel more than bond bonding pairs. You must determine the steric number (SN) - the number of bonding pairs and lone pairs about the central atom. The repulsion between valence electron pairs in the outer shell of the central atom determines the shape of the molecule. Use the VSEPR shape to determine the angles between the bonding pairs. Use the SN and VSEPR theory to determine the electron pair geometry of the molecule. That gives you the steric number (SN) - the number of bond pairs and lone pairs around the central atom. Write the Lewis dot structure of the molecule. There are three basic steps to determining the molecular shape of a molecule:

Compound molecular geometry table