Answer:
CO2
Electron pair geometry- Linear
Molecular geometry- Linear
BF3
Electron pair geometry - Trigonal planar
Molecular geometry- trigonal planar
SO2
Electron geometry - Trigonal planar
Molecular geometry - bent
SiCl4
Electron geometry- tetrahedral
Molecular geometry - tetrahedral
PF3
Electron pair geometry - tetrahedral
Molecular geometry- trigonal pyramidal
OF2
Electron pair geometry- tetrahedral
Molecular geometry- bent
Explanation:
Considering the molecule CO2, there are two regions of electron density in the molecule positioned at an angle of 180 degrees from each other hence the molecule is linear.
For BF3, the three bond pairs are arranged at the corners of a triangle to give a trigonal planar geometry at a bond angle of 120 degrees.
SO2 has two bonding groups and one lone pair giving three regions of electron density and a trigonal planar electron pair geometry. Due to the distortion to geometry caused by the presence of a lone pair, the molecule is bent.
For SiCl4, the four bonding groups are arranged at the corners of a regular tetrahedron hence it is tetrahedral both in electron pair geometry and in molecular geometry.
PF3 molecule has four regions of electron density corresponding to tetrahedral electron pair geometry. The presence of the lone pair leads to a trigonal pyramidal molecular geometry.
For OF2, there are four regions of electron density around the central oxygen atom. Two bond pairs and two lone pairs leads to a tetrahedral electron pair geometry but a bent molecular geometry is observed due to the two lone pairs.
