Determine the electron geometry, molecular geometry, and idealized bond angles for each of the following molecules. a. CF4
b. NF3
c. OF2
d. H2S

CF4- electron geometry- tetrahedral

Molecular geometry- tetrahedral

bond angle- 109 degrees

NF3- electron geometry- tetrahedral

Molecular geometry- trigonal planar

bond angle - less than 109 degrees

OF2 - electron geometry- tetrahedral

Molecular geometry- bent

bond angle- less than 109 degrees

H2S- electron geometry- tetrahedral

Molecular geometry- bent

less than 109 degrees

Explanation:

All the compounds mentioned here are based on a tetrahedron according to VSEPR theory. There are four regions of electron density in each molecule.

However, the presence of lone pairs causes a distortion away from the expected tetrahedral geometry predicted by VSEPR theory.

Hence the presence of one or more lone pairs on the valence shell of the central atom causes distortion from the expected geometry.

true

Explanation:

Because Mercury can be solidified when its temparature us brought to its freezing point. However, when returned to room temparature conditions, mercury does not exist in solid state for long, and returns back to its more common liquid form.