Applied Exercises (40 points) Answer the following questions in complete sentences. 1) In molecules with the same number of electron groups but different molecular geometries, discuss what happens to the bond angle? 2) What happens to the bond angle as you increase the number of bonding groups? 3) In 5 electron group molecules, what is the difference between axial and equatorial positions? Which groups are removed as lone pairs are added? 4) What is the difference between tetrahedral bent and

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Explanation:

In molecules with the same number of electron groups but different molecular geometries, the bond angles differ markedly owing to the presence of lone pairs on the central atom. Recall that lone pairs of electrons take up more space around the central atom and causes more repulsion thus squeezing the bond angle and making it less than the value expected on the basis of the Valence Shell Electron Pair Repulsion Theory.

As the number of bonding groups increases, the bond angle increases since the repulsion due to lone pairs of electrons is being progressively removed by increase in the number of bonding groups.

For 5 electron group molecules, the axial groups are oriented at a bond angle of 90° while the equatorial groups are oriented at a bond angle of 120°. In the presence of lone pairs, the equatorial bonds are removed because the equatorial bonds often have a greater bond length than the axial bonds.

In the tetrahedral geometry, four groups are bonded to the central atom while in a bent molecular geometry, only two groups are bonded to the central atom with two lone pairs present in the molecule.

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