The Valence Shell Electron Pair Repulsion Vsepr Theory

So , the correct answer is 5.

1. : Linear shape (sp hybridization)
2. : Linear shape (sp hybridization)
3. : Linear shape (sp hybridization)
4. : Linear shape (sp hybridization)
5. : V-shape (not linear)
6. : Linear shape (sp hybridization)
7. : V-shape (not linear)
8. (O=C=C=C=O): Linear shape (sp hybridization)

The species with a linear shape are:

Thus, the number of species with linear shape is 5.

To determine the increasing order of bond angles among , we need to understand the molecular geometry and electronic effects influencing these compounds:

1. (Boron Trifluoride) has a trigonal planar structure due to the hybridization of the boron atom. This leads to bond angles of 120°.
2. (Phosphorus Trifluoride) exhibits a trigonal pyramidal shape, with phosphorus undergoing hybridization. The presence of a lone pair causes the bond angle to decrease from the ideal tetrahedral angle (109.5°) to approximately 97°.
3. (represented as part of a radical such as in chemistry) typically has a trigonal planar arrangement similar to , but due to the presence of differing electronic factors (such as resonance or inductive effects involving fluorine), the bond angle can be slightly different from 120°.

Based on these observations, we conclude:

• The bond angle in is the largest because there are no lone pair repulsions.
• The bond angle in is smaller due to the lone pair repulsion.
• The bond angle in is influenced by both the resonance and inductive effects, which make it smaller than the ideal angles in and structures.

Thus, the increasing order of bond angles is: