Question

1. drag and drop the molecular shapes with the lewis structures.

choices
bent
linear
trigonal pyramidal
tetrahedral
trigonal planar

Explanation:

1. For $\text{PF}_3$: Central P has 3 bonding pairs + 1 lone pair, so electron repulsion forms a trigonal pyramidal shape.
2. For $\text{BeF}_2$: Central Be has 2 bonding pairs, no lone pairs, so atoms align linearly.
3. For $\text{CCl}_4$: Central C has 4 bonding pairs, no lone pairs, forming a tetrahedral shape.
4. For $\text{GeF}_2$: Central Ge has 2 bonding pairs + 1 lone pair, lone pair repulsion creates a bent shape.
5. For $\text{BF}_3$: Central B has 3 bonding pairs, no lone pairs, forming a trigonal planar shape.

Answer:

• $\text{F-P-F (with one lone pair on P, three F atoms)}$: trigonal pyramidal
• $\text{F-Be-F (with three lone pairs on each F)}$: linear
• $\text{Cl-C-Cl (four Cl atoms around C)}$: tetrahedral
• $\text{F-Ge-F (with one lone pair on Ge, two F atoms)}$: bent
• $\text{F-B-F (three F atoms around B)}$: trigonal planar