Shapes Of Molecules

Question 1

2 bonding pairs, 0 lone pairs

Answer 1

linear - 180°

Question 2

3 bonding pairs , 0 lone pairs

Answer 2

trigonal planar - 120°

Question 3

2 bonding pairs , 1 lone pair

Answer 3

bent (v - shape) 118°

Question 4

4 bonding pairs, 0 lone pairs

Answer 4

tetrahedral - 109.5°

Question 5

3 bonding pairs, 1 lone pair

Answer 5

trigonal pyramidal - 107°

Question 6

2 bonding pairs, 2 lone pairs

Answer 6

bent (v shape) - 104.5°

Question 7

5 bonding pairs, 0 lone pairs

Answer 7

trigonal bipyramidal - 90°, 120°

Question 8

4 bonding pairs, 1 lone pairs

Answer 8

trigonal pyramidal or see saw 89°

Question 9

3 bonding pairs, 2 lone pairs

Answer 9

trigonal planar/ T-shape 89°

Question 10

6 bonding pairs, 0 lone pairs

Answer 10

octrahedral -90°

Question 11

5 bonding pairs, 1 lone pair

Answer 11

square pyramid - 89°

Question 12

4 bonding pairs, 2 lone pairs

Answer 12

square planar - 90°

Question 13

why are bond angles between bonding pairs reduced?

Answer 13

Due to extra repulsion from a lone pair of electrons. Lone pairs are more compact than bonding pairs, so repel more than bonding pairs.

Question 14

how much does a lone pair reduce a bond angle by?

Answer 14

2.5°

Question 15

In square planar structures, why do the 2 lone pair of electrons not affect the bond angle?

Answer 15

As the lone pairs are opposite each other, therefore the extra repulsions cancel each other out.