Shapes Of Molecules

Question 1

2 bonded pairs of electrons

Answer 1

-Beryllium chloride /carbon dioxide
-Electron pairs repel each other equally to minimise repulsion
-shape: linear
-Angle: 180

Question 2

3 bonded pairs of electrons

Answer 2

-Boron trifluoride
-The 3 bonding pairs repel each other equally
-shape: trigonal planar
-Angle: 120

Question 3

4 bonded pairs of electrons

Answer 3

-Methane/ammonium ion
-4bonded pairs of electrons repel each other equally
-Shape: tetrahedral
-Angle: 109.5

Question 4

3 bonded pairs and 1 lone pair of electrons

Answer 4

-Ammonia
-electron pairs repel each other equally, lone pair repel more
-shape: trigonal pyramidal
-angle: 107

Question 5

2 bonded pairs and 2 lone pairs

Answer 5

-water
-electron pairs repel each other, but lone pairs of electrons have a greater repulsion
-shape: bent
-angle: 104.5

Question 6

5 bonded pairs of electrons

Answer 6

-phosphorus (v) fluoride
-electron pairs repel each other equally to minimise repulsion
-shape: trigonal bipyramidal
-angle: 120 & 90

Question 7

3 bonded pairs and 2 lone pairs

Answer 7

-chlorine trifluoride
-3 of fluorine are in a plane at 120 to each other the other 2 are at right angle to this plane
-shape: T shaped
-angle: 86

Question 8

2 bonded pairs and 3 lone pairs

Answer 8

• Tri-iodine ion
  -2 different bond angles
  -shape: linear
  -angle: 180

Question 9

6 bonded pairs of electrons

Answer 9

-Sulfur hexafluoride
-electron pairs repel each other to minimise repulsion
-shape: octahedral
-angle: 90

Question 10

4 bonded pairs and 2 lone pairs

Answer 10

-xenon (lv) fluoride
-2 of 6 pairs around xenon are lone pairs. The lone pairs are placed at 180 apart to avoid great repulsion that would result from placing the lone pairs at 90 to each other
-shape: square planar
-angle: 90 & 180