Shapes Of Molecules And VSEPR Theory

Question 1

What does VSEPR stand for?

Answer 1

V = Valence
S = Shell
E = Electron
P = Pair
R = Repulsion

Question 2

The arrangement of bonding lone electrons creates….

Answer 2

Molecular geometry

Question 3

How are the predictable shapes given names?

Answer 3

Using the VSEPR model

Question 4

Is there a fixed amount of shapes molecules can make?

Answer 4

No. There are lots and lots of shapes molecules can make

Question 5

How are VSEPR names given to molecules?

Answer 5

Names are given based on the number of bonds and the number of lone pair electrons on a central atom.

Question 6

What are the 5 more common VSEPR names?

Answer 6

1. Linear
2. Tetrahedral
3. Bent
4. Trigonal pyramidal
5. Trigonal planar

Question 7

Describe the Linear molecular shape

Answer 7

It is a straight line (180 degrees) with 2 bonds on a central atom (that are as far away from each other as possible) and no lone pairs of electons.

Question 8

Describe the Tetrahedral molecular shape

Answer 8

Molecule has 4 equal spaced out bonds on a central atom (109.5 degrees) with no lone pairs of electrons

Question 9

Describe the Bent molecular shape

Answer 9

There are 2 lone pairs of electrons. Each lone pair of electrons push everything away from itself. So the 2 bonds on the central atom get pushed away giving the molecule a bent shape.

Question 10

Describe the Trigonal Pyramidal molecular shape

Answer 10

Molecule has 1 pair of lone electrons that pushes the 3 bonds on the central atom (less than 109.5 degrees) away from itself so the molecule makes a sort of pyramid shape.

Question 11

Describe the Trigonal Planar molecular shape

Answer 11

Molecule has 3 bonds on the central atom which makes the molecule lie flat (120 degrees). It also has no lone pair electrons (no purple blob).