6) Shapes Of Molecules And Intermolecular Forces

Question 1

Give an example of a non-linear molecule.

Answer 1

H20

Question 2

Give an example of a trigonal planar molecule.

Answer 2

BF3

Question 3

Give an example of a pyramidal molecule.

Answer 3

NH3

Question 4

Give an example of a tetrahedral molecule.

Answer 4

CH4

Question 5

Give an example of an octahedral molecule.

Answer 5

SF6

Question 6

Give an example of a linear molecule.

Answer 6

C02

Question 7

What is the bond angle for non-linear molecules?

Answer 7

104.5

Question 8

What is the bond angle for trigonal planar molecules?

Answer 8

120

Question 9

What is the bond angle for pyramidal molecules?

Answer 9

107

Question 10

What is the bond angle for tetrahedral molecules?

Answer 10

109.5

Question 11

What is the bond angle for octahedral molecules?

Answer 11

90

Question 12

What is the bond angle for linear molecules?

Answer 12

180

Question 13

How many bonded pairs are there in non-linear molecules?

Answer 13

2

Question 14

How many bonded pairs are there in trigonal planar molecules?

Answer 14

3

Question 15

How many bonded pairs are there in pyramidal molecules?

Answer 15

3

Question 16

How many bonded pairs are there in tetrahedral molecules?

Answer 16

4

Question 17

How many bonded pairs are there in octahedral molecules?

Answer 17

6

Question 18

How many bonded pairs are there in linear molecules?

Answer 18

2

Question 19

How many lone pairs are there in non-linear molecules?

Answer 19

2

Question 20

How many lone pairs are there in trigonal planar molecules?

Answer 20

0

Question 21

How many lone pairs are there in pyramidal molecules?

Answer 21

1

Question 22

How many lone pairs are there in tetrahedral molecules?

Answer 22

0

Question 23

How many lone pairs are there in octahedral molecules?

Answer 23

0

Question 24

How many lone pairs are there in linear molecules?

Answer 24

0

Question 25

Define ‘permanent dipole-dipole interactions’.

Answer 25

Forces which occur between neighbouring molecules with a permanent dipole.

Question 26

Define ‘induced dipole-dipole interactions’.

Answer 26

Forces which occur when electrons moving randomly create a dipole and induce one in a neighbouring molecule.

Question 27

Which three elements can form hydrogen bonds?

Answer 27

Oxygen, nitrogen, and fluorine.

Question 28

What is the bond angle around the H atom in a hydrogen bond?

Answer 28

180

Question 29

Around which atom is the 180 degree bond angle in a hydrogen bond?

Answer 29

Hydrogen

Question 30

Are sodium, potassium, and ammonium salts soluble in water?

Answer 30

Yes

Question 31

Are nitrates soluble in water?

Answer 31

Yes

Question 32

Are chlorides soluble in water?

Answer 32

Mostly, yes

Question 33

Are sulfates soluble in water?

Answer 33

Mostly, yes

Question 34

Are silver and lead chlorides soluble in water?

Answer 34

No

Question 35

Are lead, barium, and calcium sulfates soluble in water?

Answer 35

No

Question 36

Are carbonates soluble in water?

Answer 36

Mostly, no

Question 37

Are hydroxides soluble in water?

Answer 37

Mostly, no

Question 38

Which carbonates are soluble?

Answer 38

Sodium , potassium, and ammonium

Question 39

Which hydroxides are soluble?

Answer 39

Sodium , potassium, and ammonium

Question 40

Which chlorides are insoluble?

Answer 40

Silver and lead

Question 41

Which sulfates are insoluble?

Answer 41

Lead, barium, and calcium

Question 42

What is electronegativity?

Answer 42

The ability of an atom to attract the bonding atoms in a covalent bond.

Question 43

Define electronegativity.

Answer 43

The ability of an atom to attract the bonding electrons in a covalent bond.

Question 44

Define polar bond.

Answer 44

A bond between two atoms of differing electronegativities.

Question 45

Define polar molecule.

Answer 45

A molecule with a more positive and a less positive side, due to the polarity of its bonds.

Question 46

Why is ice less dense than water?

Answer 46

Hydrogen bonds are long and the molecules are in an open lattice structure.