Bonding

Question 1

Ionic Bonding

Answer 1

Strong electrostatic force of attraction between oppositely charged ions (formed by the transfer of electrons from one atom to another)

Question 2

Covalent Bonding

Answer 2

Strong electrostatic force of attraction between the nuclei of both atoms and the shared pair of electrons

Question 3

Metallic Bonding

Answer 3

Electrostatic force of attraction between a lattice of positive ions and the sea of delocalised electrons

Question 4

Group 1 ions charge

Answer 4

1+

Question 5

Group 2 ions charge

Answer 5

2+

Question 6

Group 3 ions charge

Answer 6

3+

Question 7

Group 5 ions charge

Answer 7

3-

Question 8

Group 6 ions charge

Answer 8

2-

Question 9

Group 7 ions charge

Answer 9

1-

Question 10

Zinc ion

Answer 10

Zn2+

Question 11

Silver ion

Answer 11

Ag+

Question 12

Hydrogen ion

Answer 12

H+

Question 13

Ammonium ion

Answer 13

NH4+

Question 14

Nitrate ion

Answer 14

NO3-

Question 15

Hydroxide ion

Answer 15

OH-

Question 16

Carbonate ion

Answer 16

CO32-

Question 17

Sulfate ion

Answer 17

SO42-

Question 18

Do ionic compounds have high melting points and boiling points? (Reason)

Answer 18

Yes
- (giant ionic lattice structure
- strong electrostatic force of attraction between oppositely charged ions
- a lot of energy is required to overcome these forces)

Question 19

Why are ionic compounds crystalline and brittle?

Answer 19

• regular arrangement of the ions in the lattice
  -the arrangement of the ions is disrupted, the like charged ions repel

Question 20

Are ionic substances soluble in water?

Answer 20

Yes

Question 21

Are ionic substances soluble in organic solvents?

Answer 21

No

Question 22

Why can’t the ionic compounds conduct electricity when they are solid?

Answer 22

• the ions are fixed in state
  -the ions aren’t mobile

Question 23

Do substances with simple molecular structure have low melting and boiling points? (Reason)

Answer 23

Yes
- (weak intermolecular forces of attractions between molecules
- not much energy is required to overcome these forces)

Question 24

Why don’t covalent molecular compounds conduct electricity?

Answer 24

• there are no ions
• there are no delocalised electrons

Question 25

Are covalent molecular compounds soluble in water? Any exceptions?

Answer 25

No - ethanol, NH3 and HCl are soluble in water.

Question 26

Are covalent molecular compounds soluble in organic solvents?

Answer 26

Yes

Question 27

Explain diamond's bonding and structure

Answer 27

- each carbon atom is covalently bonded to 4 other carbon atoms - forming a tetrahedral structure

Question 28

Does diamond and graphite have high melting point? (Reason)

Answer 28

Yes - (they are substances with giant covalent structures - they have very strong carbon-carbon covalent bonds - a lot of energy is required to break these strong covalent bonds)

Question 29

Is diamond hard? (Reason)

Answer 29

Yes - (very strong covalent bonds - a lot of energy is required to break the bonds in the giant structure)

Question 30

Does diamond conduct electricity? (Reason)

Answer 30

No - (no delocalised electrons)

Question 31

Is diamond soluble?

Answer 31

No

Question 32

Explain graphite's bonding and structure

Answer 32

-each carbon is covalently bonded to 3 other carbon atoms -forming a hexagonal layer structure

Question 33

Is graphite hard? (Reason)

Answer 33

No -(weak forces of attractions between layers -not much energy is required to overcome these forces)

Question 34

Does graphite conduct electricity? (Reason)

Answer 34

Yes -(it has delocalised electrons which are free to move)

Question 35

Is graphite soluble?

Answer 35

No

Question 36

Why are metals hard and have high melting points?

Answer 36

- strong electrostatic forces of attraction between the positive ions and the delocalised electrons

Question 37

Why do metals conduct electricity?

Answer 37

- it has delocalised electrons which are free to move throughout the structure

Question 38

Why are metals malleable and ductile?

Answer 38

- the layers of positive ions slide over each other