Structure

Question 1

What is a giant ionic structure?

Answer 1

Lattice held together by electrostatic forces of attraction between positive and negative ions

Question 2

Intermolecular forces?

Answer 2

weak force between molecules

Question 3

what are the 3 properties and reasons for a giant ionic lattice?

Answer 3

1. High melting point - strong electrostatic attraction require a lot of energy to break them. These bonds are strong since the oppositely charged ions attract each other strongly
2. Conducts electricity when aqueous - Ionic compounds containing ions which attracted to the electrodes and are free to move to the electrodes when aqueous
3. Soluble in water - the poll of water molecules are attracted to the charged ions and the supplies the energy to break up the giant lattice

Question 4

Example of a giant ionic lattice

Answer 4

Sodium chloride

Question 5

Example of a simple covalent structure

Answer 5

water, hydrogen

Question 6

what are the 3 properties and reasons for a simple covalent structure?

Answer 6

1. Weak intermolecular forces are easily broken and molecules are therefore easily separated
2. Do not conduct - covalent molecules on neutral so I’m not attracted to the power supply
3. Insoluble in water. The neutral molecules are not attracted to the polar the water molecules

Question 7

what are the 3 properties and reasons for a giant molecular covalent structure?

Answer 7

1. High melting point – the strong covalent bonds need to be broken to mount the giant covalent lattice and these bonds are very difficult to break
2. Do not conduct (graphite) - giant covalent lattice do not contain free electron so cannot conduct electricity except for graphite which contains delocalised electrons
3. Insoluble in water - the strong covalent bonds are difficult to break

Question 8

Description of a diamond?

Answer 8

Diamonds use all carbon bonds, so there are no delocalised electrons every carbon atom is joined to the four others so every electron is used

Question 9

3 properties of diamond?

Answer 9

1. High melting point so there are 4 strong covalent bonds per atom and must be broken
2. Very hard to to the strong bonds since each carbon atom is joint four other carbon atoms
3. Don’t conduct as they do not have free moving electrons

Question 10

3 uses of diamond and the reason?

Answer 10

1. cutting tool as it is the hardest know in substance
2. Jewellery – crystalline structure allows it to be cut in different ways
3. Laser components, precise optical equipment

Question 11

Description of graphite?

Answer 11

Strong covalent bond in carbon atoms between each layer. Weaker forces hold layers together. So layers can slide. But Corbin is in group for but only uses three out of the four potential bonds

Question 12

3 properties of graphite?

Answer 12

1. High melting point as strong covalent bonds need to be broken
2. The hardness is very soft so the layers can slide over each other
3. Can conduct as the strong covalent bonds

Question 13

3 uses of graphite and the reason?

Answer 13

1. Lubricant so the layers can slide over each other making a soft
2. Crucibles as they can withstand high temperatures
3. Paint as it is soft because of the layers