C3 - Structure And Bonding

Question 1

What is Covalent Bonding?

Answer 1

Sharing pair(s) of electrons between non-metal atoms.

Question 2

What is Ionic Bonding?

Answer 2

Transferring electrons, (between metal and no-metal atoms) were the atoms lose or gain electrons to form charged particles (ions).

Question 3

What are Ions?

Answer 3

A charged particle.

Question 4

Sodium has 2,8,1 stabalise it using Ionic Bonding ?

Answer 4

Na[2,8]+

Question 5

Na (2,8,1) + Cl (2,8,7) stabalise it with ionic bomding.

Answer 5

Na [2,8]+ + Cl [2,8,8]-

Question 6

Group 1 want form what ions?

Answer 6

+1 ions

Question 7

Group 5 want to form what ions?

Answer 7

-3 ions

Question 8

Group 7 want to form what ions?

Answer 8

1- ions

Question 9

Calcium atom is 2,8,8,2 and Chlorine atom is 2,8,7 balance this equation.

Answer 9

Ca [2,8,8)2+ Cl [2,8,8]-
Cl [2,8,8]-
Chlorine gains 1 but calcium needs to get rid of 2 so 2 Chlorine atoms are needed.

Question 10

What is graphene?

Answer 10

A single layer of graphite one atom thick.

Question 11

What are Fullerenes?

Answer 11

Molecuoes of carbon atoms with hollow shapes, usually spherical. Fullerenes can be used as lubricants for example giving drug to the body.

Question 12

What are Carbon Nanotubes?

Answer 12

They are cylindrical fullerenes and they can be used as reinforcements such as in tennis rackets.

Question 13

Why does it take a lot of energy to break Giant Ionic Structures?

Answer 13

It takes a lot of energy to break down the giant ionic lattice because there are lots of strong ionic bonds to break. To seperate the ions you have to overcome all those electrostatic forces of attraction acting in all directions.

Question 14

When can ionic compounds conduct electricity?

Answer 14

When molten or disolved in water as there can then become mobile and carry the charge through the liquid.

Question 15

Example of Giant Convalent Structures?

Answer 15

Diamond and Graphite

Question 16

3 special properties of a Giant Convalent Strutures?

Answer 16

1) They have very high melting and boiling points
2) Insoluble in water
3) (apart from graphite) they are hard and do not conduct electricity

Question 17

Why is Graphite soft and slippery?

Answer 17

There are no covalent bonds between the layers, meaning the layers can slide over eachother.

Question 18

What are delocalised electrons?

Answer 18

The electrons in the ‘sea’ of free-moving electrons (outer most shell), they are not linked to the structure.

Question 19

What does graphites Delocalised electrons allow? (Same with metals)

Answer 19

It is able to conduct electricity as the delocalised electrons will drift towards the postive terminals. It is also a great heat conductor as the delocalised electrons will move around faster transfering energy around the material quicker.

Question 20

Why are particles made up as metals described as postivily charged?

Answer 20

Because there are more protons than electrons in the structure as they lose their outer shell elctron(s) into the delocalised electrons.

Question 21

What is a alloy?

Answer 21

Is a mixture of two or more elements, one at least a metal.

Question 22

What does mallulable mean?

Answer 22

Metal can be hammered or stretched into a different shape wtihout braking.

Question 23

Why are metals Ductile?

Answer 23

Metal can be drawn into wires as the layer of atoms can slide over eachother.

Question 24

How can a alloy make a metal harder?

Answer 24

If you distrupt the postive charged ions then it will be harder for the layer to move.