bonding, structure, properties of matter

Question 1

When a substance melts, what happens to the attractive forces between solid particles?

Answer 1

They are broken as particles break away from the solid lattice and become liquid particles.

Question 2

What happens to the temperature when a substance melts?

Answer 2

Remains constant until all bonds are broken.

Question 3

What happens to particles when liquid boils?

Answer 3

The particles overcome the attractive forces to become a gas.

Question 4

What happens to the temperature when the liquid boils?

Answer 4

Remains constant until all attractive forces are overcome.

Question 5

When are ions formed?

Answer 5

When metal atoms transfer their outer shell electrons to the outer shell of non-metal atoms. This electron transfer forms charged particles called ions.

Question 6

The electrostatic force around each ion attract several opposite charged ions. What does his form?

Answer 6

A giant lattice.

Question 7

Ionic compounds have (a) melting and boiling points because the ionic bonds are (b).

Answer 7

(a) high
(b) strong

Question 8

Do all giant structures have a high melting and boiling point?

Answer 8

Yes, because they have lots of bonds to be broken.

Question 9

Do ionic compounds have a better electrical conductivity of solid, or liquids?

Answer 9

Liquids, the ions can move around and carry the current whereas in solids they can’t.

Question 10

Covlantely bonded substances can exist as…

Answer 10

Simple molecules, giant covalent structures, polymers.

Question 11

The (a) forces increase as the molecular size (b), meaning the melting and boiling points (c).

Answer 11

(a) intermolecular
(b)increases
(c)increases

Question 12

What is broken when a simple molecular force melts?

Answer 12

The weak intermolecular forces, not strong covalent bonds.

Question 13

All of the (a) atoms in diamond, graphite and (b) are linked together by (c).

Answer 13

(a) carbon
(b) graphene
(c) strong covalent bonds

Question 14

In diamond, each carbon atom is covalently bonded to how many other carbon atoms?

Answer 14

4.

Question 15

Why does diamond have such a high melting/ boiling point?

Answer 15

It has strong covalent bonds in a giant structure.

Question 16

Can diamond conduct in a liquid/ solid state?

Answer 16

No, there are no charged particles, free electrons to carry an electrical current.

Question 17

How are carbon atoms structured in graphite?

Answer 17

In hexagonal rings, where each carbon atom is covalently bonded to 3 other carbon atoms, meaning each carbon atoms has a free electron to move around meaning graphite conducts both as a solid and liquid.

Question 18

The covalent bonds in the layers are (a) but between layers there are only (b). These are (c) to break so the layers can (d) over eachother, making graphite soft and (e)

Answer 18

(a) strong
(b) weak intermolecular forces
(c) easy
(d) slide
(e) slippery

Question 19

Does graphene have an identical structure to graphite?

Answer 19

It is identical to ONE layer of graphite, making it 1 atom thick. It has similar properties to graphite.

Question 20

What is the smallest example of a spherical fullerene?

Answer 20

Buckminsterfullerene, which is a large but simple molecular substance.

Question 21

What do buckminsterfullerene contain?

Answer 21

Mostly 6- carbon rings, but some 5- and 7-.

Question 22

What can buckminsterfullerene be used for?

Answer 22

To trap drugs and deliver them to parts of the body, lubricants and catalysts.

Question 23

Carbon nanotubes are (a), which have high length to diameter ratio. They have (b) between carbons in the layers, meaning they have (c) tensile strength. They are (d) conductors.

Answer 23

(a) cylindrical fullerenes
(b) strong covalent bonds
(c) high
(d) good

Question 24

What are polymeres

Answer 24

Polymers are very large molecules which are made up of long chains of carbon atoms joined by strong covalent bonds. As the chains are long, the intermolecular forces between each chain are quire large, meaning polymers are solids.

Question 25

Do metals form a giant lattice of positive metal ions in a sea of delocalised electrons?

Answer 25

Yes.

Question 26

What is the electrostatic attraction between the positive ions and delocalised/ free electrons called?

Answer 26

A metallic bond.

Question 27

Metallic bonds are usually (a) and need (b) of energy to overcome them, which is why most metals have (c) MP and BP.

Answer 27

(a) strong
(b) a lot
(c) high

Question 28

Where do metallic bonds operate?

Answer 28

In pure metals and alloys.

Question 29

The layers in metal ions can (a) eachother, meaning metals can be (b) meaning they are malleable and they can be (c) meaning they are ductile.

Answer 29

(a) slide over
(b) bent/ shaped
(c) drawn into wires

Question 30

Are alloys a mixture of metals?

Answer 30

Yes, they are harder than pure metals too.