C3 - Structure and Bonding

Question 1

What structure are giant ionic compounds arranged in?

Answer 1

an ionic lattice structure

Question 2

What is ionic bonding?

Answer 2

A metal and a non-metal with opposite charges are attracted to each other due to the electrostatic force.

Question 3

Three types of bonding

Answer 3

• ionic
• covalent
• metallic

Question 4

What happens to the particles in a body when it melts?

Answer 4

The particles gain more energy which breaks the bonds between the particles meaning they can more freely move around.

Question 5

Does the temperature increase, decrease or stay the same when a body is changing state? Why?

Answer 5

The temperature stays the same. The energy being transferred from the surroundings is used to break or make the bonds between the particles in the body.

Question 6

How many electrons can the first 3 shells hold?

Answer 6

1^st : 2
2^nd : 8
3^rd : 8

Question 7

Why are some atoms stable and some unstable?

Answer 7

Stable atoms have filled outer shells
Unstable atoms have incomplete outer shells

Question 8

define ion

Answer 8

an atom with a + or - electrical charge

Question 9

When can ionic compounds conduct electricity?

Answer 9

When they are molten. This is because the ions break free from the lattice structure and electrons are then free to move around - this means they can conduct an electrical current.

Question 10

Why are most ionic compounds dissolvable in water?

Answer 10

A water molecule has a slight positive and negative charge so it can break apart the ionic compound.

Question 11

What is covalent bonding?

Answer 11

Covalent bonding is when multiple non-metal atoms share electrons.

Question 12

define intramolecular

Answer 12

strong bonds inside molecules

Question 13

define intermolecular

Answer 13

a weaker force of attraction that acts between molecules

Question 14

3 examples of giant covalent structures

Answer 14

• sand (SiO₂)
• diamond (C)
• graphite (C)

Question 15

Why are simple covalent molecules gases at room temperature?

Answer 15

the molecules are so small that the intermolecular forces are very weak and don’t take much energy to break.

Question 16

properties of diamond

Answer 16

• high melting and boiling point
• crystalline shape (not lattice)
• does not conduct electricity
• very hard
• each carbon is bonded to 4 other carbons

Question 17

define hardness

Answer 17

the measure of resistance to deformation, e.g. indentation or a scratch

Question 18

properties of graphite

Answer 18

• electrical conductor - each carbon has a delocalised electron
• soft and slippery - layers slide off easily, used as a lubricant
• each carbon is bonded to 3 other carbons

Question 19

what are fullerenes

Answer 19

giant covalent molecules of carbon atoms with hollow shapes. an allotrope of carbon

Question 20

1 example of a fullerene

Answer 20

buckminsterfullerene - C₆₀

aka buckyball

Question 21

properties of fullerenes

Answer 21

• high tensile strength
• good electrical conductor
• good thermal conductor

Question 22

what is graphene

Answer 22

one atom thick layer of carbon arranged in a hexagonal lattice

Question 23

list 4:

properties of graphene

Answer 23

• excellent electrical conductor
• low density
• very reactive
• strong for its mass

Question 24

properties of metals

Answer 24

• high melting and boiling points
• good electrical conductor
• good thermal conductor
• malleable
• ductile
• sonorous
• dense
• strong

Question 25

# list 4: properties of giant ionic compounds

Answer 25

- form cubic shapes - bad electrical conductor unless molten - dissolves in water - high melting and boiling points

Question 26

How do metals bond?

Answer 26

Metallic bonding is when metals bond. They bond because there is an electrostatic attraction between the metal ions (really just the nucleus) and the sea of electrons.

Question 27

define strength

Answer 27

how much force can be applied until a body breaks apart

Question 28

Why are metallically bonded structures malleable?

Answer 28

The layers in the metal slide over each other when a force is applied.

Question 29

define alloy

Answer 29

a mixture of a metal and at least 1 other element

Question 30

Why are alloys stronger than pure metals?

Answer 30

alloys are stronger because the mixture of atoms with different radii disrupts the regular lattice structure causing more difficulty for layers to slide over each other

Question 31

Why do nanoparticles behave differently

Answer 31

- they have a large surface area : volume ratio making them more reactive - they are so small quantum mechanics govern them

Question 32

# list 6: general properties of substances

Answer 32

- Hardness - melting + boiling Points - Strength - electrical Conductor - thermal Conductor - Structure / Shape | Horrible People Say Cats Can't Sing