Strcutures

Question 1

What does a giant ionic lattice look like

Answer 1

3d dimensional lactic of alternating metal and non metal ions

Question 2

What are examples of giant ionic lattice

Answer 2

Sodium chloride
Magnesium oxide
Any metal and non metal

Question 3

Properties of giant ionic lattices

Answer 3

-Crystalline
-high melting points
-conducts electricity when liquid/molten
-does not conduct electricity when solid
-soluble in water
-high boiling points

Question 4

What does a covalent molecular look like

Answer 4

Molecules with dashed lines repenting van de waals forces in between

Question 5

What are some examples of covalent molecular

Answer 5

Iodine
Carbon dioxide
Water
Hydrogen chloride
Ammonia

Question 6

What are the properties of covalent molecular

Answer 6

Low melting and boiling points
Do not conduct electricity
Not very soluble in water
Soft when solid

Question 7

What does diamond structure look like

Answer 7

Each carbon covalent bonds to 4 other carbons in a giant tetrahedral structure. Giant covalent/ macro molecular structure.

Question 8

What are the properties of diamond

Answer 8

Very high melting and boiling points
Diamond does not conduct electricity
Insoluble in water
Extremely hard

Question 9

What does graphite look like

Answer 9

3d hexagonsl structure with layers. 3 covalent bonds between each carbon leaving one electron delocalised

Question 10

What are the properties of graphite

Answer 10

Graphite does conduct electricity as they have a delocalised electron free to carry charge
Graphite slippery soft solid layers that can slide over each other
Graphite is used as a lubricant and in pencil lead

Question 11

What does graphene look like

Answer 11

Single atom thick layer of graphite with strong covalent bonds between each carbon atom. The atoms are arranged hexagon and are two dimensions 

Question 12

What are the properties of graphene

Answer 12

Graphene does conduct electricity as it has delocalised electrons
Graphing conducts heat and electricity efficiently
nearly transparent
Graphing is 100 times stronger than steel
very thin, light and inexpensive
It is insoluble because of the 3 strong covalent bonds
It is a man-made structure 

Question 13

What is graphene used in

Answer 13

-solar cells
-light emitting diodes
-touch panels
-smart windows or phones

Question 14

Name 3 giant covalent structures

Answer 14

Diamond
Graphite
Graphene

Question 15

What do diamond graphite and graphene all have in common

Answer 15

They are all allotropes of carbon

Question 16

What does a giant metallic structure look like

Answer 16

Regular lattice of positive metal ions with delocalised electrons randomly scattered throughout the

Question 17

What are the properties of giant metallic structure

Answer 17

High melting and boiling points
Dense (tight packing makes them dense)
Conducts electricity
Conducts heat
Malleable
Ductile

Question 18

Allotrope

Answer 18

Allotropes are different forms of the same element in the same physical state

Question 19

Ductile

Answer 19

Can be drawn into wires

Question 20

Malleable

Answer 20

Can be hammered into shape

Question 21

Metallic bonding

Answer 21

The attraction between delocalised electrons and the positive ions in a regular lattice 

Question 22

Why do giant ionic lattices conduct electricity when molten but not when solid? 

Answer 22

When solid, giant ionic lattices are arranged in tight strong regular lattice structure meaning the ions can’t carry the charge of electricity because no ions are free to. But when dissolved in water or melted the strong electrostatic interactions of the giant ionic lattice are overcome and the ions are free to move and carry current/charge 

Question 23

Why do ionic compounds have high melting and boiling points?

Answer 23

Ionic compounds have high melting and boiling because ionic bonds have a strong electrostatic attraction between them which require large amounts of heat energy to break

Question 24

What is a covalent bond

Answer 24

Shared pair of electrons between two non metal atoms

Question 25

Why do molecular covalent structures have low melting points and boiling points

Answer 25

Although there are strong bonds between the atoms within the molecules there are only weak intermolecular forces of attraction between molecules. These are called Van der waals forces and require little energy to break hence the low melting + boiling point.

Question 26

How many atoms of carbon surround diamond?

Answer 26

Each atom is covalently bonded to 4 other atoms

Question 27

How many atoms of carbon surround graphite? 

Answer 27

3

Question 28

Why did diamond graphite both have high melting point boiling points

Answer 28

They have strong three-dimensional covalent bonding networks. This requires a huge amount of heat energy to break hence the high melting/boiling points

Question 29

Explain how graphites properties mean it can be used as lubricant

Answer 29

Graphite is arranged in layers that can slide over one another due to the fact the layers are only held together by weak intermolecular forces called van der waals). This is what makes them lubricant.

Question 30

Explain why graphite unlike other giant covalent substances can conduct electricity

Answer 30

In graphite carbon is covalently bonded to 3 atoms. This leaves one delocalised electron per atom which is able to move freely around the structure and therefore courage charge + conduct electricity

Question 31

Why are metallic structures malleable?

Answer 31

Malleable means can be hammered into shape. The arrangement of metallic structures means they have free delocalised electrons which allows the layers of ions to slide over each other without breaking when a force is applied therefore making it malleable. 

Question 32

Why did metallic structures conduct heat? 

Answer 32

The arrangement of metallic structures mean the delocalised electrons with high kinetic energy can move around freely to transfer the particle kinetic energy to cooler ions therefore conducting heat

Question 33

Why do metallic structures have high melting points

Answer 33

Metallic structures have strong bonding between the positive ions and delocalised electrons that require huge amounts of heat energy to break hence the high melting point

Question 34

Why are metallic structures good conductors of electricity?

Answer 34

The arrangement of metallic structures includes delocalised electrons. These delocalised electrons are free to carry the charge of an electrical current when a voltage is applied

Question 35

Use the understanding of the bonding to explain my metals can be made into the long thin wires 

Answer 35

The sea of delocalised electrons in metallic bonding allows the layers of cations to slide over each other and be held in their new place by the free electrons. This means they easily be stretched out into long wires without breaking. 

Question 36

Why is aluminium used for overhead electrical power cables

Answer 36

Good conductor of electricity Light Not liable to corroding

Question 37

What is an alloy

Answer 37

A Mixture of two or more elements, at least one of which is a metal and the resulting mixture has metallic properties

Question 38

Steel is

Answer 38

An alloy of iron and carbon

Question 39

White gold is an alloy of

Answer 39

Gold and silver

Question 40

Rose gold is an alloy of

Answer 40

Gold and copper

Question 41

Brass is an alloy of

Answer 41

Copper and zinc

Question 42

What is pure gold

Answer 42

24 carats

Question 43

How do you calculate the purity of gold

Answer 43

% of gold in alloy = number of carats ➗ by 24 x 100

Question 44

Why are alloys harder than metals?

Answer 44

Alloys also have metallic structures but some of the ions(or atoms) in the alloy are different size to those of the metal ion/atom. This distort the layers in the structure and makes it more difficult for the layers of ions to slide past each other. As a result alloys are harder than pure metals 

Question 45

What is meant by the term material science?

Answer 45

The study of how strong material is the distance between the items and other properties

Question 46

What does inert mean

Answer 46

Unreactive

Question 47

Apart from graphite and diamond, what is the name given to the other form of carbon?

Answer 47

Buckminsterfulerence (Bucky balls)

Question 48

What is a lattice

Answer 48

regular arrangements with each ion surrounded by ions of opposite charge.