Unit 2- bonding, structure and properties of matter

Question 1

In solids what are the three main features of the particles?

Answer 1

Have a regular arrangement
Are very close together
Vibrate about fixed positions

Question 2

In liquids what are the three main features of the particles?

Answer 2

Have a random arrangement
Are close together
Flow around each other

Question 3

In gases what are the three main features of the particles?

Answer 3

Have a random arrangement
Are much further apart
Move very quickly in all directions

Question 4

Name 3 limitations of the particle model

Answer 4

1. Forces between particles are not shown
2. The volume of the particles
3. The space between the particles

Question 5

Can liquids be compressed?

Answer 5

No❌❌❌❌❌

Question 6

What 3 things occur when a substance changes state

Answer 6

The particles themselves stay the same
The way the particles are arranged changes
The way particles move changes

Question 7

The amount of energy required required for a substance change to state depends on?

Answer 7

The amount of energy required to overcome the forces of attraction between the particles

Question 8

The stronger the forces of attraction?

Answer 8

The greater amount of energy needed to overcome them

The higher the melting points due to strong bonds

Question 9

What are 3 substances that have high melting points due to the strong bonds

Answer 9

Ionic compounds
Metals
Giant covalent structures eg diamond 💎

Question 10

In substances that contain small molecules ? 3 points

Answer 10

The bonds within the molecules are strong covalent bonds
The forces of attraction between the molecules are much weaker
Only a little energy is needed to overcome the forces between the molecules

Question 11

What is an ion

Answer 11

An atom that has gained or lost an electron

Question 12

Ionic bonding occurs between what?

Answer 12

Metals and none metals

Positive and negative ions

Question 13

Ions have a complete?

Answer 13

Outer shell of electrons (the same as noble gases)

Question 14

In ionic bonding, the metal ?

And the none metal?

Answer 14

The metal loses electrons to become positively charged ions

The none metal gains electrons to form a negatively charged ion

Question 15

What is an ionic bond

Answer 15

The strong electrostatic force of attraction between a positive metal and a negative none metal

Question 16

State 4 things about ionic compounds

Answer 16

1. High melting and boiling point
2. Do not conduct electricity when a solid, because ions cannot move
3. Do conduct electricity when molten or in a solution because the ions are free to move about and carry their charge
4. Dissolve in water

Question 17

Where does covalent bonding occur?

Answer 17

Between non metals

Question 18

What can be used to show covalent bonds

Answer 18

A dot and cross diagram

Question 19

Covalent bonds are very strong true or false?

Answer 19

True✅✅

Question 20

What is a covalent bond

Answer 20

A shared pair of electrons between atoms

Question 21

Can small molecules conduct electricity?why

Answer 21

No because they have no overall charge

Question 22

Why do small molecules have a low melting and boiling point

Answer 22

Because they have a weak intermolecular force

Question 23

The larger the molecules are, the stronger the?

Answer 23

Intermolecular forces between the molecules become

Question 24

In the group 7 elements, the molecules get larger and their melting and boiling points increase
What are the states at room temperature of:
Fluorine and chlorine
Bromine
Iodine

Answer 24

Fluorine and chlorine=gases☁️
Bromine=💧
Iodine=⬛️

Question 25

Giant covalent structures have high what?

Answer 25

Boiling and melting points

Question 26

Diamond and graphite are what

Answer 26

Giant covalent structures They are forms of carbon

Question 27

Name 4 points about diamond

Answer 27

It has a giant, rigid covalent structure (lattice) Each carbon atom forms 4 strong covalent bonds with other carbon atoms No charged particles, so does not conduct electricity

Question 28

4 points about graphite

Answer 28

1. Each carbon atom forms 3 covalent bonds with other carbon atoms 2. This results in a layered hexagonal structure 3. The layers are held together by intermolecular forces, this makes graphite soft and slippery 4. One electron from each carbon atom is delocalised, this allows it to CONDUCT electricity

Question 29

What is silicon dioxide also known as

Answer 29

Silica

Question 30

3 points about silica

Answer 30

Lattice structure Each oxygen atom is joined to 2 silicon atoms Each silicon atom is joined to 4 oxygen atoms

Question 31

What is graphene

Answer 31

A single layer of graphite thats atoms are arranged in a hexagonal structure, just one atom thick.

Question 32

What are three qualities of graphene

Answer 32

Very strong Good thermal and electrical conductor Nearly transparent

Question 33

What os a fullerenes

Answer 33

Carbon molecules which contain different numbers of carbon atoms

Question 34

Name three types of fullerene shapes

Answer 34

Hollow tubes, balls and cages

Question 35

What was the first fullerene to be discovered? | What are 3 points about it

Answer 35

Buckminsterfullerene C60 Consists of 60 carbon atoms that are joined together in a series of hexagons and pentagons Most stable and symmetrical fullerene

Question 36

What does the buckminsterfullerenes look like

Answer 36

A football⚽️⚽️⚽️⚽️⚽️⚽️

Question 37

What are 4 useful properties of carbon nanotubes

Answer 37

1. To deliver drugs to the body 2. In lubricants 3. As catalysts 4. For reinforcing materials eg tennis racket frames🏸🎾

Question 38

Polymers consist of what

Answer 38

Very large molecules

Question 39

Polymers are commonly known as what

Answer 39

Plastic

Question 40

How are polymers held together

Answer 40

Strong covalent bonds | Strong intermolecular forces

Question 41

Polymers are at what state at room temperature

Answer 41

Solid

Question 42

What is polythene

Answer 42

A cheap polymer produced when lots of ethane molecules are joined together in an addition polymerisation reaction

Question 43

What is polythene used for, why?

Answer 43

Plastic bottles and bags because its cheap

Question 44

What is metallic bonding

Answer 44

Metallic bonding is the attraction between the positive ions and delocalised negatively charged electrons

Question 45

Metals have a giant structure in which electrons in the outer shell are ? This produces what

Answer 45

Delocalised | This produces a lattice of positive ions held together by electrostatic attraction to the delocalised electrons.

Question 46

The delocalised electrons in metallic bonding can move freely meaning what

Answer 46

Metals are good electrical and thermal conductors

Question 47

Properties of metals- The particles in pure metals have a regular? This means what

Answer 47

Arrangement | The layers can slide over each other ie they're malleable

Question 48

Why is copper used to make water pipes?

Answer 48

Unreactive | Malleable

Question 49

What are the uses and properties of aluminium

Answer 49

Used for- high voltage cables, furniture, drink cans, kitchen foil Properties- corrosion resistant, ductile, malleable, conductive, low density

Question 50

Properties/Uses for copper

Answer 50

Uses-electrical wiring, water pipes, saucepans Properties- ductile, malleable, conductive

Question 51

Uses/properties of gold

Answer 51

Uses- jewellery, electrical junctions Properties- ductile, shiny, conductive

Question 52

Whats an alloy

Answer 52

A mixture that contains a metal and at least one other element eg stainless steel

Question 53

Why are alloys used?

Answer 53

Because pure metals are too soft

Question 54

How do alloys work?

Answer 54

The added element disturbs the regular lattice or the metal atoms so the laters do not slide over each other