Bonding, Structure and Properties of Matter

Question 1

Why does an atom lose or gain electrons?

Answer 1

To get a full outer shell and be stable

Question 2

What happens to a metal when it forms an ion?

Answer 2

They lose electrons to form positive ions

Question 3

What happens to non metals when they form an ion

Answer 3

They gain electrons to form negative ions

Question 4

If an atom lost 2 electrons to form an ion what would the charge be?

Answer 4

2+

Question 5

If an atom gains 3 electrons when turning to an ion what would the charge be?

Answer 5

3-

Question 6

What type of bonding occurs when a metal and non metal react together?

Answer 6

Ionic bonding

Question 7

What is ionic bonding?

Answer 7

When non metals and metals react together
The metal atom loses electrons to form positively charged ion
The non metal atom gains these electrons to form negatively charged ion

Question 8

What is the force called where oppositely charged ions are strongly attracted to each other?

Answer 8

Electrostatic forces

Question 9

What charge will group 1 element ions have?

Answer 9

1+

Question 10

What charge will group 2 element ions have?

Answer 10

2+

Question 11

What charge will group 6 element ions have?

Answer 11

2-

Question 12

What charge will group 7 element ions have?

Answer 12

1-

Question 13

What diagrams show ionic bonding or ions?

Answer 13

Dot and cross diagrams

Question 14

What must you always do when drawing an ion?

Answer 14

Use square brackets and state the charge

Question 15

What is the structure of ionic compounds?

Answer 15

Giant ionic lattice

Question 16

What are the properties of the ionic compound structure (giant regular lattice)?

Answer 16

Very strong electrostatic forces of attraction in all directions between oppositely charged ions

Question 17

Properties of ionic compounds

Answer 17

High melting and high boiling points due to many strong bonds between ions.
When solid can’t conduct electricity as ions are held in place
When liquid will conduct electricity as ions are free to move
Dissolve easily in water- ions superstar and are free to move

Question 18

What method do you use to write the empirical formula of an ionic compound?

Answer 18

Swap and drop

Question 19

What is covalent bonding?

Answer 19

When two non metals react together and share electron pairs to make covalent bonds

Question 20

How can you draw covalent bonds?

Answer 20

Dot and cross diagram
In shells
Line diagrams

Question 21

What is a simple molecular substance?

Answer 21

A substance made up of molecules containing a few atoms joined together by covalent bonds.
Eg/ hydrogen ( needs two atoms of hydrogen in order to both have full outer shell through covalent bonds)

Question 22

What are the properties of simple molecular substances?

Answer 22

Forces of attraction between molecules are very weak
Melting and boiling points are very low as molecules are easily parted from each other
Gases or liquids at room temperature
Don’t conduct electricity as there are no free electrons

Question 23

What is a covalent bond?

Answer 23

A chemical bond made by the sharing of a pair of electrons between two atoms

Question 24

In what states are most simple molecular substances at room temperature?

Answer 24

Gas or liquid

Question 25

What forces are stronger in simple molecular substances? Covalent bonds or intermolecular forces?

Answer 25

Covalent bonds

Question 26

What forces need to be overcome to boil a simple molecular compound?

Answer 26

Intermolecular forces

Question 27

Why may hydrogen chloride have poor electrical conductivity?

Answer 27

It doesn’t contain any ions or delocalised electrons to carry a charge

Question 28

Explain how the atoms are held together in a molecule of hydrogen chloride

Answer 28

A pair of electrons (one from hydrogen and one from chlorine) is shared between the two atoms. The atoms the held together by the strong attraction between this shared pair of negatively charged electrons and the positively charged nuclei of the atoms.

Question 29

Why may a substance have a higher boiling point than another substance?

Answer 29

They could be a larger molecule so the intermolecular forces are stronger between the bonds so it takes more energy to boil it, therefore the temperature is higher.

Question 30

What is a polymer?

Answer 30

A long chain of repeating units

Question 31

How do you draw a polymer?

Answer 31

Draw the shortest repeating section

Question 32

How do you find the molecular formula of a polymer?

Answer 32

Write down the molecular formula in brackets and put an n outside of it

Question 33

What state are polymers at room temperature?

Answer 33

Solid

Question 34

What has larger intermolecular forces, polymer molecules or simple covalent molecules and what does this mean?

Answer 34

Polymer molecules have larger intermolecular forces as they are bigger so more energy is needed to break them.

Question 35

Are the intermolecular forces weaker in polymer molecules than ionic or giant molecular compounds?

Answer 35

Yes | They have lower boiling points

Question 36

What are the bonds like in giant covalent structures?

Answer 36

All the atoms are bonded to each other by strong covalent bonds

Question 37

What are the melting and boiling points of giant covalent structures?

Answer 37

Very high as lots of energy is needed to break the covalent bonds between the atoms

Question 38

Do giant covalent structures conduct electricity?

Answer 38

No, they don’t contain charged particles so don’t conduct electricity.

Question 39

What are examples of giant covalent structures?

Answer 39

Diamond Graphite Silicon dioxide

Question 40

What is an allotrope?

Answer 40

Different structural forms of the same element in the same physical state.

Question 41

What are the properties of diamond?

Answer 41

Really hard Giant covalent structure Very high melting point Doesn’t conduct electricity as it has no free electrons or ions

Question 42

What are the allotropes of carbon?

Answer 42

Diamond Graphite Graphene Fullerenes

Question 43

What is the structure of diamond?

Answer 43

Each carbon atom has four covalent bonds | Tetrahedral

Question 44

What are the properties of Graphite?

Answer 44

Soft Slippery as no bonds between layers High melting and boiling points Conducts electricity as one delocalised electron

Question 45

What are the uses of diamond?

Answer 45

Drills and saw tops

Question 46

What are the uses of graphite?

Answer 46

Pencils | Lubricant

Question 47

What are the properties of graphene?

Answer 47

``` Hard Very strong High melting and boiling points Light Conducts electricity ```

Question 48

Uses of graphene

Answer 48

Electronics | Carbon fibres

Question 49

What is the structure of graphene

Answer 49

``` One layer of graphite Sheet of carbon atoms Joined in hexagons 2D compound One atom thick ```

Question 50

Structure of graphite

Answer 50

Sheets of hexagons

Question 51

Properties of Fullerenes

Answer 51

High melting and boiling points Hard Conducts electricity

Question 52

Structure of fullerenes

Answer 52

60 carbon atoms joined together to form a ball Can also form nanotubes Or a cage in form of ball Hollow centre

Question 53

Uses of fullerenes

Answer 53

Anti cancer drug transportation

Question 54

What is a nanotube

Answer 54

A tiny carbon cylinder

Question 55

What are the properties of nanotubes?

Answer 55

Conduct heat and electricity | High tensile strength

Question 56

True/false: metals have layers

Answer 56

True

Question 57

Do metals consist of a giant structure?

Answer 57

Yes

Question 58

How does metallic bonding work?

Answer 58

Metal atoms lose outer electrons to form positive ions. They are arranges in a lattice structure and the lost delocalised electrons move around between the metal ions. The positive ions and negative electrons have electrostatic force of attraction which is strong in metals and holds the ions together.

Question 59

What structure of metal causes it to conduct electricity and heat?

Answer 59

Having delocalised electrons

Question 60

What structure causes metals to be malleable and ductile?

Answer 60

Layers of metal ions that can slip over each other

Question 61

What structure of metal will cause it to have high melting and boiling points, be strong and hard and solid?

Answer 61

A strong force of attraction between metal ions and delocalised electrons

Question 62

What is an alloy?

Answer 62

A mixture of metals or of metals and carbon

Question 63

True/false: alloys are harder than pure metals

Answer 63

True

Question 64

How are the repeating units in a polymer bonded together?

Answer 64

Covalent bonding

Question 65

Explain why most metals are malleable

Answer 65

The layers of atoms in metals are able to slide over each other

Question 66

What are the three states of matter

Answer 66

Solid Liquid Gas

Question 67

Properties of solids

Answer 67

``` Strong forces of attraction between particles Close together in fixed positions Regular arrangement Defined shale and volume Particles vibrate and expand when heated ```

Question 68

Properties of liquids

Answer 68

``` Weak force of attraction Randomly arranged but stick close together Definite volume but don’t keep shale Constantly moving particles Move faster when hot Expands when heated ```

Question 69

Properties of gas

Answer 69

``` Very weak force of attraction Free to move far apart Travel in straight lines Don’t keep definite shape or volume Move constantly with random motion Either expand or increase pressure when heated ```

Question 70

When a solid is heated/cooled, its particles gain more energy

Answer 70

Heated

Question 71

What does aqueous mean

Answer 71

Dissolved in water

Question 72

If the temperature of a substance is below the melting point, what state is it?

Answer 72

Solid

Question 73

If the temperature of a substance is above the boiling point, what state will it be?

Answer 73

Gas

Question 74

If the temperature of the substance is between the melting and boiling points, what state will it be?

Answer 74

Liquid

Question 75

How do you work out the surface area to volume ratio?

Answer 75

Surface area/volume

Question 76

True/false as particles decrease in size, the size of their surface area increases in relation to their volume.

Answer 76

True

Question 77

Do nano particles have a high or low surface area to volume ratio?

Answer 77

High

Question 78

What are the uses of nanoparticles?

Answer 78

``` Catalysts Electric circuits Deodorants Surgical masks Wound dressings Cosmetics ```

Question 79

Is it known to doctors if nanoparticles can get into your body through suncream and damage cells?

Answer 79

No

Question 80

Sulphate ionic formula

Answer 80

SO4

Question 81

Nitrate ionic formula

Answer 81

NO3

Question 82

Hydroxide ionic formula

Answer 82

OH

Question 83

Carbonate ionic formula

Answer 83

CO3

Question 84

Ammonia ionic formula

Answer 84

NH4