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gcse chemistry > topic 2 bonding > Flashcards

topic 2 bonding Flashcards

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1
Q

what are the three states of matter

A

solid, liquid and gas

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2
Q

what is particle theory

A

a model where each particle is seen as a small, solid sphere(ball)

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3
Q

give 3 properties of solids

A
  • there are strong forces of attraction between the particles
  • the particles are held together in fixed positions to form a pattern
  • solids have a fixed shape and volume
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4
Q

give 3 properties of liquids

A
  • there are weak forces of attraction between the particles
  • randomly arranged and free to move past each other, but they stick closely together
  • have a fixed volume but dot keep a fixed shape
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5
Q

give 4 properties gases

A
  • the forces of attraction between the particles are very weak
  • the particles are free to move and are spread far apart
  • particles travel in straight lines
  • dont have a fixed shape or volume but will always fill containers
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6
Q

what does the sign “aq” mean

A

aqueous which means dissolved in water

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7
Q

a gas turning to a liquid is called

A

condensing

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8
Q

a liquid turning back into a solid is called

A

freezing

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9
Q

a solid turning into liquid is called

A

melting

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10
Q

a liquid turning into gas is called

A

boiling

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11
Q

the stronger the forces the more…

A

energy needed to break them and so the higher the melting and boiling points of the substance

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12
Q

if the temperature is below the melting point, whats its state

A

solid

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13
Q

if the temperature is above the boiling point, whats its state

A

gas

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14
Q

what are metals

A

giant structures of atoms, this means they contain lots of atoms bonded together

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15
Q

what happens to the electrons in the outer shell in metals

A

they are free to move around (delocalised)

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16
Q

between the positive metal ions and the negative electrons what kind of attraction is there

A

strong forces of electrostatic attraction

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17
Q

there are strong forces of attraction between the …

A

positive metal ions and the negative electrons these are known as metallic bonds

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18
Q

what does metallic bonding do

A

it holds the atoms together in a regular pattern

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19
Q

give 3 properties of metallic bonds

A
  • strong, so lots of energy needed to break them
  • have very high boiling and melting points
  • solids at room temp
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20
Q

what happens to the delocalised electrons in metals

A

they are free to move

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21
Q

metals are good conductors of …

A

heat and electricity

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22
Q

what happens to the layers in metals

A

they can slide over each other because of this metals can be bent or formed into different shapes

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23
Q

what is an alloy

A

a mixture of 2 or more metals or a metal and anther element

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24
Q

when you mix another element with a pure metal what happens to the layers

A

it causes the layers of the metal atoms to lose their shape because different elements have different sized atoms

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25
Q

metals are good conductors of …

A

heat and electricity

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26
Q

in a diamond each carbon atoms forms how many covalent bonds

A

4 covalent bonds- it makes diamond very hard

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27
Q

what type of melting point does diamond have

A

a high melting point as it takes a lot of energy to break the bonds

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28
Q

why does diamond not always conduct electricity

A

because it has no free electrons to move

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29
Q

graphite contains layers of what

A

carbon atoms arranged in hexagons

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30
Q

in graphite what does each carbon atom form

A

3 covalent bonds

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31
Q

why can the layers in graphite move over each other

A

because there are not any covalent bonds between the atoms, this makes graphite soft and slippery

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32
Q

what melting point does graphite have

A

a high melting point as lots of energy is needed to break the covalent bonds in the layers

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33
Q

in graphite what does each carbon atom have that is free to move

A

one free electron it is delocalised- so graphite conducts electricity and thermal energy

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34
Q

what is graphene

A

a sheet of carbon atoms joined together in hexagons- one layer of graphite

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35
Q

give 2 properties of Graphene

A
  • its covalent bonds make it very strong
  • it is very light
  • conducts electricty
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36
Q

what can graphene be added to other materials to make what

A

to make composites

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37
Q

what are fullerenes

A

molecules of carbon shaped like closed tubes o hallow balls

38
Q

what are fullerenes arranged in

A

mainly hexagons

39
Q

what can fullerenes form rings of

A

5 carbon atoms or rings of 7 carbon atoms

40
Q

what can fullerenes form

A
  • drugs

- nanotubes- tiny carbon cylinders

41
Q

what are small units in a polymer used to make

A

a large molecule

42
Q

how are all the atoms in a polymers joined by

A

covalent bonds

43
Q

what are the intermolecular forces like in polymers compared to them simple covalent molecules

A

larger- so more energy needed to break them

44
Q

what are polymers at room temp

A

solids

45
Q

what are intermolecular forces like in polymmers compared to ionic or covalent bonds

A

weaker- so have a lower melting and boiling point

46
Q

give 3 examples of giant covalent structures

A
  • diamond
  • graphite
  • graphene
47
Q

in giant covalent bonds, how are all the atoms bonded together

A

by strong covalent bonds

48
Q

give 2 things that are common about giant covalent structures

A
  • they all have high melting points as lots of energy is needed to break them
  • they don’t conduct electricity (except graphite)
49
Q

what are simple molecular substances made out of

A

molecules that contain a few atoms joined together by covalent bonds

50
Q

what are the forces of attraction like between the simple molecular substances

A

very weak

51
Q

simple molecular substances have low …

A

melting and boiling points

52
Q

what are most simple molecular substances at room temp

A

liquids or gases

53
Q

what is covalent bonding

A

when a non-metal and a metal atom bonds together and share a pair of electrons

54
Q

what type of electrostatic forces do covalent bonds have

A

very strong

55
Q

what are ionic compounds arranged in and what are they called

A

in patterns called giant ionic lattice

56
Q

what are there between oppositely charged ions

A

strong electrostatic forces of attraction

57
Q

give 3 properties of ionic compounds

A

-have high melting and boiling points
-when solid they don’t conduct electricity
when melted, the ions are free to move and conduct electricity

58
Q

what is ionic compounds

A

when a metal and a non-metal atom reacts together

59
Q

when metal atoms lose an electron what ion do they form

A

positively charged ions

60
Q

when non-metal atoms lose an electron what ion do they form

A

negatively charged ions

61
Q

what are ions

A

charged particles

62
Q

when are ions formed

A

when atoms lose or gain electrons

63
Q

solid to a liquid is called

A

melting

64
Q

liquid to a gas is called

A

boiling

65
Q

gas to a liquid is called

A

condensing

66
Q

liquid to a solid is called

A

freezing

67
Q

in diamond each carbon atom is forms how many covalent bonds

A

4

68
Q

why does diamond not conduct electricity

A

because it has no free electrons to move

69
Q

how many covalent bonds does graphite form

A

3

70
Q

what are fullerenes

A

molecules of carbon shaped like closed tubes or hallow balls

71
Q

give the name of the first fullerene delivered

A

buckministerfullerene

72
Q

how are fullerenes good

A
  • they have a huge surface area, so they could help to make great industrial catalysts
  • they make great lubricants
73
Q

how are fullerenes arranged

A

made of carbon atoms arranged in hexagons, pentagons and heptagons

74
Q

how can fullerenes be used to deliver drugs

A

because it is used to CAGE other molecules. The fullerene structure forms around another atom or molecule, which is then trapped inside

75
Q

solid to a liquid is called

A

melting

76
Q

liquid to a gas is called

A

boiling

77
Q

gas to a liquid is called

A

condensing

78
Q

liquid to a solid is called

A

freezing

79
Q

in diamond each carbon atom is forms how many covalent bonds

A

4

80
Q

why does diamond not conduct electricity

A

because it has no free electrons to move

81
Q

how many covalent bonds does graphite form

A

3

82
Q

what are fullerenes

A

molecules of carbon shaped like closed tubes or hallow balls

83
Q

give the name of the first fullerene delivered

A

buckministerfullerene

84
Q

how are fullerenes good

A
  • they have a huge surface area, so they could help to make great industrial catalysts
  • they make great lubricants
85
Q

how are fullerenes arranged

A

made of carbon atoms arranged in hexagons, pentagons and heptagons

86
Q

how can fullerenes be used to deliver drugs

A

because it is used to CAGE other molecules. The fullerene structure forms around another atom or molecule, which is then trapped inside

87
Q

give 3 properties of metallic bonds

A
  • strong, so lots of energy needed to break them
  • have very high boiling and melting points
  • solids at room temp
88
Q

what happens to the delocalised electrons in metals

A

they are free to move

89
Q

what happens to the layers in metals

A

they can slide over each other because of this metals can be bent or formed into different shapes

90
Q

what is an alloy

A

a mixture of 2 or more metals or a metal and anther element

91
Q

when you mix another element with a pure metal what happens to the layers

A

it causes the layers of the metal atoms to lose their shape because different elements have different sized atoms

gcse chemistry (15 decks)

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