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Chemistry Paper 1 > Topic 2 Bonding, Structure And Properties Of Matter > Flashcards

Topic 2 Bonding, Structure And Properties Of Matter Flashcards

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1
Q

What does ionic bonding occur between?

A

Metals and non-metals

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2
Q

What does covalent bonding occur between?

A

Non-metals

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3
Q

Where does metallic bonding occur?

A

In metallic elements and alloys

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4
Q

What are the electrostatic forces of attraction between in an ionic compound?

A

Oppositely charged ions

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5
Q

What is an ionic compound?

A

Giant structure of ions

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6
Q

What arrangement do the ions form in an ionic compound?

A

Regular lattice

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7
Q

What is the structure of an ionic compound called?

A

Giant ionic lattice

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8
Q

What are the 2 properties of ionic compounds?

A
  • High melting and boiling points
  • can conduct electricity when melted/dissolved in water
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9
Q

Why can ionic compounds conduct electricity when melted or dissolved in water?

A

Ions free to move - can carry charge/charge can flow

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10
Q

Why are covalent bonds strong?

A

positively charged nuclei of the bonded atoms are attracted to shaired pair of electrons by electrostatic forces

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11
Q

How does the displayed formula represent covalent bonds?

A

as single lines between atoms

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12
Q

What is a simple molecular substance?

A

made up of molecules containing a few atoms joined by covalent bonds

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13
Q

What is the formula for ammonia?

A

NH3

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14
Q

What are 8 examples of simple molecular substances?

A
  • hydrogen
  • chlorine
  • oxygen
  • nitrogen
  • methane
  • water
  • hydrogen chloride
  • ammonia
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15
Q

What are 3 ways covalent bonds can be represented?

A
  • dot and cross diagrams
  • displayed formula
  • 3D model
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16
Q

What are the atoms within molecules in simple molecular substances held together by?

A

very strong covalent bonds

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17
Q

What are the forces of attraction between molecules in simple molecular substances?

A

intermolecular forces

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18
Q

What forces are overcome when a simple molecular substance is melted or boiled?

A

intermolecular forces

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19
Q

Why do simple molecular substances have low melting and boiling points?

A

weak intermolecular forces are easily overcome

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20
Q

What state are simple molecular substances usually in at room temperature?

A

gases or liquids

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21
Q

Why do molecular compounds not conduct electricity?

A

not charged so there are no free electrons or ions

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22
Q

Why do larger molecules have higher melting and boiling points?

A

as molecules get bigger, the strength of intermolecular forces increases

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23
Q

What are 3 bulk properties of simple molecular substances?

A
  • usually gases/liquids at room temp
  • don’t conduct electricity
  • low melting and boiling points
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24
Q

What are polymers?

A

long chains of repeating units

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25
Q

What are the atoms in polymer molecules joined by?

A

strong covalent bonds

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26
Q

Why are most polymers solids at room temp?

A

larger intermolecular forces between polymer molecules than between simple covalent molecules so more energy needed to break them

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27
Q

What are all the atoms in giant covalent structures bonded together by?

A

strong covalent bonds

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28
Q

Why do giant covalent structures have very high melting and boiling points?

A

lots of energy needed to break strong covalent bonds

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29
Q

What are 3 examples of giant covalent structures?

A
  • diamond
  • graphite
  • silicon dioxide
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30
Q

In diamond, how many covalent bonds does each carbon atom form?

A

4 covalent bonds

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31
Q

What are 3 properties of diamond?

A
  • very hard
  • very high melting point
  • doesn’t conduct electricity
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32
Q

Why is diamond very hard?

A

carbon atoms each form 4 covalent bonds

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33
Q

Why does diamond not conduct electricity?

A

no free electrons or ions

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34
Q

Why does diamond have a very high melting point?

A

strong covalent bonds take a lot of energy to break

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35
Q

In graphite, how many covalent bonds does each carbon atom form?

A

3 covalent bonds

36
Q

In graphite, what do the 3 covalent bonds each carbon atom forms, create?

A

layers of carbon atoms arranged in hexagons

37
Q

Why can the layers in graphite move over each other?

A

no covalent bonds between layers - held together weakly

38
Q

Why is graphite a good lubricating material?

A

its soft and slippery (layers can slide over eachother)

39
Q

Why has graphite got a high melting point?

A

covalent bonds in layers need lots of energy to break

40
Q

In graphite, why does each carbon atom have one delocalised electron?

A

only 3 out of carbons 4 outer electrons are used in bonds

41
Q

Why does graphite conduct electricity and thermal energy?

A

each carbon atom has one delocalised electron that can move and carry charge

42
Q

What property of graphene makes it useful in electronics?

A

Contains delocalised electrons- can conduct electricity through whole structure

43
Q

What property of graphene makes it useful to add to composite materials?

A

Strong covalent bonds - very strong but also light

44
Q

What are fullerenes?

A

Molecules of carbon with hollow shapes

45
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene

46
Q

What shape does Buckminsterfullerene have?

A

Hollow sphere

47
Q

What is the molecular formula of Buckminsterfullerene?

A

C(60)

48
Q

What is the structure of fullerenes?

A

Mainly made up of hexagonal rings of carbon atoms but can also contain pentagons and heptagons

49
Q

Why are fullerenes useful in delivering drugs into the human body?

A

Fullerenes can ’cage’ other molecules

50
Q

Why do fullerenes make great industrial catalysts?

A

huge surface area- Individual catalyst molecules can be attached

51
Q

What are 3 examples of uses of fullerenes?

A
  • deliver drugs into the body
  • make lubricants
  • make industrial catalysts
52
Q

What are carbon nanotubes?

A

Tiny carbon cylinders (fullerenes)

53
Q

What are 4 properties of carbon nanotubes?

A
  • very high length to diameter ratio
  • conduct electricity
  • conduct heat
  • high tensile strength (don’t break when stretched)
54
Q

What is nanotechnology?

A

Technology that uses very small particles such as nanotubes

55
Q

What are 3 examples of uses of nanotubes?

A
  • in nanotechnology
  • in electronics
  • to strengthen materials (eg tennis rackets)
56
Q

Why are nanotubes useful in strengthening materials?

A

Don’t add much weight

57
Q

What do metals consist of?

A

Giant structures of atoms arranged in a regular pattern

58
Q

Which electrons are delocalised and free to move around in metals?

A

Outer shell electrons of the metal atoms

59
Q

What is metallic bonding?

A

Strong electrostatic attraction between sea of negative delocalised electrons and positive metal ions

60
Q

What holds the atoms of a metal together in a regular structure?

A

Electrostatic forces of attraction

61
Q

Are metallic bonds strong or weak?

A

Very strong

62
Q

What are 2 substances that are held together by metallic bonding?

A

metallic elements and alloys

63
Q

Why are most metals solid at room temperature?

A

Have high melting and boiling points

64
Q

What do most metals have high melting and boiling points?

A

Strong metallic bonds- lots of energy to be broken

65
Q

Why are metals good conductors of electricity?

A

Delocalised electrons carry charge through whole structure

66
Q

Why are metals good conductors of thermal energy (heat)?

A

Energy transferred by delocalised electrons

67
Q

Why are most metals malleable?

A

Layers of atoms can slide over each other- metals can be bent or shaped

68
Q

Why are pure metals mixed with other metals?

A

Too soft for many uses so mixed with other metals to make alloys which are harder

69
Q

What are alloys?

A

Mixture of two or more metals or a metal and another element

70
Q

Why are alloys harder than pure metals?

A
  • different elements have different sized atoms
  • new metal atoms distort layers of metal atoms- harder for layers to slide over each other
71
Q

What are the 2 limitations of the particle theory model?

A
  • there are no forces shown (no way of knowing their strength)
  • particles represented as solid inelastic spheres (instead of atoms, ions or molecules)
72
Q

What are the categories particles are put in based on?

A

Their diameter

73
Q

What are the diameters of nanoparticles?

A

1-100nm

74
Q

What is nanoscience?

A

area of science that investigates uses and properties of nanoparticles

75
Q

What are the diameters of fine particles?

A

100-2500nm

76
Q

What are the diameters of coarse particles?

A

2500-10000nm

77
Q

What are coarse particles also referred to as?

A

Dust

78
Q

What is the main property of nanoparticles?

A

Large surface area to volume ratio

79
Q

What happens to the surface area as particles decrease in size?

A

Surface area increases in relation to their volume- surface area to volume ratio increases

80
Q

What is the equation to find the surface area to volume ratio?

A

Surface area to volume ratio = surface area/volume

81
Q

What is the rule for surface area to volume ratio as particles decrease in size?

A

As the side of a cube is decreased by factor of 10, surface area to volume ratio increases by factor of 10

82
Q

What causes the properties of a material to be different if it’s a nanoparticle rather than in bulk?

A

Nanoparticles have a high surface area to volume ratio

83
Q

Why are smaller quantities of a material made up of nanoparticles needed to work as an effective catalyst than for materials made up of ‘normal’ sized particles?

A

Nanoparticles have a high surface area to volume ratio

84
Q

What are 6 applications of nanoparticles?

A
  • as catalysts
  • in medicine
  • in electronics
  • in cosmetics
  • in sun creams
  • in deodorants
85
Q

What is a disadvantage of nanoparticles?

A

Effects of nanoparticles on human health isn’t fully understood

Chemistry Paper 1 (6 decks)

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