Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

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

Bonding, Structure And Properties Of Matter Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What are the particles of solids like?

A
  • Regular arrangement
  • Very close together
  • Vibrate about fixed positions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the particles of liquids like?

A
  • Random arrangement
  • Close together
  • Flow around each other
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the particles of gases like?

A
  • Random arrangement
  • Far apart
  • Move very quickly, in different directions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

When a particle changes state:

A
  • Particles themselves stay the same
  • The way the particles are arranged changes
  • The way the particles move changes
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What does a pure substance always have?

A

A melting and boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What does the amount of energy required for a substance to change state depends on?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

The stronger the forces of attraction in a substance…

A
  • The greater the amount of energy needed to overcome them.

- The higher the melting and boiling points will be.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Which substances have a high melting point due to strong bonds?

A

Ionic compounds, metals and giant covalent structures.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are the limitations of the particle model?

A

Does not take into account:

1) Forces between particles
2) The volume of the particles
3) Space between particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the 3 types of chemical bonds?

A
  • Ionic
  • Covalent
  • Metallic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are ions?

A

Atoms that have lost or gained electrons. Losing and gaining electrons gives them an overall charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What do ionic bonds occur between?

A

Positive and negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Why are ions stable?

A

The have a complete outer shell of electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What happens when a metal atom reacts with a non metal atom?

A

Electrons in the outer shell of the metal atoms are transferred.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What happens when metal atoms lose electrons?

A

They become positively charged ions and non metal gain electrons to become negative ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Which groups form ions most readily?

A

Groups 1,2,6,7 because they have one or are missing 1 electron in their outer shell.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What sort of diagram is used to show ionic bonds?

A

Dot and cross diagrams.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is an ionic bond?

A

The attraction between oppositely charge ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

How are ionic compounds held together?

A

By strong forces of attraction (electrostatic forces) that act in all directions between oppositely charged ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What are the properties of ionic compounds?

A
  • High melting and boiling points (strong forces of attraction)
  • Do not conduct electricity when solid because ions can’t move
  • Conduct electricity when molten or in a solution because charged ions are free to move around and carry charge
  • Regular lattice structure
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What are lattices?

A

When oppositely charge ions are attracted, it gets bigger and bigger- held together by electrostatic forces.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How do you work out the empirical formula?

e.g. work out the empirical formula of potassium oxide

A
  • Potassium is in group 1 so it forms 1+ ions
  • Oxygen is in group 6 so it forms 2- ions

A potassium ions only has 1+ charge so you’ll need two of them to balance out the 2- charge. The empirical formula = K2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What does metallic bonding occur in?

A
  • Metallic elements e.g. iron and copper

- Alloys e.g. stainless steel

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What sort of structure do metals have?

A

A giant structure in which electrons in the outer shells are delocalised (not bound to one atom). This produces a regular arrangement (lattice) of positive ions held together by electrostatic attraction to the delocalised electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What is a metallic bond?

A

The attraction between positive ions and the delocalised negatively charge ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What are the properties of metallic bonds?

A
  • Very strong and most metals have high melting and boiling points- they are useful structural materials.
  • Thermal and electrical conductors because they have delocalised electrons.
  • Particles in pure metals have a regular arrangement- layers can slide over each other quite easily, which mean they can be bent and shaped.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Why is copper traditionally used to make water pipes?

A
  • It is unreactive so it does not react with water.

- It can easily be shaped.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is aluminium used for?

A
  • High voltage power cables
  • Furniture
  • Drink cans
  • Foil food wraps
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What are the properties of aluminium?

A
  • Corrosion resistant
  • Ductile
  • Malleable
  • Good conductivity
  • Low density
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What are the uses of copper?

A
  • Electrical wiring
  • Water pipes
  • Saucepans
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What are the properties of copper?

A
  • Ductile
  • Malleable
  • Good conductivity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What are the uses of gold?

A
  • Jewellery

- Electrical junctions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What are the properties of gold?

A
  • Ductile
  • Shiny
  • Good conductivity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What are alloys and how are they different to pure metals?

A

In pure metals, atoms are arranged in layers, which allows metals to be bent and shaped. Pure metals are too soft for many uses and so are mixed with other metals to make alloys which are harder.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What is steel?

A

An alloy made from iron

36
Q

How can iron oxide be reduced?

A

In a blast furnace to produce iron. Molten iron obtained from a blast furnace contains roughly 96% iron and 4% impurities including carbon, phosphorous and silica.

37
Q

Why does iron have limited uses?

A

It is impure and very brittle

38
Q

Why is iron too soft for many practical uses?

A

The atoms in pure irons are arranged in layers that can slide over each other making it soft and malleable- therefore it is too soft for many practical uses.

39
Q

How can iron’s properties be changed?

A

By mixing it with small quantities of carbon or other metals to make steel.

40
Q

What are alloys developed to have?

A

The required properties for a specific purpose.

41
Q

What determines the properties of steel?

A

The amount of carbon and/ or other metals.

42
Q

What is steel with a high carbon content like?

A

Hard and strong

43
Q

What is steel with a low carbon content like?

A

Soft and easily shaped

44
Q

What does stainless steel contain?

A

Chromium and nickel and is hard and resistant to corrosion.

45
Q

How are pure copper, gold and aluminium made into alloys?

A

They are too soft for many uses, they are mixed with similar metals to make them harder for everyday uses e.g. coins.

46
Q

What does the carat system show?

A

The amount of gold in an alloy.

24 carat gold= 100% gold
18 carat gold= 18/24 x 100= 75% gold

47
Q

What do aluminium alloys combine?

A

Low density with high strength so are used to make aeroplanes.

48
Q

What are the uses of bronze and what sort of alloy is it?

A
  • Alloy of copper and tin

- Bright gold colour and is used to make statues and decorative objects.

49
Q

What are the uses of brass and what sort of alloy is it?

A
  • Alloy of copper and zinc
  • Very hardwearing and resistant to corrosion
  • Used to make taps and door fittings
50
Q

What is a covalent bond?

A

A shared pair of electrons between non-metals or compounds of non-metal atoms to gain a full outershell of electrons.

51
Q

What is the strength of a covalent bond like?

A

Very strong

52
Q

What sort of diagrams can be used to show covalent bonds?

A

Dot and cross diagrams

53
Q

What do simple molecule contain?

A

A relatively small amount of non-metal atoms joined together by covalent bonds.

54
Q

Why can’t simple molecules conduct electricity?

A

They have no overall charge.

55
Q

What are substances that consist of simple molecules usually?

A

Liquids and gases that have relatively low boiling points because they have weak intermolecular forces which can be easily overcome.

56
Q

What are the intermolecular forces of simple molecules like?

A

They are very weak compared to the strength of the covalent bonds in the molecules themselves.

57
Q

Why do larger molecules have a higher melting and boiling points?

A

The larger the molecules are, the stronger the intermolecular forces between the molecules become. Going down group 7 of the periodic table, the molecules get larger and their melting and boiling points increase.

58
Q

What are the states of fluorine and chlorine like at room temperature?

A

Gases

59
Q

What is the state of bromine at room temperature?

A

Liquid

60
Q

What is the state of iodine at room temperature?

A

Solid

61
Q

What are all the atoms in covalent structures linked by?

A

Strong covalent bonds. These bonds must be broken for the substance to melt or boil. This means that giant covalent study urges are solids with very high melting and boiling points.

62
Q

What is the structure if silicon dioxide or silica (SiO2) like?

A

Has a structure similar to diamonds- each oxygen atoms is joined to 2 silicon atoms. Each silicon atom is joined to 4 oxygen atoms.

63
Q

What is graphene?

A

A singular layer of graphite.

64
Q

How are atoms arranged in graphene?

A

In a hexagonal structure, just one atom thick.

65
Q

What are the properties of graphene?

A
  • Very strong
  • Good thermal and electrical conductor
  • Nearly transparent
66
Q

What do the properties of graphene make it useful in?

A

Electronics and composite materials

67
Q

What are fullerenes?

A

A form of carbon which contains different numbers of carbon atoms.

68
Q

What is the structure of fullerenes based on?

A

Hexagonal rings of carbon atoms. Sometimes these rings contain 5 or 7 carbon atoms.

69
Q

What are the different shapes that fullerene molecules often have?

A

They have hollow shapes including tubes, balls and cages.

70
Q

What is buckminster fullerene (C60)?

A

The first fullerene to be discovered:

  • Consists of 60 carbon atoms
  • The atoms are joined together in a series of hexagons and pentagons
  • The most symmetrical and, therefore, most stable fullerene
71
Q

What are carbon nanotubes?

A

Cylindrical fullerenes with very high length to diameter ratios.

72
Q

What do the properties of carbon nanotubes make them very useful for?

A

Use in nanotechnology, electrons and materials.

73
Q

What are some of the uses of fullerenes?

A
  • Deliver drugs in the body
  • In lubricants
  • As catalysts
  • For reinforcing materials e.g. the frames of tennis rackets, so they are strong but still lightweight
74
Q

What do polymers consist of?

A

Very large molecules

75
Q

What are plastics?

A

Synthetic (man-made) polymers.

76
Q

What are the atoms within the polymer molecules held together by?

A

Strong covalent bonds

77
Q

What are the intermolecular forces between the large polymer molecules like?

A

Quite strong so polymers are solid as room temperature.

78
Q

When is polyethene produced?

A

Commonly know as polythene is produced when lots of ethene molecules are joined together in an addition polymerisation reaction. It is cheap, strong and used to make plastic bags and bottles.

79
Q

What is nanoscience?

A

The study of these very small structures

80
Q

What is the surface area to volume ratio of small particles like?

A

High- changing the size of particles has a dramatic effect on this ratio. For example if the length of side of cube decrease by a factor of 10:

  • SA decreases by 10x10= 100
  • Volume decreases by 10x10x10= 1000
  • SA to volume ratio increased tenfold
81
Q

Why is surface area important for catalysts?

A

Having a large surface area improves their effectiveness.

82
Q

How many atoms do nanoparticles contain?

A

Only a few hundred atoms.

83
Q

How are nanostructures formed?

A

When nanoparticles combine to form nanostructures, which can be manipulated so material can be developed that have new and specific properties.

84
Q

What are the properties of nanoparticles?

A

The properties of nanoparticles are different to the properties of the same materials in bulk e.g. nanoparticles are more sensitive to light, heat and magnetism.

85
Q

Why are nanoparticles used in sun creams?

A

They provide better skin coverage and, therefore, more effective protection from the sun is harmful ultraviolet rays.

86
Q

What concerns are there about nanoparticles?

A

Concerns remain that these particles are so small they could get into and damage human cells and cause problems in the environment.

87
Q

What Is research into nano particles leading to the development of?

A
  • New drug delivery systems
  • Synthetic skin for burns victims
  • Computers and technology
  • Catalysts for fuel cells
  • Stronger and lighter construction materials
  • Cosmetic and deodorants
  • Fabrics that prevent growth of bacteria

Chemistry Paper 1 (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions