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Chemistry AQA Triple > Bonding, Structure and the Properties of Matter > Flashcards

Bonding, Structure and the Properties of Matter Flashcards

Paper 1 - C2

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1
Q

What are the 3 states of matter?

A

Solid, Liquid and Gas

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2
Q

What are the features of solids and how are the particles arranged in solids?

A

-Solids are extremely hard to compress, this is because the particles in a solid are packed together in a regular pattern.
-Solids have a fixed shape and they cannot flow from place to place, this is because in a solid the particles can vibrate but they cannot move from place to place.

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3
Q

What are the features of liquids and how are the particles arranged in liquids?

A

-Liquids are extremely hard to compress, that is because the particles are close together with not many spaces between them.
-Liquids take the shape of their container and they can flow from place to place, this is because the particles in a liquid can move.

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4
Q

What are the features of gases and how are the particles arranged in gases?

A

-Gases are extremely easy to compress, that is because particles in gases are widely spaced.
-Gases spread out and fill the space of their container, that is because the particles in a gas move quickly and randomly.

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5
Q

How can we change states?

A

By putting in or taking out energy.

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6
Q

What happens when we heat a solid?

A

-It can change state to a liquid (Melting) and this takes place at the melting point.
-During the state change the particles in a liquid are moving around so they’ve got more kinetic energy than the particles in a solid.
-Which means that we have to put energy in to convert a solid into a liquid.
-This energy is needed to break the forces of attraction between the particles in a solid and once they are broken the particles can now move around.

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7
Q

Key Fact:

A

The stronger the forces of attraction between the particles the more energy we have to put in to break these forces and the higher the melting point.

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8
Q

What happens when we cool a liquid?

A

-It can change state from a liquid to a solid (Freezing), freezing takes place when we cool a liquid back down to its melting point.
-When a substance freezes the forces of attraction between the particles reform.

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9
Q

What happens when we heat a liquid?

A

-It will change state from a liquid into a gas (Boiling), boiling takes place at the boiling point.
-And if there are strong forces of attraction between the particles then the boiling point will be high.
-That is because it takes a lot of energy to break those strong forces of attraction and boil the liquid.

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10
Q

What happens when we cool a gas?

A

-It can change state from a gas into a liquid (Condensing), condensing takes place at the same temperature as boiling (boiling point).
-And when a substance condenses the forces of attraction between the particles reform.

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11
Q

Key Facts:

A

-Elements react in order to achieve a full outer energy level.
-By doing this, they achieve the stable electronic structure of a noble gas.

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12
Q

What happens when a Group 1 metal and a Group 7 non-metal react?

A

Ionic bonding takes place, Group 1 metals lose one electron forming one positive ion, Group 7 non-metals gain one electron forming one negative ion, now both ions have a full outer shell.

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13
Q

What happens when a Group 2 metal and a Group 6 non-metal react?

A

Ionic bonding takes place, Group 2 metals lose two electron forming a 2+ positive ion, Group 6 non-metals gain two electron forming 2- negative ion, now both ions have a full outer shell.

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14
Q

What do ionic compounds form?

A

They form Giant structures called a giant ionic lattice and they are three dimensional structures.

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15
Q

What is in a giant ionic lattice?

A

-In a giant ionic lattice, every positive ion is surrounded by negative ions and every negative ion is surrounded by positive ions.
-There are also strong forces of attraction between the positive and negative ions called electrostatic forces of attraction and are also called ionic bonds.
-These forces hold the positive and negative ions in place.

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16
Q

What directions do ionic bonds act in?

A

All directions

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17
Q

What are the properties of Ionic Compounds?

A

-Ionic compounds have very high melting and boiling points. That is because the strong electrostatic forces of attraction require a great deal of heat energy to break.
-They cannot conduct electricity when they are solids because the ions are locked in place by the strong electrostatic forces of attraction.
-But they can conduct electricity when they are melted or dissolved in water because the ions can now move and carry the electrical charge.

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18
Q

What happens when we heat an ionic solid?

A

The particles vibrate and when the particles vibrate with enough energy the electrostatic forces of attraction break and the solid melts. It also takes a great deal of heat energy for these to break as the electrostatic forces between the ions are very strong.

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19
Q

What is covalent bonding?

A

When non-metal atoms bond together and is a strong bond.

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20
Q

How can we show covalent bonding?

A

Dot and Cross diagrams or Stick diagrams

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21
Q

What are the properties of small covalent molecules?

A

-They have a low melting and boiling point and this means that they are usually gases or liquids at room temperature.
-They do not conduct electricity as they do not have an overall electric charge.

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22
Q

Why do small covalent molecules have a low melting and boiling point?

A

-The atoms in each molecules are held together by strong covalent bonds.
-Secondly there are very weak intermolecular forces between one molecule and another.
-As we increase the temperature the vibration of the molecules increases and at a certain point it will break the weak intermolecular forces holding the molecules to each other.
-At this point the molecules turn to a gas (boil) and the bonds do not take a great deal of energy to break because of the weak intermolecular forces.

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23
Q

Why are Giant covalent substances are always solid at room temperature?

A

Because all giant covalent substances have high melting and boiling points as they have millions of strong covalent bonds and it takes a great deal of energy to break all of the bonds.

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24
Q

What is diamond formed by?

A

Carbon

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25
Q

What does diamond consist of?

A

Huge number of carbon atoms joined by covalent bonds which makes diamond an extremely hard substance.

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26
Q

Why does it take a great deal of energy to melt diamond?

A

We need to break the huge number of covalent bonds in the diamond which makes diamond have a very high melting and boiling point.

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27
Q

Why can diamond not conduct electricity?

A

All of the outer electrons are in covalent bonds which means that diamond has no free electrons to carry electrical charge

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28
Q

What is Silicon dioxide formed out of?

A

Silicon and oxygen covalently bonded together

29
Q

Why does Silicon dioxide have a high melting and boiling point?

A

Because silicon dioxide has a huge number of strong covalent bonds.

30
Q

What is Graphite formed by?

A

Carbon, and each carbon atom forms covalent bonds to three other carbon atoms and the carbon atoms form hexagonal rings (six carbon atoms) and are arranged into layers.

31
Q

What are the properties of graphite?

A

-Soft and Slippery
-Very high melting and boiling point
-Good conductor of electricity and heat

32
Q

Why is Graphite soft and slippery?

A

There are no covalent bonds between the layers which means the layers can slide over each other.

33
Q

What is graphite used in?

A

Lubricant in machines reducing friction between the moving parts.

34
Q

Why does graphite have a very high melting and boiling point?

A

If we want to melt graphite we need to break the covalent bonds which takes a great deal of energy.

35
Q

Why is graphite a good conductor of electricity and heat?

A

There are delocalised electrons in the graphite can move which means they can conduct both electricity and heat because each carbon atom has one electron in its outer shell which is not affected by the covalent bonds.

36
Q

What is Graphene?

A

A single layer of graphite and is one atom thick.

37
Q

What are the properties of Graphene?

A

-Excellent conductor of electricity because it has delocalised electrons.
-Extremely strong

38
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes and have hexagonal rings of carbon atoms.

39
Q

How many carbon atoms does Buckminsterfullerene have?

A

60 (C₆₀)

40
Q

What are the uses of fullerenes?

A

-Pharmaceutical delivery
-Lubricants
-Catalysts

41
Q

What are the properties of Carbon Nanotubes?

A

-Have high tensile strength (can be stretched without breaking)
-Excellent conductors of heat and electricity

42
Q

What are the uses of Carbon Nanotubes?

A

Used to reinforce materials e.g. In tennis rackets

43
Q

What is a polymer made up of?

A

Polymers are made by joining together thousands of small, identical molecules (monomers).

44
Q

What are the properties of Polymers?

A

-Most polymers are solids at room temperature. That is because the intermolecular forces of attraction between the polymer molecules are relatively strong.
-High melting and boiling point.

45
Q

Why does it take a lot of energy to break down the intermolecular forces between polymer molecules?

A

Because the intermolecular forces are relatively strong.

46
Q

What do metals consist of?

A

Giant structure of atoms arranged in regular layers and the electrons in the outer energy level of each atom are delocalised.

47
Q

What is metallic bonding?

A

A strong electrostatic attraction between the sea of delocalised negative electrons and the positive metal ions. Metallic bonds are strong as well as they are in metals.

48
Q

What are the properties of metals?

A

-High melting and boiling point
-Excellent conductors of heat and electricity
-Can be bent and shaped

49
Q

Why do metals have a high melting and boiling point?

A

Because a great deal of energy is required to break the strong metallic bonds.

50
Q

Why are metals excellent conductors of heat and electricity?

A

Because the delocalised electrons can move and because electrons are charged these moving electrons can carry an electric current and thermal energy which allows metals to conduct heat.

51
Q

Why can metals be bent and shaped?

A

In metals, the layers of atoms are able to slide over each other.

52
Q

What is an alloy?

A

Mixture of metals

53
Q

Why are alloys harder than pure metals?

A

The different sizes of atoms distorts the layers, making it more difficult for them to slide over each other meaning alloys are harder than pure metals.

54
Q

(Triple only) What is the size of a micrometre?

A

0.001mm or 1 x 10^-6m

55
Q

(Triple only) What is the size of a nanometre?

A

0.000000001mm or 10^-9m

56
Q

(Triple only) What is a Coarse Particle and what is its diameter?

A

Coarse particles contain many thousands of atoms and have a diameter of between 1 x 10^-5m and 2.5 x 10^6m.

57
Q

(Triple only) What is a Fine Particle and what is its diameter?

A

Fine particles contain several thousand atoms and have a diameter of between 100 - 2500 nanometres (1 x 10^-7m and 2.5 x 10^-6).

58
Q

(Triple only) What is a Nano Particle and what is its diameter?

A

Nanoparticles only contain a few hundred atom and have a diameter between 1 - 100 nanometres.

59
Q

(Triple only) Key fact on Nanoparticles:

A

As the particle size decreases by ten times, the surface area : volume ration increases by ten times.

60
Q

(Triple only) What is the size of the surface are to volume ratio for nanoparticles? And why do we need a much smaller quantity of nanoparticles compared to martials with normal particle size?

A

Huge, and even a small amount of nanoparticles has a massive surface area which means we need a much smaller quantity of nanoparticles compared to materials with normal particle size. E.g. a catalyst

61
Q

(Triple only) What are the uses of nanoparticles?

A

-Medicines
-Sun creams
-Cosmetics
-Deodorants
-Electronics
-Catalysts

62
Q

(Triple only) What are the risks of nanoparticles

A

-It’s possible that nanoparticles can be absorbed into the body and enter our cells.
-No-one knows the potential long term effects of this
-So its important that nanoparticles are studied and used carefully.

63
Q

What is a problem with dot and cross diagrams?

A

It does not tell us about the shape of the molecule.

64
Q

What are the problems with stick diagrams?

A

-Because a covalent bond is shown as a stick we cannot
tell which electron in the bond came from which atom.
-Also stick diagrams give us no idea of outer electrons that are not in bonds.
-And the 2 dimensional stick diagrams do not give us accurate information on the shape of the molecule.

65
Q

Why is the benefit to use a 3 dimensional sick diagram?

A

It shows us the shape of the molecule

66
Q

What is the benefit of a ball and stick diagram?

A

It allows us to clearly see the ions in 3 dimensions

67
Q

What is the problem of the ball and stick diagram?

A

It shows the ions as widely spread when in reality the ions are packed together

68
Q

Why is sometimes better to use a space filling diagram than a ball and stick diagram?

A

-Because space filling diagrams give us a better idea of how closely packed the ions are.
-However, it can be difficult to see the three dimensional packing with a space filling diagram.

69
Q

What is the problem of the space filling diagram and the ball and stick diagram?

A

They only show a tiny part of the giant crystal lattice so both these diagrams give a mistaken impression about the sizes of these structures.

Chemistry AQA Triple (17 decks)

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