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Chemistry > 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 is the nature of ions in ionic bonding?

A

Ions are oppositely charged

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2
Q

What is covalent bonding?

A

Atoms share pairs of electrons

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3
Q

What is metallic bonding?

A

Atoms which share delocalised electrons

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4
Q

What does ionic bonding occur between?

A

Metals combined with non-metals

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5
Q

Where does covalent bonding occur?

A

Non-metal elements

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6
Q

Where does metallic bonding occur?

A

Metallic elements and alloys

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7
Q

Explain what happens in ionic bonding [4]

A
  1. A metal atom reacts with a non-metal atom
  2. Electrons in the outer shell of the metal are transferred
  3. Metal atoms lose electrons to become positively charged ions
  4. Non-metal atoms gain electrons to become negatively charged ions
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8
Q

What is the diagram called for ionic bonding?

A

Dot and cross diagrams

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9
Q

What is the name of the structure for ionic compounds?

A

Giant ionic lattice

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10
Q

What hold the ions together in a giant ionic lattice?

A

Strong electrostatic forces of attraction

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11
Q

Why do ionic compounds have high melting and boiling points? [2]

A
  1. Numerous strong ionic bonds
  2. Large amount of energy is needed to break them apart
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12
Q

Why can ionic compounds conduct electricity when liquid? [2]

A
  1. Ions are free to move
  2. Can carry an electrical charge
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13
Q

Why can’t ionic compounds conduct electricity when solid? [2]

A
  1. Ions are held in place
  2. So can’t carry an electrical charge
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14
Q

Why are ionic compounds brittle?

A

When they are broken apart, opposite charges in the lattice repel each other and break the lattice

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15
Q

Why are the limitations of using a 3D model to show an ionic compound?

A

Only shows the outer layer of the compound

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16
Q

Why are the limitations of using a ball and stick model to show an ionic compound? [2]

A
  1. Relative sizes of the ions not shown
  2. No gaps between ions irl
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17
Q

Why are the limitations of using a dot and cross diagram to show an ionic compound?

A

Doesn’t show the structure of the compound

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18
Q

Why are the limitations of using a dot and cross diagram to show covalent bonding?

A

Don’t show the relative sizes of the atoms

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19
Q

Why are the limitations of using a displayed formula to show covalent bonding?

A

Don’t show the 3D structure of the molecule

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20
Q

Why are the limitations of using a 3D model to show covalent bonding?

A

Don’t show where the electrons have come from

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21
Q

Why do simple molecules have low melting and boiling points? [2]

A
  1. The covalent bonds are not broken
  2. However, the forces holding neighbouring particles together are weak and easily overcome
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22
Q

Why don’t simple molecules conduct electricity?

A

They are not charged, so there are no free electrons or ions

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23
Q

What kind of structure is diamond, graphite and silicon dioxide?

A

Giant covalent structures

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24
Q

Why does diamond have a high meting and boiling point? [2]

A
  1. Strong covalent bonds
  2. Much energy needed to break them
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25
Q

Why can’t diamond conduct electricity? [2]

A
  1. Doesn’t contain charged particles
  2. So can’t carry an electrical charge
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26
Q

How many bonds does diamond make per carbon?

A

4

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27
Q

Why does graphite have a high melting and boiling point? [2]

A
  1. Strong covalent bonds
  2. Much energy needed to break them
28
Q

Why can graphite conduct electricity? [2]

A
  1. Delocalised electrons between layers
  2. Can carry an electrical charge
29
Q

Why is graphite soft?

A

Only weak intermolecular forces betwee layers which slide

30
Q

How many bonds does graphite make per carbon?

A

3

31
Q

What is graphene?

A

One layer of graphite

32
Q

Why can graphene conduct electricity? [2]

A
  1. Contains delocalised electrons
  2. So can carry an electrical charge
33
Q

Uses of graphene? [2]

A
  1. Composite materials (add strength without added weight)
  2. Electronics
34
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes

35
Q

What is the structure of fullerenes based on?

A

Hexagonal rings of carbon atoms

36
Q

What is the formula for Buckminsterfullerene?

A

C₆₀

37
Q

Explain how fullerenes can be used to deliver drugs into the body [2]

A
  1. Fullerenes can ‘cage’ other molecules
  2. Fullerene structure forms around another atom or molecule, which is then trapped inside
38
Q

Why can fullerenes make industrial catalysts?

A

Have a large surface area

39
Q

What are nanotubes?

A

Tiny carbon cylinders

40
Q

What are the useful properties of nanotubes? [3]

A
  1. Length:diameter very high
  2. Can conduct electricity and heat
  3. High tensile strength
41
Q

Uses of nanotubes? [2]

A
  1. Electronics
  2. Strengthen materials without adding weight (tennis racket frames)
42
Q

Why do giant metallic structures have high melting and boiling points? [2]

A
  1. Strong metallic bonds
  2. Much energy needed to break them
43
Q

Why can giant metallic structures conduct electricity? [2]

A
  1. Sea of delocalised electrons
  2. Can carry an electrical charge
44
Q

Why are giant metallic structures malleable?

A

Layers can slide over each other

45
Q

Why are alloys used instead of pure metals?

A

They are harder

46
Q

Why are alloys stronger than pure metals? [4]

A
  1. An alloy is a mixture of two or more metals
  2. Different elements have different sized atoms
  3. Therefore, the layers are distorted making it more difficult for them to slide over each other
  4. This makes alloys harder than pure metals
47
Q

What is an alloy?

A

A mixture of two or more metals or a metal and another element

48
Q

What 3 things does the strength of forces in solids, liquids and gases depend on?

A
  1. Material
  2. Temperature
  3. Pressure
49
Q

Describe the structure of a solid
i) forces of attraction
ii) volume and shape
iii) movement

A

i) Strong forces of attraction between particles, which holds them together in fixed positions to form a regular lattice shape
ii) Particles don’t move from their positions, so keep a definite shape and volume
iii) Particles vibrate about their positions

50
Q

Describe the structure of a liquid
i) forces of attraction
ii) volume and shape
iii) movement

A

i) Weak forces of attraction between particles, free to move past each other but stay quite close together
ii) Have a definite volume but don’t keep a definite shape
iii) Particles contantly moving with random motion

51
Q

Describe the structure of a gas
i) forces of attraction
ii) volume and shape
iii) movement

A

i) Very weak forces of attraction between particles, free to move and are far apart
ii) Don’t keep a definite shape or volume
iii) Particles constantly moving with random motion

52
Q

What are the limitations of the particle theory? [2]

A
  1. Doesn’t show forces
  2. Particles are represented as solid spheres
53
Q

Explain why a solid melts [4]

A
  1. When a solid is heated, its particles gain more energy
  2. This makes the particles vibrate more, which weakens the forces that hold the solid together
  3. At a certain temperature, the particles have enough energy to break free from their positions
  4. This is called melting
54
Q

Explain why a liquid boils [4]

A
  1. When a liquid is heated, the particles gain even more energy
  2. This energy makes the particles move faster, which weakens and breaks bonds holding the liquid together
  3. At a certain temperature, the particles have enough energy to break their bonds
  4. This is boiling
55
Q

Explain why a gas condenses [4]

A
  1. As a gas cools, the particles no longer have enough energy to overcome the forces of attraction between them
  2. Bonds form between the particles
  3. At a certain temperature, so many bonds have formed that the gas becomes a liquid
  4. This is condensing
56
Q

Explain why a liquid freezes [4]

A
  1. When a liquid cools, the particles have less energy so move around less
  2. There’s not enough energy to overcome the attraction between the particles, so more bonds form between them
  3. At a certain temperature, so many bonds have formed that they’re helf in place
  4. This is freezing
57
Q

What is the diameter of coarse particles?

A

2500 nm to 10 000 nm

58
Q

What is the every day name for coarse particles?

A

Dust

59
Q

What is the diameter of fine particles?

A

100 nm and 2500 nm

60
Q

What is the diameter of nanoparticles?

A

1 nm and 100 nm

61
Q

How would you calaculate surface area to volume ratio?

A

surface area / volume

62
Q

What are silver nanoparticles used for? [2]

A
  1. They have antibacterial properties
  2. Can be added to polymer fibres to make surgical masks and wound dressings
63
Q

Why are nanoparticles used in mositurisers?

A

Can improve them without making them oily

64
Q

Dangers of nanoparticles [2]

A
  1. Don’t know the long-term impacts on health
  2. May cause damage to the environment
65
Q

What is nanoscience?

A

Area of science which investigates the uses and properties of nanoparticles

66
Q

Why are nanoparticles used in sun creams? [2]

A
  1. Better at protecting skin from harmful UV rays
  2. Give better skin coverage

Chemistry (10 decks)

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