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GCSE WJEC Chemistry > Topic 7 - Bonding > Flashcards

Topic 7 - Bonding Flashcards

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1
Q

What are the 3 types of bonding?

A

Ionic bonding, covalent bonding and metallic bonding.

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2
Q

What is ionic bonding?

A

An attraction between oppositely charged ions.

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3
Q

Where are ionic bonds found?

A

In compounds made of metals and non-metals.

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4
Q

What is covalent bonding?

A

2 atoms sharing 1 or more pairs of electrons.

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5
Q

Where are covalent bonds found?

A

In most non-metal elements and in non-metal compounds.

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6
Q

What is metallic bonding?

A

An attraction between positively charged ions and negatively charged delocalised electrons.

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7
Q

Where are metallic bonds found?

A

Metallic bonds are found in metals and alloys.

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8
Q

What is an alloy?

A

A mixture of metals and other substances.

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9
Q

What is an ion?

A

Particles that have a charge, created when an atom or molecule gains or loses electrons.

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10
Q

What causes a negative ion?

A

Gaining electrons

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11
Q

What causes a positive ion?

A

Losing electrons

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12
Q

What is a positive ion called?

A

Cation

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13
Q

What is a negative ion called?

A

Anion

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14
Q

What happens during ionic bonding?

A

In ionic bonding, a metal atom transfers electrons to a non-metal atom, allowing both to have a full outer shell.

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15
Q

What are the properties of materials with ionic bonds?

A

Only conduct electricity when molten/dissolved, high melting points.

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16
Q

What are dot-and-cross diagrams used for?

A

To show electrons being transferred and ions being formed in covalent or ionic bonding.

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17
Q

What do the dots represent?

A

Electrons from 1 atom.

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18
Q

What do the crosses represent?

A

Electrons from the other atom.

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19
Q

What else must a dot-and-cross diagram have?

A

Square brackets and a charge (e.g. 2+) to represent ions.

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20
Q

When are ionic compounds formed?

A

When millions of metal atoms transfer electrons to millions of non-metal atoms at the same time, resulting in ionic lattices.

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21
Q

What are ionic lattices?

A

Giant structures held together by large electrostatic forces between positive and negative ions.

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22
Q

What are electrostatic forces?

A

Ionic bonds that extend in all directions.

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23
Q

What are empirical formulae?

A

The simplest ratio of ions possible where charges are balanced.

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24
Q

Examples of covalent bonds?

A

Small molecules (e.g. Water), large molecules (e.g. polymers) and giant covalent structures (e.g. diamond).

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25
Q

What are delocalised electrons?

A

Delocalised electrons are NOT bound to an atom and are free to move around within the lattice because metals have a low number of electrons in their outer shells.

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26
Q

In metals, what do electrostatic attractions form between?

A

Metal ions and delocalised electrons.

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27
Q

What is the difference between a single and a double/triple covalent bond?

A

Double/triple bonds are normally stronger and require more energy to break.

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28
Q

How can covalent bonds be represented by lines?

A

The atomic symbol represents the atom. Lines between the atoms represent a covalent bond.

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29
Q

Why do electrons become delocalised in metals?

A

Because the electron orbitals in metal atoms overlap.

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30
Q

What are the properties of ionic compounds?

A

High melting/boiling points, conduct electricity if liquid or dissolved.

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31
Q

Why do ionic compounds have high melting/boiling points?

A

Significant energy is needed to break the electrostatic forces between the ions and electrons in the lattice so the melting and boiling points of ionic compounds are high.

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32
Q

Why don’t ionic compounds conduct electricity if solid?

A

When solid, the ions in the lattice are fixed in place therefore charges cannot flow, so electricity cannot be conducted.

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33
Q

Why do ionic compounds conduct electricity if liquid or dissolved?

A

When molten, or dissolved in water, the ions in the lattice can move freely so the charge can flow and electricity can be conducted.

34
Q

What are intermolecular forces?

A

Forces between different molecules that are often easy to break.

35
Q

What are intramolecular forces?

A

The strong covalent bonds found within small molecules which are often difficult to break.

36
Q

Why do small covalent molecules have low melting/boiling points?

A

Lots of small covalent molecules can be held together by intermolecular forces but these forces are weak and easy to break.

37
Q

What state are small molecules in at room temperature?

A

Liquids or gases because they have weak intermolecular forces.

38
Q

Why don’t small molecules conduct electricity?

A

They don’t contain delocalised electrons.

39
Q

Why do large molecules have higher melting/boiling points than small molecules?

A

Bigger molecules attract other molecules with stronger intermolecular forces.

40
Q

Why don’t large molecules conduct electricity?

A

They don’t contain delocalised electrons.

41
Q

What are polymers?

A

Polymers are large, chain-like molecules that can extend for thousands of atoms.

42
Q

What are polymers held together by?

A

Strong covalent bonds between atoms in molecules but weak intermolecular forces between molecules.

43
Q

What are the intermolecular forces of a polymer like?

A

Because of the large size of polymer molecules, the intermolecular forces add up to be quite strong.

44
Q

What are the properties of a polymer?

A

Polymers are usually solid when at room temperature but many polymers melt easily because the intermolecular forces remain less strong than chemical bonds.

45
Q

Why don’t giant covalent structures have a specific formula?

A

The structure can be any size.

46
Q

Why do giant covalent structures have very high melting points?

A

Strong covalent bonds between atoms make them solids at room temperature. High temperatures and significant energy are required to break the structure’s covalent bonds.

47
Q

Why are there no intermolecular forces in giant covalent structures?

A

There is only 1 molecule.

48
Q

What is the structure of pure metals like?

A

Giant structures with strong electrostatic forces between positive ions and delocalised electrons. All ions are the same size and arranged in layers.

49
Q

Why are pure metals soft and malleable?

A

The ions are arranged in layers, they easily move over each other when a force is applied.

50
Q

Why do pure metals have high melting/boiling points?

A

There are strong electrostatic forces between the positive metal ions and the negative delocalised electrons.

51
Q

What is an alloy?

A

A combination of 2+ elements, where at least 1 is a metal.

52
Q

Why are alloys stronger than pure metals?

A

The ions of the different elements are different sizes, making it harder for the layers to slide across each other when a force is applied to the alloy. This makes alloys stronger than pure metals, and so they are often used in construction.

53
Q

Why are metals good electrical and heat conductors?

A

Their delocalised electrons can carry a charge/heat energy from the negative terminal to the positive terminal.

54
Q

What are the covalent bonds in diamond like?

A

Every carbon atom in diamond is bonded to 4 other carbon atoms by strong covalent bonds, creating a giant covalent structure.

55
Q

Is diamond hard?

A

There are lots of strong covalent bonds in diamond, making it very hard and useful as a cutting tool to cut other materials.

56
Q

Why does diamond have a high melting point?

A

Diamond has lots of strong covalent bonds which need lots of energy to break resulting in a high melting point.

57
Q

Does diamond conduct electricity?

A

Diamond is NOT an electrical conductor because it has no delocalised electrons.

58
Q

What are the covalent bonds in graphite like?

A

Every carbon atom in graphite is bonded to 3 other carbon atoms by strong covalent bonds, creating a giant covalent structure.

59
Q

Is graphite soft?

A

The carbon atoms form layers of hexagonal (6-sided) rings, with weak intermolecular forces ergo the layers easily slide over one another, so graphite is very soft and useful as ‘lead’.

60
Q

Does graphite conduct electricity?

A

Each carbon atom forms 3 bonds ergo there is 1 delocalised electron from every carbon atom which can move freely, so graphite is a good electrical conductor.

61
Q

Does graphene conduct electricity?

A

Graphene is a single layer of graphite so it also conducts electricity because of each carbon atoms’ one delocalised electron.

62
Q

Is graphene light?

A

Graphene has a thickness of just 1 atom meaning that it is almost a 2-dimensional structure, and so graphene is very light.
But, the strong covalent bonds between carbon atoms mean that it is also very strong.

63
Q

What is graphene used for?

A

Graphene makes materials stronger without making them much heavier so can be used in solar panels, batteries and much more.

64
Q

What is graphene?

A

A single layer of graphite.

65
Q

What is a fullerene?

A

Single layers of graphene that make up hollow structures, usually carbon atoms arranged in hexagonal rings.

66
Q

What is a buckminsterfullerene?

A

It has a spherical shape and its formula is C60; it’s technically a simple molecule because of its fixed size.

67
Q

What are fullerenes used for?

A

As catalysts, lubricants and as vehicles for transporting drugs into our bodies.

68
Q

What are carbon nanotubes?

A

Cylindrical fullerenes

69
Q

Is a carbon nanotube strong?

A

Nanotubes are exceptionally strong for their size, because of the strong covalent bonds between carbon atoms.

70
Q

What are carbon nanotubes used for?

A

In electronics, nanotechnology and strengthening materials (e.g. tennis racket frames).

71
Q

What is 1nm in m?

A

1x10-9 m

72
Q

What size are nanoparticles?

A

1 - 100 nm long

73
Q

How many atoms make up nanoparticles?

A

10 - 1,000 atoms

74
Q

What size are fine particles?

A

100 - 2,500 nm long

75
Q

How many atoms make up fine particles?

A

1,000 - 25,000 atoms

76
Q

What size are coarse particles (dust)?

A

2,500 - 10,000 nm long

77
Q

How many atoms make up coarse particles (dust)?

A

25,000 - 100,000 atoms

78
Q

What are the advantages of nanoparticles?

A

High surface area to volume ratio i.e. smaller amounts of materials can be used for our desired purpose (e.g. as catalysts or in sun cream) so they are cheaper and more efficient than larger particles.

79
Q

What are the disadvantages of nanoparticles?

A

Nanoscience is still a very new area of research, we do not know the long-term effects on the environment or human health.

80
Q

What are the uses of nanoparticles?

A

Catalysts (high surface area), deodorants (anti-microbial/transparent)

GCSE WJEC Chemistry (9 decks)

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