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

Bonding, Structure, And Properties Of Matter Flashcards

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1
Q

What are ions?

A

Charged atom

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2
Q

How are ions formed?

A

Losing or gaining an electron

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3
Q

Why are Group 1 and 2 more likely to become ions?

A

Requires less energy to stabilise (lose electrons).

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4
Q

Ionic bonding is likely to occur with…

A

…a metal and a non-metal.

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5
Q

How does ionic bonding happen (in terms of electrons)?

A

There’s a transfer of electrons, where one gains electrons while the other loses electrons.
This makes one of the ions positive, and the other negative.
Because of the opposite charges, they are attracted to each other due to electrostatic forces.

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6
Q

What is an ionic compound?

A

They involve lots of ions. Positive and negative ions alternate so each ion is attracted to all of those around them.

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7
Q

What does an ionic compound form?

A

A regular lattice structure

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8
Q

Properties of ionic compound.

A

-Very high melting and boiling points
-Strong bonds
-Conducts electricity when melted or dissolved in water

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9
Q

Why do ionic compounds have very high melting and boiling points?

A

The ionic bonds are really strong(due to electrostatic forces). It takes a lot of energy to break/ weaken the bonds. The high temperatures provide the energy needed.

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10
Q

Why do ionic compounds have strong bonds?

A

The electrostatic forces.

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11
Q

Why do ionic compounds have a crystal structure?

A

Due to their repeating lattice structure.

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12
Q

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

A

The ions are free to move, which allows them to conduct electricity.

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13
Q

Covalent bonding happens between…

A

…a non-metal and another non-metal

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14
Q

How does Covalent bonding happen (in terms of electrons)?

A

Both the atoms share electrons to get a full outer shell.

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15
Q

What is the displayed formula?

A

E.g
Cl - Cl
(1 line to show them sharing one pair of electrons)

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16
Q

What are the disadvantages of the displayed formula?

A

Doesn’t show/ represent the 3D shape of the molecule
(Use 3D model)

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17
Q

What are the advantages of the displayed formula?

A

Can show complex molecules in a simpler form.

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18
Q

What is a disadvantage of the 3D model?

A

Hard to predict the shape of the molecule.

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19
Q

What is a simple molecular substance?

A

Small molecules in which the atoms of the molecules are bonded by strong covalent bonds.

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20
Q

Examples of simple molecular substances:

A

-Water
-Methane
-Chlorine
-Ammonia

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21
Q

In a simple molecular substance, do they have:

A) strong intermolecular forces but weak covalent bonds
B) weak intermolecular forces but strong covalent bonds

A

B
The have very strong covalent bonds however they’re intermolecular forces are weak, which is why they have low melting and boiling points.

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22
Q

What are the properties of simple molecular substances?

A

Low melting and boiling points
As the molecules get bigger,melting and boiling points increase
Doesn’t conduct electricity or heat

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23
Q

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

A

Weak intermolecular forces require less energy to break them.

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24
Q

Why do simple molecular substances not conduct electricity or heat?

A

There are no free electrons or ions

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25
Q

What are large molecular structures?

A

Giant covalent structures and polymers

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26
Q

What is a giant covalent structure?

A

Huge numbers of non-metal atoms that are all bonded together by covalent bonds.
Arrange a regular repeating lattice structure

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27
Q

Examples of giant covalent structures:

A

Diamond
Graphite
Silicon dioxide

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28
Q

What are the properties of giant covalent structures?

A

Very strong
High melting and boiling points
Generally don’t conduct electricity (except for graphite)

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29
Q

Why are giant covalent structures strong?

A

strong covalent bonds

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30
Q

Why do giant covalent bonds have high melting and boiling points?

A

A lot of energy is required to break/ weaken all the strong covalent bonds.

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31
Q

Why do most giant covalent bonds not conduct electricity?

A

No free ions or free electrons

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32
Q

What is silicon dioxide (silica)

A

Silicon and Oxygen atoms
(1:2 ratio)

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33
Q

What is an allotrope?

A

Different structural forms of the same element in the same physical state.

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34
Q

Examples of allotropes of Carbon:

A

Diamond
Fullerenes
Graphite/ Graphene

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35
Q

Describe the structure of diamond.

A

Each carbon atom is covalently bonded to 4 other carbon atoms, which is the maximum amount of bonds a carbon can make.
This creates a 3D pattern.

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36
Q

What are the properties of diamond?

A

Strong
High melting and boiling points
Doesn’t conduct heat nor electricity

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37
Q

Why is diamond very strong?

A

There are lots of strong covalent bonds.

38
Q

Why does diamond have high melting and boiling points?

A

There are lots of covalent bonds which all require lots of energy to break.

39
Q

Why does diamond not conduct electricity or heat?

A

There are no free ions or free electrons.
(Because every carbon is bonded to 4 other carbons)

40
Q

Describe the structure of graphite.

A

Each carbon atom is covalently bonded to 3 other carbon atoms and therefore they make hexagons.
These hexagons are formed into large flat sheets, which are layered on top of each other to form lots of layers.
However the forces of attraction between the layers are weak.

41
Q

What are the properties of graphite?

A

Soft
High melting and boiling points
Can conduct heat and electricity

42
Q

Why is graphite soft?

A

The layers of graphene are held together by weak forces of attraction.
This allows the layers to slide over each other, therefore graphite is soft.

43
Q

Why does graphite have high melting and boiling points?

A

Due to graphites many covalent bonds, a lot of energy is required to break these bonds

44
Q

Why can graphite conduct electricity?

A

Since every carbon atom is covalently bonded to 3 other carbon atoms, there’s 1 free electron in each carbon atom.
This electron becomes delocalised and is free to move. All the delocalised electron can carry charge/ electric charge.

45
Q

What is graphene?

A

A single layer of graphite

46
Q

What is graphite used for?

A

Lubricant and in pencils.

47
Q

What are the properties of graphene?

A

Can conduct electricity
Strong

48
Q

Why is graphene strong?

A

Many strong covalent bonds between all the carbons.

49
Q

Why can graphene conduct electricity?

A

Sea of delocalised electrons.

50
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes.
Their structures are based on the hexagon shapes of carbon (covalently bonded together), basically a graphene.

51
Q

Describe what the first fullerenes was?

A

Buckminsterfullerene, had 60 carbons covalently bonded together.
It was a molecule of C60, and is spherical.
Has a low melting point due to weak intermolecular forces

52
Q

What is a nanotube?

A

Graphene rolled into a cylinder.

53
Q

Properties of nanotubes:

A

Large surface area : volume ratio
Large length : diameter ratio (long and thin)
High tensile strength
Strong
Can conduct electricity (free electrons)

54
Q

Metallic bonding occurs between…

A

…a metal and another metal.

55
Q

Describe what metallic bonding is.

A

Giant structure of atoms arranged in a regular pattern. (lattice structure)

56
Q

Describe metallic bonding (in terms of electrons).

A

The metal atoms lose the electrons on the outer shell, therefore the electrons are delocalised and the metal atoms become cations.
(There’s a sea of delocalised electrons which are shared across all the cations.)

57
Q

How does metallic bonding form a lattice structure?

A

The delocalised electrons and cations have a strong electrostatic attraction between them and these forces of attraction keeps the regular structure.

58
Q

What are the properties of metallic bonding?

A

High melting and boiling points
Strong
Can conduct heat and electricity
Malleable

59
Q

Why do metallic bonds have high melting and boiling points?

A

There are lots of strong electrostatic forces between the cations and electrons. Therefore more energy is required to weaken these forces.

60
Q

Why are pure metals malleable (easily bent into shape)?

A

The regular structure allows layers of metal to slide over each other (not fixed)

61
Q

How can you make a metal not malleable?

A

Alloys.
The different sized atoms disrupt the regular structure so the layers can no longer slide over each other, therefore it is harder than pure metal.

62
Q

What is an alloy?

A

2 or more different elements mixed together (can be metal and non-metal).
Remember: it is a mixture!!

63
Q

What is particle(kinetic) theory?

A

Particles are small, inelastic spheres.

64
Q

Name the 3 states of matter:

A

Solid
Liquid
Gas

65
Q

Describe a solid using particle theory.

A

They vibrate in a fixed position and has a definite shape and volume.
There are strong forces of attraction between the particles.

66
Q

Describe the change in state from solid to liquid (in terms of particle theory).

A

Energy is transferred to the particles internal energy (via heating) and the energy increases until the melting point- where it has enough energy to overcome the bonds.

67
Q

Describe a liquid using particle theory.

A

The particles are free to move around because they have weaker forces of attraction (yet they stick together).
They are randomly arranged but have a definite volume.

68
Q

Describe the change in state from liquid to gas (in terms of particle theory).

A

The liquid is heated and energy is transferred to the particles internal energy store.
The particles gain energy and they move faster.
The bonds weaken and at the boiling point, the particles have enough energy to break the bonds.
(The liquid has evapourated)

69
Q

Describe a gas using particle theory.

A

The forces of attraction are very weak so the gas particles are free to move around themselves.
They are constantly moving in random motion.
They don’t keep a definite volume or shape and they always fill a container.

70
Q

In a closed system, while changing state, does the number of particles change?

A

No, the number of particles will stay the same.

71
Q

If a gas is heated, what happens?

A

Expandable container: the gas will expand
Fixed container: the pressure will increase

72
Q

What happens when a gas condenses (in terms of particle theory)?

A

The particles don’t have enough energy to overcome the forces and therefore condenses into a liquid.

73
Q

What are the disadvantages of the particle model?

A

Particles aren’t solid, inelastic spheres
Doesn’t include the details of forces between the particles.
(But it’s a useful simplification)

74
Q

What are nanoparticles?

A

Really small particles
Used in nanoscience

75
Q

What is the size for nanoparticles?

A

1 - 100 nm

76
Q

What are the properties for nanoparticles?

A

Very large surface area : volume ratio
Can conduct electricity

77
Q

How can we use nanoparticles, in medicine?

A

Using fullerenes to transport drugs directly inside a cell of our body.

78
Q

How can we use nanoparticles, in chemistry?

A

Use as catalysts in chemical reactions, and nanoparticles have a high surface area: volume ratio therefore we need less of that material.

79
Q

How can we use nanoparticles, in circuits?

A

Can conduct electricity, therefore we can make smaller chips (computer chips)

80
Q

What are potential disadvantages of nanoparticles?

A

Relatively new (so we don’t fully understand their affect on our bodies)
However there’s no evidence that they cause harm.
They could damage our cells (since they can get into them)
We don’t know the harm they cause to the environment.
Could be breathed in and cause problems inside our bodies.

81
Q

What is a polymer?

A

A large molecule formed by many individual smaller molecules

82
Q

How are atoms in a molecule formed?

A

Covalently bonds

83
Q

Give an example of a polymer

A

Poly(ethene) has thousands of Carbon atoms

84
Q

What are the properties of polymers?

A

Strong intermolecular forces between polymer molecules.
High melting point

85
Q

What are nanoparticulate materials?

A

A substance that contains nanoparticles

86
Q

What are bulk materials?

A

Atoms with a larger dimension than nanoparticles (100nm +)

87
Q

Are nanoparticulate materials properties the same as the properties of the same material in bulk?

A

No, some of the properties of nanoparticulate materials are different to the same material in bulk.

88
Q

Why do nanoparticulate materials have different properties to materials in bulk?

A

The size of nanoparticles are much smaller compared to them in bulk
The surface area: volume of nanoparticulate materials compared to the same material in bulk
(Bulk materials have lower ratio)

89
Q

What are properties of nanoparticulate materials.

A

Medicine treatments
Cosmetics + deodorants + sunscreen
Electronics
Catalysts

90
Q

What does the difference in surface area: volume ratio between nanoparticulate substances and substances in bulk change as catalysts?

A

The higher surface area: volume ratio will catalyse the reaction more effectively
Catalyse different reactions that produce different products

91
Q

List the smallest particle to the largest:

A

Atoms + small molecules
Nanoparticles
Fine particles
Course particles

92
Q

If an atom had a diameter of 0.28nm and the nanoparticle for the same atom had a diameter of 32nm.
How would you work out how much larger the nanoparticle is?

A

32/0.28 = x
x = number of times larger it is.

Chemistry (6 decks)

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