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Gsce Chemistry > C3 Structure and bonding > Flashcards

C3 Structure and bonding Flashcards

1
Q

What are the 3 common states of matter

A

Solid, liquid, gas

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2
Q

Describe a solid

A

-Hard to compress due to the particles being packed together in a regular pattern with almost no space in between
-fixed shape
-so cannot flow due to the fact they can’t move from place to place but can vibrate

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3
Q

Describe a liquid

A

-hard to compress due to particles being close together with not many spaces in between
-liquids take the shape of the container
-flow from place to place due to particles in liquid can move

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4
Q

Describe a gas

A

-Easy to compress due to particles being widely spaced
-Gases spread out to fill container due particles in gases moving quickly and randomly

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5
Q

How can you change state of a substance

A

By putting in or taking away energy

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6
Q

Describe melting

A

-Takes place at melting point / freezing point
-particles in liquid move around so have more kinetic energy than a solid so we have to put in energy to convert a solid to a liquid, this energy is needed to break down the forces of attraction between particles of a solid
-when forces are broken, particles can move around / we’ve changed the solid to a liquid

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7
Q

The stronger the forces of attraction between the particles the more / less energy we have to put in to break them.what does this mean about the melting point?

A

More
Higher

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8
Q

Solid -> liquid

A

Melting

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9
Q

Solid -> liquid

A

Melting

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10
Q

Liquid -> solid

A

Freezing

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11
Q

Liquid -> gas

A

Boiling

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12
Q

Gas -> liquid

A

Condensing

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13
Q

What are the limitations of the simple particle model

A

-assumes all particles are solid spheres (particles have lots of different shapes, not solid)
-assumes no forces between the particles (forces on particles have big impact on boiling and melting point of substance)

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14
Q

How many electrons are in first outer shell

A

2

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15
Q

How many electrons are in the 2nd and 3rd outer shell

A

8th

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16
Q

How many electrons are in 4th outer shell

A

18

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17
Q

Which group has a full outer shell?

A

Group 0

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18
Q

What are group 0 called?

A

Noble gases

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19
Q

Why do elements react?

A

To achieve a full outer shell

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20
Q

When a metal reacts with a non metal it is what type of bonding?

A

Ionic

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21
Q

Draw a dot cross diagram of lithium and flourine

A
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22
Q

Group 1 metals …………… forming a ….. ion

A

Lose 1 electron
1+

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23
Q

Group 7 metals …………… forming a ….. ion

A

Gain 1 electron
1-

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24
Q

Describe what is happening in the reaction of sodium chloride [4]

A

One electron passes from the sodium atom to the chlorine atom. Both atoms achieve a full outer shell.

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25
Q

Give the electronic structure of magnesium element

A

[2,8,2]

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26
Q

Draw the dot cross diagram for magnesium and oxygen

A
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27
Q

Group 2 metals ………….. forming a ….. Ion

A

Lose 2 electrons
2+ ion

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28
Q

Group 6 metals ………….forming a ….. ion

A

Gain 2 electrons
2- ion

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29
Q

Ionic compounds form what?

A

Giant structures where every positive ion is surrounded by negative ions and vice versa called a giant ionic lattice w

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30
Q

What are giant ionic lattices

A

Three dimensional
Very strong forces of attraction between positive and negative ions (electrostatic forces)
The strong electrostatic forces hold the ions in place
The electrostatic forces are also called ionic bonds and act in all directions

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31
Q

Properties of ionic compounds

A

-very high melting and boiling points due to electrostatic forces requiring a great deal of heat energy to break
-can’t conduct electricity as solid because ions can’t move due to being locked in place by electrostatic forces of attraction.
-can conduct when melted or dissolved in water due to ions being free to move and carry charge

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32
Q

Draw Energy level diagram for H2

A
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33
Q

What is a single covalent bond

A

One shared pair of electrons

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34
Q

Draw dot cross diagram for H2

A
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35
Q

Draw stick diagram for H2

A

H—H

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36
Q

Covalent bonding takes place between what type of elements?

A

Non-metals

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37
Q

Draw dot cross diagram for NH3

A
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38
Q

Draw energy level diagram for H2O

A
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39
Q

Draw stick diagram for CH4

A
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40
Q

Draw stick diagram for O2

A

O=O

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41
Q

Describe properties of small covalent molecules

A

-low melting and boiling points
-usually gases or liquids at room temperature
-weak intermolecular forces which don’t require lots of energy to break

42
Q

Why do small covalent molecules have low melting points

A

They have weak intermolecular forces in between the covalent bonds

43
Q

Conductivity of small covalent molecules

A

-don’t conduct electricity
-don’t have an overall eletric charge

44
Q

Describe giant covalent molecules

A

-solids at room temperature
-millions of strong covalent bonds
-high melting and boiling points

45
Q

What is diamond formed from

A

Element of carbon

46
Q

How many covalent bonds does each carbon atom bond to in diamond

A

4 other carbon atoms

47
Q

Can diamond conduct electricity?

A

No due to there being no delocalised electrons

48
Q

What is the properties of silicon dioxide

A

Very high melting and boiling point due to huge number of strong covalent bonds which have to be broke requiring lots of energy

49
Q

Properties of graphite

A

High melting and boiling points
Soft and slippery
Excellent conductor of electricity and heat

50
Q

What is graphite formed from

A

Carbon

51
Q

How many bonds do each carbon atom have in graphite

A

3

52
Q

What shape do carbon atoms form in graphite

A

Hexagonal rings

53
Q

How are the hexagonal rings in graphite arranged in?

A

Layers

54
Q

What keeps the layers of graphite together?

A

There are no covalent bonds so only weak intermolecular forces, due to this they can slide over each other

55
Q

What is the 4th electron in graphite called

A

Delocalised electrons because it is not in an outer shell

56
Q

What can delocalised electrons do

A

Conduct thermal energy and electricity

57
Q

Is graphite a metal or non metal

A

Non metal

58
Q

What do graphites properties align with? Metals or non metals

A

Metals

59
Q

What can delocalised electrons do

A

Move around

60
Q

What is graphene

A

A single layer of graphite, one atom thick

61
Q

Does graphene conduct electricity?

A

Yes due to it having a delocalised electron

62
Q

What is the strength of graphene

A

Extremely strong

63
Q

What are fullerenes

A

Molecules of carbon atoms with hollow shapes

64
Q

What types of carbon rings do fullerenes have

A

Rings with 5, 6 or 7 carbon atoms

65
Q

Give 3 uses of fullerenes

A

-pharmaceutical delivery
-lubricants
-catalysts

66
Q

Properties of carbon nanotubes

A

-High tensile strength
-excellent conductor of heat and electricity

67
Q

Give 1 use of nanotubes

A

Reinforce materials like strings of a tennis racket

68
Q

What are polymers

A

-Made by joining small, identical molecules (monomers)
-monomers are often alkaline molecules e.g. ethene

69
Q

Join 5 ethene molecules together

A
70
Q

What is the difference in carbon bonds between monomers and polymers

A

Monomers have double carbon covalent bonds whereas polymers have single carbon covalent bonds

71
Q

Draw a polymer of polythene short hand

A
72
Q

Properties of polymers

A

-solids at room temperature
-intermolecular forces between polymer molecules are relatively strong
-high melting and boiling point due to intermolecular forces requiring a lot of energy to break

73
Q

What do metals consist of?

A

A giant structure of atoms arranged in regular layers

74
Q

What are the electrons in the outer shell of each atom

A

Delocalised

75
Q

Metallic bonding

A

-Strong electrostatic attraction between sea of delocalised electrons and positive metal ions

76
Q

Why do metals have a high melting and boiling point?

A

Due to great deal of energy required to break strong metallic bonds

77
Q

What is the conductivity of metals

A

Good conductors of heat and electricity because the delocalised electrons can move

78
Q

Why can metals be bent and shaped?

A

Due to the layers of a metal being able to slide over each other

79
Q

What is an alloy?

A

A mixture of metals

80
Q

Why are alloys less malleable than pure metals?

A

Due to the different size of atoms distorting the layers, making it more difficult for them to slide over each other. Alloys are harder than pure metals

81
Q

What is a millimetre in standard form compared to a metre

A

1x10-3

82
Q

What is a micrometre in standard form compared to a metre

A

1x10-6

83
Q

What is a nanometre in standard form compared to a metre

A

1x10-9

84
Q

What are other names of coarse particles

A

PM10 or dust

85
Q

What is the diameter of coarse particles

A

1x10-5 - 2.5x10-6

86
Q

How many atoms can coarse particles contain

A

Many thousands of

87
Q

What is another name for fine particles

A

PM2.5

88
Q

What is the diameter of fine particles

A

100 - 2500 nanometres

89
Q

How many atoms are contained in fine particles

A

Several thousands

90
Q

What is the diameter of a nanoparticle

A

1-100 nanometres

91
Q

How many atoms are in nanoparticles

A

A few hundred

92
Q

As the particle size decreases by ten times, what happens to the surface area : volume ratio?

A

Increases by ten times

93
Q

What is the surface area to volume ratio of a nanoparticle like?

A

Huge surface area : volume ratio so even a small amount of nanoparticles have a huge surface area therefore much smaller quantity of nanoparticles needed to catalyse something

94
Q

How can nanoparticles be used?

A

Medicine, sun cream, cosmetics, deodorants, electronics, catalysts

95
Q

What are the risks of nanoparticles

A

-can be absorbed into our body and enter our cells
-unknown long term effects of absorption into cells

96
Q

Drawbacks of dot cross diagrams?

A

Don’t tell us shape of the moelcule

97
Q

Drawback of a stick diagram

A

Can’t tell which electron came from which atom as they are sticks
No idea outer electrons that are not in bonds

98
Q

Benefit of 3D stick diagram

A

Shows where the electron came fron

99
Q

Draw 3D stick diagram for ammonia

A
100
Q

Drawback of ball and stick diagram

A

Shows the ions as widely spaced

101
Q

Drawback of space filling diagram

A

Can be hard to see 3D packaging

102
Q

Problem with both ball and stick diagram and space filling diagrams

A

Only show tiny part of lattice, give mistaken impression of size of the lattices

Gsce Chemistry (15 decks)

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