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Chemistry > C3 Structure And Bonding > Flashcards

C3 Structure And Bonding Flashcards

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1
Q

Process of melting

A

As solid is heated particles gain energy and vibrate more

As temperature increases when it reaches melting point there’s enough energy to break free from their positions

This is called melting when solid becomes liquid

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2
Q

Process of freezing

A

Liquid turns to a solid as a result of lowered energy in particles

Result of colling to point where liquid solidifies

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3
Q

Process of boiling

A

When liquid heated particles gain more energy

Energy makes particles move faster which weakens and breaks the bonds holding liquid together

When it reaches the boiling point the particles have enough energy to break their bonds

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4
Q

Process of condensing

A

As gas cools particles no longer have enough energy to overcome the forces of attraction between them

Bonds form between the particles

At boiling point so many bonds have formed between the gas particles the gas becomes liquid

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5
Q

How do particles act at melting point

A

Particles start to move about staying close to other particles

Then move freely

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6
Q

How do particles behave at its boiling point

A

Particles gain energy to overcome bonding forces

They become free, fast moving, individual particles in a gas

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7
Q

Solid to liquid

A

Melting

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8
Q

Liquid to solid

A

Freezing

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9
Q

Liquid to gas

A

Evaporating

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10
Q

Gas to liquid

A

Condensing

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11
Q

Solid to gas

A

Sublimation

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12
Q

Gas to solid

A

Deposition

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13
Q

Why substances have different melting and boiling points from each other

A

The stronger the forces between particles, the higher its melting and boiling points

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14
Q

The factors that affect rate of evaportaion

A

Temperature

Surface area

Wind speed

Humidity

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15
Q

The particles involved in ionic bonding

A

Cation

Anion

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16
Q

When is ionic bonding formed

A

When a metal loses an electron or gains electrons

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17
Q

Cation

Anion

A

Cation - a metal which loses electrons

Anion - a non-metal gains electrons

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18
Q

How electron transfer allows ionic bonding to occur in the compound formed when a Group metal reacts with a Group 7 non-metal

A

Metals lose electrons to become positively charged ions

non‐metals gain electrons to become negatively charged ions

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19
Q

What do opposite charges do

A

Attract

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20
Q

With an example, how a Group 7 non-metal atom becomes a negative ion

A

-
Fluorine will gain an electron forming F

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21
Q

Suggest the charge on unfamiliar ions using the position of the element in the periodic table

A

Elements on left metals form positive ions

Those on the right non-metals form negative ions

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22
Q

Charges of ions of Groups 1-7

A

Group 1 = 1+

Group 2 = 2+

Group 3 = 3+

Group 4 = 4-

Group 5 = 3-

Group 6 = 2-

Group 7 = 1-

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23
Q

How unfamiliar elements become ions

A

Atoms lose electrons to form positively charged ions

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24
Q

Ratio of metal and non- metal ions in compounds

A

2:1

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25
Q

Ionic lattice

A

Regular repeating arrangement of ions

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26
Q

Properties of ionic compounds

A

High melting points

Can conduct electricity when molten or dissolved in water

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27
Q

Why ionic compounds have a high melting point

A

Large amounts of energy needed to break the many strong bonds

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28
Q

Ionic bond

A

Forms between metal and non-metal

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29
Q

Covalent

A

Non-metals

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30
Q

The movement of ions in solutions or when molten

A

Free to move

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31
Q

How a covalent bond forms in terms of electronic structure

A

When pairs of electrons are shared by atoms

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32
Q

How double and triple covalent bonds can be formed

A

If 2 pairs of electrons are shared forms double bond

If 3 pairs of electrons are shared forms triple bond

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33
Q

Examples of covalent bonds

A

H2O

CO2

NH3

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34
Q

Examples of ionic bonds

A

Sodium chloride

Sodium bromide

Sodium iodide

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35
Q

Metallic bond examples

A

Na

Al

Mg

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36
Q

How the properties of a double bond could be different to the properties of a single covalent bond

A

Double bonds are stronger than single covalent bonds

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37
Q

Properties of small molecules

A

Low melting and boiling points

Don’t conduct electricity

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38
Q

Phyiscal properties of covalent bonds

A

Low boiling/melting points

Soft

Don’t possess electrical conductivity

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39
Q

Why small molecules and polymers do not conduct electricity

A

Small molecules have no overall electric charge

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40
Q

Intermolecular force

A

Forces of attraction between particles

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41
Q

How to identify substances that would have weak intermolecular forces

A

If it has low boiling point

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42
Q

Physical properties of graphite

A

High melting and boiling points

Good conductors of heat and electricity

Soft

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43
Q

Phycial properties of diamond

A

Hard

Giant covalent structure

High melting and boiling points

Bad conductor of electricity

Good conductor of heat

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44
Q

Properties of giant covalent structures

A

High melting points

Do not conduct electricity as no overall charge

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45
Q

A use for graphite based on its properties

A

Used as a lubricant for fast-moving parts of machinery

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46
Q

Structure of graphite

A

Giant covalent structure

Each carbon atom forms 3 covalent bonds creating sheets of carbon atoms arranged in hexagons

Carbon atoms form layers with hexagonal arrangement of atoms with weak forces

There aren’t any covalent bonds between the layers

Only 3 out of carbon’s 4 outer electrons are used in bonds so each carbon atom has 1 delocalised electron

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47
Q

Use for diamond

A

Embedded into saw blades

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48
Q

Relationship between graphite and graphene

A

Graphite is made up of hundreds of thousands of layers of graphene

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49
Q

Structure of a fullerene

A

Hexagonal rings of carbon atoms joined by covalent bonds but can also contain pentagons or heptagons

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50
Q

Uses of fullerenes

A

Drug delivery in the body

Sports equipment (tennis racket)

Antioxidant

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51
Q

Main physical properties of fullerenes

A

Good conductors of heat and electricity

Very strong

Highly ductile

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52
Q

Molecular formula of buckminsterfullerene

A

C60

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53
Q

Use of graphene

A

Construction

Health

Electronics sector

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54
Q

Use of nanotubes

A

Used in electronics

Strengthen materials without adding much weight

Used in space and aircraft to reduce the weight and stress of the various components working together

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55
Q

Nanotube

A

Tiny carbon cylinders

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56
Q

What structures do metals form

A

Giant structure

57
Q

Metallic bonding

A

Bonding from electrostatic attractive forces between conduction electrons

58
Q

How metal atoms form giant structures

A

The electrons in the outer shell of metal atoms are delocalised and so are free to move

59
Q

Physical properties of metals

A

Malleable

Ductile

Good conductors of heat and electricity

Lustrous (shiny)

Strong

60
Q

How alloying affects the structure and bonding in metals and its effect on properties

A

The smaller or bigger atoms distort the layers of atoms in the pure metal

Making it harder them to slide over each other

61
Q

Pure metals

A

Metals that have not been alloyed with other metallic elements

62
Q

Structure of pure metal

A

Giant metallic structure

63
Q

Why metals are alloyed

A

Increase strength

Reduce costs

Increase corrosion resistance

Harder

64
Q

Nanoscience

A

The study of structures between 1 and 100 nanometres in size

65
Q

Size of nanoparticles

A

1 to 100 nanometres

66
Q

How to classify a particles as coarse, fine or nanoparticles based on their size

A

Fine = diameter of 100nm to 2500nm

Coarse = diameter of 2500nm to 10,000nm

67
Q

How surface area to volume increases as particle size reduces

A

The surface area to volume ratio increases as the radius of the sphere decreases

68
Q

Uses of nanoparticles

A

Paints

Cosmetics

Sunscreens

69
Q

Advantages of using nanoparticles

A

Increased strength

Increased durability

Enhanced catalytic activity

70
Q

Disadvantages of using nanoparticles

A

Difficult to manufacture

Very small

Very expensive

71
Q

Why nanoparticles can have new applications

A

Produces stronger and lighter wind turbines

Imrpoves fuel efficiency

Can save energy

72
Q

Why nanotechnology research should continue

A

Can be used for the development of newer materials with better properties

73
Q

Explain why chlorine (Cl2) is a gas at room temperature, but sodium chloride (NaCl)
is a solid at room temperature

A

There are weak attractions between molecules of Cl2 so little energy is needed to break these forces of attraction

74
Q

Why metals are good conductors of heat and electricity

A

Due to the metallic bonding

In metallic bonding outer electrons are delocalised

The delocalised electrons carry electric charge and thermal energy through the whole structure

75
Q

Iron reacts with halogen in gaseous form give 1 reason why the experiment should be done in a fume cupboard

A

Both the reactants and products are hazardous

76
Q

Why is it not correct to say the boiling point of a single bromine molecule is 59 degrees

A

Boiling point is a bulk property of a substance and is not applicable to individual molecules

77
Q

Why C70 molecules is good for the uses in medicine to move drugs from around the body

A

It is hollow

78
Q

Why diamond has a very high melting point

A

4 valence electrons surrounding each carbon atom which are strong covalent bonds making them hard to break. Requires very high energy to break

79
Q

Element dull solid with melting point 44

Does not conduct electricity

Where most likely found on periodic table

A

Far right end

80
Q

Buckminister fullerene

A

A fullerene with formula C60 with a cage-like structure made of twenty hexagons and twelve pentagons

81
Q

Avogadro’s number of C70

A

21
8.6 x 10

82
Q

How to work out molar mass

A

Moles of 1 reactant
_________________________

Moles of other reactant

83
Q

How are opposite charged ions strongly attracted to each other

A

Electrostatic force

This attraction is called an ionic bond

84
Q

What arrangements do ions form

A

Regular lattice

85
Q

Regular lattice structure

A

Strong electrostatic forces of attraction between oppositly charged ions in all directions of lattice

86
Q

Structure of a single sodium chloride (salt)

A

Giant ionic lattice

87
Q

Why can ion not conduct electricity when a solid but can when molten or dissolve in water

A

Not free to move in a solid

When ionic compound molten or dissolve in water the ions are free to move so they’ll carry an electric charge

88
Q

Empirical formula

A

The simplest whole number ratio of atoms in each elements in a compound

89
Q

What do all covalent bonds provide

A

1 extra shared electron for each atom

90
Q

Where does covalent bond happen

A

In compounds of non-metals

91
Q

What are simple molecular substances made up of

A

Molecules containing a few atoms joined together by covalent bonds

92
Q

Structure of simple molecular substance

A

Atoms held together by strong covalent bonds

Forces of attraction between these molecules are very weak

93
Q

Why are boilng/melting points of simple molecular substances very low

A

Molecules easily parted from each other

94
Q

What state are most simple molecular substances at room temperature

A

Gases or liquids

95
Q

What happens as molecular substances get bigger

A

The strength of intermolecular increases so more energy needed to break them so melting and boiling points increase

96
Q

Why don’t molecular compounds conduct electricity

A

They aren’t charged so there are no free electrons or ions

97
Q

What bonds do polymers have

A

Covalent bonds

98
Q

Polymers

A

Large molecules made up of repeating units called monomers

99
Q

What are polymers used for

A

Plastic bags

Ropes

Water pipes

100
Q

Properties of polymers

A

Strong

Low density

Waterproof

101
Q

Why do polymers have low melting/boiling points

A

Intermolecular forces are weak

102
Q

Why are most polymers solid at room temperature

A

Intermolecular forces are larger between polymer molecules than in between simple covalent bonds so more energy needed to break them making them solids

103
Q

Structures of polymers

A

Large molecule made up of repeating units known as monomers

All atoms joined by strong covalent bonds

104
Q

Molecular formula of polymer poly(ethene)

A

(C2H4)n

105
Q

Examples of polymers

A

Nylon

Epoxy

Teflon

106
Q

Describe giant covalent structure

A

All atoms bonded together by strong covalent bonds

High melting boiling points as lots of energy needed to break bonds between atoms

Don’t conduct electricity

107
Q

Why don’t giant covalent structures conduct electricity

A

They don’t contain charged particles

108
Q

Examples of giant covalent structures

A

Diamond

Graphite

109
Q

Structure of diamond

A

Diamond is a giant covalent structure

Each carbon atom is joined to four other carbon atoms by strong covalent bonds

The carbon atoms have a regular lattice

110
Q

Silicon dioxide structure

A

Giant covalent structure

Each silicon atom forms four covalent bonds with four oxygen atoms

This forms a tetrahedral arrangement

111
Q

Why silicon dioxide can’t conduct electricity

A

No delocalised electrons in the structure

112
Q

Why do diamonds not conduct electricity

A

Has no free electrons or ions

113
Q

How does graphite conduct electricity and thermal energy

A

Graphite has delocalised electrons which are free to move between the layers in graphite

114
Q

Graphene

A

A single layer of graphite

115
Q

Properties of graphene that make it useful

A

It is incredibly light

It is strong

116
Q

Structure of graphene

A

Giant covalent structure

A single layer of carbon atoms arranged in a hexagonal lattice

The sheet is 1 atom thick so it’s a two-dimensional substance

117
Q

How does graphene conduct electricity

A

Contains delocalised electrons so can conduct electricity through whole structure

118
Q

Fullerene

A

Molecules of carbon shaped like closed tubes or hollow balls

119
Q

Why are fullerenes good for drug delivery in the body

A

It can be absorbed more easily by the body

120
Q

How can fullerenes make good lubricants

A

Fullerenes can reduce friction between two surfaces

121
Q

Advantage to fullerenes having large surface area

A

They could make great indrustrial catalysts

122
Q

Which substances are held together by metallic bonding

A

Metallic elements and alloys

123
Q

Which part of metallic bonding produces all the properties of metals

A

Delocalised electrons

124
Q

Why are metals solid at room temperature

A

Electrostatic forces between the positive metal ions and shared negative electrons

125
Q

Why metals are malleable

A

The layers of atoms in a metal can slide over each other

126
Q

Alloys

A

A mixture of 2 or more metals or a metal and another element

127
Q

Do different elements have different sized atoms

A

True

128
Q

What 3 things do strength of attraction between particles depend on

A

The material (structure)

Temperature

Pressure

129
Q

Structure of solids

A

Strong forces of attraction between particles holding them close together to form regular repeating lattice

130
Q

Structure of liquids

A

Weak force of attraction between particles

Randomely arranged

Free to move past each other

131
Q

Structure of gas

A

Force of attraction between particles is very weak

Free to move and far apart

Particles in gas travel in straight lines

132
Q

Name a model for explaining the 3 states of matter

A

Particles thery

The disgrams of solids liquids gas as circles

133
Q

What does energy needed for substance to change state depend on

A

How strong the forces between the particles are

134
Q

How to know state of a substance

A

If temperature is below melting point it’ll be solid

If above boiling point it’s a gas

If between a liquid

135
Q

What happens to surface area as particle decreases in size

A

Surface area increases

136
Q

What does very high surface area to volume ratio mean

A

Surface area is very large compared to the volume

137
Q

What are nanoparticles used in

A

Tiny electric circuits for computer chips

Can help make surgical masks

138
Q

Why should new products containing nanoparticles be tested

A

To minimise risk as the way they affect the human body isn’t fully understood

Chemistry (10 decks)

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