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GCSE Chemistry > C3 - Structure and Bonding > Flashcards

C3 - Structure and Bonding Flashcards

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1
Q

What is it called when a SOLID turns into a GAS

A

Sublimation

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2
Q

What is it called when a SOLID turns into a LIQUID?

A

Melting

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3
Q

What is it called when a LIQUID turns into a SOLID?

A

Freezing

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4
Q

What is it called when a LIQUID turns into a GAS?

A

Boiling

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5
Q

What is it called when a GAS turns into a SOLID?

A

Deposition

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6
Q

What is it called when a GAS turns into a LIQUID?

A

condensing

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7
Q

What is a covalent bond?

A

When electrons are shared between non metal atoms

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8
Q

Why do atoms need full outershells?

A

To be stable

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9
Q

What is the definition of Ionic Bonding?

A

The electrostatic force of attraction between two oppositely charged ions

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10
Q

Why do lattices have very high melting and boiling points?

A

They have lots of ionic bonds
This means that the bonds are very strong
Requiring alot of energy to break

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11
Q

What is the formula of hydroxide ions?

A

_
OH

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12
Q

What is the formula of Sulfate?

A

2-
SO4

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13
Q

What happens when two non metal elements try and attract? For example Cl and Cl

A

They share electrons

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14
Q

Which types of elements combine in ionic bonding?

A

Metals combine with non metals

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15
Q

Why do metals combine with non metals in ionic bonding? For example, Li and Cl

A

So both elements can have a full outer shell

Li (+1) + Cl (-1) = LiCl

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16
Q

What is an ionic compound?

A

A giant structure of ions

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17
Q

How are ionic compound held together?

A

Electrostatic forces of attraction between oppositely charged ions (ionic bonding)

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18
Q

What happens when ionic compounds are melted or dissolved in water?

A

They conduct electricity

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19
Q

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

A

The ions are free and their charge can flow

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20
Q

Where does covalent bonding occur?

A

Between non - metal elements and compounds of non metals

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21
Q

How are covalent bonds formed?

A

When atoms share pairs of electrons

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22
Q

What is metallic bonding?

A

Atoms which share delocalised electrons

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23
Q

What are some examples of giant covalent structures?

A

Diamond
Graphite

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24
Q

What is an example of a simple molecullar structure?

A

Water

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25
Q

Why do ionic substances not conduct electricicty when they are a solid?

A

The ions are in a fixed position and are not free to flow

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26
Q

What does it mean when an atom is delocalised?

A

It is free to move around the whole structure

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27
Q

Why do positive metal ions attract to delocalised elctrons?

A

Electrostatic force of attraction

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28
Q

What are the properties of giant covalents?

A

High melting and boiling points

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29
Q

What are the three main types of covalent structures?

A

Giant covalents
Small molecules
Large molecules

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30
Q

What are the properties of covalent small molecules?

A

Low melting and boiling poit

The intermolecular forces are weak so do not require energy

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31
Q

What are the properties of covalent large molecules?

A

Melting and boiling points are low but still stronger than small molecules

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32
Q

What is the state of giant covalents at room temperature?

A

Solid

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33
Q

What is the state of covalent small molecules at room temperature?

A

Gaseous or liquid

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34
Q

What is the state of covalent large molecules at room temperature?

A

Normally solid

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35
Q

Why do most covalent structures not conduct electricity?

A

They do not have delocalised electrons or ions that are free to move

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36
Q

What type of covalent structure is Graphite?

A

Giant Covalent

37
Q

Can Graphite conduct electricity?

A

Yes

38
Q

What is the structure of graphite in more depth?

A

Each carbon arom forms three covalent bonds to create Hexagonal layers
Layers are not covalently bonded so they slide
Each carbon atom has one delocalised electron

39
Q

What is the structure of fullerenes in more depth?

A

Hollow sphere of carbon atoms held by weak intermollecular forces

40
Q

What is an allotrope?

A

Different structural forms of the same element

41
Q

What are the allotropes of carbon?

A

diamond, graphite, graphene and fullerene

42
Q

What is the carbon structure in a diamond?

A

Each carbon atom is covalently bonded to 4 other carbon atoms

43
Q

What are the uses of fullerene?

A

Industrial catalyst
To strengthen materials
Nanotechnology

44
Q

What is an alloy?

A

The resulting mixture of adding a different element to a pure metal to make it harder

45
Q

How are ions made?

A

When electrons are transferred

46
Q

What do atoms need to do to get a “stable electronic structure”?

A

loses or gains electrons

47
Q

How do metals form ions?

A

They lose electrons from their outershell to form postive ions

48
Q

How do non-metals form ions?

A

They gain electrons into their outershell to form negative ions

49
Q

Which groups are most likely form ions?

A

Groups 1 & 2, and 6 & 7

50
Q

What what type of ions do group 1 elements form?

A

1+ ions

51
Q

What what type of ions do group 2 elements form?

A

2+

52
Q

What what type of ions do group 6 elements form?

A

2-

53
Q

What type of ions do group 7 elements form?

A

1-

54
Q

What happens in ionic bonding?

A

When a metal and a non-metal react together

55
Q

Why do metals and non-metals transfer electron in Ionic Bonding?

A

There oppositely charged ions are strongly attracted to each other by electrostatic forces

56
Q

What is the name of the structure of ionic compounds?

A

A Giant ionic lattice

57
Q

Why are the ions in a giant ionic lattice so strong?

A

Because of the electrostatic forces of attraction between oppositely charged ions (EXTREME STRENGTH)

58
Q

What does the structure of a single crystal of sodium chloride look like?

A

one giant ionic lattice
A similar ratio of positive and negative ions
Very strong electrostaic forces of sttraction

59
Q

What are the properties of solid ionic compounds?

A

High Melting and Boiling points (Electrostatic force of attraction)
Cant conduct electricity (ions are held in place)

60
Q

Why are covalent bonds so strong?

A

The atoms are attracted to the shared pair of electrons by electrostatic forces

61
Q

Why, in covalent bonding, do atoms share electrons in their outsrshells?

A

They have the highest energy levels

62
Q

What are simple molecular substance made up of?

A

molecules that contain a few atoms joined together by covalent bonds

63
Q

What are some examples of simple molecula substances?

A

Hydrogen
Chlorine
Oxygen
Nitrogen

64
Q

Why do simple molecular substances have low melting and boiling points if they have strong covalent bonds?

A

The intermolecular forces between the covalent bonds are very weak

65
Q

Why dont molecular compounds like H20 or CO2, conduct electricity?

A

They have no delocalised electrons

66
Q

What are the properties of simple molecular substances?

A

Strong covalent bonds within the molecules held together by weak intermolecular forces
Very Low melting and boiling points
Dont conduct electricity

67
Q

What is the diametere of a nanoparticle?

A

Between 1nm and 100nm

68
Q

What ratio do nanoparticles have?

A

Large surface area to volume ratio

69
Q

What are some uses of nano particles?

A

Nanomedicine
Making new catalysts
Tiny electric circuits

70
Q

Why is nanomedicine popular?

A

nanoparticles are tiny so can be absorbed more easily by the body
This means they can deliver drugs right into the specific cells

71
Q

Why are nanoparticles used in tiny electric circuits?

A

Some nanoparticles conduct electricity

72
Q

What is a disadvantage of nanomedicine?

A

Long term effects on health arent fully understood as it is new

73
Q

What are polymers?

A

Long chains of repeating units

74
Q

What is an example of a polymer?

A

Poly(propene) - one of the main polymers in plastic

75
Q

What is the molecular formula for Polypropene?

A

(C3H6)n

76
Q

Each Polymer Molecule is made up of smaller units called ___________

A

Monomers

77
Q

What type of bonds are within polymers?

A

Covalent bonds

78
Q

What are you breaking when melting or boiling a Polymer?

A

The weak intermolecular forces

79
Q

Why do Polymers have a higher melting point and boiling point than simple molecular substances even though they both have very weak intermolecular forces?

A

Polymers have a large surface area
So theres more intermolecular forces to break

80
Q

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

A

Alot of energy is needed to break the strong covalent bonds

81
Q

Why dont giant covalent structures conduct electricity?

A

They dont contain charged particles - even when molten

82
Q

Why does diamond have a very high melting point?

A

Many strong covalent bond
Require alot of energy to break

83
Q

Why does diamond not conduct electricity?

A

No delocalised electrons

84
Q

Why is graphite the only giant covalent structure that can conduct electricity?

A

Only three out of each carbons four outer electrons are used
So each carbon has one delocalised electron

85
Q

What can graphite conduct?

A

Electricity and thermal energy

86
Q

What is graphene

A

One layer of Graphite

87
Q

Give an example of a fullerene molecular formula

A

C60

88
Q

A molecule such as C70 can be used in medicine to move drugs around the body
Why is this C70 molecule suitable for this use?

A

Its a fullerene so its hollow and unreactive

89
Q

What is an ion?

A

Charged particles

GCSE Chemistry (9 decks)

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