P1. Topic 2- Bonding, Structure And Properties Of Matter Flashcards
1
Q
What are the three states of matter?
A
Solid, liquid, gas
2
Q
What is the particle model?
A
A diagram used to show how particles are arranged and how they move in a state of matter
3
Q
What does the particle model not take into account?
A
the forces between particles, the volume of the particles and the space between particles
4
Q
What happens to the particles when a substance changes state?
A
They change arrangement and they change the way they move
5
Q
What is the name of the temperature a pure substance melts and freezes at?
A
Melting point
6
Q
What is the name of the temperature a pure substance boils and condenses at?
A
Boiling point
7
Q
What is the amount of energy needed for a state change dependent on?
A
The amount of energy needed to overcome the forces of attraction between the particles
8
Q
What happens at the forces of attraction increase?
A
The more energy needed to overcome the forces of attraction so the higher the melting and boiling point
9
Q
What substances have high melting and boiling points due to strong bonds?
A
Ionic compounds, metals and giant covalent structures
10
Q
Why are the melting and boiling points of simple molecules low?
A
Because the bonds between molecules are strong covalent bonds but the forces of attraction between molecules are weak so little energy is needed to overcome them
11
Q
What is this state symbol? (s)
A
Solid
12
Q
What is this state symbol? (g)
A
Gas
13
Q
What is this state symbol? (l)
A
Liquid
14
Q
What is this state symbol? (aq)
A
Aqueous (dissolved in water)
15
Q
What are the three types of bonding?
A
Covalent, ionic and metallic
16
Q
What type of substances does ionic bonding involve?
A
Metal and non-metal
17
Q
Which type of substance gives away electrons in ionic bonding?
A
The metal
18
Q
Describe ionic bonding
A
Chemical bonding that results from the electrical attraction between cations (positively charged ions) and anions (negatively charged ions)
19
Q
What sort of force do ionic compounds have that keep them together?
A
Strong electrostatic force of attraction
20
Q
Why do atoms in ionic bonding transfer electrons?
A
To gain a full outer shell
21
Q
What are ionic compounds?
A
Giant structures of ions
22
Q
How are ionic compounds held together?
A
By strong electrostatic forces of attraction acting in all directions between positive and negative ions in a giant lattice
23
Q
Are ionic compounds boiling and melting points high or low?
A
High
24
Q
Why are ionic compounds boiling and melting points high?
A
Because ionic compounds contain strong electrostatic forces of attraction between oppositely charged ions that require a lot of energy to overcome
25
Can ionic compounds conduct electricity?
Only when molten (not as a solid)
26
Why can ionic compounds only conduct electricity when molten?
Because the charged ions are free to move about and carry their charge
ionic lattice has been broken up as it dissolves
27
Why are smaller particles effective catalysts?
They have a high surace area:volume ratio
28
Why can pure metals be easily shaped?
The particles have a regular arrangement so the layers can easily slide over each other
29
What is iron obtained from a blast furnace like?
Brittle because it is still impure. It only contains 96% iron
30
What are the properties of stainless steel?
Hard and resistant to corrosion
31
How many carbon atoms does buckminsterfullerene have?
60
32
Why are nanoparticles used in sun cream?
They help to provide better coverage hence protecting skin better
33
Do giant covalent structures conduct electricity?
No (except graphite)
34
Are ionic compounds brittle?
yes
however you move the ionic compounds, you will always shift the lattice
35
What causes a metal to have a giant lattice structure?
The delocalised electrons causes there to be positive ions. It is held together by the electrostatic forces between the delocalised electrons and the positive ions
36
Are covalent bonds strong or weak?
Strong
37
What is brass
An alloy of copper and zinc
38
Why do we use alloys?
Pure metals are too soft for many purposes
39
What is a gold alloy made of?
Gold, silver and zinc
40
What is a fullerene?
A covalently bonded form of carbon that contains different numbers of carbon atoms
41
do fullerenes conduct electricity ?
no
it has delocalised electrons but they can't move from one molecule to another
42
What is the diameter of nanoparticles?
Between 1x10^-9 and 1x10^-7
43
What sort of substances does metallic bonding occur in?
Metallic elements and alloys
44
Why do simple (covalent) structures have low melting and boiling points?
Because they have weak intermolecular forces between molecules that are overcome easily
45
What are the functions of fullerenes?
To deliver drugs in the body, in lubricants, as catalysts, for reinforcing materials
46
What type of substances does covalent bonding occur in?
Non-metallic elements and compounds
47
What is the structure of diamond?
A giant covalent lattice
48
Structure of diamond
Giant covalent
49
What is the name of the structures nanoparticles combine to form?
Nanostructures
50
Do polymers have large or small molecules?
Large
51
What is the diameter of fine particles?
Between 1x10^-7 m and 2.5x10^-6 m
52
Do metals have high or low melting and boiling points?
High
53
Why do giant covalent structures have high melting and boiling points?
Because lots of energy is needed to break the many covalent bonds between the atoms
54
how many covalent bonds does each carbon make in graphene?
3
55
What is bronze used for?
Statues and decorative objects
56
What is an alloy?
Mixtures that contain a metal and at least one other element
57
Why are aluminium alloys used to make aeroplanes?
They are strong but low density
58
Does diamond conduct electricity?
No because there are no charged particles
59
Why is graphite soft?
The weak intermolecular forces between layers allow the layers to slide over each other
60
What is stainless steel?
Steel that also contains chromium and nickle
61
What was the first fullerene to be discovered?
Buckministerfullerene
62
Why does diamond have a high melting point?
There are many strong covalent bonds so a lot of energy would be needed to overcome them
63
are fullerenes hard or soft?
Soft
64
What is a polymer
A long molecule consisting of many similar or identical monomers linked together
65
What is steel?
An alloy made from iron and carbon
66
Is graphite hard or soft?
soft
weak intermolecular forces between planes
67
What are the properties of brass?
It is hard wearing and resistant to corrosion
68
What is a giant covalent structure?
All the atoms are linked by strong covalent bonds
69
Is diamond hard or soft?
Hard
70
What are simple (covalent) molecules?
Covalent molecules that contain a relatively small number f non-metal atoms
71
Giant covalent structure
A structure with many atoms joined to each other by lots of strong, covalent bonds in a continuous network
giant lattice
72
Why are polymers a solid at room temperature?
Because the intermolecular forces are strong
73
Why are nonostructures different?
The properties are different than if the material were in bulk
74
What are plastics?
Man-made polymers
75
Why are metals good thermal and electrical conductors?
Because the delocalised electrons can move around freely and transfer energy through the structure
76
How many bonds does each carbon atom make in diamond?
4
77
What are the properties of steel with a high carbon content?
Hard and strong
78
What are the bonds in silicon dioxide (silica)?
Each oxygen atom is bonded to 2 silicon atoms and each silicon atom is bonded to 4 oxygen atoms
79
Why are alloys harder than pure metals?
Because adding another element disrupts the regular arrangement (different sized atoms )so the layers don't slide over each other as easily
80
why do fullerenes have low melting and boiling point?
they're hollow so need to overcome relatively weak intermolecular forces
no covalent bonds broken
81
Does graphite conduct electricity?
yes as it contains delocalised that are free to move along the layers and carry charge through the structure
82
What is diamond a form of?
Carbon
83
What is 24 carat gold?
Pure gold
84
What is a covalent bond?
A shared pair of electrons between atoms
85
How are atoms in a polymer held together?
Strong covalent bonds
86
How many atoms do nanoparticles contain?
Only a few hundred
87
What are the concerns of nanoparticles?
That they could get into the body and damage cells
88
What shapes do fullerenes form?
Hollow shapes including balls, tubes and cages
89
How are the required properties /effects of nanoparticles achieved?
Each individual atom can be placed in the correct position
90
Structure of fullerenes
Simple molecular
91
What is the structure of a metal?
A giant metallic lattice in which electrons from the outermost shells are delocalised (not bound to one atom) and are free to move through the whole structure
92
What are carbon nanotubes?
Cylindrical fullerenes
93
What are the properties if graphene?
Very strong, good thermal and electrical conductor, nearly transparent
94
Does diamond conduct electricity?
No, it has no delocalised electron.
95
how are the layer of graphite held together?
Weak intermolecular forces
96
Do simple (covalent) structures have high or low boiling and melting points?
Low
97
Is graphene strong or weak?
very strong
it's a single layer of graphite
98
Do giant covalent structures have high or low melting points?
High
99
Can simple (covalent) molecules conduct electricity?
No because the molecule has no overall charge
100
Why do we make steel?
The atoms in pure iron are arranged in layers that can slide over each other so is malleable. But it is too soft for many purposes
101
structure of graphene
Giant covalent
102
What is the diameter of coarse particles?
Between 1x10^-5 m and 2.5x10^-6 m
103
does graphene conduct electricity
yes as it contains one delocalised electron that is free to move and carry the charge through the substance
104
How many bonds does each carbon atom make in graphite?
3
105
Why is buckminsterfullerene the most stable fullerene?
It is the most symmetrical
106
Why is copper used for water pipes?
It is unreactive and can be easily shaped
107
What is the structure of buckminsterfullerene?
The atoms are joined together in a series of pentagons and hexagons
108
Why do metals have high melting and boiling point?
Because metals have many strong bonds ( sea of delocalised electrons strongly attracted to the positive nuclei of the metal atoms) and so need a lot of energy to overcome them
109
Why aren't giant covalent substances electrically conductive ?
most aren't as they don't contain any delocalised electrons as graphite does
delocalised electrons are free to move and carry charge through the substance
110
What are the properties of steel with a low carbon content?
Soft and easily shaped
111
What is a metallic bond?
The attraction between the positive nucleus of the metal and the delocalised electrons
112
What is bronze?
An alloy of copper and tin
113
What is graphene?
A single layer of graphite
114
Why can graphite conduct heat and electricity?
Because there is one delocalised electron per atom
115
What is the structure of graphite?
A layered, hexagonal lattice
116
What is brass used for?
To make water taps and door fittings
117
how many covalent bonds does each carbon form in fullerene?
3
118
Structure of graphite
Giant covalent
119
What is nanoscience?
the study of particles between 1-100nm in size
120
How does a bulk material differ to the nanoparticle of that material
Nanoparticles have higher SA:V ratios than bulk material so have a greater proportion of particles exposed at the surface making them highly reactive
121
What can gold nanoparticles be used for?
To catalyse some chemical reactions
122
What are carbon nanotubes?
cylindrical fullerenes with very high length to diameter ratios
123
Properties of carbon nanotubes
High tensile strength due to many strong covalent bonds through its structure
High thermal and electrical conductance
124
Why are nanoparticles harmful ?
Some may be able to penetrate cell membranes to enter cells
May breathe some in then they may catalyse reactions that are harmful
Toxic substances could bing to them due to large SA:V
125
properties of ionic compounds
-brittle
-high melting points and boiling point
-electrically conductive
126
Properties of simple molecules
Low melting and boiling points
127
Properties of giant covalent structures
- Very high melting and boiling points
- Only graphite conducts electricity
128
Properties of polymers
High melting and boiling points
129
properties of metallic bonds
malleable and ductility
Soft
high thermal and electrical conductivity
High melting and boiling points
130
Properties of alloys
-melting point lower than that of components
-harder than metals that compose it
