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Structure and bonding Flashcards

1
Q

Electrostatic forces

A

Force between the oppositely charged particles
which causes covalent and ionic bonds to be strong.

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2
Q

Intermolecular forces

A

Force between each simple covalent molecule. When broken, doesn’t break the bonds but causes a change in state.

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3
Q

Ionic compounds - what melting + boiling points and why?

A

High
Because the oppositely charged ions are held together by strong electrostatic forces
It takes a lot of energy to break these forces between ions
So it has a high melting point so solid at room temperature

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4
Q

Ionic compounds - do they conduct electricity and why?

A

Only when dissolved in water or molten
Because it has a giant ionic lattice structure
When it is solid the ions are in a fixed place and cannot move
Therefore they cannot carry a charge
When melted or dissolved the ions are free to move
So they can therefore carry a charge

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5
Q

Why are covalent bonds strong?

A

Both the nucleus in each atoms (positive) is strongly attracted to the shared electrons in the outer shell (negative).
So electrostatic attraction

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6
Q

Simple molecules - what melting and boiling points and why?

A

Low
Because it has weak intermolecular forces
Little energy is needed to overcome these weak forces
So it has a low boiling point and is a gas at room temperature

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7
Q

Simple molecules - do they conduct electricity and why?

A

No
It has no delocalised electrons or ions
So has no particles to carry a charge

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8
Q

What is a giant covalent structure?

A

Millions of atoms joined together by covalent bonds that are arranged in a lattice shape.

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9
Q

Do giant covalent structures have high or low boiling/melting points? Why?

A

Very high
Because it has a giant covalent structure
With millions of covalent bonds between the many atoms
So a lot of energy is needed to overcome their strong covalent bonds
So has high melting/boiling point and a solid at room temperature

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10
Q

Metallic bonding

A

Bonding in metal elements due to sea of delocalised electrons moving
And the electrostatic attraction between the electrons and positive metal ions

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11
Q

Do metal bonds conduct electricity?

A

Yes
They have a giant metallic lattice structure
So has delocalised electrons
That can move through a structure carrying a charge

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12
Q

Do metal bonds have high or low melting/boiling points?

A

High
Have a giant metallic lattice structure
The positive metal ions are held together by delocalised electrons
This strong electrostatic attraction takes a lot of energy to overcome and pull the ions apart
So have a high melting point

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13
Q

Are metal bonds soft?

A

Yes, because the metal atoms are arranged in layers so when a force is applied they slide over each other

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14
Q

Alloy

A

Mixture of 2 or more elements, where at least one is a metal. Usually 2 metals in order to increase hardness of pure metals.

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15
Q

Why are alloys harder than pure metals?

A

Many different sized atoms due to multiple elements so greater force needed to make layers slide over each other
The layers are DISTORTED

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16
Q

What bonding forms giant structures?

A

All 3: giant ionic lattices, giant covalent structures and giant metallic structures

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17
Q

Polymer

A

A large molecule made up of many small units (monomers)

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18
Q

Are the bonds between atoms in a polymer weak or strong?

A

Strong because it’s joined by covalent bonds which are strong

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19
Q

What holds ionic compounds together?

A

Electrostatic forces

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20
Q

How can metals and graphite conduct electricity?

A

Because they both have delocalised electrons that can conduct heat

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21
Q

Fullerene

A

Molecules of carbon atoms with hollow shapes
Normally made out of hexagonal rings

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22
Q

Are ionic compounds molecules?

A

No because a molecules is 2 or more atoms held together by COVALENT bonds

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23
Q

What forms graphite?

A

Carbon atom covalently bonded to 3 other carbon atoms
In hexagonal rings
Then large rings are in layers with no bonds between

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24
Q

Properties of graphite

A

High melting and boiling point
Soft and slippery
Good conductor of heat and elec

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25
Why does graphite have high melting and boiling points?
It takes a lot of energy to break covalent bonds
26
Why is graphite slippery?
The hexagonal rings the carbon atoms are in are in layers No covalent bonds between the layers = they can slide Therefore it’s slippery
27
Why is graphite good conductor of heat and elec?
Because the C atoms form 3 other singular covalent bonds So has a spare electron that isn’t shared as carbon has 4 electrons in outer shell therefore there is one free electron Which is released in the outer shell To be delocalised and move between layers and conduct electricity
28
What makes up diamond?
4 carbon atoms covalently bonded with 4 other carbons Millions of these
29
Properties of diamond
High melting and boiling point Cannot conduct electricity
30
Why does diamond have high melting and boiling points?
Because it contains millions of carbon atoms covalently bonded To melt requires breaking these millions of bonds Which require a lot of energy
31
Why does diamond not conduct electricity?
It has no free electrons to carry electrical charge
32
What makes up silicon dioxide?
Silicon atom bonded covalently with 4 oxygen atoms Millions of these
33
Properties of silicon dioxide
Very high melting and boiling point
34
Why does silicon dioxide have high melting and boiling point?
Because it contains many covalent bonds that require a lot of energy to break
35
What makes up graphene?
Single layer of graphite Aka a layer of hexagonal rings of carbon atoms covalently bonded to 3 other carbon atoms
36
Properties of graphene
Only 1 atom thick Good conductor of elec Extremely strong
37
Why is graphene a good conductor of elec?
Because it is a giant covalent structure Each carbon atom forms 3 bonds This means there is 1 delocalised electron per carbon atom These delocalised electrons can move through the structure carrying a charge
38
Why is graphene strong?
Not in layers so can’t Slide Over each other
39
Fullerenes
Molecules of carbon atoms with hollow shapes
40
Buckminsterfullerene
Contains 60 carbon atoms in hollow sphere Can have a ring of 5 carbon atoms or 6 carbon atoms Each bonded 3 times
41
Fullerenes use
Delivery drugs into the body Lubricants to reduce friction Catalysts
42
Carbon nanotubes
Carbon rings forming a long hollow cylinder
43
Carbon nanotubes properties
Have high tensile strength Conduct electricity and heat
44
Carbon nanotubes uses
Reinforce materials
45
Polymer vs monomer
The monomer has a double carbon to carbon covalent bond Whereas the polymer has singular carbon to carbon bonds
46
Repeating unit
Short hand way of writing a polymer Has brackets around one section of the polymer (with its single carbon to carbon bond) and an n outside it The bonds extend outside the bracket
47
Why are polymers solid at room temperature?
Because the intermolecular forces of attraction between polymer molecules are quite strong Since they are arranged in layers It takes a lot of energy to break these many forces
48
Micrometer
1x10⁻⁶ of a Metre
49
Nanometre
1x10⁻⁹ of a metre
50
Coarse particles
Dust Have a diameter of between 2500 to 10000 nanometres Contain thousands of atoms
51
Coarse particles name
PM ₁₀
52
Fine particles name
PM2.5
53
Fine particles size
100 to 2500 nanometres Contain several thousand atoms
54
Nano particles
Diameter between 1-100 nanometre Only contain a few hundred atoms
55
Relationship between particles size and surface area:volume ratio
As it decreases by 10 times The surface area to volume ratio increases 10 times Aka the difference gets bigger between surface area and volume increases by x10
56
Nano particles surface area to volume ratio
Huge because they are the smallest So have a very large surface area compared to its volume So we don’t need many of them when using it
57
Uses of nano particles
Medicine Suncream Cosmetics Deodorant Electronics Catalysts
58
Risks of nano particles
Can be absorbed and enter our cells
59
Dot and cross diagram
Using dots and crosses to represent the electrons in different atoms when bonding
60
Advantage of dot and cross diagrams
Clear which electrons belong to which atom and where they are coming from
61
Stick diagram
Using one line to represent a covalent bond
62
Stick diagram disadvantage
Don’t tell us which electron came from where/which atom Don’t tell us about outer electrons not in a bond Don’t tell us shape of molecule
63
3d stick diagram
Uses dotted lines and thicker lines to show which bonds are closer and what direction
64
3d stick diagram advantages
Shows shape of molecule
65
Ball and stick diagram
Used for giant structures Where balls are ions and the sticks are bonds
66
Advantage of ball and stick diagram
Shows ions clearly in 3 dimensions
67
Ball and stick diagram disadvantage
Shows ions as widely spaced but in reality they are packed closely together Only shows a tiny part so give inaccurate sizing
68
Space filling diagram
Where the ions are shown as large balls in 3D with no sticks
69
Advantage of space filling diagrams
Shows how closely ions are packed together
70
Disadvantage of space filling diagram
Difficult to see how they’re 3D Only shows a tiny part of the lattice = inaccurate sizing
71
Disadvantage of a dot and cross diagram
Don’t tell us the shape of molecule

Chemistry (46 decks)

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