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Chemistry C1-C6 revision > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

1
Q

What are Ions?

A

They are Atoms with a Charge

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2
Q

What Ions do Metals make?

A

Positive ions

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3
Q

What Ions do Non-Metals make?

A

Negative ions

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4
Q

Atoms with full outer shells are what?

A

Very stable

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5
Q

What is Ionic bonding?

A

An electrostatic attractions between oppositely charged ions.

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6
Q

Why are atoms neutral?

A

Because they have the same number of protons and electrons

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7
Q

What do many ionic compounds form?

A

salts

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8
Q

What do Ionic Compounds form?

A

Giant ionic lattice structures where every postie ion is surrounded by every negative ions.

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9
Q

What do Giant ionic lattices have?

A

They have strong forces electrostatic of attraction between negative and positive charged ions in all directions in the lattice.

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10
Q

Name two Properties of Ionic compounds

A

Have very high melting and boiling points

Cannot conduct electricity when solids

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11
Q

Why do Ionic compounds have High melting and boiling points?

A

The strong electrostatic forces require a great deal of energy to break.

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12
Q

Why cant ionic compounds conduct electricity when solids?

A

This is because ions cannot move and they are locked together in place by strong electrostatic forces forces of attraction.

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13
Q

Why can Ionic compounds conduct electricity when they are dissolved in water or melted?

A

This is because ions can move freely and carry a charge.

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14
Q

What is a covalent bond?

A

When non-metals react together to share electrons.

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15
Q

Give an example of a Small covalent bond?

A

Oxygen

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16
Q

What are the two properties of small covalent bonds?

A

Have low melting and boiling points

Doesn’t conduct electricity

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17
Q

Why do small covalent bonds have low melting and boiling points?

A

The weak intermolecular forces between the molecules do not require a lot of energy to break

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18
Q

Do Small covalent bonds have strong Covalent bonds?

A

Yes

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19
Q

Why can’t small covalent bonds conduct electricity?

A

This is because the molecules do not have an overall electric charge.

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20
Q

Are small covalent bonds gas at room temperature?

A

Yes

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21
Q

Name 2 properties of Giant covalent bonds?

A

Very high melting and boiling points

Don’t conduct electricity

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22
Q

Why do Giant covalent bonds have very high melting and boiling points?

A

They have millions of strong covalent bonds so a lot of heat energy is required to break the covalent bonds.

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23
Q

Why cant Giant covalent bonds conduct electricity?

A

This is because the molecules do not have an overall electric charge, not even when they are molten.

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24
Q

Name 3 examples of Giant Covalent bonds.

A

Diamond, graphite and Silicon dioxide

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25
Are giant Covalent bonds gases or Solids at room temperature?
Always solids at room temperature
26
What element is Diamond formed from?
Carbon
27
In diamond how many Covalent bonds are made from one carbon atoms
4 Covalent bonds
28
Why do diamonds have high melting and boiling points?
They have a huge amount of carbon atoms joined by Covalent bonds which means it requires a lot of energy to break the bonds
29
Why cant Diamonds conduct electricity?
This is because there are no free electrons to carry a charge.
30
What elements do Silicon dioxide have?
Silicon and Oxygen which have been Covalently bonded together.
31
In Silicon dioxide how many Covalent bonds are made from one carbon atoms
One giant structure
32
What is Silicon dioxide?
Sand is made from it.
33
In Graphite how many Covalent bonds are made from one carbon atoms
three Covalent bonds .
34
Name 3 properties of Graphite.
Have melting and boiling points. It is soft and slippery Great conductors of heat and electricity
35
What do the carbon atoms in Graphite form.
Hexagonal rings
36
Why does Graphite have high melting and boiling points
They have many strong covalent bonds so it takes a great deal of energy to break the bonds.
37
Why is Graphite slippery?
They have hexagonal rings in layers which have no covalent bonds in between them so they can slide and be slippery.
38
Why is Graphite great conductors of Electricity and Heat?
They have delocalised electrons that can move.
39
What is Graphene?
It is a single layer of graphite and is one atom thick.
40
Name 2 properties of Graphene
Good conductors of electricity. | Extremely strong.
41
Why are Graphene good conductors of electricity?
Because they have delocalised electrons that can move.
42
What can Graphene be used for?
It can be added to composite materials to improve strength without adding too much weight.
43
What are fullerenes?
Molecules of carbon atoms which are shaped like closed tubes or hollow balls.
44
How are Carbon atoms in fullerenes usually arranged?
In hexagons or sometimes in pentagons(rings of five carbon atoms) or heptagons (rings of 7 carbon atoms)
45
What was the first fullerene to be Discovered?
Buckministerfullerene
46
How many carbon atoms do fullerenes contain
60 carbon atoms
47
Name 2 uses of Fullerenes
Lubricants | Catalysts
48
Name one group of Fullerenes.
Carbon nanotubes
49
What are Carbon nanotubes?
Fullerenes shaped into long cylinders.
50
Name 2 properties of Carbon nanotubes.
Excellent conductors of electricity | have high tensile strength (stretched without breaking)
51
Name one use of Carbon nanotubes
To reinforce materials like Tennis rackets
52
What are Polymers?
Are very long molecules of of repeating units joined by strong covalent bonding.
53
What is it called when scientists draw draw long polymers in a short hand way?
Repeating unit
54
Are polymers Solids or gases at room temperature?
Solids
55
Name 2 properties of Polymers.
High melting points | Lower boiling points
56
Why do Polymers have High melting points?
This is because the Intermolecular forces between each polymer atom are strong so it requires a lot of energy to break the bonds.
57
What is Metallic bonding?
The bonding between electrostatic attraction between a lattice of positive metal ions and a sea of decoliased electrons
58
Are metallic bonds weak or strong?
Strong
59
Why are do Metals have high melting and boiling points?
This is because it requires a lot of energy to break the bonds.
60
Why are metals good conductors of heat and electricity?
This is because the decoliased electron can move carrying electrical current and heat energy.
61
Why are metals malleable?
This is because in metals the layers of atoms are able to slide over each other.
62
What is a Alloy?
a mixture of metals
63
Why are Alloys harder than pure metals?
The different size of atoms changes the length of the layers making it more difficult for them to slide over each other.
64
3 Features of Solids?
Fixed shape Strong forces of attraction The particles vibrate about their positions
65
3 Features of Liquids?
Weaker forces of attraction Fixed volume/ Randomly arranged No fixed shape
66
3 features of Gases?
No forces of Attraction No fixed shape or volume Move randomly.
67
If the temperature is below its melting point of a substance is it a solid liquid or gas?
Solid
68
If the temperature is above the boiling point of a substances is it a liquid solid or gas?
Gas
69
If the temperature is between its melting and boiling point of a substance is it a solid liquid or gas?
Liquid

Chemistry C1-C6 revision (14 decks)

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