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

Bonding, Structure and Properties of Matter Flashcards

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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
Q

Are giant Covalent bonds gases or Solids at room temperature?

A

Always solids at room temperature

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26
Q

What element is Diamond formed from?

A

Carbon

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27
Q

In diamond how many Covalent bonds are made from one carbon atoms

A

4 Covalent bonds

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28
Q

Why do diamonds have high melting and boiling points?

A

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
Q

Why cant Diamonds conduct electricity?

A

This is because there are no free electrons to carry a charge.

30
Q

What elements do Silicon dioxide have?

A

Silicon and Oxygen which have been Covalently bonded together.

31
Q

In Silicon dioxide how many Covalent bonds are made from one carbon atoms

A

One giant structure

32
Q

What is Silicon dioxide?

A

Sand is made from it.

33
Q

In Graphite how many Covalent bonds are made from one carbon atoms

A

three Covalent bonds .

34
Q

Name 3 properties of Graphite.

A

Have melting and boiling points.
It is soft and slippery
Great conductors of heat and electricity

35
Q

What do the carbon atoms in Graphite form.

A

Hexagonal rings

36
Q

Why does Graphite have high melting and boiling points

A

They have many strong covalent bonds so it takes a great deal of energy to break the bonds.

37
Q

Why is Graphite slippery?

A

They have hexagonal rings in layers which have no covalent bonds in between them so they can slide and be slippery.

38
Q

Why is Graphite great conductors of Electricity and Heat?

A

They have delocalised electrons that can move.

39
Q

What is Graphene?

A

It is a single layer of graphite and is one atom thick.

40
Q

Name 2 properties of Graphene

A

Good conductors of electricity.

Extremely strong.

41
Q

Why are Graphene good conductors of electricity?

A

Because they have delocalised electrons that can move.

42
Q

What can Graphene be used for?

A

It can be added to composite materials to improve strength without adding too much weight.

43
Q

What are fullerenes?

A

Molecules of carbon atoms which are shaped like closed tubes or hollow balls.

44
Q

How are Carbon atoms in fullerenes usually arranged?

A

In hexagons or sometimes in pentagons(rings of five carbon atoms) or heptagons (rings of 7 carbon atoms)

45
Q

What was the first fullerene to be Discovered?

A

Buckministerfullerene

46
Q

How many carbon atoms do fullerenes contain

A

60 carbon atoms

47
Q

Name 2 uses of Fullerenes

A

Lubricants

Catalysts

48
Q

Name one group of Fullerenes.

A

Carbon nanotubes

49
Q

What are Carbon nanotubes?

A

Fullerenes shaped into long cylinders.

50
Q

Name 2 properties of Carbon nanotubes.

A

Excellent conductors of electricity

have high tensile strength (stretched without breaking)

51
Q

Name one use of Carbon nanotubes

A

To reinforce materials like Tennis rackets

52
Q

What are Polymers?

A

Are very long molecules of of repeating units joined by strong covalent bonding.

53
Q

What is it called when scientists draw draw long polymers in a short hand way?

A

Repeating unit

54
Q

Are polymers Solids or gases at room temperature?

A

Solids

55
Q

Name 2 properties of Polymers.

A

High melting points

Lower boiling points

56
Q

Why do Polymers have High melting points?

A

This is because the Intermolecular forces between each polymer atom are strong so it requires a lot of energy to break the bonds.

57
Q

What is Metallic bonding?

A

The bonding between electrostatic attraction between a lattice of positive metal ions and a sea of decoliased electrons

58
Q

Are metallic bonds weak or strong?

A

Strong

59
Q

Why are do Metals have high melting and boiling points?

A

This is because it requires a lot of energy to break the bonds.

60
Q

Why are metals good conductors of heat and electricity?

A

This is because the decoliased electron can move carrying electrical current and heat energy.

61
Q

Why are metals malleable?

A

This is because in metals the layers of atoms are able to slide over each other.

62
Q

What is a Alloy?

A

a mixture of metals

63
Q

Why are Alloys harder than pure metals?

A

The different size of atoms changes the length of the layers making it more difficult for them to slide over each other.

64
Q

3 Features of Solids?

A

Fixed shape
Strong forces of attraction
The particles vibrate about their positions

65
Q

3 Features of Liquids?

A

Weaker forces of attraction
Fixed volume/ Randomly arranged
No fixed shape

66
Q

3 features of Gases?

A

No forces of Attraction
No fixed shape or volume
Move randomly.

67
Q

If the temperature is below its melting point of a substance is it a solid liquid or gas?

A

Solid

68
Q

If the temperature is above the boiling point of a substances is it a liquid solid or gas?

A

Gas

69
Q

If the temperature is between its melting and boiling point of a substance is it a solid liquid or gas?

A

Liquid

Chemistry C1-C6 revision (14 decks)

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