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Pro Chem > C3 > Flashcards

C3 Flashcards

1
Q

Why are solids hard to compress?

A
  • The particles are packed together in a regular pattern with no space between them
  • Have a fixed shape and cannot flow from place to place
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2
Q

Why can’t solids move from place to place?

A

The particles can vibrate but not move

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3
Q

Why are liquids hard to compress?

A

Particles are close together with no space between them

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4
Q

Why are gases easy to compress?

A

The particles in a gas are widely spread and fill the spaces of the container

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5
Q

How do gases move?

A

Quickly and randomly

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6
Q

How can you change the state of a substance?

A

Putting in or taking out energy

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7
Q

What do you have to do to convert a solid to a liquid?

A

Put energy in as the particles in a liquid move. The energy is used to break the forces of attraction

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8
Q

What does stronger the forces of attraction mean?

A

More energy needed to break them and higher the melting point

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9
Q

Why do substances have low boiling points?

A

Have low forces of attraction

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10
Q

How do you turn gas into a liquid?

A

Condense

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11
Q

What are the limitations of the simple particle model?

A
  • All particles are solid spheres
  • No forces between particles
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12
Q

Why do elements react?

A

To form a full outer energy level

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13
Q

What is ionic bonding?

A

When a metal reacts with a non metal

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14
Q

What do ionic compounds form?

A

Giant structures

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15
Q

What are giant ionic lattices?

A

When negative ios are surrounded by positive ions

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16
Q

What are electrostatic forces?

A

Giant ionic lattices have strong forces of attraction between positive and negative ions

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17
Q

What are ionic bonds?

A

Electrostatic forces that hold negative and positive ions together

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18
Q

Facts about ionic compounds?

A
  • Have high melting and boiling points
  • Cannot conduct electricity when solids
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19
Q

Why do ionic compounds have high melting and boiling points?

A

The electrostatic forces require a lot of heat energy to break

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20
Q

Why can’t ionic compounds conduct electricity?

A

Ions cannot move and locked in strong electrostatic forces of attraction

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21
Q

When can ionic compounds conduct electricity?

A

Melted or dissolved in water (the ions can move and carry the charge)

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22
Q

What are facts about ionic compounds?

A
  • Form giant structures where every positive ion is surrounded by negative ions
  • Giant ionic lattices have strong forces of attraction (electrostatic forces)
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23
Q

What is covalent bonding?

A

Sharing electrons

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24
Q

When does covalent bonding happen?

A

Between non metal elements

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25
Q

Properties of small covalent molecules?

A

Have low melting and boiling points (usually gases or liquids at room temp)

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26
Q

Why do small molecules have low melting and boiling point?

A
  • atoms are held by strong covalent bonds
  • Very weak forces between intermolecular forces
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27
Q

What does intermolecular mean?

A

Betwen forces

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28
Q

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

A

Weak intermolecular forces and does not require a lot of energy to break

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29
Q

Why is it when alkanes get larger the boiling point increases?

A

The intermolecular forces increase and require more energy

30
Q

Why do small covalent molecules not conduct electricity?

A

Molecules do not have an overall electric charge

31
Q

Facts about giant covalent molecules?

A

Always solid at room temperature

32
Q

Why do giant covalents always have high melting and boiling points?

A

Millions of strong covalent bonds

33
Q

How is diamond formed?

A

From carbon

34
Q

How is diamond formed?

A

Each carbon atom forms 4 strong covalent bonds

35
Q

Why does diamond have a high melting point?

A

It has a lot of carbon covalent bonds so requires a lot of energy

36
Q

Why can’t diamond conducts electricity?

A

No free electrons to carry out electrical charge

37
Q

Why does silicone dioxide have a high melting and boiling point?

A

Huge number of strong covalent bonds must be broken and requires energy

38
Q

Graphite properties?

A
  • High melting and boiling point
  • Soft and slippery
  • Great conductor for electricity and heat
39
Q

How is graphite formed?

A

Element carbon and forms 3 covalent bonds from hexagonal rings

40
Q

Why does graphite have a high boiling and melting point?

A

Has strong covalent bonds

41
Q

Why is graphite slippery?

A

No covalent bonds between layers so they can slide

42
Q

What can delocalised electrons do?

A

Conduct heat and electricity

43
Q

Why is graphite not a metal?

A

Based on element carbon

44
Q

Why is graphite a good conductor to heat and electricity?

A

Have delocalised electrons which can move

45
Q

What is graphene?

A

A single layer of graphite
One atom thick

46
Q

Graphene properties?

A
  • Good conductor of electricity
  • Very strong
47
Q

Why is graphene a good conductor of electricity?

A

It has delocalised electrons

48
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes

49
Q

How are fullerenes formed?

A

Hexagonal rings of carbon atoms

50
Q

Whats c60?

A

Buckminsterfullerene

51
Q

What are the uses of fullerenes?

A
  • Pharmaceutical delivery
  • Lubricants
  • Catalysts
52
Q

Carbon nanotubes properties?

A
  • High strength and can be stretched
  • Excellent conductors of heat and electricity
53
Q

Uses of carbon nanotubes?

A

Reinforce materials eg tennis rackets

54
Q

How are polymers made?

A

Joining thousands of small identical molecules

55
Q

What are monomers?

A

Alkene molecules

56
Q

Why are most polymers solids at room temperature?

A

The intermolecular forces between polymers are strong

57
Q

What are the electrons on the outer energy level of a metal?

A

Delocalised

58
Q

Whats between the sea delocalised electroms and positive metal ions?

A

Strong electrostatic attraction

59
Q

Whats a metallic bond?

A

Electrostatic bond in metals

60
Q

Why are metals great conductors of heat?

A
  • Delocalised electrons can move
  • Charged metals carry electricity
61
Q

Why can metals be bent and shaped?

A

Able to slide over each other

62
Q

Metal properties?

A
  • Bent and shapes
  • Good heat and electricty conductors
63
Q

What is an alloy?

A

A mixture of metals

64
Q

How are alloys harder than metals?

A

Different sizes of atoms distorts the layers making it harder to slide over

65
Q

What is a micrometer?

A

1 x 10-6

66
Q

What is a nanometer?

A

1 x 10-9

67
Q

Coarse particle diameter?

A

1x10-5 and 2.5 x 10-6

68
Q

What is the diameter of nano particles?

A

1 -100 nanometeres
Contain few hundred atoms

69
Q

What happens when particle size decreases 10 times?

A

SA - VR increases 10 times

70
Q

Uses of nanoparticles?

A
  • Medicines
  • Suncreams
  • Cosmetics
  • Deodrants
  • Electronics
  • Catalysts
71
Q

Risks of nanoparticles?

A
  • can be absorbed by our body and enter our cells
  • No one knows long term effects

Pro Chem (11 decks)

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