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AQA Chemistry GCSE > Bonding, Structure and Properties of matter > Flashcards

Bonding, Structure and Properties of matter Flashcards

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1
Q

What are ions?

A

charged particles

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2
Q

What is made when electrons are transferred?

A

ions

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3
Q

What happens when metals form ions?

A

They lose electrons from their outer shells to form positive ions.

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4
Q

What happens when non-metals form ions?

A

They gain electrons into their outer shells to form negative ions.

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5
Q

What charged ions do metals form?

A

positive

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6
Q

What charged ions do non-metals form?

A

negative

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7
Q

What is ionic bonding?

A

When a metal and non-metal react together. The metal loses electrons and the non-metal gains these electrons.

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8
Q

What are oppositely charged ions strongly attracted to one another by?

A

electrostatic forces of attraction

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9
Q

What is the attraction between oppositely charger ions called?

A

An ionic bond

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10
Q

What groups are most likely to form ions?

A

1&2 and 6&7

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11
Q

What are positive ions called?

A

cations

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12
Q

What are negative ions called?

A

Anions

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13
Q

Draw a dot and cross diagram for sodium chloride.

A

Your diagram should show:
Sodium loses 1 electron from its outer shell, forming a +1 charged ion.
Chlorine gains the electron into its outer shell, forming a -1 charged ion.

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14
Q

Draw a dot and cross diagram for magnesium chloride.

A

Your diagram should show:
Magnesium loses two electrons from its outer shell, forming a +2 charged ion. Each chlorine atom gains one electron into its outer shell forming a -1 charged ion.

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15
Q

What structures are ionic compounds?

A

Regular lattice structure/ giant ionic lattice

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16
Q

What are the properties of ionic compounds?

A

High melting and boiling points
(strong bonds means lots of energy needed to break them)

Can’t conduct electricity when solid

When melted, can carry electric current

Some dissolve easily in water

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17
Q

What two ways can ionic compounds conduct electricity?

A

When melted/molten
When dissolved in water

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18
Q

What is covalent bonding?

A

When non-metal atoms bond together, they share electrons.

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19
Q

True or false: Covalent bonds are weak.

A

False- covalent bonds are strong as the positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces.

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20
Q

Complete the sentence: Each single covalent bond provides _______ extra shared ______ for each atom.

A

one, electron

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21
Q

True or false : Covalent bonds fill up the atom’s outer shell making it very stable.

A

True

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22
Q

What are the different ways of drawing covalent bonds?

A
  • Dot and cross diagrams
  • Displayed formulas
  • 3D Models
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23
Q

What are the factors of a giant covalent structure?

A
  • High melting and boiling points
  • Don’t conduct electricity (no charged particles) except graphite
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24
Q

What type of structures do covalent bonds usually have?

A

simple molecular structures

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25
Q

In simple molecular structures, what are the atoms held together by?

A

very strong covalent bonds

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26
Q

How strong are the forces of attraction in simple molecular structures?

A

very weak

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27
Q

What are the properties of simple molecular structures?

A
  • Low melting and boiling points due to weak forces of attraction
  • mostly gases or liquids at room temp
  • As molecules get bigger, forces increase so melting and boiling points increase
  • Don’t conduct electricity
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28
Q

Give two examples of giant covalent structures.

A

Diamond and Graphite

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29
Q

What are the properties of diamond?

A
  • Strong covalent bonds so high melting and boiling point
  • Doesn’t conduct electricity
  • Very hard as each carbon atom forms 4 covalent bonds
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30
Q

How many covalent bonds does each carbon atom in diamond form?

A

4

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31
Q

Why does diamond not conduct electricity?

A

There are no free electrons (delocalised) or ions

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32
Q

How many covalent bonds does each carbon atom in graphite form?

A

3

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33
Q

What are the properties of graphite?

A
  • Soft & slippery
  • high melting point
  • good conductor of heat and electricity
34
Q

Why can graphite conduct electricity?

A

Each carbon atom only forms three covalent bonds, so each atom has one delocalised electron that is free to move. Therefore charge can flow so it conducts heat and electricity.

35
Q

Why is graphite slippery?

A

There aren’t any covalent bonds between the layers so they are weakly held together meaning they can move over each other.

36
Q

What is graphene?

A

A sheet of carbon atoms joined together in hexagons.

37
Q

What is a polymer?

A

Long chains of repeating units

38
Q

What are atoms in a polymer joined by?

A

Strong covalent bonds

39
Q

Do polymers have higher or lower boiling points than ionic compounds?

A

Low - weak intermolecular forces

40
Q

What state are most polymers at room temperature?

A

Solid- larger intermolecular forces than simple covalent molecules

41
Q

What are giant covalent structures?

A

All atoms are bonded to each other by strong covalent bonds.

42
Q

What are giant covalent structures also known as?

A

Macromolecules

43
Q

What are the properties of giant covalent structures?

A
  • Very high melting and boiling points
  • Don’t conduct electricity, except graphite
44
Q

What are allotropes?

A

Different structural forms of the same element in the same physical state.

45
Q

Give 3 examples of carbon allotropes.

A

Diamond, Graphite, Graphene

46
Q

What are fullerenes?

A

Molecules of carbon, shaped like closed tubes or hollow balls.

47
Q

In fullerenes, what are the carbon atoms typically arranged in?

A

hexagons but can contain pentagons or heptagons

48
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene

49
Q

Why can fullerenes be used in medicine?

A

They can be used to cage other molecules, this can be used to deliver a drug into the body.

50
Q

Why do fullerenes help to make good catalysts?

A

They have a huge surface area, individual catalyst molecules could be attached to them.

51
Q

Complete the sentence : Fullerenes make good l___________.

A

lubricants

52
Q

What can fullerenes form (tiny carbon cylinders)?

A

nanotubes

53
Q

What are nanotubes?

A

Tiny carbon cylinders

54
Q

What are the properties of nanotubes?

A
  • Conduct electricity and heat
  • High tensile strength
  • High ratio of length and diameter
55
Q

How can nanotubes be used in technology?

A

They can strengthen materials without adding much weight.

56
Q

What is the name of the technology involving nanotubes?

A

nanotechnology

57
Q

What is metallic bonding?

A

Bonding between two metals
Electrons in the outershell are delocalised

58
Q

What are the forces of attraction in metallic bonding?

A

Strong forces of electrostatic attraction between positive ions and negative electrons

59
Q

What are the properties of metals?

A
  • Solid at room temp
  • High melting and boiling points
  • Good conductors of electricity and heat
  • Malleable
60
Q

Why are most metals malleable?

A

The layers of atoms slide over each other.

61
Q

Why are alloys harder than pure metals?

A

Pure metals are often too soft. When pure metals are mixed with other elements, the layers of metal atoms are distorted making it more difficult for them to slide over each other.

62
Q

What is an alloy?

A

A mixture of two or more metals or a metal and another element.

63
Q

What are the three states of matter?

A

Solid, Liquid, Gas

64
Q

What does the state of something depend on?

A

How strong the forces of attraction are between the particles of the material.

65
Q

What does the strength of forces in an atom depend on?

A
  • The material (structure & bonds)
  • The temperature
  • The pressure
66
Q

Describe the structure of a solid.

A
  • Strong forces of attraction between particles
  • Fixed position forms a regular lattice arrangement
  • Definite shape and volume
  • Vibrate about their positions
67
Q

Describe the structure of liquids.

A
  • Weak forces of attraction
  • Randomly arranged and free to move
  • Definite volume but not definite shape
  • Constantly moving with random motion
68
Q

Describe the structure of gases.

A
  • Very weak forces of attraction
  • No definite shape or volume
  • Constantly moving with random motion
69
Q

Describe the change from a solid to a liquid.

A

Melting:
- Solid is heated, particles gain more energy
- Particles vibrate more, weakening the forces of attraction
- At the melting point, particles break free and form a liquid

70
Q

Describe the change from a liquid to a gas.

A

Boiling:
- Liquid is heated, particles gain more energy
- Particles move faster, weakens and breaks the bonds holding the liquid together
- At boiling point, particles break bonds forming a gas

71
Q

Describe the change from a gas to a liquid.

A

Condensing:
- As gas cools, particles lose energy so don’t have enough to overcome forces of attraction
- Bonds form between particles
- At boiling point, so many bonds have formed causing the particles to become a liquid

72
Q

Describe the change from a liquid to a solid.

A

Freezing:
- Particles have less energy so move around less
- Not enough energy to overcome forces of attraction
- At melting point, bonds have formed and are held in place, particles become a solid

73
Q

What are coarse particles?

A

Particles with a diameter between 2500nm and 10,000nm.
Also called dust.

74
Q

What are fine particles?

A

Particles with a diameter between 100nm and 2500nm.

75
Q

What are nanoparticles?

A

Particles with a diameter between 1nm and 100nm.

76
Q

List coarse particles, nanoparticles and fine particles in order of size. Start with the smallest.

A

Nanoparticles (1x10^-9m), Fine particles (1x10^-7m), Coarse particles (1x10^-5m)

77
Q

What do nanoparticles have?

A

A large surface area to volume ratio.

78
Q

What is the equation for surface area to volume ratio?

A

Surface area/ volume

79
Q

Give 5 uses of nanoparticles.

A
  • Catalysts
  • Nanomedicine
  • Electric circuits
  • Added to polymer fibres to make surgical masks, wound dressings and deodrants
  • Cosmetics
80
Q

True or false: Nanoparticles can conduct electricity.

A

True

81
Q

Why are some people against nanoparticles in health/medicine?

A

The effects aren’t fully understood yet.

AQA Chemistry GCSE (9 decks)

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