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Chemistry 9-1 iGCSE Oxford AQA > Structure, Bonding & Properties of Matter > Flashcards

Structure, Bonding & Properties of Matter Flashcards

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1
Q

How are ions made?

A

Made when electrons are transferred

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2
Q

What are ions?

A

Charged particles

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3
Q

When atoms lose or gain electrons to form ions, what are they trying to do?

A

To get a full outer shell (stable electronic structure)

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4
Q

When metals form ions, what happens to their electrons and what type of ions do they form?

A

They lose electrons from their outer shell to form positive ions

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5
Q

When non-metals form ions, what happens to their electrons and what type of ions do they form?

A

They gain electrons into their outer shell to form negative ions

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6
Q

What does the charge on the ion represent?

A

Number of electrons lost or gained

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7
Q

Explain ionic bonding

A
  1. Non-metal gains electrons = negatively charged ion
  2. Metal atom loses electrons = positively charged ion
  3. Opposite charged ions are strongly attracted to one another by electrostatic forces
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8
Q

What the structure of an ionic compounds called?

A

Giant ionic lattice

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9
Q

How ions arranged in a giant ionic lattice? (forces?)

A

They’re closely packed with very strong electrostatic forces of attraction between oppositely charged ions - in all directions

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10
Q

Name 3 properties of ionic compounds

A
  1. High melting points
  2. High boiling points
  3. Dissolve easily in water
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11
Q

When ionic compounds melt, what can they do and why?

A

Carry electric current bc ions are free to move

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12
Q

Why do ionic compounds have high melting/boiling points?

A

Due to MANY strong bonds between ions = takes a lot energy to overcome this attraction (electrostatic forces)

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13
Q

Draw the structure of sodium chloride

A

See mind map

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14
Q

What is covalent bonding?

A

When non-metals bond together: share a pair of electrons to make covalent bonds

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15
Q

Why are covalent bonds very strong?

A

Positively charged nuclei of bonded atoms are attracted to the shared pair of electrons by electrostatic forces

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16
Q

Atoms only share electrons in their…

A

outer shells (highest energy levels)

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17
Q

What does each covalent bond provide for each atom?

A

1 extra shared electron

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18
Q

Atom involved generally makes enough covalent bonds…

A

to fill up its outer shell

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19
Q

Draw the covalent bonds for water

A

See mind map

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20
Q

Draw the covalent bonds for water in this form Cl-Cl

A

See mind map

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21
Q

Draw the covalent bonds for ammonia

A

See mind map

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22
Q

Draw the covalent bonds for ammonia in this form Cl-Cl

A

See mind map

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23
Q

Draw the covalent bonds for hydrogen

A

See mind map

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24
Q

Draw the covalent bonds for hydrogen in this form Cl-Cl

A

See mind map

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25
Q

Draw the covalent bonds for hydrogen chloride

A

See mind map

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26
Q

Draw the covalent bonds for hydrogen chloride in this form Cl-Cl

A

See mind map

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27
Q

Draw the covalent bonds for methane

A

See mind map

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28
Q

Draw the covalent bonds for methane in this form Cl-Cl

A

See mind map

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29
Q

Draw the covalent bonds for oxygen

A

See mind map

30
Q

Draw the covalent bonds for oxygen in this form Cl-Cl

A

See mind map

31
Q

Usually substances containing covalent bonds, have what kind of structure?

A

Simple molecular structures

32
Q

For covalent compounds with a simple molecular structures, what the intramolecular forces like?

A

Very strong (covalent bonds)

33
Q

For covalent compounds with a simple molecular structures, what the intermolecular forces like?

A

Very weak (forces of attraction between molecules)

34
Q

Why do simple molecular substances have low melting/boiling points?

A

Feeble intermolecular forces need to be broken (NOT covalent bonds) = molecules are easily parted (little energy to overcome)

35
Q

What states are simple molecular substances at room temperature?

A

Most are gases or liquids

36
Q

Why is it that as a simple molecular substance gets larger, the melting/boiling points increases?

A

Strength of intermolecular forces increases = more energy needed to break them

37
Q

Why don’t simple molecular substances conduct electricity?

A

Because they aren’t charged = no free electrons or ions

38
Q

In giant covalent structures (macromolecules), how are all atoms bonded together?

A

By strong covalent bonds

39
Q

Why do macromolecules have very high melting/boiling points?

A

Lots of energy is needed to break covalent bonds between atoms

40
Q

Why don’t macromolecules conduct electricity?

A

Don’t contain charged particles = don’t conduct electricity (not even when molten)

41
Q

How many covalent bonds can carbon have?

A

4

42
Q

Why is diamond really hard?

A

Giant covalent structure - made up of carbon atoms that form four covalent bonds = makes it really hard

43
Q

Why does diamond have a really high melting point?

A

Strong covalent bonds take a lot of energy to break

44
Q

Why doesn’t diamond conduct electricity?

A

Because it has no free electrons/ions

45
Q

Describe the structure of graphite

A

Carbon atoms forms three covalent bonds = creating sheets of carbon atoms arranged in hexagons

46
Q

Why is graphite an ideal lubricating material?

A
  1. Aren’t any covalent bonds between layers - only held together with weak forces
  2. Layers can slide over each other = graphite slipperily
47
Q

Why doe graphite have a high melting point?

A

Covalent bonds in layers need a lot of energy to break

48
Q

Why can graphite conducts electricity and thermal energy?

A

Only three out of each carbon’s four outer electrons are used in bonds = carbon atoms has one electron that’s delocalised (free) and can move THROUGH whole structure

49
Q

What is graphene?

A

Sheet of carbon atoms joined together in hexagons (sheet is one atom thick)

50
Q

What do metals consist of?

A

Giant structures of atoms arranged in a regular pattern

51
Q

Explain metallic bonding

A
  1. Electrons in outer shell are delocalised
  2. Strong forces of electrostatic attraction between the positive metal ions and shared negative electrons
  3. These forces of attraction hold the atoms together in a regular structure (known as metallic bonding)
52
Q

What produces the properties of metals?

A

Delocalised electrons in metallic bonds

53
Q

What does the condition of a metal depend on?

A

The ability of electrons to move through the metal

54
Q

Why are metals malleable?

A

Layers of atoms can slide over each other

55
Q

Why are metals solid at room temperature?

A

Electrostatic forces between metal atoms and delocalised electrons are very strong - lots of energy needed to broken
∴ Most have very high melting and boiling points

56
Q

Why are metals a good conductor of electricity and heat?

A

Delocalised electrons carry electrical current and thermal

energy through whole structure

57
Q

What are intermolecular forces?

A

Are forces that exist between molecules

58
Q

What are intramolecular forces?

A

Are the forces that hold atoms together within a molecule

59
Q

What are fullerenes?

A

Molecules of carbon, shaped like closed tubes or hollow balls

60
Q

What is the structure of fullerene like?

A

Made up of hexagon rings of carbon atoms

61
Q

What can fullerenes be used for? Name 4 things

A
  1. Deliver a drug into body
  2. Catalysts
  3. Lubricants
  4. Nanotubes
62
Q

How can fullerenes be used to deliver a drug into body?

A

They ‘cage’ other molecules = structure forms around another atom/molecule

63
Q

How can fullerenes be used as catalysts?

A

Individual molecules could be attached to fullerenes

64
Q

Why would fullerenes help make great industrial catalysts?

A

Because they have a large surface area

65
Q

Name 3 properties of nanotubes

A
  1. Ratio between length and diameter of nanotubes = very high
  2. Have high tensile strength (don’t break when stretched)
  3. Conduct both electricity and thermal energy
66
Q

What can nanotubes be used for? Name 2 things

A
  1. In electronics

2. Strengthen materials without adding much weight E.g. tennis racket frames

67
Q

How large a nanoparticles? (length and no. of atoms)

A

1-100nm, contain only a few hundred atoms

68
Q

Nanoparticles have a…

A

Large surface area to volume ratio

69
Q

As particles decrease in size…

A

size of surface area increases in relation to their volume

70
Q

What can having large surface area to volume ratio cause for nanoparticles?

A

For them to have different properties for the same material in bulk

71
Q

Why are some people worried about products containing nanoparticles?

A

Bc they’ve been made available before effects on human health have been investigated properly = we don’t know long term impacts on health will be

Chemistry 9-1 iGCSE Oxford AQA (11 decks)

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