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GCSE AQA Chemistry 9-1 > C3 Structure and Bonding > Flashcards

C3 Structure and Bonding Flashcards

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1
Q

What is an ion?

A

A charged particle when an atom loses or gains electrons

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2
Q

What happens when metals form ions?

A

They lose electrons to form positive ions

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3
Q

What happens when nonmetals form ions?

A

They gain electrons to form negative ions

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4
Q

What happens in ionic bonding?

A

When a metal and nonmetal react together the metal atom transfers electrons to the nonmetal forming a positive metal ion and negative nonmetal ion. These particles are strongly attracted by electrostatic forces

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5
Q

What do groups one and two lose in ionic bonding?

A

Electrons to form positive ions

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6
Q

What do groups six and seven gain in ionic bonding?

A

Electrons to form negative ions

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7
Q

What is the structure of ionic compounds?

A

A giant ionic lattice
Ions form closely packed regular lattice with very strong electrostatic forces of attraction between the oppositely charged ions in all directions.

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8
Q

What are the properties of ionic compounds?

A

High melting points and boiling points due to the strong bonds
When solid they cannot conduct electricity
When they melt they can carry electric charge
Some dissolve easily so can carry electric charge

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9
Q

Why can solid ionic structures not carry electric current?

A

The ions are held in place so cannot conduct electricity

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10
Q

What is covalent bonding?

A

When nonmetals bond together and share pairs of electrons

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11
Q

What are some limits of drawing covalent bonds?

A

In dot and cross diagram you cannot see the relative size of the atom or how it is arranged in space
In displayed formulas you cannot see the 3-D structure or where electrons come from
3D models can get confusing with large molecules

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12
Q

What are some properties of simple molecular substances that are covalently bonded?

A

They have strong covalent bonds but weak intermolecular forces
Melting and boiling points are very low as the intermolecular forces are weak
Larger molecules have stronger intermolecular forces so the melting and boiling points of these molecules increases
They do not conduct electricity as they are not charged

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13
Q

What is a polymer?

A

A long chain molecule that is formed by joining lots of small molecules (monomers) together

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14
Q

What state are polymers at room temperature and why?

A

Solid as polymers have larger intermolecular forces so more energy is needed to break them apart

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15
Q

Why are the boiling points of polymers lower than ionic or giant molecular compounds?

A

The intermolecular forces are weaker than ionic or covalent bonds

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16
Q

What is the structure of a giant covalent structure?

A

All atoms are bonded to each other by strong covalent bonds

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17
Q

What are the properties of giant covalent structures?

A

They have very high melting and boiling points
They don’t conduct electricity

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18
Q

What is an allotrope?

A

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

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19
Q

What is the structure of diamond?

A

Each carbon atom is bonded to 4 other carbon atoms with covalent bonds

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20
Q

Why does diamond have a very high melting point?

A

Strong covalent bonds take a lot of energy to break

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21
Q

Why does diamonds not conduct electricity?

A

There are no free ions

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22
Q

What is the structure of graphite?

A

Each carbon atom is covalently bonded to 3 other carbon atoms.
There is one delocalised electron.
There are no covalent bonds between layers so they are free to move over each other

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23
Q

What are the properties of graphite?

A

Graphite is soft
It has a high melting point
It conducts electricity and Thermal energy

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24
Q

What is graphene?

A

A sheet of carbon atoms join together in hexagons
It is just one atom thick

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25
Q

What are the properties of graphene?

A

It is very strong and light
It conducts electricity through the whole structure

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26
Q

What are fullerenes?

A

Molecules of carbon shaped like closed tubes or hollow balls

27
Q

What is the structural arrangement of fullerenes?

A

Mainly arranged and hexagons but also pentagons and heptagons

28
Q

What can fullerenes be used for?

A

Deliver drugs
Industrial catalysts
Lubricants
Electronics
Strength and composite materials

29
Q

what are the three common states of matter?

A

solids
liquids
gases

30
Q

what are the properties of solids?

A

hard to compress - particles are packed together in a regular pattern with no spaces
fixed shape and cannot flow - particles cannot move from place to place

31
Q

what are the properties of liquids?

A

hard to compress - particles are close together with not many spaces
take the shape of a container + can flow - particles can move

32
Q

what are the properties of gases?

A

easy to compress - widely spaced particles
spread out and fill container - particles move quickly and randomly

33
Q

how can you change the state of a substance?

A

put in or take away energy

34
Q

what happens when a substance changes from a solid to a liquid? (or a liquid to a gas)

A

energy is put into the solid (liquid)
this breaks the forces of attraction between the particles in the solid (liquid)
allowing the particles to move around

35
Q

what causes a melting point/boiling point to be higher?

A

the stronger the forces of attraction between the particles, the greater amount of energy needed to break them

36
Q

what are the limitations of the particle model?

A

it assumes all particles are solid spheres - particles actually have different shapes and are not solid
it is assumed that there are no forces in between the particles

37
Q

what types of elements does ionic bonding ivolve?

A

metals and non-metals

38
Q

why do small covalent molecules have low melting and boiling points?

A

they have weak intermolecular forces between the the molecules which do not require a lot of energy to break

39
Q

why are giant covalent molecules solid at room temperature?

A

they have millions of strong covalent bonds so they have high melting and boiling points

40
Q

what is diamond formed from?

A

carbon

41
Q

Can diamonds conduct electricity? why? why not?

A

no
there are no free electrons to carry the charge

42
Q

why does silicon dioxide have high melting and boiling points?

A

there are a huge number of strong covalent bonds which take a lot of energy to break

43
Q

what are the properties of carbon nanotubes?

A

they have high tensile strength
good conductors

44
Q

what is the difference between the bonding of a monomer and a polymer?

A

the monomer has a double carbon to carbon bond
the polymer has single carbon to carbon bonds

45
Q

what are some key facts about repeating units of polymers?

A

only one carbon to carbon bond
the bonds on either side of the molecule have to extend out of the brackets
the n represents a large number

46
Q

how are atoms in metals arranged?

A

giant structures in regular layers

47
Q

what is metallic bonding?

A

the strong electrostatic attraction between the ‘sea’ of negative delocalised electrons and the positive metal ions

48
Q

why do metals have high melting and boiling points?

A

it takes a lot of energy to break the metallic bonds

49
Q

why are metals good conductors of heat and electricity?

A

the delocalised electrons can move and transfer energy

50
Q

why are metals malleable?

A

the layers of atoms are able to slide over each other

51
Q

what is an alloy?

A

a mixture of metals?

52
Q

why are alloys harder than pure metals?

A

they different sizes of atoms distorts the layers, making it more difficult for them to slide over each other

53
Q

what is the size of a micrometre in metres?

A

1 x 10^-6

54
Q

what is the size of a nanometre in metres?

A

1 x 10^9

55
Q

what is the size of coarse particles (PM10 or dust)?

A

1 x 10^-5 to 2.5 x 10^-6 metres

56
Q

what is the diameter of fine particles?

A

100 to 2500 nanometres
or
1 x 10^-7 to 2.5 x 10^-6 metres

57
Q

what is the diameter of nanoparticles?

A

1 - 100 nanometres

58
Q

how many atoms do nanoparticles contain?

A

only a few hundred atoms

59
Q

what happens to the surface area : volume ratio when the size of the particle falls?

A

as the size of the particle decreases by 10 times, the surface area : volume ratio increases by 10 times

60
Q

why do you need a much smaller amount of nanoparticles compared to materials with normal particle sizes?

A

nanoparticles have a huge surface area to volume ratio so even a small amount of nanoparticles have a massive surface area

61
Q

what are some uses of nanoparticles?

A

medicines
cosmetics
suncreams
deodorants
electronics
catalysts

62
Q

what are some uses of nanoparticles?

A

medicines
cosmetics
suncreams
deodorants
electronics
catalysts

63
Q

what are some risks of nanoparticles?

A

it is possible they can be absorbed into the body and enter the cells

64
Q

what is an advantage of dot and cross diagrams?

A

it is clear where the electrons of each atom comes from as they are represented by dots and crosses

GCSE AQA Chemistry 9-1 (16 decks)

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