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Chemistry > C2 > Flashcards

C2 Flashcards

solid, liquid,gas not done dot& cross diagram

1
Q

(FSL) - what forces of attraction are in a giant ionic lattice?

A

strong electrostatic forces of attraction between positive and negative ions
- holds ions in place

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2
Q

(FSL) does ionic compounds have high or low mp/bp?

A

high

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3
Q

(FSL) what can move when ionic compounds can conduct electrcity?

A

ions NOT electrons

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4
Q

(FSL) do simple covalent molecules have high or low mp/bp?

A

low

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5
Q

(FSL) what bonds do small covalent molecules have? strong/weak?

A

strong covalent bonds BUT weak intermolecular forces of attraction between molecules

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6
Q

(FSL) what state are small covalent molecules at room temp?

A

gas/ liquids

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7
Q

(FSL) what happens when you increase the size of small covalent molecules?

A

intermolecular forces of attraction becomes stronger —> so higher mp/bp

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8
Q

(FSL) can small covalent molecules conduct electricity? why?

A

NO because molecules do not have an overall electric charge

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9
Q

(FSL) what state are giant covalent molecules at room temp? why?

A

Solids
- they have millions of strong covalent bonds –> high mp/bp

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10
Q

(FSL) does silicon dioxide have high or low mp/bp? why?

A

High because it has many covalent bonds

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11
Q

(FSL) what state are polymers at room temp?

A

solids

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12
Q

(FSL) how are polymers made?

A

by joining thousands of identical molecules (monomers)

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13
Q

(FSL) what forces of attractions are between polymers? high or low mp/bp?

A

strong intermolecular forces of attraction between molecules

  • high mp/bp
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14
Q

what are the 3 types of chemical bonding

A

ionic: metals and non-metals
covalent: non metals
metallic: metals

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15
Q

what is an ion

A

an atom or group of atoms that has lost or gained 1 or more electrons and therefore gaining a charge

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16
Q

what is a cation

A

a positively charged ion

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17
Q

what is an anion

A

a negatively charged iom

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18
Q

what is ionic bonding?

A

the transfer of electrons between metals and non-metals

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19
Q

what the 3 properties of ionic compounds?

A

1.high melting and boiling points
2. soluble in water
3. don’t conduct electricity

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20
Q

Do ionic compounds have high or low melting and boiling points? why?

A

High
- bcus they have are held together by strong electrostatic forces of attraction —-> so lots of energy is needed to overcome these

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21
Q

are ionic compounds soluble in water? why?

A

yes, bcus the water molecules are charged and attract ions away from the lattice to dissolve in water

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22
Q

do ionic compounds conduct electricity as solids? why?

A

No, not as solids bcus the ions are in fixed positions and can’t move

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23
Q

do ionic compounds conduct electricity as liquids

A

yes, bcus the ions are free to move and carry a charge

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24
Q
  • ionic compounds have a regular structure called a giant ionic lattice.

describe a giant ionic lattice?

A

the ions form a closely packed regular lattice arrangement and there are very strong electrostatic forces of attraction between oppositely charged ion in all directions in the lattice

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25
Q

what are polymers?

A

long chains made up of repeating units
- atoms joined togteher by covalent bonds
- are linked together to form molecules called monomers

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26
Q

what state are polymers at room temp? why?

A

solid, because the intermolecular forces of attraction between polymer molecules are relatively strong —> so lots of energy to break —> so high melting and boiling points

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27
Q

what are (4) properties of graphite?

A
  1. soft —> layers are free to slide over one another
  2. slippery —> ideal as lubricating material
  3. high melting point —> individual layers held together by strong covalent bonds so lots of energy is needed for them to break
  4. conducts electricity and thermal energy
28
Q

why does graphite conduct electricity?

A

graphite atoms have 3 covalent bonds meaning each carbon atom in graphite has 1 spare electron that isn’t bonding—> that 1 electron becomes delocalised —> allowing it to conduct electricity

29
Q

Graphite (4)
-bonded to…
- creates…
- held together..
- covalent bonds?

A

-bonded to only 3 other carbon atoms
-creates sheets of carbon atoms arranged in hexagons
- held together weakly so free to slide over one another ( makes it softer than diamond)
-no covalent bonds between layers

30
Q

what are 3 properties of diamond?

A
  1. really hard —> each carbon atom is covalently bonded to 4 other carbon atoms
    - forms regular 3D structure
  2. high melting and boiling point —-> strong covalent bonds so lots of energy needed to break
  3. doesn’t conduct electricity —> bcus no free ions/ electrons
31
Q

what is an allotrope?

A

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

32
Q

what is an alloy?

A

a mixture of 2 or more different elements
- either mix of 2 metals or metal and non-metal

  • elements of different sized atoms —> disrupt regular structure so layers can’t slide past each other —> this makes it hard
33
Q

what are fullerenes?

A

molecules of carbon —> shaped like hollow balls

  • arranged in hexagons/ heptagons (5/7 rings of carbon)
34
Q

what are fullerene tubes known as?

35
Q

properties of fullerene?

36
Q

what is graphene?

A

a single layer of graphite
- a sheet of carbon atoms joined together in hexagons

37
Q

what is covalent bonds?

A

the sharing of electrons between non-metals

38
Q

what are giant covalent structures?
- made up of…
- all joined together by…
- arranged into…

A
  • made up of huge number of non-metal atoms
  • all joined together by strong covalent bonds
  • generally arranged into repeating lattices
39
Q

what are 3 examples of giant covalent structures?

A

diamond, graphite, silicone dioxide

40
Q

what are 2 properties of giant covalent structures?

A
  1. very high melting and boiling points —> lots of energy needed to break strong covalent bonds
  2. don’t conduct electricity —> don’t contain charged particles even when molten (except graphite)
41
Q

what are covalent bonds?

A

bonds between non-metals
- sharing electrons

42
Q

what are 2 properties of graphene?

A
  1. strong but light —> can increase strength without adding weight
  2. conducts electricity—> contains delocalised electrons ( potential to be used in electronics)
43
Q

what are 3 properties of metalic bonding?

A

1.conducts electricity and heat
2. high melting and boiling points
3. malleable

44
Q

why can metalic bonds conduct electricity and heat?

A

because delocalised electrons carry electric current and thermal energy throughout structure

45
Q

why do metalic bonds have high melting and boiling points?

A

because has giant lattice of very strong electrostatic forces of attraction between metal ions and electrons ( so solid at room temp)

46
Q

why are metalic bonds malleable?

A

layers of atom can slide over one another making to soft as well,

47
Q

what is metalic bonding?

A
  • between metals and metals
  • consists of giant structures
  • there are strong forces of electrostatic attraction between positive metal ions and shared negative ions
48
Q

what are simple molecular substances made of?

A

they are made up of molecules containing few atoms joined together by covalent bonds.

49
Q

what are 6 properties of simple molecular substances?

A
  1. the atoms within the molecules are held together by very strong covalent bonds (2) but the forces of attraction between the molecules are very weak
  2. low melting and boiling points
  3. they are mostly gas or liquid at room temperature
  4. don’t conduct electricity
  5. as the molecules get bigger the strength of the intermolecular forces increases.
50
Q

what bonds are the atoms in within simple molecular substances held by?

A

very strong covalent bonds

51
Q

why are the melting and boiling points low in simple molecular substances?

A

to melt or boil a simple molecular substance you only need break the week intermolecular forces of attraction so the molecules are easily parted

52
Q

why do the melting and boiling points increase as the molecules in simple molecular substances get bigger?

A

as the molecules get bigger, the strength of the intermolecular forces increase, so more energy is needed to break them so the mp and bp increase

53
Q

simple molecular substances: do molecular compounds conduct electricity? why?

A

no, because they aren’t charged so there are no free electrons or ions

54
Q

describe the 3 properties of solids

A
  1. strong electrostatic forces of attraction between the particles
  2. particles don’t move positions so keep definite shape and volume
  3. particles vibrate in fixed positions
55
Q

describe 3 properties of liquids

A

1.weak force of attraction between the particles
2. definite volume but not definite shape
3. particles constantly move in random motion

56
Q

describe 3 properties of gases?

A

very weak forces of attraction between the particles
2. dont keep definite shape or volume
3. particles move constantly in random motion

57
Q

what is gas –> liquid?

A

condensing

58
Q

what is liquid —> gas?

A

evaporation/ boiling

59
Q

what is gas —> solid?

A

deposition

60
Q

what is solid —> gas?

A

sublimation

61
Q

what are 2 limitations of of simple particle models?

A
  1. assumes all particles are solid spheres when that is not the case because they are different shapes
  2. doesn’t show the forces between the particles
62
Q

do small covalent molecules have high or low mp and bp?

63
Q

exam questions- what are 2 advantages of using nano particles in sun cream?

A
  1. more protection from the sun’s ultraviolet rays
  2. better coverage
64
Q

exam questions- what are 2 disadvantages of using nano particles in sun cream?

A
  1. potential cell damage to the body
  2. harmful effects to the environment

Chemistry (13 decks)

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