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AQA GCSE chemistry > Paper 2 stuff :) > Flashcards

Paper 2 stuff :) Flashcards

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1
Q

concentration =

A

moles/ volume

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2
Q

Volume =

A

moles x 24

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3
Q

What are titrations used for?

A

finding out exactly how much acid is needed to neutralise a quantity of alkali

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4
Q

Explain the process of a titration?

A
  • using a pipette and pipette filler add some alkali to a conical flask along with two or three drops of indicator
  • fill a burette with acid, making sure its done at eye-level
  • use burette, add acid to alkali a bit at a time giving conical flask a swirl
  • the indicator changes colour when all the alkali has been neutralised
  • record volume of acid needed to neutralise acid. repeat this to check results
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5
Q

How do you make insoluble salts?

A

precipitation experiment, using two soluble salts

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6
Q

What two things are needed to make lead sulfate?

A

lead nitrate and magnesium sulfate

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7
Q

What is solubility?

A

a measure of how much solute will dissolve in a solvent

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8
Q

What is solubility measured in?

A

grams of solute per 100 grams of solvent

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9
Q

How does temperature effect solubility?

A

increases solubility

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10
Q

What can you use a solubility curve for?

A

to see the solubility of a substance at a specific temperature

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11
Q

What is the solubility equation?

A

solubility = mass of solid / mass of water removed x100

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12
Q

Explain how you would investigate how the solubility of ammonium chloride is effected by temperature?

A
  • make a saturated solution by adding excess of ammonium chloride to 10cm cubed of water to a boiling tube
  • stir and place in water bath at 25C
  • after 5 mins check that all of the excess solid has sunk to the bottom of the tube and check solution is at 25C
  • weigh empty evaporating basin, pour some solution on (no undissolved solid)
  • reweigh basin and contents then gently heat using bunsen burner until all water removed
  • reweigh evaporating basin and contents
  • repeat at two more temperatures
  • plot results
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13
Q

What are ions?

A

charged particles

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14
Q

What structure do ionic compounds have?

A

lattice structure/ giant ionic structures

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15
Q

Descibe ionic compounds?

A
  • ions held together in closely packed 3D lattice by strong electrostatic attraction between oppositely charged ions
  • high melting and boiling points
  • not electrical conductors when solid, if you melt or dissolve them in water they are able to conduct electricity
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16
Q

Define a covalent bond?

A

strong electrostatic attraction between the negatively charged shared electrons and the positively charged nuclei of the atoms involved

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17
Q

What are the features of a simple molecular structure?

A
  • atoms within molecule held together by strong covalant
  • forces of attraction between molecules are very weak
  • feeble intermolecular forces
  • low melting and boiling due to weak intermolecular
  • intermolecular forces are stronger with a high Mr
  • usually gases or liquids
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18
Q

Describe giant covalant?

A
  • no charged ions
  • atoms bonded by strong covalent bonds
  • high melting and boiling point
  • insoluble in water
  • dont conduct electricity
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19
Q

What is the reactivity series?

A 
potassium
sodium
lithium
calcium
magnesium
aluminium
zinc
iron
copper
silver 
gold
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20
Q

What is oxidation?

A

loss of electrons

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21
Q

what is reduction?

A

gain of electrons

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22
Q

How are most metals found?

A

in ores

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23
Q

What is the alcohol functional group?

A

OH

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24
Q

WHat is the alcohol general formula?

A

CnH2n+1OH

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25
Q

What are the first four alcohols?

A

methanol, ethanol, propanol, butanol

26
Q

What can alcohols be oxidised to form?

A

carboxylic acids

27
Q

What do you need to make carboxylic acids?

A

potassium dichromate in dilute sulfuric acid

28
Q

What is formed when ethanol is heated with potassium dichromate in dilute sulfuric acid?

A

ethanoic acid

29
Q

What forms carboxylic acids from alcohol?

A

microbial oxidation

30
Q

Explain microbial oxidation?

A

some microorganisms are able to use alcohols as an energy source. to do this they used oxygen in the air to oxidise alcohols

carboxylic acids are made as a by product of this

31
Q

When alcohols are burned what happens?

A

they are oxidised

32
Q

What happens when alcohols are burned in enough oxygen?

A

undergo complete combustion

33
Q

What is complete combustion of alcohols equation?

A

ethanol + oxygen –> carbon dioxide + water

34
Q

What are the two ways of producing ethanol?

A
  • ethene and steam

- fermentation

35
Q

Explain ethanol production from ethene and steam?

A
  • ethene is produced from crude oil
  • ethene reacts with steam to form ethanol - addition reaction
  • temp is 300 and pressure is 60-70 atmospheres
  • phosphoric acid used as catalyst
36
Q

What are the benefits and drawbacks of producing ethanol from ethene and steam?

A
  • cheap process becuase ethene is cheap and not wasted

- crude oil is non- renewable which means it will start running out - could become expensive

37
Q

fermentation equation?

A

C6H1206 —> 2C2H5OH + 2CO2

38
Q

Explain fermentation method?

A
  • raw material of sugar (glucose) is converted to ethanol using yeast
  • yeast cells contain enzymes- naturally occuring catalysts
  • 30C to optimise rate but not denature enzymes
  • keep in anaerobic conditions so that the ethanol isnt converted to ethanoic acid
39
Q

What are the advantages to fermentation?

A
  • raw materials are all from renewable source

- sugar is grown in crops around world and yeast is easy to grow

40
Q

What are the disadvantages of fermentation?

A
  • ethanol isnt very concentrated so needs to be distilled to increase strength and needs purifying
41
Q

equation for ethene and steam?

A

C2H4 + H20 —> C2H5OH

42
Q

Explain steps in finding out concentration of acid in titration?

A
  • work out moles of known substance
  • write out equation and compare ratio
  • use concentration formula
43
Q

What is a metal ore?

A

if a compound contains enough of metal worth extracting

44
Q

If a metal is more reactive, is it harder or easy to extract?

A

harder

45
Q

What type of reaction is usually used for extraction?

A

reduction reaction

46
Q

What is the problem with reduction reactions with carbon?

A

only metals that are less reactive then carbon can be extracted

47
Q

How are elements more reactive then carbon extracted?

A

using electrolysis

48
Q

What is electrolysis?

A

using electricity to extract a metal

49
Q

Explain steps in working out water of crystalisation?

A
  • work out mass of all substances
  • calculate number of moles of water lost
  • calculate moles of anhydrous salt
  • work out ratio of salt to water
  • whole number
50
Q

Explain diamond structure?

A
  • network of carbon atoms that each form four covalant bonds
  • strong covalant bonds mean high melting point
  • strong bonds mean rigid lattice structure so hard
  • no delocalised electrons so doesnt conduct
51
Q

Explain graphite?

A
  • each carbon forms three covalant creating layers of carbon atoms
  • layers have weak intermolecular forces so slide over each other making it soft and slippery
  • high melting point due to covalant bonds in layers
  • only three out of carbon four outer electrons are used so one delocalised to conduct electricity
52
Q

Explain C60 fullerene?

A
  • hollow sphere of 60 carbon atoms
  • made of large covalent molecules
  • weak intermolecular forces so can slide over eachother making it soft
  • one delocalised electron but electrons can move between molecules so poor conductor
53
Q

WHat is electric current?

A

flow of electrons or ions

54
Q

What happens when electrons or ions move?

A

cause material they are in to conduct electricity

55
Q

Do solid ionic compounds conduct electricity?

A

no - ions can move around

56
Q

Explain why ionic compounds can conduct electricity as a solution?

A
  • when dissolved the ions are separate and are able to move in the solution
57
Q

Explain why ionic compounds can conduct in molten state?

A

when compound melts, ions are able to move and can conduct

58
Q

What are metals held together by?

A

metallic bonding

59
Q

Explain metal structure?

A
  • giant structure of positive ions surrounded by sea of delocalised electrons
  • electrostatic attraction between positive ions and electrons is called metallic bonding
60
Q

Definition of metallic bonding?

A

electrostatic attraction between positive ions and the electrons

61
Q

Why are most metals malleable?

A
  • layers of ions in a metal can slide over each other making metals malleable, can be hammered or rolled into flat sheets

AQA GCSE chemistry (10 decks)

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