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Chemistry: Paper 2 > Separate Chemistry > Flashcards

Separate Chemistry Flashcards

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1
Q

Why must the test for ions be unique

A

As you wouldn’t be able to know the specific ion if more than one ion gave the same result

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2
Q

What colour is lithium ions in the flame test

A

Red

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3
Q

What colour is sodium ions in the flame test

A

yellow

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4
Q

What colour is potassium ions in the flame test

A

lilac

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5
Q

What colour is calcium ions in the flame test

A

orange-red

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6
Q

What colour is copper ions in the flame test

A

blue-green

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7
Q

How do you preform a flame test

A

Hold a sample you wish to test on a wire in a roaring Bunsen flame and observe colour change

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8
Q

Describe tests to show the presence of the following ions in solids or solutions

A
  • Add a few drops of sodium hydroxide solution to a solution of your unknown compound
  • Forms an insoluble hydroxide
  • Depending on the colour of precipitate produced from the metal ion it can be identified
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9
Q

What colour precipitates form when sodium hydroxide reacts with aluminium ions

A

White precipitate (dissolves when excess NaOH is added)

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10
Q

What colour precipitates form when sodium hydroxide reacts with calcium ions

A

White precipitate

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11
Q

What colour precipitates form when sodium hydroxide reacts with copper(II) ions

A

Blue precipitate

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12
Q

What colour precipitates form when sodium hydroxide reacts with iron(II) ions

A

Green precipitate

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13
Q

What colour precipitates form when sodium hydroxide reacts with iron(III) ions

A

Brown precipitate

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14
Q

What is observed when sodium hydroxide reacts with ammonium ions

A
  • Pungent-smelling gas produced
  • Gas produced turns damp red litmus paper blue
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15
Q

What is the test for ammonium ions

A
  1. Add a few drops of dilute sodium hydroxide solution, then warm gently.
  2. Ammonia gas is produced if ammonium ions are present.
  3. Confirm that the gas is ammonia - damp red litmus paper turns blue.
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16
Q

What is the test for carbonate ions

A
  1. Add a few drops of dilute hydrochloric acid.
  2. Bubbles are produced if carbonate ions are present.
  3. Confirm that the gas is carbon dioxide - limewater turns milky.
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17
Q

What is the test for sulphate ions

A
  1. Add a few drops of dilute hydrochloric acid,
  2. add a few drops of barium chloride solution.
  3. A white precipitate forms if sulfate ions are present.
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18
Q

What is the test for halide ions

A
  1. Add a few drops of dilute nitric acid,
  2. Add a few drops of silver nitrate solution.
  3. Observe and record the colour of any precipitate formed.
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19
Q

What colour precipitate does does chloride form in dilute nitric acid and silver nitrate solution

A

White precipitate

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20
Q

What colour precipitate does does bromide form in dilute nitric acid and silver nitrate solution

A

cream precipitate

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21
Q

What colour precipitate does does iodide form in dilute nitric acid and silver nitrate solution

A

yellow precipitate

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22
Q

What are two examples of instrumental analysis

A
  • gas chromatography
  • mass spectrometry
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23
Q

What are the positives of instrumental analysis

A
  • Improve sensitivity
  • Improve accuracy
  • Increases speed of the test
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24
Q

What is a flame photometer used for

A
  • Identifying metal ions in a sample
  • determining the concentration of metal ions in a solution
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25
Q

How does a photometer work

A
  • Sample is put into a flame and the light given out is passed through a photometer
  • Output is a line spectrum that can be analysed to identify metal ions in the solution and measure their concentrations
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26
Q

What are the first 4 alkanes

A
  1. Methane
  2. Ethane
  3. Propane
  4. Butane
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27
Q

Why are alkanes saturated hydrocarbons

A
  • They don’t possess any double or triple bonds
  • Are compounds made of hydrogen and carbon only
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28
Q

What are the first 3 alkenes

A
  • Ethene
  • Propene
  • Butene
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29
Q

Why are alkenes unsaturated hydrocarbons

A
  • Contain 1 or more C=C bonds
  • Are compounds made of hydrogen and carbon only
30
Q

What is the reaction of ethene + bromine

A

Ethene + bromine -> 1,2-dibromoethane
this reaction works the same for any alkene or any halogen

31
Q

How is bromine water used to distinguish between alkenes and alkanes

A
  • Alkenes react with bromine water (go from orange to colourless)
  • Alkanes don’t react with bromine water
32
Q

Describe complete combustion of alkanes/alkenes

A
  • Alkane/alkene + oxygen → carbon dioxide + water
  • Hydrocarbons oxidise to produce products
33
Q

What is a polymer

A

A substance made from long chains of
small repeating units

34
Q

What is addition polymerisation

A

A reaction where many small molecules (monomers) join to create large molecules (polymers)

35
Q

Why can any alkene be used as a monomer

A

They contain a C=C bond

36
Q

What is the difference between the structure of a monomer and the structure of an addition polymer

A

all monomers involved in addition polymerisation have a double bond

37
Q

What is the properties of Poly(ethene)

A
  • Flexible
  • Cheap
  • Electrical insulator
38
Q

What are the uses of Poly(ethene)

A
  • Plastic bags & bottles
  • Coating on electrical wires
39
Q

Properties of poly(propene)

A
  • Flexible
  • Strong
40
Q

Uses of poly propene

A

Buckets and crates

41
Q

Properties of chloroethene (PVC)

A
  • Tough
  • Cheap
  • Long lasting
42
Q

Uses of poly chloroethene (PVC)

A

Window frames

43
Q

Properties of PTFE

A
  • Tough
  • Non-stick
44
Q

Uses of PTFE

A

Non stick coating on pans

45
Q

Why are polyesters condensation polymers

A

dicarboxylic acid and diol molecules join releasing a water molecule for every ester link made

46
Q

How is a polyester formed when a monomer molecule containing two carboxylic acid groups is reacted with a monomer molecule containing two alcohol groups

A
  • the dicarboxylic acid loses the OH group off of each COOH group
  • the di-alcohol loses the H off of each OH group
  • the remaining molecules join together to make a polyester
47
Q

How a molecule of water is formed each time an ester link is formed

A

the OH and H groups combine to make H2O

48
Q

Advantages of recycling polymers

A
  • Better for the environment
  • Saves crude oil
  • More economically viable
49
Q

disadvantages of recyling polymers

A
  • Difficult and expensive to seperate
50
Q

What are different types of polymers and how

A
  • DNA - nucleotides
  • Starch - sugars
  • Proteins - amino acids
51
Q

What are the first 4 alcohols

A
  1. Methanol
  2. Ethanol
  3. Propanol
  4. Butanol
52
Q

What is the functional group of alcohols

A

-OH

53
Q

Core practical: Investigate temperature rise by the combustion of alcohols

A
  • the temperature is raised more as the
    chain length of the alcohols increases
  • Combustion of longer chain alcohols release more energy
54
Q

What is the functional group for carbolic acids

A

-COOH

55
Q

What are the first 4 four members of the carboxylic acids

A
  • Methanolic
  • Ethanoic
  • Propanoic
  • Butanoic
56
Q

What happens when you oxidise an alcohol

A

It becomes a carboxylic acid

57
Q

How can ethanol be produced

A
  • Fermentation with yeast
  • It is produced from carbohydrates
  • Kept under anaerobic conditions
58
Q

What is the anaerobic equation

A

Glucose -> ethanol + carbon dioxide

59
Q

How do you obtain a concentrated solution of ethanol by fractional distillation

A
  • Ethanol conc = 15% from fermentation
  • Water and ethanol solution are heated
  • Ethanol evaporates first - having a lower boiling point - cools then condenses
  • Water left evaporates
60
Q

What is the size of an atom

A

0.1 nm

61
Q

What is the size of a nanoparticle

A

1 nm to 100 nm

62
Q

Why are nanoparticles useful for their uses

A
  • Contains fullerenes
  • High SA:V ratio ( good catalysts)
  • Layers slide over each other so is good for sunscreen
  • Can conduct electricity
63
Q

What are the risks of nanopaticles

A
  • Could enter the bloodstream and cause harm (cataylse reactions)
  • A lot of effects are unknown
64
Q

What are the properties of glass ceramics

A
  • Transparent
  • Hard
  • Brittle
  • Poor heat and electrical conductors
65
Q

Uses of glass ceramics

A
  • Windows
  • Bottles
66
Q

Qualities of clay ceramics

A
  • Opaque
  • Hard
  • Brittle
  • Poor heat and electrical conductors
67
Q

Uses of clay ceramics

A
  • Bricks
  • Porcelain
68
Q

Qualities of polymers

A
  • Can be made transparent/translucent/opaque
  • Poor heat and electrical conductors
  • Can be tough or doctile
69
Q

Uses of polymers

A
  • Plastic bags
  • Bottles
70
Q

Qualities of metals

A
  • Shiny
  • Good heat and electrical conductors
  • Hard
  • Tough
71
Q

Uses of metals

A
  • Cars
  • Bridges
  • Electrical cables

Chemistry: Paper 2 (8 decks)

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