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Chemistry: Paper 2 > Separate Chemistry > Flashcards

Separate Chemistry Flashcards

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
How does a photometer work
- 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
26
What are the first 4 alkanes
1. Methane 2. Ethane 3. Propane 4. Butane
27
Why are alkanes saturated hydrocarbons
* They don't possess any double or triple bonds * Are compounds made of hydrogen and carbon only
28
What are the first 3 alkenes
* Ethene * Propene * Butene
29
Why are alkenes unsaturated hydrocarbons
* Contain 1 or more C=C bonds * Are compounds made of hydrogen and carbon only
30
What is the reaction of ethene + bromine
Ethene + bromine -> 1,2-dibromoethane this reaction works the same for any alkene or any halogen
31
How is bromine water used to distinguish between alkenes and alkanes
* Alkenes react with bromine water (go from orange to colourless) * Alkanes don't react with bromine water
32
Describe complete combustion of alkanes/alkenes
* Alkane/alkene + oxygen → carbon dioxide + water * Hydrocarbons oxidise to produce products
33
What is a polymer
A substance made from long chains of small repeating units
34
What is addition polymerisation
A reaction where many small molecules (monomers) join to create large molecules (polymers)
35
Why can any alkene be used as a monomer
They contain a C=C bond
36
What is the difference between the structure of a monomer and the structure of an addition polymer
all monomers involved in addition polymerisation have a double bond
37
What is the properties of Poly(ethene)
* Flexible * Cheap * Electrical insulator
38
What are the uses of Poly(ethene)
* Plastic bags & bottles * Coating on electrical wires
39
Properties of poly(propene)
* Flexible * Strong
40
Uses of poly propene
Buckets and crates
41
Properties of chloroethene (PVC)
* Tough * Cheap * Long lasting
42
Uses of poly chloroethene (PVC)
Window frames
43
Properties of PTFE
* Tough * Non-stick
44
Uses of PTFE
Non stick coating on pans
45
Why are polyesters condensation polymers
dicarboxylic acid and diol molecules join releasing a water molecule for every ester link made
46
How is a polyester formed when a monomer molecule containing two carboxylic acid groups is reacted with a monomer molecule containing two alcohol groups
* 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
How a molecule of water is formed each time an ester link is formed
the OH and H groups combine to make H2O
48
Advantages of recycling polymers
* Better for the environment * Saves crude oil * More economically viable
49
disadvantages of recyling polymers
* Difficult and expensive to seperate
50
What are different types of polymers and how
* DNA - nucleotides * Starch - sugars * Proteins - amino acids
51
What are the first 4 alcohols
1. Methanol 2. Ethanol 3. Propanol 4. Butanol
52
What is the functional group of alcohols
-OH
53
Core practical: Investigate temperature rise by the combustion of alcohols
* the temperature is raised more as the chain length of the alcohols increases * Combustion of longer chain alcohols release more energy
54
What is the functional group for carbolic acids
-COOH
55
What are the first 4 four members of the carboxylic acids
* Methanolic * Ethanoic * Propanoic * Butanoic
56
What happens when you oxidise an alcohol
It becomes a carboxylic acid
57
How can ethanol be produced
* Fermentation with yeast * It is produced from carbohydrates * Kept under anaerobic conditions
58
What is the anaerobic equation
Glucose -> ethanol + carbon dioxide
59
How do you obtain a concentrated solution of ethanol by fractional distillation
* 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
What is the size of an atom
0.1 nm
61
What is the size of a nanoparticle
1 nm to 100 nm
62
Why are nanoparticles useful for their uses
* Contains fullerenes * High SA:V ratio ( good catalysts) * Layers slide over each other so is good for sunscreen * Can conduct electricity
63
What are the risks of nanopaticles
* Could enter the bloodstream and cause harm (cataylse reactions) * A lot of effects are unknown
64
What are the properties of glass ceramics
* Transparent * Hard * Brittle * Poor heat and electrical conductors
65
Uses of glass ceramics
* Windows * Bottles
66
Qualities of clay ceramics
* Opaque * Hard * Brittle * Poor heat and electrical conductors
67
Uses of clay ceramics
* Bricks * Porcelain
68
Qualities of polymers
* Can be made transparent/translucent/opaque * Poor heat and electrical conductors * Can be tough or doctile
69
Uses of polymers
* Plastic bags * Bottles
70
Qualities of metals
* Shiny * Good heat and electrical conductors * Hard * Tough
71
Uses of metals
* Cars * Bridges * Electrical cables

Chemistry: Paper 2 (8 decks)

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