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Edexcel GCSE Chemistry Triple > TOPIC 9 - Separate Chemistry 2 > Flashcards

TOPIC 9 - Separate Chemistry 2 Flashcards

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1
Q

Colour of lithium ion flame

A

Red

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2
Q

Colour of sodium ion flame

A

Yellow

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3
Q

Potassium ion flame color

A

Lilac

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4
Q

Calcium ion flame

A

Orange-red

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5
Q

Copper ion flame color

A

Blue-green

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6
Q

Test for metal ions involving precipitate

A

Add sodium hydroxide solution to the solution and metal hydroxide may precipitate out of solution.

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7
Q

Aluminium precipitate color and ionic equation

A

White before redissolving in excess sodium hydroxide w colourless solution.
Al3+ + 3OH-&raquo_space; Al(OH)3

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8
Q

Calcium precipitate color and ionic equation

A

White

Ca2+ + 2OH-&raquo_space; Ca(OH)2

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9
Q

Copper precipitate color and ionic equation

A

Blue

Cu2+ + 2OH-&raquo_space; Ca(OH)2

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10
Q

Iron(II) precipitate color and ionic equation

A

Green

Fe2+ + 2OH-&raquo_space; Fe(OH)2

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11
Q

Iron(II) precipitate color and ionic equation

A

Brown

Fe3+ + 3OH-&raquo_space; Fe(OH)3

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12
Q

How do you work out whether a substance contains ammonium ions?

A

Add sodium hydroxide solution and gently heat, ammonia gas will be given off.

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13
Q

How do you test for ammonia gas?

A

Hold a piece of damp red litmus paper over and ammonia gas will turn it blue.

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14
Q

How do you test for halide ions?

A

Add dilute nitric acid before a few drops of silver nitrate solution.

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15
Q

Chloride precipitate

When testing for anions

A

White precipitate of silver chloride

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16
Q

Bromide precipitate

When testing for anions

A

Cream precipitate of silver bromide

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17
Q

Iodide precipitate

When testing for anions

A

Yellow precipitate of silver iodide

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18
Q

How do you test for carbonate ions?

Symbol equation?

A

Add dilute acid and mixture will fizz as it will produce carbon dioxide gas.
CO32- + 2H+&raquo_space; CO2 + H2O

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19
Q

How do you test for sulphate ions?

A

Add dilute hydrochloric acid before adding barium chloride solution, sulfate ions will produce a white precipitate of barium sulfate.

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20
Q

Flame photometry

A

Instrumental method allowing identification of ions in a dilute solution. Each ion produced a unique line spectrum.

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21
Q

Why is flame photometry better than flame tests on specific occasions?

A

As can identify ions within a mixture which flame tests can’t.

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22
Q

Advantages of using machines to analyse unknown substances

A

V sensitive
V fast
V accurate

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23
Q

Homologous series

A

A group of chemicals w similar chemical structures and functional group while sharing a trend in chemical properties.

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24
Q

Alkanes

A

Homologous series of hydrocarbons w general formula CnH2n+2. They are saturated.

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25
Q

Functional group

A

A group of atoms that determine how a molecule reacts.

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26
Q

Alkenes

A

Homologous series of hydrocarbons w a C=C functional group, unsaturated .
CnH2n

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27
Q

How do you test for an alkene?

What reaction does it involve? Why?

A

Place in Bromine water, alkene will decolourise (orange to transparent).
Addition reaction occurs as bromine is added across the alkene double bond.

28
Q

Complete combustion of hydrocarbons

A

Hydrocarbon+ oxygen» carbon dioxide + water

29
Q

Polymers

A

Substances of high average relative molecular mass, composed of monomers.

30
Q

Monomers in addition polymers

A

Have double bond

31
Q

Addition polymerisation

A

Unsaturated monomer molecules opening up their double bonds to form polymer chains.

32
Q

How are formulas of polymers written?

A

(Monomer formula)n

33
Q

How do you draw the displayed formula of an addition polymer?

A

Join monomer carbons together w no double bonds w brackets on each side and stick n on end

34
Q

How do you draw the displayed formula of an addition monomer?

A

Draw out unsaturated monomer and stick n before it

35
Q

Condensation polymerisation

A

2 different monomers (w 2 functional groups) reacting together to create long chains of alternating monomers. For each new bond formed, a small molecule (like water) is lost.

36
Q

Polyesters

A

Di carboxylic acid monomers reacted with diol monomers.

37
Q

Ester link

A

A carboxylic acid group reacting with an alcohol group.

Molecule of water is formed each time an Ester link is made.

38
Q

Examples of non-synthetic polymers

A

DNA (nucleotide monomers)
Proteins (amino acid monomers in condensation polymerisation)
Starch / cellulose (sugar monomers)

39
Q

2 methods of disposing polymers

A

Landfill

Incineration

40
Q

Positives and negatives of landfill

A

:) polymers can be difficult and expensive to separate and recycle.
:( valuable land is used up and most polymers are no biodegradable

41
Q

Positives and negatives of incineration

A

:) produces much energy to generate electricity.

:( produces toxic gases and CO2, contributing to global warming

42
Q

Advantages of recycling

A

Reduces amount of a non-biodegradable waste filling up landfill sites.
Reduces emissions.
Uses less water and energy resources than when making new plastics.
Reduces amount of crude oil needed to produce more plastics.
Saves money and creates jobs

43
Q

Disadvantages of recycling

A

Separation of polymers can be difficult/expensive.
Quality of polymer product is reduced when mixed.
Finite number of times through which a polymer can be recycled.
Melting down polymers can release dangerous gases

44
Q

Alcohols

A

Have an -OH functional group w the same general formula (CnH2n+1)

45
Q

What is formed by the oxidation of alcohols?

A

Carboxylic acids

46
Q

Carboxylic acids

A

Have a -COOH functional group w the general formula Cn-1H2n-1COOH.

47
Q

Fermentation

A

The process of using yeast to convert a type of carbohydrate (sugars) into alcohol.

48
Q

Equation for fermentation

A

C6H12O6 >yeast> 2C2H5OH + 2CO2

Glucose> ethanol + carbon dioxide

49
Q

How do you make a solution of ethanol via fermentation?

A

Mix yeast and carbohydrate solution in sealed, clean container in warmth (between 30/40°C). Needs to be kept in anaerobic conditions
When concentrated of alcohol reaches 10-20%, fermentation will stop as yeast is killed by alcohol, falling to bottom of container.

50
Q

How do you produce a more concentrated alcohol?

A

Fractional Distillation

51
Q

Why does fractional distillation work on the solution of alcohol?

A

Ethanol has a lower boiling point than water so evaporates up fractionating column while water stays as liquid.

52
Q

What equipment is used to condense the ethanol vapour

A

A Liebig condenser.

53
Q

How do you measure the efficiency of alcohol as a fuel?

A

Put alcohol in spirit burner and measure mass of burner w fuel (using mass balance).
Measure 100 cm cubed of distilled water into copper calorimeter and insulate w draught excluder, covering w insulating lid after putting thermometer inside.
Take initial temp of water and light wick.
Stir throughout w a thermometer and blow out burner when water temp has risen by 20°C.
Reweigh burner and fuel.
Repeat w other alcohols

54
Q

Variables to keep same when burning alchol

A

Volume of water
Height of container above wick.
Length of wick.
Moles of alcohol.

55
Q

How does chain length of alcohol affect efficiency

A

Longer chain length = more efficient fuel.

56
Q

Size of nanoparticles

How many atoms do they contain?

A

1-100 nanometers

Roughly few hundred atoms.

57
Q

Surface area to volume ratio of nanoparticles

A

As particles decrease in size, surface area to volume ratio increases.
Therefore can act as catalyst as much more of atom is available to interact w substances they come into contact w.

58
Q

Uses of nanoparticles

A

CATALYST (large surface area to volume ratio)
COSMETICS (transparent but work)
NANOMEDICINE (can hold medicine and transport into body)
LUBRICANT (artificial joints and gears)
CONDUCTORS (electric circuits)
SPORTS EQUIPMENT (strengthens plastics)
Surgical masks (silver nanoparticles have antibacterial properties)

59
Q

Risks of nanoparticles

A

health implicationsUnaware of long-term

Could build up in cells

60
Q

Uses of polymers

A

Water pipes
Plastic bags and squeeze bottles
Thermal insulators
Plastic kettles

61
Q

Properties of polymers

A 
Strong, rigid, 
light, stretchy
Heat-resistant
Insulator
Cheaper
Less dense
Degrade and break down over time
62
Q

Clay uses

A

Building material (bricks)

63
Q

Clay properties

A

Easily mouldable

Strong

64
Q

Glass properties

A

Transparent strong brittle

Easily mouldable

65
Q

Composites

A

Reinforcement embedded in matrix
Properties depend on materials mixed.
Expensive

66
Q

Metals properties and uses

A 
Conductor of heat and electricity
High density
Malleable
Can form alloys
Corrosion resistant
67
Q

Examples of ceramics

Properties

A

Clay
Glass

Brittle, stiff, strong, hard-wearing, don’t degrade or corrode

Edexcel GCSE Chemistry Triple (14 decks)

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