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Chemistry > Separate Chemistry 2 > Flashcards

Separate Chemistry 2 Flashcards

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1
Q

Homologous series definition

A

Group of chemicals with similar chemical structures

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2
Q

Alkane general formula

A

CnH2n+2

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3
Q

Functional group of alkenes

A

C=C

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4
Q

Why are alkenes unsaturated?

A

Double bonds are present and can open up and bond further

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5
Q

How to test for alkenes

A

Add orange bromine water to alkene and shake
If bromine water becomes colourless, alkenes are present
Addition reaction has occurred

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6
Q

Complete combustion of hydrocarbons word equation

A

Hydrocarbon + oxygen -> carbon dioxide + water

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7
Q

Addition polymerisation method

A

Lots of unsaturated smaller monomers open up their double bonds
They join together to form polymer chains

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8
Q

Propane as a polymer symbol

A

(C3H6)n

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9
Q

Formula for alkenes

A

CnH2n

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10
Q

Properties of poly(ethene)

A

Flexible
Electrical insulator
Cheap

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11
Q

Properties of poly(propene)

A

Flexible
Strong
Tough
Mouldable

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12
Q

Properties of poly(chloroethene) (PVC)

A

Tough

Cheap

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13
Q

Properties of poly(tetrafluoroethene) (PTFE)

A

Un reactive
Tough
Non-stick

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14
Q

Uses of poly(ethene)

A

Plastic bags, bottled, wire insulation

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15
Q

Uses of poly(propene)

A

Crates
Furniture
Ropes

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16
Q

Uses of poly(chloroethene) (PVC)

A

Window frames

Water pipes

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17
Q

Uses of poly(tetrafluoroethene) (PTFE)

A

Non-stick pans

Waterproof clothing

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18
Q

Condensation polymerisation method

A

Involves 2 different types of monomers
Each monomer contains at least 2 functional groups
Each functional group reacts with the functional group of another monomer, creating long chains of alternating monomers
Small molecule is lost per new bond made (e.g. water)

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19
Q

Polyester method

A

Dicarboxylic acid monomers contain 2 carboxylic acid (-COOH) groups
Diol monomers contain 2 alcohol groups (-OH) groups
Carboxylic acid groups react with alcohol groups to form an ester link
Molecule of water is lost per ester link made
Type of condensation polymerisation

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20
Q

Important naturally occurring monomers

A

Nucleotides -> DNA
Amino acid -> proteins and enzymes
Carbohydrates -> starch and cellulose

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21
Q

General formula for alcohols

A

CnH2n+1OH

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22
Q

Alcohol functional group

A

(-OH)

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23
Q

General formula for carboxylic acids

A

Cn-1H2n-1COOH

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24
Q

carboxylic acid functional group

A

(-COOH)

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25
Q

Fermentation formula

A

C6H12O6 -> yeast -> 2C2H5OH + 2CO2

Glucose -> yeast -> ethanol + carbon dioxide

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26
Q

Fermentation process

A

Carbohydrate (from sugar cane or sugar beet) is used
Yeast cells are mixed carbohydrate in clean container
Mixture is sealed and stored in a warm place (ideally between 30°C - 40°C)
Must have no oxygen present (oxidised ethanol turns into ethanoic acid)
Alcohol concentration gets high enough to kill off yeast
Distill mixture to get more concentrated alcohol

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27
Q

How to make concentrated ethanol

A

Fractional distillation
Ethanol has lower boiling point so will evaporate before water
This can then condense and be collected in a beaker while water stays as a liquid

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28
Q

Colour flame turns with lithium ions

A

Crimson red

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29
Q

Colour flame turns with calcium ions

A

Orange-red

30
Q

Colour flame turns with sodium ions

A

Yellow

31
Q

Colour flame turns with copper ions

A

Blue-green

32
Q

Colour flame turns with potassium ions

A

Lilac (purple)

33
Q

How to carry out flame test

A

Clean nichrome wire loop by dipping into hydrochloric acid and rinsing with distilled water
Dip wire loop into sample of metal compound
Place loop in clear blue part of Bunsen burner

34
Q

How to test for cations with precipitates

A

Add sodium hydroxide solution to compound

If hydroxide precipitate forms, colour correlates to metal ion in compound

35
Q

Colour of precipitate made with sodium hydroxide solution + aluminium

A

White at first then dissolves in excess NAOH to form colourless solution

36
Q

Colour of precipitate made with sodium hydroxide solution + calcium

A

White

37
Q

Colour of precipitate made with sodium hydroxide solution + copper

A

Blue

38
Q

Colour of precipitate made with sodium hydroxide solution + iron

A

Green if Fe2+

Brown if Fe3+

39
Q

How to test for ammonium ions (NH4 +)

A

Add sodium hydroxide solution to mystery solution
Hold damp red litmus paper over solution
If paper turns blue, ammonia is present

40
Q

How to test for halide ions

A

Add nitric acid
Add silver nitrate solution
Check colour of precipitate

41
Q

Colour of precipitate made with silver nitrate + chloride

A

White (silver chloride)

42
Q

Colour of precipitate made with silver nitrate + bromide

A

Cream (silver bromide)

43
Q

Colour of precipitate made with silver nitrate + iodide

A

Yellow (silver iodide)

44
Q

How to test for carbonates

A

Add dilute acid
Fizzes if carbonate is present (carbon dioxide)
Use limewater to test for carbon dioxide

45
Q

How to test for sulfate ions

A

Add dilute hydrochloric acid to stop precipitation reactions not involving sulfate ions
Add barium chloride solution
If sulfate ions present, precipitate made will be white (barium sulfate)

46
Q

Why each ion test has to be unique

A

If each test gave the same response, ions present wouldn’t be able to be differentiated from each other

47
Q

How flame photometry works

A

Each ion produced a unique line spectrum (how to identify what ion)
Intensity of measured wavelength correlates to ion’s concentration
Also can be used in mixtures

48
Q

Advantages of machines in instrumental analysis

A 
Very sensitive (can detect tiniest amounts of substance)
Very fast (can be automated)
Very accurate (no human error)
49
Q

Disposal of polymers in landfills facts

A

Done because polymers are too difficult or expensive to separate and recycle
Valuable land is used up as landfill sites
Polymers are non-biodegradable so they will stay in landfill for thousands of years

50
Q

Disposal of polymers by combustion facts

A

Burning plastics produces a lot of heat and can be used to generate electricity
Toxic gases can be released from combustion of plastics
Carbon dioxide produced can contribute to global warming

51
Q

Advantages of recycling polymers

A

Reduces amount of non-biodegradable waste on landfill sites
Reduces emissions of greenhouse and toxic gases from burning polymers
Generally uses less water and energy resources than making new plastics
Reduces amount of crude oil needed to produce more plastics
Germany saves money and creates jobs

52
Q

Disadvantages of recycling

A

Separating polymers can be difficult and expensive
Quality of final recycled polymer reduced if polymers are mixed together
Polymers can only be recycled a certain amount of times
Melting down polymers can release dangerous gases

53
Q

How to check which alcohol is best as a fuel

A

Put some alcohol in a spirit burner and measure mass
Put 100cm3 of distilled water into a copper calorimeter
Insulate calorimeter with drought excluder
Place thermometer into calorimeter and cover with insulating lid
Record initial temperature of water and light wick
Stir water through using thermometer
When temperature of water rises to 20°C, blow out spirit burner
Reweigh burner and fuel
Repeat with other alcohols

54
Q

Nanoparticles definition

A

Particles 1-100 manometers across

Have different properties from the “bulk” chemical it’s made from due to a high surface area to volume ratio

55
Q

Uses of nanoparticles

A

Good catalysts (higher surface area = more collisions)
Cosmetics e.g. sunscreen (don’t leave white marks on skin)
Nanomedicine (tiny fullerenes can deliver drugs more easily than most particles)
Lubricant
Nanotubes for conducting electricity
Enforcing plastics in sports equipment
Silver nanoparticles added in medical equipment for antibacterial uses

56
Q

Risks of nanoparticles

A

Their effect on the body aren’t fully understood e.g. some nanoparticles don’t break down easily
can cause problems e.g. lung inflammation if breathed in

57
Q

Use of high-density poly(ethene)

A

Strong and rigid so used in water pipes

58
Q

Use of low-density poly(ethene)

A

Light and stretchy so used for plastic bags and squeezy bottles

59
Q

Use of poly(styrene) foam

A

Packaging and thermal insulation

60
Q

Use of heat-resistant polymers e.g. melamine and poly(propene)

A

Plastic kettled

61
Q

Clay facts

A

Mineral formed from weather and decomposed rock
Soft when dug up so can be moulded into different shapes
Hardens when fired at high temperatures
Used in pottery and as a building material

62
Q

Glass facts

A

Transparent and strong
Can be moulded when hot
Brittle when thin
Usually made when limestone, sand and sodium carbonate are melted together

63
Q

Composite definition

A

Things made of one material (reinforcement) embedded in another (matrix/binder)
Properties depend on properties of the materials it is made from

64
Q

Properties of metal as a material

A

Good heat and electric conductor
High density
Malleable
Can be mixed with other elements to form alloys

65
Q

Advantages of polymers as a material

A

Very adaptable (often flexible and be moulded into almost any shape)
Cheaper
Thermal and electrical insulators

66
Q

Disadvantages of polymers as a material

A

Degrade and break down over time (don’t last as long)

Hard to dispose of properly

67
Q

Advantages of ceramics as a material

A

Electric and heat insulator
Strong and hard-wearing
Don’t degrade over time so they last longer

68
Q

Disadvantages of ceramics as a material

A

Brittle and stiff

Dense

69
Q

Advantages of metals as a material

A

Good conductor of heat and electricity
Malleable
Corrosion-resistant metals last for a very long time
Less brittle (don’t shatter)

70
Q

Disadvantages of metals as a material

A 
Some metals corrode easily 
Less brittle (likely to deform)
71
Q

Advantages of composites as a material

A

Can be made for specific purpose (properties purely rely on materials they are made from)

72
Q

Disadvantages of composites as a material

A

Much more expensive than other materials

Chemistry (10 decks)

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