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Paper 2 Flashcards

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1
Q

Group 1

2 qualities of Alkali metals

A

Soft

Low mp/bp

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2
Q

Group 1

As you go down, reactivity…

A

…increases

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3
Q

Group 1

Reactions with water include:

A 
Lithium = move around surface fizzing
Sodium = melts in heat of reaction
Potassium = ignites the H2 producued
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4
Q

Group 7

Colour of chlorine

A

Green poisonous gas

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5
Q

Group 7

Colour of bromine

A

Red-brown liquid / orange vapour at room temp.

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6
Q

Group 7

Colour of iodine

A

Dark grey crystalline solid / purple vapour when heated

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7
Q

Group 7

Qualities of halogens

A

diatomic, mp/bp increases as you go down the group

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8
Q

Group 7

As you go down, reactivity…

A

…decreases

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9
Q

Test for chlorine

A

Damp blue litmus paper will be bleached, turning it white

May turn red for a moment as solution of chlorine is acidic

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10
Q

Group 7

What is formed when a halogen and metal react?

A

A salt called metal halides

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11
Q

Group 7

What is formed when halogens react with hydrogen?

A

Hydrogen halides, which dissolve in water to form acidic solutions

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12
Q

Group 0

Qualities to noble gases

A

monatomic, inert, colourless gases, non-flammable

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13
Q

Group 0

Use of argon

A

Provides inert atmosphere in filament lamps to stop hot filament burning

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14
Q

Group 0

Use of noble gases in flash photography

A

Argon, krypton and xenon stop flash filament from burning up during high temperatures of flash

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15
Q

Group 0

Uses of helium

A

Airships / party balloons as it has a lower density than air so can float

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16
Q

Group 0

As you go down the group, bp/mp and density…

A

…increase

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17
Q

How SA affects rate

The finer the particles of marble chips…

A

…the faster the reaction, meaning the powered chips on a graph goes up steeper

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18
Q

How conc. affects rate

The more conc. a solution…

A

… the faster the reaction occurs, so the steeper the line on a graph

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19
Q

How temp. affects rate

The higher the temperature…

A

…the faster the reaction

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20
Q

Sodium thiosulfate and HCL

What is the experiment?

A

Use different temperature solutions and time how long it takes for them to react - the reaction is finished when you can’t see a black cross underneath beaker

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21
Q

What does IFOSC

A

Increased frequency of successful collisions

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22
Q

What are enzymes?

A

Biological catalysts

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23
Q

How are enzymes used to produce alcoholic drinks?

A

Enzymes from yeast cells are used in the fermentation process of alcoholic drinks

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24
Q

How do catalysts affect activation energy?

A

Decrease activity ion energy by providing an alternative reaction pathway that has a lower AE, so more particles have at least the minimum energy to react

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25
Q

Qualities of catalysts

A

Doesn’t alter products / is unchanged itself / doesn’t use up its mass

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26
Q

Formula for rate of reaction

A

Amount of reactant used / formed
————————————————
Time

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27
Q

What can be used to measure how much gas is given off?

A

Gas syringe

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28
Q

What 3 factors impact collision theory?

A

Temperature / concentration (pressure) / SA

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29
Q

Define an exothermic reaction

A

One which gives out energy to the surroundings, usually shown by a rise in temp of surroundings

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30
Q

Define an endothermic reaction

A

One which takes energy in from the surroundings, usually shown by a fall in temp of the surroundings

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31
Q

Graphs of endo- and exo- thermic reactions

A

Picture 6

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32
Q

Define activation energy

A

The minimum amount of energy needed for bonds to break and a reaction to start

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33
Q

What is activation energy on a reaction profile

A

The energy difference between the reactants and the highest point on the curve

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34
Q

Formula for overall energy change

A

Energy required to break bonds - energy required to make bonds

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35
Q

What reaction is bond breaking?

A

Endothermic as energy used to break bonds is greater than the energy released by forming them

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36
Q

What reaction is bond making?

A

Exothermic as the energy released by forming bonds is greater than the energy used to break them

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37
Q

Temperature change

Dissolving salts in water experiment

A

Adding the salt to a polystyrene cup of water and measuring the change in temp when the salt had dissolved

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38
Q

Dissolving salts in water experiment

Ammonium chloride =

A

Decreases the temperature of the reaction mixture - its endothermic

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39
Q

Dissolving salts in water experiment

Calcium chloride =

A

Causes temp of solution to rise = exothermic

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40
Q

Temperature changes

Neutralisation reactions

A

Most are exothermic

Reaction between ethanoic acid and sodium carbonate is endothermic

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41
Q

Temperature changes

Displacement reactions

A

Release of energy - exothermic

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42
Q

Temperature changes

Precipitation reactions

A

Exothermic

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43
Q

What do hydrocarbons contain?

A

Hydrogen and carbon

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44
Q

Crude oil is:

A
  • a complex mixture of hydrocarbons
  • containing molecules in which carbon atoms are in chains or rings
  • an important source of useful substances
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45
Q

Is crude oil renewable?

A

No it’s finite

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46
Q

Qualities of longer hydrocarbons

A

Higher bp so turn into liquids and drain out of the column early on when they’re near the bottom

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47
Q

Qualities of shorter hydrocarbons

A

Lower bp so then to liquid and drain out much later on, near to the top of the column where it’s cooler

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48
Q

Use of gases at top of colouring

A

Domestic heating and cooking

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49
Q

Use of petrol

A

Used as fuel in cars

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50
Q

Use of kerosene

A

Used as fuel in aircraft

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51
Q

Use of diesel oil

A

Fuel in larger vehicles (trains) and some cars

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52
Q

Use of fuel oil

A

Fuel for large ships and in some power stations

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53
Q

Use of bitumen at bottom of column

A

To surface roads and roofs

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54
Q

Define a homologous series

A

A family of molecules which have the same general formula and share similar chemical properties

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55
Q

Neighbouring homologous series differ by:

A

a CH2 unit

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56
Q

What is viscosity?

A

The measure of how easily a substance flows

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57
Q

Which fractions have a higher viscosity?

A

Longer hydrocarbons - thick like treacle

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58
Q

Which fractions have lower viscosity?

A

Shorter hydrocarbons - runnier

59
Q

Which hydrocarbons are easy to ignite and why?

A

Shorter hydrocarbons - have lower bp so tend to be gases at room temp

60
Q

What state are longer hydrocarbons usually in at room temperature?

A

Liquid

61
Q

How do inter molecules forces break in smaller molecules?

A

Easily as the forces are much stronger in big molecules than in small ones

62
Q

What is complete combustion?

A

burning hydrocarbons in plenty of oxygen to produce CO2 and wayer

63
Q

What sort of reaction is complete combustion?

A

Exothermic

64
Q

What is incomplete combustion?

A

Not enough oxygen is present so the products are:

Carbon dioxide, water, carbon monoxide and carbon (soot)

65
Q

Why is carbon monoxide dangerous?

A

Can combine with red blood cells and stop blood from carrying oxygen

A lack of oxygen in blood to brain can lead to fainting, a coma, or death

66
Q

What is the issues with soot?

A

Makes buildings look dirty, reduces air quality, can cause or worsen respiratory problems

67
Q

Where does sulfur dioxide actually come from?

A

Sulfur impurities in fossil fuels

68
Q

What happens when sulfur dioxide mixes with clouds?

A

It forms dilute sulfuric acid, and falls as acid rain

69
Q

Why is acid rain harmful?

A

Causes lakes to become acidic so fish and plants die

Kills trees, damages limestone buildings, causes metal to corrode

70
Q

How are nitrogen oxides formed?

A

From a reaction between nitrogen and oxygen in the air, caused by the energy released by combustion reactions

71
Q

Why are nitrogen oxides harmful?

A

Contribute to acid rain / cause photochemical smog

72
Q

What is photochemical smog?

A

A type of air pollution that causes breathing difficulties, headaches and tiredness

73
Q

Cons to hydrogen as a fuel to power vehicles

A

Special, expensive engine needed
Expensive to manufacture hydrogen
Hard to store
Not widely availble

74
Q

Pros to hydrogen as a fuel to power vehicles

A

Very clean = only water waste product
Renewable
Can be obtained from the water produced by the cell when used in fuel cells

75
Q

What is cracking

A

Turning long saturated (alkane) molecules into smaller unsaturated (alkene) and alkane molecules

76
Q

What happens in cracking

A

A form of thermal decomposition when one substance breaks down into two new ones when heated

77
Q

What conditions does cracking need?

A

Heat, moderate pressure and a catalyst

78
Q

Why is cracking important?

A

To meet supply and demand by breaking down unwanted hydrocarbons into wanted ones

79
Q

What was the earth’s atmosphere in the first billion years?

A

Volcanoes erupting, releasing gases mainly CO2, steam, methane and ammonia

80
Q

What gases made up the atmosphere in the first billion years?

A

Mostly CO2 and water vapour which later condensed to form oceans

81
Q

What was the Earth’s atmosphere from 1-3 billion years?

A

A lot of CO2 dissolved into oceans

Green plants evolved over the earth, removing more CO2 and adding O2

82
Q

How was nitrogen added to the atmosphere 1-3 billion years ago?

A

N2 gas was formed by ammonia reacting with oxygen, and was also released by denitrifying bacteria

Not reactive so was being made but not broken down

83
Q

Where did CO2 in the 1-3billion year atmosphere get trapped?

A

In fossils and sedimentary rocks

84
Q

What has the presence of oxygen in the last billion years meant for animals?

A
  • early organisms died who couldn’t cope with oxygen in air

- evolution of more complex organisms

85
Q

What has the presence of O2 in the last billion years made in the atmosphere?

A

Created the ozone layer O3 blocking harmful rays from the Sun, there is virtually no CO2 left jow

86
Q

What is the test for oxygen

A

If the gas is present, it will relight a glowing splint

87
Q

What is the greenhouse gas effect stages?

A
  1. Earth radiates some of the heat radiation it absorbs as longer wavelength = IR
  2. Some of this IR is absorbed by GG
  3. Some IR is re-emitted back towards Earth by GG
  4. Some IR is re-emitted back into space
  5. The absorption and remission of IR by GG keeps the Earth warm
88
Q

What is the enchanted greenhouse effect?

A

Conc of GG increases, more heat radiation from the Earth is absorbed and less is reemitted back into space

89
Q

How has the increasing human population affected the composition of air?

A

more people = more land for housing and crops = less trees = less removal of CO2 and production of O2

more energy (fossil fuels) used as well

90
Q

How has the concentration of methane increased in the atmosphere?

A

Methane is produced in digestive processes of certain livestock

More livestock to feed growing population means more methane is produced

91
Q

How can carbon dioxide emissions be reduced?

A

Limit use of fossil fuels and become more energy efficient

92
Q

How can data be collected about what the atmosphere was like?

A
  • fossils
  • tree rings
  • gas bubbles trapped in ice sheets
93
Q

How do you carry out a flame test?

A
  • clean a nichrome wire loop by dipping it in HCL and rinsing it with distilled water
  • dip wire loop in metal compound
  • put loop in clear blue part of flame
94
Q

Flame test for lithium and sodium

A 
Lithium = crimson red
Sodium = yellow
95
Q

Flame test for potassium and calcium

A 
Potassium = lilac
Calcium = orange-red
96
Q

Flame test for copper

A

Green flame

97
Q

Metal Ions - Precipitate with NaOH

Colour of aluminium precipitate

A

White at first, but redissolves in excess NaOH to form a colourless solution

98
Q

Metal Ions - Precipitate with NaOH

Colour of calcium precipitate

A

White

99
Q

Metal Ions - Precipitate with NaOH

Colour of copper precipitate

A

Blue

100
Q

Metal Ions - Precipitate with NaOH

Colour of iron(II) precipitate

A

Green

101
Q

Metal Ions - Precipitate with NaOH

Colour of iron(III) precipitate

A

Brown

102
Q

What is the test for ammonia gas?

A

Damp red litmus paper will turn blue

103
Q

Qualities of ammonia

A

Strong smell, is an irritant and toxic

104
Q

How do you tell if a substance contains ammonium ions?

A

Add sodium hydroxide solution to a solution of mystery substance and gently heat it - if ammonia has is given off then it has ammonium ions in it

105
Q

How do you test for halide ions?

A

Add some dilute nitric acid followed by a few drops of silver nitrate solution to the halide

106
Q

Halide Ion Test

Colour of chloride precipitate of silver chloride

A

White precipitate

107
Q

Halide Ion Test

Colour of bromide precipitate of silver bromide

A

Cream precipitate

108
Q

Halide Ion Test

Colour of iodide precipitate of silver iodide

A

Yellow precipitate

109
Q

What is the test for carbonate ions?

A

Add some dilute acid - if carbonate ions are present, the mixture will fizz as carbonate will react with the acid to produce CO2 gas

110
Q

What is the test for sulfate ions?

A

Add dilute HCL to sample - this stops any precipitation reactions not involving the sulfate ions happening

Then add some barium chloride solution - if there are sulfate ions, a white precipitate will form

111
Q

What is flame photometry?

A

An instrumental method that allows you to identify ions in a dilute solution

112
Q

How do you work out which ion is present in flame photometry?

A

Each ion produces a unique line spectrum with different lines present in different places

113
Q

How do you work out the concentration of an ion present in flame photometry?

A

The intensity of the measured wavelength indicates conc.

The intensity can be found using a calibration curve (reading off a graph)

114
Q

Why is flame photometry better than flame tests?

A

Can identify different ions in mixtures, but flame tests only identify a single metal ion

115
Q

Why do chemists often use instrumental analysis (machines) to analyse unknown substances?

A

Very sensitive - detects tiny amounts
Very fast - automated
Very accurate - no human error

116
Q

How small are nanoparticles?

A

1-100nm across, contain a few hundred atoms - so they’re bigger than atoms and simple molecules

117
Q

What are fullerenes?

A

Nanoparticles, including nanotubes = tiny hollow carbon tubes - all the carbon bonds make them very string

118
Q

What is nanoparticles SA:V?

A

Big SA:V

119
Q

Why are nanoparticles good catalysts?

A

Reactions take place on the surface of catalysts, so the big SA gives more space for collisions

120
Q

How are nanoparticles used cosmetically?

A

In sunscreens as the small particles provide better protection but don’t leave white marks on the skin

121
Q

What is the idea behind nanomedicine?

A

Tiny fullerenes are absorbed more easily by the body than most particles, so they could deliver drugs right into the cells needed

122
Q

What could lubricant coatings using fullerenes be used in?

A

Artificial joints and gears

123
Q

How are nanotubes used in computer chips?

A

They conduct electricity so can be used in tiny electric circuits

124
Q

How do nanoparticles improve plastics?

A

Make them stronger, more durable, without adding much mass

125
Q

What and why are silver nanoparticles?

A

Added to polymer fibres used to make surgical masks and wound dressings - gives the fibres antibacterial properties

126
Q

What are the worries about nanoparticles?

A

We don’t know the side effects or long-term impacts on health, so they must be tested thoroughly

127
Q

What is high-density poly(ethene) used for and it’s qualities?

A

Make water pipes - strong/rigid

128
Q

What is low-density poly(ethene) used for and it’s qualities?

A

Plastic bars and squeeze water btls - light/stretchy

129
Q

What is poly(styrene) used for?

A

Packing to protect breakable things and as a thermal insulator

130
Q

What is used to make plastic kettles due to its heat-resistant quality?

A

Melamine resin and poly(propane)

131
Q

Qualities of glass

A

Transparent, strong, can be moulded when hot, brittle when thin

132
Q

How is glass made?

A

Soda-lime glass is made by heating limestone, sand and sodium carbonate until they melt - when it cools it is glass

133
Q

Qualities of clay

A

Soft when dug up, easy to mould, hardened by high temp, withstands weight

134
Q

What is clay actually made from?

A

A mineral formed from weathered and decomposed rock

135
Q

What are composites?

A

One material (the reinforcement) embedded in another (the matrix/binder)

136
Q

Qualities of metals

A

Good conductors, high density, malleable

137
Q

Pros to polymers

A

Flexible, less dense, cheap, insulators

138
Q

Cons to polymers

A

Degrade and break down over time so don’t always last long

139
Q

Pros to ceramics

A

Insulators, brittle, stiff, strong, hard-wearing, don’t degrade nor corrode

140
Q

Pros to metals

A

Conductors, malleable, corrosion resistant metals last a long time

141
Q

Cons to metal

A

Corrosion, less brittle so likely to deform but stay in one piece (not shatter)

142
Q

Cons to composites

A

Very expensive

143
Q

Pros to composites

A

Mix of qualities of two different materials which can be changed for specific pirposes

Chemistry (16 decks)

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