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Chemistry Paper 2 > All topics > Flashcards

All topics Flashcards

1
Q

what do you call the elements in Group 1?

A

alkali metals

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2
Q

how are the physical properties of alkali metals different to other metals

A

are soft - can be cut with a knifehave low melting points - but are still solid at room temp

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3
Q

how does reactivity change in alkali metals?

A

as you go down the group the reactivity increases

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4
Q

what happens to the metals lithium, sodium and potassium when reacting with water

A
  • lithium fizzes steadily- sodium melts into a ball from the heat released- potassium gives off sparks and the hydrogen produces burns with a lilac coloured flame
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5
Q

alkali metals react with water to create…

A

an alkaline metal hydroxide and hydrogen

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6
Q

what are the densities of alkali metals like

A

they are less dense than water so they float

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7
Q

how are alkali metals stored and why?

A

they are stored in oil to keep oxygen and water away

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8
Q

why do alkali metals become less reactive as they move down the group?

A

all alkali metals have 1 electron on their outer shell. this means in reaction it is given away. the larger the atom, the further away the final electron is from the nucleus which means there is a weaker force of attraction between the electron and nuclear. this means larger alkali metals give away their final electron easier and are therefore more reactive

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9
Q

what do you call the elements in group 7?

A

halogens

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10
Q

give 4 halogens

A

fluorine, chlorine, bromine, iodine

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11
Q

true or false? halogens are never molecules

A

false, they are always molecules

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12
Q

how do the melting/boiling points change when going down the halogen group and why?

A

they both increase as the intermolecular forces between each molecule become much stronger

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13
Q

how does the colour change as you go down group 7, give examples.

A

it gets darker, for example, chlorine is yellow-green, while iodine is dark grey

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14
Q

how does reactivity change as you go down the halogen group? why?

A

it gets less reactive, this is because each halogen has 7 electrons in its outer electron, the easier it gains an electron the more reactive it is. As you go down the group the atoms get larger meaning the force of attraction is weaker by the time it reaches the outer electron. therefore the smallest atoms find it easier to attract electrons therefore as you go down the group the atom gets less reactive

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15
Q

metals and halogens react to create…

A

metal halides

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16
Q

sodium + chlorine –>

A

SODIUM CHLORIDE

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17
Q

give an example of a halogen displacement reaction

A

chlorine water will displace the bromine in sodium bromide to create a sodium chloride solution

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18
Q

give the redox reaction for the halogen displacement reaction between bromine and chlorine

A

2Cl + 2e –> 2CL- (reduced)2Br- –> Br2 + 2e- (oxidised)

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19
Q

what do you call elements in group 0?

A

noble gases

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20
Q

what is the most important chemical property of noble gases? and why?

A

they are inert - because they have full outer electrons they do not tend to lose, gain or share electrons

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21
Q

what is helium used for and why?

A

helium is used as a lifting gas in party balloons and airships. this is because how it is less dense than air so it causes airships to rise., it is also non-flammable so will not ignite

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22
Q

what are argon, krypton and xenon used for and why?

A

it is used as a filling gas in filament lamps. its inertness stops it from burning away

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23
Q

what is argon used for and why?

A

it is a shielding gas during welding as it is denser than air so it keeps air away from the metal during welding, it is inert so it won’t oxidise the metal

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24
Q

what is the test for chlorine?

A

damp blue litmus paper will turn red and then go white

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25
Q

what are the factors that affect the rate of a reaction?

A

concentration and pressuretemperaturesurface area: volume ratiocatalyst

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26
Q

how do concentration and pressure affect the rate of reaction?

A

it increases as the conc increases which means that there are more particles in the same volume which increases the number of successful collisions between reacting particlesit also increases as the pressure increases which means that there is less space for the particles to move around which means that there will be more successful collisions

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27
Q

how does temperature affect the rate of reaction?

A

an increase in temperature increases the kinetic energy of the particles which means that the particles will be moving faster the frequency of collisions increases and so does the energy of each collision. this increases the rate of reaction as it means there will be more successful collisions

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28
Q

how does the surface area: volume ratio affect the rate of reaction

A

the rate of reaction increases when the surface area to volume ratio increases (for example when lumps are made into powder). this is because the larger surface area allows there to be more particles of the reactant available for the reaction, which increases the frequency of successful collisions

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29
Q

what is the equation for the rate of reaction?

A

change/time

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30
Q

what are the two types of reaction (temp)

A

exothermic and endothermic

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31
Q

what is an exothermic reaction?

A

a reaction where heat energy is given out which causes the surroundings to increase in temperature

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32
Q

what is an endothermic reaction?

A

a reaction that takes in heat energy, and decreases the temperature of its surroundings

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33
Q

is a displacement reaction an endothermic or exothermic reaction

A

exothermic

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34
Q

explain why energy is released or used up in reactions

A

Breaking bonds in endothermic (energy is needed)making bonds in exothermic(energy is released)

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35
Q

what is the activation energy?

A

the minimum energy required to start a reaction

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36
Q

what does the energy profile for an exothermic reaction look like

A
  • the energy level of the reactants is greater than the energy of the products- there is negative energy change as energy has been lost to the surroundings
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37
Q

what does the energy profile of an endothermic reaction look like

A
  • the energy level of the reactants is less than the energy level of the products- there is a positive energy change as the energy is transferred from the surroundings
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38
Q

what is bond energy?

A

the energy needed to break 1 mol of a particular bond

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39
Q

what is crude oil?

A

a type of fossil feul formed over millions of years from the remains of marine organisms

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40
Q

what are hydrocarbons

A

compounds that are made of hydrogen and carbon atoms only.

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41
Q

what is a finite source?

A

will eventually run out as they are no longer being made or are being made extremely slowly

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42
Q

what are 2 uses of crude oil?

A
  • fuel- feedstock from the petrochemical industry (uses oil to make things such as plastic)
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43
Q

what is fractional distillation for crude oil?

A

a method used to separate crude oil into simple mode useful mixtures

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44
Q

what are the 4 steps to using fractional distillation on crude oil?

A
  • oil is heated to evaporate it- vapours rise in a fractionating column- the column has a temperature gradient, hot at the bottom and cool at the top.- each fraction condenses where it becomes cool enough and is piped out of the column
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45
Q

what features does a fraction of crude ould will a small number of atoms show?

A

lowest boiling point, most flammable, runny - least viscous

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46
Q

what features does a fraction of crude ould will a high number of atoms show?

A

highest boiling point, least flammable, most vicious

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47
Q

what is the use of gases from crude oil?

A

domestic heating and cooking

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48
Q

what is the use of petrol from crude oil?

A

fuel for cars

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49
Q

what is the use of kerosene from crude oil?

A

fuel for aircraft

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50
Q

what is the use of diesel from crude oil?

A

fuel for larger vehicles and trains

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51
Q

what is the use of fuel oil from crude oil?

A

fuel for large ships and power stations

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52
Q

what is the use of bitumen from crude oil?

A

surfacing roads and roofs

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53
Q

what are the properties of homologous series?

A
  • all members have similar chemical properties- show a gradual variations in physical properties
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54
Q

what are some chemical properties of alkanes?

A
  • undergo complete combustion when they react with oxygen- use only single bonds
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55
Q

what is the general formula for alkanes

A

Cn + H2n+2

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56
Q

what are the first 8 alkanes?

A

methaneethanepropanebutane pentanehexaneheptaneoctane

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57
Q

how does incomplete combustion happen

A

when there is a lack of oxygen

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58
Q

compare the products of complete and incomplete combustion

A

complete -> water + carbon dioxideincomplete -> water + carbon monoxide + carbon (soot) + less energy

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59
Q

why is carbon monoxide dangerous?

A

produced in incomplete combustion it is a colourless and odourless gas. when breathed in it can attach to haemoglobin in blood, reducing the amount of oxygen being carried around the blood

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60
Q

what are the 3 problems caused by soot?

A

soot can build up in chimneys where it can cause fireblackens buildingssoot particles can be breathed in which can cause lung disease

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61
Q

how is acid rain formed?

A

when sulfur dioxide (from the combustion of hydrocarbon fuels) dissolves in water

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62
Q

what are 3 ways can the environmental damage from acid rain be reduced?

A
  • removing sulfur from oil (refining at oil refinery) before selling it- preventing sulfur dioxide from leaving the power station chimneys- adding calcium carbonate to fields and lakes to neutralise the excess acid
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63
Q

what are some of the effects of acid rain?

A
  • acid rain speeds up the weathering of buildings and statues- trees are damaged- rivers, lakes and soils are more acidic which harms organisms living in them
64
Q

how is nitrogen oxide produced when using hydrocarbons?

A

airt goes into the engine so that the fuel can burn, this means that nitrogen and oxygen from the air can react together in the high temperatures of the engine to produce nitrogen

65
Q

what is a non-renewable resource?

A

a recourse that is being used up faster than it is being formed

66
Q

what are 3 features of a good fuel?

A

burn easily - it should be easy to ignite and stay alightnot produce soot, smoke or ashrelease a lot of energy when it burnseasy to store and transport

67
Q

give the word equation for the combustion of hydrogen

A

hydrogen + oxygen –> water (+energy)

68
Q

what are 2 ways that hydrogen is manufactured?

A

electrolysis of water cracking oild fractionsreaction of natural gas and steam

69
Q

what are 4 positives of petrol?

A
  • burns easily- does not produce ash- releases more energy than coal or wood- is a liquid so is easy to store and transport
70
Q

what are 2 negatives of petrol?

A
  • produces Carbon dioxide and carbon monoxide- non-renewable
71
Q

what are the 4 positives of hydrogen as a fuel?

A
  • burns easily- does not produce ash or smoke- only produces water when burned (no carbon dioxide)- releases 3 times as much energy as petrol
72
Q

what are 2 negatives of hydrogen as a fuel?

A

is a gas so is hard to store as it needs to be stored at high pressuresnew infrastructure needs to be created

73
Q

what is cracking

A

breaking down loner alkanes into smaller and more useful alkenes/alkanes

74
Q

what was the most prominent gas in the Earth’s early atmosphere give 2 pieces of evidence

A

carbon dioxideCO2 is produced by the volcanoessimilar planets also have CO2

75
Q

what elements make up our atmosphere today (percentages)

A

78% nitrogen21% oxygen1% other

76
Q

give 2 reasons why levels of CO2 decreased in the early atmosphere

A
  • carbon dioxide dissolved in the oceans- Marine organisms used up the dissolved carbon for their wheels which allowed for more carbon to dissolve
77
Q

give 2 reasons why levels of oxygen increased in the early atmosphere

A

photosynthesis in organisms produces more oxygen

78
Q

how do very old iron rocks show proof of a change in the early atmosphere?

A

it proves that the early atmosphere contained no oxygen as the iron would not have been oxidised. Later rocks would have had their iron oxidised which shows that oxygen was now present in the atmosphere

79
Q

what is the test for oxygen?

A

a glowing wooden splint relights in oxygen

80
Q

what is global warming?

A

the increase in temperatures of the world due to the greenhouse effect

81
Q

what is the greenhouse effect?

A

when greenhouse gases stop the heat emitted from the earth from escaping by reflecting them towards the earth, causing an increase in temperature

82
Q

what is climate change?

A

long term changes to weather patterns or the climate in a certain area

83
Q

what 2 tests are there for metal ions

A

flame testshydroxide precipitates

84
Q

what are the 5 ions that can be tested for using the metal flame test and what colours do they go?

A

lithium - Li+ - red sodium - Na+ - yellowpotassium - K+ - lilaccalcium - Ca2+ - orangey-redcopper - Cu2+ - blue-green

85
Q

how do hydroxide precipitates help you identify metal ions?

A

some metal ions form coloured hydroxide precipitates. add few drops of sodium hydroxide solution

86
Q

what are the 5 ions that can be tested for using the metal hydroxide precipitates and what colours do they go?

A

copper - blueiron(II) - greenIron(III) - browncalcium - whitealuminium - white

87
Q

how can you identify calcium and aluminium using the hydroxide precipitates test?

A

add excess sodium hydroxide, aluminium would dissolve and form a colourless solution while the calcium would stay white

88
Q

how can you test for sulfate ions?

A

add hydrochloric acid, followed by barium chloride. if sulfate ions are present they will form a white precipitate of barium sulfate

89
Q

how can you test for carbonate ions?

A

add acid, if present bubbles of CO2 will show

90
Q

how do you test for halide ions?

A

add dilute nitic acid, followed by silver nitrate solution. if present a coloured precipitate would form

91
Q

what are the 3 halide ions that can be tested and what colour do they go?

A

chloride - white (milk)bromide - cream (cream)iodide - yellow (butter)

92
Q

what is the test for ammonium ions?

A

add sodium hydroxide solution and heat, if present ammonia will be produced as a gas

93
Q

what are the 3 ways to detect ammonia gas?

A
  • damp red litmus paper turns blue- hydrogen chloride gas reacts with ammonia to form white smokes of ammonium chloride- ammonia has a characteristic sharp smell
94
Q

what are the 3 advantages of using instrumental methods to detect substances?

A
  1. sensitivity - they can detect and analyse very small amounts of different substances2. accuracy - they measure amounts of different substances very accurate3. speed - they can carry out each analysis quickly and the machines can run all the time
95
Q

what is flame photometry and what data does it allow you to get?

A

is a type of instrumental substance analysis. it allows you to identify the substance. calculate the concentration of each solution using a calibration curve

96
Q

what is the general formula for alkenes?

A

CnH2n

97
Q

what is the function group for alkenes?

A

C=C

98
Q

how do you test for alkenes and how does it work

A

Add a few drops of bromine water, since alkenes are unsaturated they will react with the bromine and form a colourless solution

99
Q

what is an isomer?

A

a hydrocarbon where the functional group is in a different place

100
Q

what is a polymer?

A

a polymer is a substance that is made up of small repeating units called monomers. They usually have very high formula mass

101
Q

what is addition polymerisation?

A

combining smaller alkenes to make large polymers

102
Q

how do you show a polymer

A

you show one monomer in brackets with an N next to it

103
Q

what are the 4 polymers we need to know

A

poly(ethene)poly(propene)poly(chloroethene)poly(tetrafluoroethene)

104
Q

what are some properties and uses for poly(ethene)

A

Properties- flexible - cheap- electrical insulatorUses- plastic bags and bottles- clingfilm

105
Q

what are some properties and uses for poly(propene)

A

Properties-flexible- shatterproof- has a high softening pointUses- buckets - bowls

106
Q

what are some properties and uses for poly(chloroethene)

A

Properties- touch, long-lasting- cheap- electrical insulatorUses- window frames- gutters and pipes- electrical wire insulator

107
Q

what are some properties and uses for poly(tetrafluoroethene)

A

Properties- tough- slippery- resistant to corrosion- electrical insulatorUses- non-stick coatings for frying pans- containers for corrosive substances- electrical insulator

108
Q

how are polyesters formed?

A

condensation polymerisation

109
Q

what 2 types of monomers are needed in condensation polymerisation

A

molecule containing carboxylic acida molecule containing an alcohol group

110
Q

what is a by-product of condensation polymerisation?

A

water

111
Q

what are 2 biological polymers?

A

DNA and protein show

112
Q

what process do biological polymers use

A

condensation polymerisation

113
Q

what are the monomers of DNA?

A

nucleotides - made up of a phosphate, sugar and group

114
Q

what shape is the DNA sugar in diagrams

A

pentagon

115
Q

what are the monomers of Proteins?

A

amino acids

116
Q

what are reactive groups in condensation polymerisation?

A

the 2 ends of a monomer that react to join the monomers together

117
Q

what materials are used to make polymers and what are the problems

A

Crude Oil - finite - non-renewable - damages natural habitats

118
Q

what are an advantage and disadvantages of polymers not being biodegradable?

A
  • lasts a long time- will take a long to break when disposed of
119
Q

what are 2 negative ways of disposing of polymers?

A
  • landfills- burning
120
Q

what are the 3 negatives of using landfills to dispose of polymers?

A
  • not biodegradable- look ugly and attract pests- running out of landfill sites
121
Q

what is the problem with burning polymers?

A

many polymers release toxic gases when they burn

122
Q

what are biodegradable polymers?

A

they will rot away

123
Q

what are 2 positives of landfills?

A

waste is disposed of quicklyout of sight one it is covered over

124
Q

what is the functional group of alcohol?

A

OH

125
Q

what is the naming convention for alcohols?

A

end in -ol

126
Q

what is the result of ethanol being oxidised?

A

ethanoic acid

127
Q

name two drinking alcohols that contain ethanol

A

wine and beer

128
Q

what process is used to create ethanol

A

fermentation

129
Q

what is used to create enzymes for fermentation

A

yeast

130
Q

what is yeast

A

a single-celled fungus

131
Q

what is the process of fermentation?

A

a carbohydrate (such as glucose) in aqueous solution is put with yeast

132
Q

what is a by-product of fermentation?

A

carbon dioxide

133
Q

what are the conditions yeast need for fermentation and why

A
  • warm temp = if it is too cold the reaction will be too slow and if it is too warm the enzymes will denature- anaerobic respiration = is oxygen is present yeast will use aerobic respiration and form only water and carbon dioxide
134
Q

what process is used to obtain concentrated ethanol from an ethanol-water solution and why does it work

A

fractional distillation - ethanol has a lower boiling point than water

135
Q

what is the functional group for carboxylic acids?

A

-COOH

136
Q

how do you name carboxylic acids?

A

end in -anoic

137
Q

what are 3 chemical properties of carboxylic acids (similar to acids)?

A
  • react with carbonates to produce salt, water and carbon dioxide- react with magnesium (and other reactive metals) to produce a salt and hydrogen- dissolve in water to produce acidic solutions
138
Q

why are carboxylic acids weak?

A

this is because they only partially dissociate into ions when they dissolve in water

139
Q

what is the structural diagram for the functional group of carboxylic acid?

A

O=C-O-H

140
Q

what are nono-particles

A

structures containing only a few hundred atoms

141
Q

why do nanoparticles have different properties from the same substance in larger pieces?

A

because of its size

142
Q

what are 3 uses of nano-particles

A

sunscreensfuture drug deliverycatalysts

143
Q

why are nano-particles used in sunscreens?

A

they absorb the UV but cannot be seen on the skin

144
Q

why are nano-particles used in drug delivery?

A

buckyballs are hollow balls made up of carbon atoms that can be used to carry drugs

145
Q

why are nano-particles used as catalysts?

A

they are very small so have a very large surface area: volume ratio

146
Q

give 2 properties of nanoparticles

A

strong and light

147
Q

what are the 3 dangers of nanoparticles?

A
  • if breathed in, they are so small that they can be absorbed through the skin or transported into cells- take a long time to break down- attract toxic substances to their surfaces
148
Q

what is the size of a nanoparticle?

A

1-100 nanometres

149
Q

what are 4 bulk materials?

A

glass ceramicsclay ceramicspolymersmetals

150
Q

what are some properties of glass ceramics?

A

transparenthard but brittlepoor conductors of heat and electricity

151
Q

what are some properties of clay ceramics?

A

opaquehard but brittlepoor conductors of heat and electricity

152
Q

what are some properties of polymers?

A

can be transparent, translucent or opaquepoor conductors of heat and electricityoften touch and ductile

153
Q

what are some properties of metals?

A

can be polished to a shinegood conductors of heat and electricityhard, tough and ductile

154
Q

what is the definition of brittle

A

will crack or break when hit

155
Q

what is the definition of ductile

A

can be bent, twisted or stretched without cracking or breaking

Chemistry Paper 2 (11 decks)

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