Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

gcse notes > chem paper 2 > Flashcards

chem paper 2 Flashcards

(94 cards)

Start Studying
1
Q

group 1 characteristics

A

shiny when freshly cut
good conductors
solid at room temp
soft
produce white/colourless ionic compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

group 1 melting point trend

A

melting point decreases as you go down the group
more distance between nucleus and valence electron
decreased electrostatic forces
metallic bond weakens
easier to break

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

group 1 reactivity trend

A

reactivity increases down the group
outer electron becomes easier to lose because more distance weaker bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

how does lithium, sodium and potassium react in water

A

lithium - fizzes steadily and slowly disappears

sodium - melts to form a silvery ball, fizzes vigorously and quickly disappears

potassium - immediately ignites, burns with a lilac flame, very quickly disappears

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

group 7 characteristics

A

brittle in solid state
poor conductors

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

group 7 elements appearance

A

flourine - pale yellow gas
chlorine - green gas
bromine - orange-brown liquid
iodine - shiny grey-black crystalline solid and purple vapour

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

group 7/0 melting point trend

A

melting point increases as you go down
gain extra electron shells
so intermolecular forces are stronger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

group 7 reactivity trend

A

reactivity decreases as you go down
increased electron shielding
reduces attractive forces of nucleus
so can’t get an electron to react

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

halide colours

A

chloride - white
bromide - cream
iodide - yellow

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

transition metals characteristics

A

shiny when freshly cut
good conductors
strong
malleable
produce coloured ionic compounds
good catalysts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

metals that arent solid at room temp

A

mecury (liquid)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

how to detect chlorine

A

dampen blue litmus paper
paper turns blue to red to white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

how to detect hydrogen and oxygen

A

hydrogen: lit splint should make a squeaky pop

oxygen: glowing splint should relight

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

flame test colours

A

lithium - red
sodium - yellow
potassium - lilac
calcium - orange
copper - green

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

how to do a hydroxide precipitate test

A

add a few drops of sodium hydroxide solution to a solution containing metal ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

hydroxide precipitate colours

A

iron 2 - green
iron 3 - orange brown
copper 2 - blue
calcium - white
zinc - white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

how to differentiate between calcium and zinc hydroxide

A

add excess sodium hydroxide
zinc becomes colourless and calcium stays white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

how to detect sulfate ions

A

add a few drops of hydrochloric acid
then few drops of barium chloride solution

if sulfate present then you get a white precipitate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

how to detect halide ions

A

add a few drops of dilute nitric acid

then a few drops of silver nitrate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

how to interpret mass spectra

A

each peak is a fragment of the molecule

the peak on the far right represents the molecular ion

the mass:charge of the molecular in peak is the Mr of the molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what affects percentage yield

A

reactants may react unexpectedly
reaction may not complete
may lose product when you separate it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

atom economy

A

sum of Mr of desired product/ sum of Mr of all products x 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

factors for reaction pathway

A

product yield
atom economy
usefulness of by-products
rate of reaction
equilibrium position

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

how to carry out a titration

A

measure out 25cm2 of alkali solution using a volumetric pipette and pour into your conical flask
add a few drops of phenolphthalein
ensure your burette is closed and pour your acid solution in until it hits zero
put an empty beaker underneath and run the burette tap through to get rid of any air bubbles and refill the burette
the burette should be clamped, at the bottom of the clamp stand you should have a white tile underneath your conical flask
run your acid solution through in intervals and swirl your flask
repeat until the mixture turns clear
then read off the titre at the bottom of the meniscus
repeat until you obtain at least 2 concordant results

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
mole calculations using avogadro's constant
number of particles = avogadro's constant x number of moles
25
gas volume formula
volume in dm3 = amount in mol x 24dm3/mol
25
molar volume
the volume that one mole of any substance occupies at the same temp and pressure 24dm3/mol = 24000cm3/mol
26
why do reactions go faster at higher temps (exact wording)
particles have more energy so move faster so increased collision frequency so more successful collisions
26
why do reactions go faster at higher concentrations (exact wording)
more crowded particles in same volume increased collision frequency so more successful collisions
27
why do reactions go faster with powders (exact wording)
more surface area so more particles available to come into contact so increased collision frequency so more successful collisions
28
how to investigate the effect of temperature
sodium thiosulfate solution and hydrochloric acid Na2S2O2 aq + 2HCl aq -> 2NaCl aq + H2O l + SO2 g + S s beakers should be placed in an ice bath to reduce acidic fumes place beaker on paper with a cross mix reactants in beaker record how long it takes for the cross to disappear vary the temp by warming up one of the solutions before mixing
29
how to investigate the effect of powders
calcium carbonate and hydrochloric acid CaCO3 s + 2HCl aq -> CaCl2 aq + H2O l + CO2 (g) gas syringe measure volume of co2 produced in certain amount of time
30
how to use reaction times
1/reaction time = rate of reaction
31
investigating a catalyst
manganese (IV) oxide catalyses decomposition of hydrogen peroxide 2H2O2 aq -> 2H2O l + O2 g hydrogen peroxide solution in a conical flask with a stopper with a gas syringe put catalyst in, stop it, start stopwatch record time and volume of oxygen at regular intervals
32
how do catalysts work
they provide an alternative reaction pathway with a lower activation energy a greater portion of colliding particles now meet the activation energy so the rate of successful collisions increases
33
what happens at equilibrium
forwards and backwards reaction rates become equal concentration of all reacting substances are constant
33
the equilibrium yield
amount of desired product present in a reaction at equilibrium
34
elements needed in plants
nitrogen poor growth yellow leaves phosphorus poor root growth discoloured potassium poor fruit growth discoloured leaves
35
water soluble form of elements for fertilisers
nitrate NO3- ammonium NH4+ phosphate PO4 3- potassium ions K-
36
raw materials needed
phosphate rock sulfur natural gas air water potassium chloride
37
making potassium sulfate
titration but alkali is potassium hydroxide indicator is phenolphthalein acid is sulfuric acid add activated charcoal then filter it out to remove indicator warm filtrate to evaporate don't heat to dryness
38
making ammonium sulfate
titration but alkali is ammonia solution indicator is methyl orange (yellow to red) acid is sulfuric acid ammonia gives off sharp irritating smell and excess gives off gas don't breathe it in
39
what is an ore
rock and mineral that contains enough metal/metal compound to make it economical to extract it
40
ore examples
malachite - copper carbonate bauxite - aluminium oxide haematite - iron 2 oxide
41
acid mine drainage
metal sulfides oxidise underwater making sulfuric acid reacts with other metal ores and leave with water as it drains from the mine
42
bioleaching
bacteria respire oxidising iron 2 and sulfide ions making sulfuric acid which breaks down other minerals releasing metal ions
43
phytoextraction
crop grows on soil with metal complexing agent added to enhance metal uptake by crop crops burned ash treated like a high grade ore
44
corrosion and rusting
corrosion is reaction of metal with surroundings rusting is just iron and steel corroding
45
rusting equation
iron + oxygen + water -> hydrated iron 3 oxide
46
how to investigate rusting
3 test tubes with an iron nail in each 1st anhydrous calcium chloride and bung 2nd boiled water and bung 3rd half filled with water and no bung record appearance of nails after a day
47
how to reduce rusting
painting coating with oil grease or plastic galvanising (zinc plating) tin plating
48
sacrificial protection
the more reactive metal, loses electrons more easily and so is more readily oxidised and corroded
49
alkenes addition reactions
ethene + bromine -> dibromoethane decolourisation reaction alkene, bromine water goes colourless alkane, bromine water stays orange brown ethene + hydrogen -> ethane (only happens with a nickel catalyst)
49
alcohols
CnH2n+1OH ethanol + oxygen (burning) -> carbon dioxide and water
50
carboxylic acid trends
CnH2n+1COOH
51
how are carboxylic acids made
alcohols react with oxidising agent to make carboxylic acids oxidising agent - potassium mangante (VII) solution purple reduced to manganese (II) ions pale pink violent reaction ethanol is harmful and flammable oxidising agent stains hands/clothing
52
cracking and its conditions
600 to 700 degrees hot catalyst of alumina or silica
52
small alkanes vs big alkanes (characteristics)
small: low bp flow easily easy to ignite big: opposite
53
how did the atmosphere form
lots of volcanic activity during earth's early years releases lots of water vapour and co2 earth cools water vapour condenses forming oceans algae and plants photosynthesised using all the co2 and releasing lots of oxygen
54
pollutants meaning
substances released into the environment that may harm living things
55
why is carbon monoxide a problem
toxic colourless no taste smell attaches to haemoglobin reduces oxygen in bloodstream drowsiness difficulting breathing death
56
why are particulates a problem
settle deep in lungs when breathed in causing bronchitis and other breathing problems increases chance of heart disease
57
why are acidic oxides a problem
nitrogen monoxide dissolves in cloud moisture and become acid rain sulfur dioxide does the same
58
greenhouse gas effect
energy from sun reaches earth's surface warms up the earth infrared radiation is emitted back some of it is absorbed by ghg ghg emit infrared radiation absorbed in all directions warms atmosphere and surface
59
common ions
ammonium NH4+ nitrate No3- carbonate CO3 2- sulfate SO4 2-
60
haber process equation
N2 g + 3H g = 2NH3 g
61
raw materials and conditions for haber process
liquified air natural gas steam 200 atmospheres 450 degrees iron catalyst
62
raw materials for contact process
sulfur air water
63
contact process stage 1
sulfur burns in air to make sulfur dioxide S s + O2 g -> SO2 g
64
contact process stage 2
sulfur dioxide and more oxygen to make sulfur trioxide 2SO2 g O2 g = 2SO 3 g
64
contact process stage 3
sulfur trioxide is converted to sulfuric acid (H2O l + SO3 g -> H2SO4 aq) in two steps sulfur trioxide passed through sulfuric acid to make oleum H2SO4 l + SO3 g -> H2S2O7 l oleum added to water to make sulfuric acid H2S2O7 l + H2O l -> 2H2SO4 aq
65
conditions for contact process
2 atmospheres 450 degrees vanadium (V) oxide catalyst
66
how to make alcohol using ethene
ethene + steam = ethanol C2H4 g + H2O g = C2H5OH g 60 atmospheres 300 degrees phosphoric acid catalyst
67
how is copper extracted
copper sulfide is burned in air to make copper oxide and sulfur dioxide copper oxide is then put in a crucible with charcoal lid on, let it do its thing copper sinks to the bottom and charcoal is in the water so separate copper by washing it
68
raw materials for a blast furnace
iron ore (haematite) coke limestone hot air
69
extracting iron stages
coke (carbon) burns in the air (oxygen) making co2 coke reacts with co2 making carbon monoxide carbon monoxide reudces iron 3 oxide to iron
69
removing impurities from blast furnace
impurities in the iron are removed using limestone (calcium carbonate) calcium carbonate becomes calcium oxide and co2 calcium oxide reacts with silica (SiO2 g) to form calcium silicate (CaSiO3 l) calcium silicate is known as slag
70
conditions for aluminium electrolysis
aluminium oxide is dissolved in molten cryolite insulation then carbon lining of cell (cathode) then what we're separating then molten aluminium with a tapping hole at the top carbon anodes
71
steel
iron buildings bridges, cars
72
duralumin
aluminium and copper aircraft parts
73
solder
tin and copper joining electrical components
74
brass
copper and zinc musical instruments and coins
75
bronze
copper and tin bells, propellers for ships
76
alloy meaning
mixture of two or more elements, at least one of which is a metal
77
ceramics
hard non metallic materials brick china porcelain glass high melting points hard stiff brittle poor conductors unreactive because mostly oxides
78
composite materials
material made from two or more materials combined resin fibreglass (glass fibres in resin) for boats, canoes, surfboards carbon fibre (carbon fibres in resin) used for sports equiment, racing cars, aircraft parts concrete (small stones, sand, cement, water) buildings, foundations
79
what is a LCA
cradle to grave analysis of impact of making using and disposing a manufactured product
80
why recycle
conserve limited raw materials conserve limited energy resources reduce release of pollutants reduce waste
81
factors for recycling
how easily collected and sorted amount and type of by products cost of recycling amount of energy
82
how are materials recycled
metal melted and poured into blocks to make ingots paper mixed with water cleaned rolled heated to make new paper glass melted and moulded into new things polymers are melted into new things
83
addition polymers conditions
carbon carbon double bond high pressures catalyst
84
how to make a Daniell cell
zinc sulfate and zins strip in one beaker copper 2 sulfate and copper strip in another connect two with filter paper soaked in potassium nitrate connect voltmeter
85
fuel cell steps
hydrogen reacts with oxygen to make water vapour hydrogen molecules lose electrons 2H2 g -> 4H+ aq + 4e- at ANODE hydrogen ions combine with oxygen and electrons to make water vapour 4H+ aq + O2 g + 4e- -> 2H2O g at CATHODE
86
how is fresh water treated
passes through a metal screen to get rid of large objects (twigs leaves) sand and soil settle out aluminium sulfate and line added to get rid of dirt passes through sand to get rid of mud chlorine to kill bacteria pH checked then given

gcse notes (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions