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Stuff To Remember (C1,C2,C3) using OCR Gateway Chemistry for GCSE revision guide

Terms in this set (60)

Eggs & Meat
Protein molecules denature when cooked; Transparent Liquid --> White Solid
2NaHCO3 -->
Na2CO3 + H2O + CO2
Hydrophilic ...?
Head
Hydrophobic ...?
Tail
Making an Ester
Alcohol+Organic Acid--> Ester+water
Ethanol + Ethanoic acid
Ethyl ethanoate
Properties of Esters
Volatile, Insoluble, Not toxic, doesn't react with perspiration/water and doesn't irritate skin
Alkenes
unsaturated as contain one or more c=c
Alkanes
saturated, only c-c bonds
Cracking
high temperature (400 to 700oC) and pressure aluminium oxide catalyst.Large ALkanes to smaller ones + Alkene. Produces more petrol fractions
monomers are used to make polymers in a ... ?
Addition polymerisation - high pressure using catalyst
alkanes
c x2 + 2
alkenes
c x 2
Bromine water changes colour in?
unsaturated solutions. Orange-brown --> colourless
Polymers are stronger with?
covalent crosslinking bridges between adjacent polymer molecules
nylon laminated in ptfe/polyurethane membrane?
Gore-Tex
Complete combustion?
CH4 + 2O2 --> Co2 + 2H2O, Blue flame
Incomplete Combustion?
4CH4 +5O2 --> 2CO + 2C + 8H2, Yellow flame
Energy/g fuel
Energy (J) = mass of water (g) x Temperature change x 4.2
Energy/1000 = KJ

KJ/mass of fuel = kj/gram of fuel
oil-based
Oil oxidised by O2 in air before solid, longer, indoor and outdoor woodwork
water-based
Solvent evaporates leaving a thin film of solvent and binding medium
Brick
Clay
Cement
limestone heated with clay
Concrete
limestone heated with clay then gravel or sand added with water, when solidifies concrete
reinforced concrete
Steel rod reinforcement to add steel strength to hardness of concrete
Oceanic plates slide under continental plates when they collide
due to oceanic plates being more dense than continental plates
Silica rich magma
explosive lava, rhyolite (small crystals), granite (large crystals)
Iron rich magma
runny lava runs slowly from volcano, basalt (small crystals), gabbro (large crystals)
electrolyte in copper electrolysis
copper (II) sulphate solution
copper electrolysis anode
impure copper
copper electrolysis cathode
pure copper
Amalgam
mercury
Brass
Copper and zinc
Solder
lead and tin
steel
iron and carbon (1%)
Bronze
copper and tin
Rusting
iron + oxygen + water --> hydrated iron (III) oxide
Composition of air
78% Nitrogen, 21% Oxygen, 0.0035% Carbon Dioxide
Carbon monoxide
incomplete combustion of petrol or diesel in car creates this poisonous gas
oxides of nitrates
in car engines from reaction of Nitrogen and oxygen
Photochemical smog
Sunlight causes nitrogen oxide to combine causing ground-level smog
Sulphur dioxide
due to sulphur impurities in fossil fuel (e.g. coal)
Acid rain
oxides of nitrogen and sulphur dioxide mix with clouds to form dilute sulphuric acid and nitric acid, falling as acid rain, damages metal, buildings and statues, main cause power stations and internal combustion engines
Group 1
Alkali metals, more reactive down group, all have one e- in outer shell
Group 7
Halogens, less reactive down the group, all have 7 e- in their outer shell
reaction of alkali metals with water
2M + 2H2O --> 2MOH + H2
Flame test
Lithium = red
Sodium = yellow/orange
Potassium = lilac
Halogen + Alkali Metal --> alkali metal halide
2K + 2Cl --> 2KCl
Displacement of Br in NaBr by Cl
Cl2 +2NaBr --> 2NaCl + Br2
2Al2O3-->?
Al3+ + 3e- --> Al at cathode
2O2- --> O2 + 4e-
Electrolysis of dilute sulphuric acid
2H+ + 2e- --> H2 cathode
4OH- --> 2H20 + O2 + 4e-
Transition metal compounds
copper compounds = blue
iron (II) compounds = light green
iron (III) compounds = orange/brown
Thermal decomposition of Calcium Carbonate
CaCO3 --> CaO + CO2
Precipitation reactions
insoluble solid precipitate forms. Sodium hydroxide added to a solution of a transition element compound.
Precipitations
copper (II) ions = blue
Iron (II) = grey-green
Iron (III) = orange-brown
Precipitation ionic equations
One OH- ion per positive charge on the metal ion.
Cu2+ + 2OH- --> Cu(OH)2
copper (II) ion + hydroxide ions --> copper (II) hydroxide

Fe3+ + 3OH- --> Fe(OH)3
iron (II) ion + hydroxide ions --> iron (III) hydroxide
Metallic bonding
Lattice of positive metal ions is held together by a 'sea' of free, mobile/delocalised e-. the e- can move throughout the regular structure of positive metal cations allowing electrical conduction
Properties of metal
High mpt and bpt -> Due to the large amount of energy needed to overcome the strong attraction between the delocalised e- and the positive metal cations

Good Electrical conductivity - The e- can move throughout the regular structure of positive metal cations allowing electrical conduction when the metal is connected to a power supply.

Metals that have a higher tensile strength -> due to stronger electrostatic attraction between delocalised e- and positive metal ions

Metals which are better conductors --> must have e- which move more easily
In Metal
Not all e- delocalised, as positive ions contains some as it is not just atomic nuclei but an ion
Superconductors
used to;
make powerful electromagnets
make superfast electronic circuits
transmit power with minimal energy loss

Problem is that with many superconductor they only work at extremely low temperatures. This is expensive as to do so special cooling equipment is needed aswell as a large amount of power to maintain the cooling of the cables.

That is why scientists are interested in developing superconductors which can work at 20 degrees celsius
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