Methane CH4
Ethane C2H6
Fractional
Distillation
Separating mixtures of liquids
because they boil (and condense)
at different temperatures
Examples: crude and vegetable oil
separation
Alkane (CnH2n+2)
Dodecane
C12H26
Alkane (CnH2n+2)
Rule: any liquid will boil and
condense at the same
temperature
Ethene C2H4
Cracking
Type of
thermal decomposition
that requires
heat and catalyst
Alkane (CnH2n+2)
Alkene (CnH2n)
Propene C3H6
Propane C3H8
Heating breaks down the chemical
bonds between the carbon atoms
of the hydrocarbon compound to
make new smaller sized
hydrocarbon compounds
CaCO3
CaO+CO2
Thermal decomposition
Process requires
Alkene (CnH2n)
Alkane (CnH2n+2)
heat
Carbon
Carbon Dioxide
C
Also exists as
Carbon Coke or as
Carbon particulates
Calcium
Carbonate
Complete
Combustion
CO2
(burning with
plenty of oxygen)
Calcium Oxide
C+O2CO2
e.g. carbon coke in blast
CaCO3
Also known as
CaO
Exothermic
limestone
Also is the cloudy
white
precipitate when CO2 gas
furnace
Also known as
Quicklime
reaction
(generates heat)
reacts with limewater
Calcium Hydroxide
Water
Ca(OH)2
H20
Also known as
limewater
Thermal
Decomposition
Heating breaks down the
chemical bonds in the
compound to make new
substances
Octane C8H18
also known as
Gasoline (Petrol)
Alkane (CnH2n+2)
Poly(ethene)
Ethanol C2H5OH
Made from renewable and
non-renewable sources
C12H26
C8H18+2C2H4
Cracking
dodecane to give
octane(petrol)
Polymerisation
Hydration
polymerisation
equation
Incomplete
Combustion
(burning with
limited oxygen)
Multiple monomer
molecules (e.g.
ethene) are joined
together to make a
longer molecule called
a polymer
CH4+2O2
CO2+2H20
H20 formed in U-tube
turns blue cobalt
chloride paper pink
Chemical reaction
in which
water (H20) is added
C2H4+H20
C2H5OH
Ethene reacts with steam
Requires 300C, 60atm
and phosphoric acid
catalyst
Non-renewable source
Glucose
C6H12O6
Energy source in most
organisms
Is a product of plant
photosynthesis
Plants store glucose as starch
C6H12O6
2C2H5OH+2CO2
Formation of ethanol
from glucose by
fermentation
Renewable source of
ethanol
Hydrogen gas
Fermentation
H2
H-H
Anaerobic
(without oxygen)
respiration of yeast
Single covalent bond
Carbon
Monoxide
CO
Made from combustion of
carbon (coke) or incomplete
combustion of hydrocarbons
Cell
Respiration
Aerobic
(with oxygen)
Toxic clear odourless gas
Electrolysis
Carbon Dimming
Global Warming
Caused by excessive
Caused by excessive
atmospheric Carbon
atmospheric CO2
particulates (soot)
Fe2O3 + 3CO
2Fe + 3CO2
Redox
C+O2CO2
2C+CO22CO
2C+O22CO
Reduction &
Oxidation
Reactions occurring in
a Blast Furnace
Type of chemical
Reaction
C6H12O6+6O2
6CO2+6H20
Generates energy(heat) in all
living organisms
Technically, cellular
respiration is a combustion
reaction
Occurs in cell mitochondria
Fossil fuels
Coal
Crude oil
Natural gas
formed by natural processes such
as anaerobic decomposition of
buried dead organisms
Electrolysis of brine
(sodium chloride, NaCl)
2NaCl+2H20
Cl2+H2+2NaOH
6CO2+6H20
C6H12O6+6O2
Reaction occurring in
plant chloroplasts that
contain chlorophyll
pigments
Photosynthesis
Light-dependent reaction
Sulfur dioxide
SO2
Sulfur can be removed from
fuels prior to burning the fuel
Sulfur dioxide emissions from
fossil fuel power plants can
Contain hydrocarbons
be reduced by reacting SO2
with CaO (quicklime)
Also contain sulfur and heavy
metal (e.g. lead) impurities
2NO22O2+N2
2CO+O22CO2
Redox reaction
occurring in a platinum
or palladium catalytic
converter
Nitrogen gas
Nitrogen dioxide
N2
NO2
78% of atmosphere is N2
For use by industry, nitrogen
is made by the fractional
distillation of liquid air
Liquid nitrogen is a cryogenic
liquid (boils at -195 C, 78 K)
Sulfuric Acid
H2SO4
Formed naturally from
SO2 emissions
(burning fossil fuels)
Formed industrially by
combining SO2 with O2 to
make sulfur trioxide SO3
CaCO3+H2SO4
CaSO4+H2O+CO2
Explains why limestone
statues corrode
(gradually dissolve away)
by acid rain
(e.g sulfuric acid)
Catalytic converter
(e.g. in car exhaust)
Air pollutant that arise
from any combustion
process that uses air
N2+O22NO
2NO+O22NO2
Acid Rain
Biodiesel
Formed when SO2 or
NO2 gases, produced
from combustion
processes, dissolve in
atmospheric water
vapour
Renewable source of
energy made from
plant (e.g palm oil) or
animal products (e.g.
animal fats, sewage)
Bromine water test
Br2
Bromine water is ORANGE
Test which shows the difference
between unsaturated and
saturated carbon bonds in organic
compounds
Br2 water, stays orange (saturated
e.g. alkanes, single C-C bond)
Br2 water, turns clear (unsaturated
e.g. alkenes, double C=C bond)
Hydrogen-oxygen
fuel cell
2H2 + O2 → 2H2O
CaO(s)+H20(l)
Ca(OH)2(s)
Quicklime reacts exothermically
(generates heat) with water to
produce slaked lime Ca(OH)2(s)
Recycling plastic
polymers
2H2 + O2
→ 2H2O
Combustion of hydrogen gas
Ca(OH)2(s) + (aq) 
Ca(OH)2(aq)
Hydrogen is a clean fuel as
the product (water) is nonpollutant
Solid slaked lime dissolves in
Highly exothermic
(generates heat) reaction
water (aq) to give aqueous
limewater Ca(OH)2(aq)
Ca(OH)2+CO2
CaCO3+H2O
Bubble CO2 gas
through limewater to
give the cloudy white
precipitate of calcium
carbonate
Compound
A molecule that is made up
of two or more different
atoms (elements) that are
joined together by chemical
bonds
Examples include:
Sodium Chloride (NaCl),
Water (H2O), hydrocarbons
(e.g. methane CH4)
Unsaturated
vegetable oils
Extracted from seeds, nuts
and fruits by pressing or by
distillation
Hydrogenation
Hardening of
unsaturated
vegetable oils
Contain C=C double bonds
Higher boiling points than
water (food cooks at higher
temp in oils so food cooks
faster in oil than in water)
Hydrogenated
oils
have higher melting points
because they are more
saturated
so they are solids at room
temperature, making them
useful as spreads and in
cakes and pastries.
by reacting them with
hydrogen at 60C with a
nickel catalyst
Mixture
A combination of two or
more elements or
compounds which are
NOT chemically combined
Examples include:
crude oil (a mixture of
alkanes), sand & water,
breakfast!