Cambridge IGCSE® Chemistry (0620)
N
O
N
O
C
H 2O
Na
S
O
N
O
O
O
C
O
He
O
Ne
Ar
Kr
O
Xe
Rn
1
Unit
links
Particles, atomic structure,
ionic bonding and the Periodic Table
2
Experimental techniques
1
2
3
4
5
6
7
8
9
10
11
12
Unit
links
3
1
2
3
4
5
6
7
8
9
10
11
12
Air and water
Unit
links
CaO
EXO
OH –
CaCO3
SO2
1
2
3
4
5
6
7
8
9
10
11
12
Cl
Cl
H
C
N
?
7
H
H
H
C
C
H
H
H
O
C
C
1
2
3
4
5
6
7
8
9
10
11
12
H
O
H
H
O
H
H
C
C
C
C
H
H
O
H
O
H
O
C
H
H
H
C
C
H
H
H
O
5
6
7
8
9
10
11
12
3
4
5
6
7
8
9
10
11
12
Mg
Ca
H
H
C
C
H
H
Unit
links
Fe + CuSO4
C
N
B
H
Cu
Cu
Fe
Zn
2
3
4
5
6
7
8
9
10
11
12
Cu + FeSO4
F
reduction
Cl
oxidation
Br
+
–
1
2
3
4
5
6
7
8
9
10
11
12
+
–
Cu
–
Fe
+
–
+
Fe2O3
Metals and the reactivity series
+
O
1
2
3
4
5
6
7
8
9
10
11
12
Cu
O
Cu
O
O
24 dm3
Fe
56 g
23
Amount of substance
Unit
links
1
2
3
4
5
6
7
8
9
10
11
12
N2 + 3H2
2NH3
H2SO4
1
2
3
4
5
6
7
8
9
10
11
12
12
Equilibria
Unit
links
1
2
3
4
5
6
7
8
9
10
11
12
Highlighted numbers in the ‘unit links’ boxes indicate significant links between the different units.
®IGCSE is a registered trademark
Copyright © UCLES 2017
H2
At
Redox, electrochemistry and Group VII
Unit
links
–
+
I
Fe
11
+
–
9
1
n
+
+
–
6.022 × 10
n
N
H
–
+
–
–
Unit
links
Cu
C
Organic 1
H
Organic 2
Unit
links
4
Fe2+ + 2e –
H
10
H
O
A
3
8
Covalent bonding
Unit
links
H
N
2
C
H
H
H
1
H
H
–
+
6
Reaction rates
Unit
links
+
–
–
+
B
A
B
5
Acids, bases and salts
Unit
links
B
A
Ca(OH)2
B
H
NO2
A
H
4
CO2
+
H
Na2O MgO ZnO
2
Na+
Cu2+
H
H+
Na
K
ENDO
1
Experimental techniques
Measuring melting and boiling points
13:03
Measurement
2.1
distance travelled by compound
distance travelled by solvent
chromatography
drug purity
melting points
Criteria of purity
Purification techniques
2.6 cm
2.1 cm
Rf =
2.2.1
1.23
out
in
condenser
HEAT
distillate
HEAT
2.2.2
Copyright © UCLES 2017
Methods of purification
Measuring temperature, mass and volume
1
Particles, atomic structure, ionic bonding
and the Periodic Table
2
atomic number
proton
Particles and atoms
3
neutron
Li
symbol
7
solid
1.1
liquid
electron
gas
3.1
Atomic structure and the Periodic Table
Changes of state
Isotopes
The particulate nature of matter
mass number
235
U
element
Energy transfer
Reactions
Cl
Metals and non-metals
Na
Ions and ionic bonds
3.2.2
Metals and non-metals
Physical and chemical changes
Alloys
T
W
O PENC
O
steel
2
NE
PE N
C
E
7.1
chemical change
alloys
E
physical change
Ionic bonding
HEAT
mixture
Bonding: the structure of matter
3.2.1
Atomic structure and the Periodic Table
6.2
compound
1
Properties of metals
10.1
Ea
EXO
ENDO
A
∆H
B
Energetics of a reaction
6.1
number of electrons in outer shell
O
O2
O
C
O
CO2
Al 3+ O 2- Al 2 O 3
4.1
Copyright © UCLES 2017
6
C
12
Stoichiometry
2 electrons
3 electrons
7 electrons
8 electrons
Na
Mg
Al
Cl
Ar
gas
Periodic trends
9.2
8
O
16
Li
K
Cs
9.3
melting point
density
Na
Rb
Group properties
reactivity
Periodic Table trends
liquid
The Periodic Table
9.1
O
solid
non-metal
Periodic Table trends
Working out formulae
metal
1 electron
Air and water
3
N2
78%
O2
Cl
cobalt(II)
chloride
Cl
OTHERS
He
C
−190 °C
Ne
O
Pollutant gases in air
Noble gases in the atmosphere
He
Ar
Kr
Ar
GAS
He
Combustion reaction products
Ne
Xe
Rn
Noble gases
C
O
9.5
O
H
H
C
H
11.4
Copyright © UCLES 2017
−185 °C
air
Air
11.2
EXO
EXO
OIL
6.2
CaCO3 CaO + CO2
C
H
COAL
THE
CARBON
CYCLE
0.4% CO2
Carbon dioxide and methane
N
O
the composition of dry air
treatment
Water
11.1
1%
O
Ar
Energy transfer
Fossil fuels and global warming
H 2O
21%
N
O
4
Acids, bases and salts
Cu
Cu
+
O
O
12
0
Ar = 12
C
O
Cu
Cu
O
Cu
O
2
3
H+
Mr = 80
4
5
6
H+
acids
Masses of compounds
8
9
10 11 12 13 14
bases
OH –
Stoichiometry
The characteristic properties
of acids and bases
Uses
Equations
8.1
Neutralisation reactions
HCl
NaOH
NaCl
+
phosphorus
H2O
potassium
Salts and their uses
NH4NO3
PO43–
KNO3
Ca(OH)2 + 2NH4Cl 2NH3 + CaCl2 + H2O
ACID + BASE SALT + WATER
Preparation of salts
8.3
ACID + BASE
SALT + WATER
nitrogen
+
OH –
methyl orange
FeCl3 + 3NaOH Fe(OH)3 + 3NaCl
4.1
1
Nitrogen and fertilisers
11.3
Reactions of carbonates and acids
CuCO 3
metal elements
CO 2
non-metal elements
MgO
ZnO
CO2
NO2
SO2
Indicators
heat
Types of oxides
8.2
CaCO3
CaCO3
Thermal decomposition
Na2O
CaO
13.1
CuO
Ca(OH)2
Carbonates
AgNO3
Cu2+
Na+
K+
Li+
Cl– Br– I–
Testing for ions and gases
O2
CO2
8.4
Copyright © UCLES 2017
Testing for carbonates
Cl2
NH3
Identification of ions and gases
H2
5
Reaction rates
factors affecting rate
1 / time
x
x
x
x
x
x
A
B
temperature
Catalysis
Activation energy
Temperature changes
Rate (speed) of reaction
7.2
A
EXO
A
A
B
∆H
B
A
B
ENERGY
B
ENERGY
A
B
breaking bonds
Ea
∆H
A
making bonds
ENDO
Ea
B
B
mexobendo
∑ ∆H (bonds broken) − ∑ ∆H (bonds formed)
6.1
Copyright © UCLES 2017
Energetics of a reaction
6
Metals and the reactivity series
+
W
3432°C
Au
1064°C
Al
660 °C
Explaining properties
+
–
–
–
–
conduct heat
and electricity
Properties of metals
Zn
Fe
OH–
H2
NO3–
CO32–
Copyright © UCLES 2017
–
mobile free
electrons
+
Al 3+
–
Ca2+
Na+
W
O PENC
NE
2
PE N
C
1
Uses of metals
10.4
Transition metal uses
Extraction and reactivity
10.3
+
E
thermal
decomposition
Transition metal reactivity
Fe
C
Galvanising
O
electrolysis
Fe2O3
fixed positive
cations
Cu
Reactivity series
10.2
+
–
+
Metallic bonding
T
Mg
C
H 2O
–
–
+
Properties and uses
Transition metal properties
Ca
–
–
+
E
HCl
Na
+
–
+
3.2.5
Reactions of metals
10.1
K
+
malleable and
ductile
+
–
Explaining properties
high melting
points
shiny
+
Fe2+
Na
Fe3+
Mn7+
Cu2+
Al
C
+
–
Extraction of metals
heat metal
oxide with
carbon
Zn
Fe
Fe
Cu
Extracting transition metals
2+
9.4
Cu
3+
1+
Rh
Mn
2+
2+
7+
Transition elements
Pt
Pd
7
Covalent bonding
Cl
H
C
more volatile
than ionic
compounds
do not
conduct
electricity
generally
insoluble in
water
C
H
H
H
low melting and boiling points
N
H
Cl
N
Explaining properties
Covalent bonding
Valence electrons
Comparing properties
Molecules and covalent bonds
3.2.3
diamond does not conduct
graphite does conduct
C
high melting and boiling points
graphite
3.2.4
Copyright © UCLES 2017
diamond
Macromolecules
insoluble
in water
Organic 1
8
C
C
H
H
H
H
H
H
C
H
C
H
C
C
H
H
H
H
H
H
H
alkane
alkene
H
H
O
2
3
4
meth–
eth–
prop–
but–
O
C
C
H
H
H
O
Naming compounds
carboxylic acid
H
H
O
C
C
O
H
H
H
H
H
C
C
H
H
methane
H
ester
Names of compounds
H
H
C
C
H
H
H
H
ethane
H
H
H
C
C
C
H
H
H
H
H
H
H
H
H
C
C
H
C
HC
H
H
H
H
propane
alkanes
alkenes
CnH2n+2
CnH2n
H
butane
1C
2C
3C
4C
increasing boiling point
Homologous series
14.3
H
H
H2
H
+
H
–
hydrogen
C
H
Energy transfer
Fuels
14.2
Cracking
6.2
H
Increasing molecule size
Alternative fuels
Increasing boiling point
H2 + O2 2H2O
Increasing temperature
Properties
14.1
C
H
H
alcohol
1
H
Fuels and combustion
Alternative fuels
H
C
C
H
H
H
Cl
H
H
Cl
Cl
14.5
Naming compounds
H
C
H
O
H
C
+
O
O
H
H
H
H
H
H
C
C
H
H
O
Combustion reactions
sugar
14.6
Copyright © UCLES 2017
C
Br
Alkanes
14.4
C
C
H
Alcohols
C
+
Br
Br
H
Br
H
C
Alkenes
H
ethanol
O
C
O
H
H
H
O
C
H
H
H
Hydration of ethene
C
H
complete combustion
H
C4H10 + C2H4
H
C
H
H
H
C6H14
H
H
H
H
C
O
C
substitution
reactions
H
O
H
H
H
H
H
H
C
C
Br
Br
H
H
H
C
C
H
H
n
Amount of substance
9
O2
O
Al O
3+
6
C
2-
C
CO2
O
Al 2 O 3
8
29
16
64
Relative formula mass
Relative atomic mass
6.022 × 10 1 Mole
23
Au 197 g
4.2
Copyright © UCLES 2017
+
O
Cu
O
Cu
O
O
C
O
C
12
O
44
Stoichiometry
4.1
18 g
Cu
Cu
O Cu
12
H2O
Cu
Fe
56 g
Ag 108 g
O2
He
4g
Molecular formulae
O
Balanced equations
O
24 dm3
mol/dm3
g/dm3
32 g
Cu 64 g
% yield =
The mole concept
actual yield
theoretical yield
Organic 2
10
H
C
C
H
H
O
ethanol
H
H
H
C
C
H
H
O
C
C
OXIDATION
H
O
H
ethanoic acid
H
O
+
H
O
C
H
O
C
C
H
O
H
H
O
C
C
O
H
O
H
ethyl ethanoate (ester)
H
H
H
C
C
H
H
H
H
C
C
H
H
H
H
H
O
C
C
H
H
H
C
C
C
H
H
H
H
H
H
H
O
CH
C
C
H
H
propyl ethanoate
C2H5OH + CH3COOH
H
O
H
ethyl ethanoate
Naming compounds
ETHYL ETHANOATE
Carboxylic acids
14.7
H
C
Fermentation or acidified
potassium manganate(VII)
H
H
H
H
C
C
H
H
C
C
H
H
addition
polymerisation
C
Esterification
Condensation polymers
poly(ethene)
C
C
monomer
polymer
H
H
C
N
B
N
C
A
B
O
N
B
H
O
O
C
H
O
A
C
O
C
C
O
X
C
N
Y
N
H
H
O
14.8.2
C
X
O
C
N
Y
H
H
A
C
O
B
terylene
O
H
n
carbohydrates
O
Synthetic polymers
N
O
O
Polyamides
O
n
14.8.3
n
O
O
proteins
Polymerisation
nylon
N
n
O
H
Natural polymers
H
FROM ACID
n
O
Copyright © UCLES 2017
A
O
C
Polymers
H
CH3COOCH2CH3
FROM ALCOHOL
O
O
H
H
ethene
14.8.1
O
poly(styrene)
n
H
C
Names of compounds
14.1
Amino acids and proteins
H
H
n
H
H
C
ethyl propanoate
Forming polyamides
H
O
Naming polymers
H
H
11
Redox, electrochemistry and Group VII
Fe + CuSO4
Fe + Cu2+
Cu + FeSO4
Cu + Fe2+
reduction
oxidation
Fe = reducing agent
Cu2+ = oxidising agent
Oxidation and reduction
Ionic equations
anode
cathode
non-metals
metal or hydrogen
bromine
chlorine
+
chlorine
oxygen
PbBr2
HCl
NaCl
H2SO4
–
graphite
–
cryolite
Electrolysis
aluminium
hydrogen
Extraction of metals
10.3
Making halogens
At
9.3
Copyright © UCLES 2017
REACTIVITY
DENSITY
BOILING point
Melting point
–
hydrogen
F2
Cl2
Br2
I2
Group properties
H2 + O2 2H2O
H
I
graphite
H
Br
Rate (speed) of reaction
7.2
–
hydrogen
photosynthesis
6CO2 + 6H2O C6H12O6 + 6O2
lead
–
Ag
Hydrogen fuel cells
F
Cl
silver salts in photography
Electricity and chemistry
5.1
Ag+ + e–
Ionic equations
Oxidation and reduction in displacement reactions
Redox
7.4
O
I
L
R
I
G
H2
+
–
hydrogen
6.2
Energy transfer
12
Equilibria
A+B
C+D
RATE
EXO
N2 + 3H2
N
AIR
2NH3
N
Haber
process
450 °C
N
200 atm
P
NATURAL
GAS
K
PbS
S
S
12.1
H
CAT
Fe
iron catalyst
Nitrogen and fertilisers
11.3
S
H
400–450 atm
ZnS
S
S
S
Industrial processes
Equilibrium conditions
INCREASE CONC.
OF PRODUCTS
Reversible reactions
7.3
Copyright © UCLES 2017
MORE GAS MORE GAS
MOLES ON MOLES ON
RATE
LEFT
RIGHT
atm
ENDO
INCREASE CONC.
OF REACTANTS
1–2 atm
S
H2SO4
S
Sulfur
CAT
V2O5 catalyst
SO2
PAPER
BLEACHING