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Chemistry Overall Revision Notes +
Revision Tables
Electrolysis Examples to Study
1. Concentrated Sodium Chloride
2. Dilute Sodium Chloride
3. Concentrated Aqueous Copper Sulfate
4. Dilute Copper Sulfate
5. Dilute Sulfuric Acid
6. Concentated Sulfuric Acid
7. Concentrated Aqueous Hydrochloric Acid
8. Dilute Hydrochloric Acid
9. Lead Bromide
10. Copper Chloride Solution
11. Sodium Hydroxide Solution
12. Potassium Iodide
13. Copper Bromide
14. Sodium Sulfate
15. Silver Nitrate
16. Copper Nitrate
Acid base reactions
Base + acid --> salt + water
metal + acid --> salt + hydrogen
metal carbonate + acid --> salt + carbon dioxide + water
metal oxide/hydroxide + acid --> salt + water
Physical change in matter
sublimation - solid to gas
deposition - gas to solid
freezing - liquid to solid
Chemistry Overall Revision Notes + Revision Tables
1
melting - solid to liquid
vaporization- liquid to gas
condensation - gas to liquid
Reactions in hydrocarbons
Making esters: heat(no specified temp) - sulfuric acid
Dehydration; sulfuric acid
Esters: alcohol + carboxylic acid --> ester + water
Synthesis of plastics
Chemistry Overall Revision Notes + Revision Tables
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Nylon formation
Terylene formation
Amino acid structure
Chemistry Overall Revision Notes + Revision Tables
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Carbohydrate structure
Protein formation - (amino acid joining together with another amino acid, by peptide bond) (check pic 6)
Thermal Decomposition
Oxidation reduction
Chemistry Overall Revision Notes + Revision Tables
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OIL RIG
OIL --> Oxidation Is Loss (of electrons)
RIG --> Reduction Is Gain (of electrons)
Main Reactions
1. Synthesis
2. Combustion
3. Displacement
a. Single
b. Double
i. Acid-Base
ii. Ionic Precipitation
4. Decomposition
Le Chatelier:
Left and Right basically means whether the reaction shifts towards the reactants and products.
For an exothermic reaction, an increase in temperature decreases the amount of product formed (i.e
moves to the left) and a decrease in temperature increases product (moves to the right)
For an endothermic reaction, an increase in temperature increases the product formed (moves to the
right) and a decrease in temperature decreases the product (moves to the left)
Basically as a standard rule remember:
Increasing the temperature favours the endothermic reaction to absorb the extra heat. Decreasing the
temperature favours the exothermic reaction to produce more heat.
Group 1
Group 7
Density Increases Down the Group
Density Increases Down the Group
Chemistry Overall Revision Notes + Revision Tables
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Melting Points Decreases Down the Group
Melting Point Increases Down the Group
Reactivity Increases Down the Group
Reactivity Decreases Down the Group
Boiling Points Decreases Down the Group
Boiling Point Increases Down the Group
Property Type
Group 1 Metals
1. soft / can be cut
(with a knife) 2.
low density / light
3. low melting
point / fixed points
Physical
4. (good)
conductor (heat or
electricity) 5. shiny
(when freshly cut)
6. malleable /
ductile / tarnishes
Group 7 Halogens
Fluorine (F) is a pale
yellow gas Chlorine (Cl) is
a greenish gas Bromine
(Br) is a dark red liquid
Iodine (I) is a black solid
and when heated it forms a
purple vapour Astatine (At)
is a black solid Strong /
nasty smell Toxic Poor
conductors of heat and
electricity Low melting and
boiling points
Transition
Elements
What to write about
hard / high density
/ dense / high
tensile strength /
high mp or bp /
fixed points/
(good) conductor
(heat or electricity)
/ strong / malleable
Softness, Density,
Conductivity, Melting
Points, Colour, Smell
Other Props
/ ductile / silver or
grey or lustrous or
shiny solid
react with water
Chemical
(not steam) / (very)
reactive / forms
more than one
oxidation state or
salts with halogens
/ react vigorously
valency (accept
many oxides) /
with acid / forms
an alkaline or
basic oxide / fixed
oxidation state or
oxidation number
Diatomic Molecules /
Seven Valence Electrons/
Weak Intermolecular
Forces
or valency of +1 /
has one valency or
forms coloured
compounds or ions
/ forms complex
ions / behave as a
catalyst / less
Reactivity with
Elements/Compounds,
Existing Molecular
State, Molecular
Structure, Oxidation
State / Valenc
reactive than
group 1
outer shell electron
Physical Properties : Softness, Density, Conductivity, Melting Points, Colour, Smell Other Props
Chemical Properties: Reactivity with Elements/Compounds, Existing Molecular State, Molecular
Structure, Oxidation State / Valency
What does Oxidation State mean?
Ans: does not form compounds / does not accept and does not lose electrons / has full outer
shell/has 8e in outer shell / it is a Noble Gas / it is in Group 0/8
What does Lattice mean?
Ans: regular arrangement of ions / particles / positive and negative ions alternate;
Habers Process:
N2(g) + 3H2(g) ↽ −− ⇀ 2NH3(g)
Reaction Type
Exothermic
Forward Reaction
Exothermic Forward Reaction
Change
Lower
Increase Temperature
Chemistry Overall Revision Notes + Revision Tables
Increase
Reduce
6
Temperature
Which Side
Effect
Favour Exothermic
Favour Endothermic (Moves to Left)
(Moves to Right)
Less Ammonia Produced - More
More Ammonia
Nitrogen and Hydrogen Gas
Produced
Produced
Pressure
Pressure
(Moves to Right)
(Moves to Leftt)
(Lesser Moles)
(More Moles)
More Ammonia
Less Ammonia
Produced
Produced
Contact Process:
2SO2(g) + O2(g) ⇌ SO3(g) ΔH = −196KJ mol − 1
Reaction Type
Exothermic Forward
Reaction
Exothermic Forward Reaction
Change
Lower Temperature
Increase Temperature
Favour Exothermic to
Favour Endothermic to use
increase the temperature
up the extra heat (Moves to
(Moves to Right)
Left)
Which Side
Effect
More Sulfur Trioxide
Produced
Less Sulfur Trioxide Produced
- More Oxygen and Sulfur
Oxide Produced
Increase
Reduce
Pressure
Pressure
(Moves to Right)
(Moves to Left)
(Lesser Moles)
(More Moles)
More Sulfur
Less Sulfur
Produced
Produced
Organic Chemistry
Homologous Series
Functional Group
Alkanes
General Formula
Suffix
CnH2n+2
-ane
Alkenes
C=C
CnH2n
-ene
Alchohols
-OH
CnH2n+1+OH
-anol
Carboxylic Acids
-COOH
CnH2n+1+COOH
-anoic acid
Halogenoalkane
Halogonoethene
Amine
R-NH2
-amine
Ester
-R-COOR
-yl -anoate
Number of
Name
Number of C
Number of H
Formula
Methane
1
4
CH4
1
Ethane
2
6
C2H6
1
Propane
3
8
C3H8
1
Butane
4
10
C4H10
2
2 methyl-propane
Pentane
5
12
C5H12
3
2 methyl-butane, 22dimethylepropane
Isomers
Isomer
2 methyl-pentane, 3
Hexane
6
14
Ch6H14
5
methyl-pentane,
2,2dimethylebutane,
2,3dimethylbutane
Chemistry Overall Revision Notes + Revision Tables
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Number of
Name
Number of C
Number of H
Formula
Ethene
2
4
C2H4
1
Propene
3
6
C3H6
1
Butene
4
8
C4H8
4
Isomers
Isomer
but 2-ene, 2 methyl
prop 1-ene
2-pentene, 2-methyl
Pentene
5
10
C5H10
5
but-1-ene, 3-methyl
but-1-ene, 2-methyl
but-2-ene
hex-2-ene hex-3ene 2-methylpent-1ene 3-methylpent-1ene 4-methylpent-1ene 2-methylpent-2ene 3-methylpent-2-
Hexene
6
12
C6H12
13
ene 4-methylpent-2ene 2,3dimethylbut-1-ene
3,3-dimethylbut-1ene 2-ethylbut-1ene 2,3dimethylbut-2-ene
Number of
Name
Number of C
Number of H
Formula
Methanol
1
3
CH3OH
1
Ethanol
2
5
C2H5OH or
C2H6
1
Propanol
3
7
C3H8OH
1
Isomers
Isomer
butan-2-ol, 2Butanol
4
9
C4H10OH
2
Pentanol
5
11
C5H12OH
3
Hexanol
6
13
Ch6H14OH
5
Name
Number of C
Number of H
Formula
Methanoic Acid
1
2
Ethanoic Acid
2
4
CH₃COOH
2
6
C3H6O2 or
CH3CH2COOH
2
Propanoic Acid
3
CH2O2 or
HCOOH
Number of
Isomers
4
8
Chemistry Overall Revision Notes + Revision Tables
C4H8COOH or
C3H7COOH
and 2-methylpropan-2-ol
Isomer
1
or C2H5COOH
Butanoic Acid
methylpropan-1-ol
Methyl Methanoate
Methyl Ethanoate
Ethyl Methanoate
Ethyl Ethanoate,
2
Propyl Methanoate,
Methyl Propanoate,
8
Name
Number of C
Number of H
Formula
Pentanoic Acid
5
10
C5H10O2 or
C4H9COOH
Gas
Sources
Example
Complete
Carbon Dioxide
Methane: CH4 + O2 —
Carbon containing
→ CO2 + 2H2O
Fuels
Carbon
Monoxide
Particulates
Incomplete Combustion
Incomplete
Combustion of Carbon
containing Fuels
Incomplete
Combustion of Carbon
containing Fuels
Isomers
3
Adverse Effect
Combustion of
Combustions of
Number of
of Gasoline: C8H18 +
9O2 → 5CO + 2CO2 +
9H2O
Incomplete Combustion
of Methane 2CH4 +
3O2→ 2CO + 4H2O
CH4 + O2→ C + 2H2O
Global Warming,
Climate Change
Toxic, combining
with haemoglobin
in the blood and
prevents it from
carrying oxygen
Isomer
Propyl Ethanoate,
Methyl Butanoate,
Solution
Renewable Energy
Sources, Plant More
Trees
Oxidised Unburned
Hydrocarbons:
C8H18 + 12½O2 →
8CO2 + 9H2O
Respiratory
Problems and
Cancer
Digestive processes of
Methane
organisms,
~
decomposition of
Global Warming,
Reduce Life-Stock
Climate Change
Farming
plants, bacterial action
Photochemical
Reaction between
Nitrogen and Oxygen
Nitrogen Oxides
in car engines, hightemperature furnace
and bacterial action in
smog Acid Rain
nitrogen + oxygen →
nitrogen dioxide N2 +
Pollutes crops and
water supplies
2O2 → 2NO2
Causes respiratory
problems and
the soil
Catalytic Converters:
Redox reactions to
neutralise gases: 2NO
+ 2CO → N2 + 2CO2
irritation
Using Low Sulfur
Sulfur Oxide
combustion of fossil
Acid rain
fuels
Fuels, Flue Gas
Desulfurisation by
reacting with CaO
The Group 2 carbonates break down (decompose) when they are heated to form the metal
oxide and give off carbon dioxide gas
The general equation for the decomposition of Group 2 carbonates is:
XCO3 (s) XO(s) + CO2 (g)
HEAT
⎯⎯⎯⎯⎯⎯
X = Group 2 element
Chemistry Overall Revision Notes + Revision Tables
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The only Group 1 nitrate that will decompose to produce nitrogen dioxide (which is a brown toxic
gas) and oxygen is lithium nitrate LiNO3
4LiNO3 (s) 2Li2O(s) + 4NO2 (g) + O2 (g)
HEAT
⎯⎯⎯⎯⎯⎯
The rest of the Group don't decompose so completely producing the metal nitrite (NO2-) and
oxygen, but no nitrogen dioxide
2XNO3 (s) 2XNO2 (s) + O2 (g)
HEAT
⎯⎯⎯⎯⎯⎯
Red litmus paper:
Acidic:red
Neutral: red
Alkaline:blue
Blue litmus paper:
Acidic:red
Neutral: blue
Alkaline:blue
Thymolphthalein:
Acidic: colorless
Neutral: colorless
Alkaline: blue
Phenolphthalein:
Acidic: colorless
Neutral: colorless
Alkaline: pink
Methyl orange:
Acidic: red
Neutral: orange
Alkaline: yellow
Hydrocarbon Reactions
Alkane —→ Chloroalkane
Substitution, UV Light
Chemistry Overall Revision Notes + Revision Tables
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Alkane —→ Alkene
Cracking, Heat(500 - 700) + Catalyst(Zeolite, Alumimium Silicate, Alumina or Silica)
Alkene —> Bromoalkene
Bromination, Bromine Decolourises
Alkene —> Alkane
Hydrogenation, Heat (150c), Nickel Catalyst + H2
Alkene —> Alcohol
Hyration, + H20 (Steam) , Heat (300), Pressure 60, H3PO4 catalyst (Any acid catalyst)
Glucose —→ Ethanol
Fermentation, Yeast
Alcohol —→ Carboxylic Acid
Oxidation
Fermentation
Acidified Potassium Manganate
Carboxylic Acid + Alcohol
Ester: Heat, Sulfuric Acid catalyst
Alcohyl + Carboxanoate
Chemistry Overall Revision Notes + Revision Tables
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