Table Of ContentIGCSE CHEMISTRY
AN INTERACTIVE REVISION GUIDE
ANDREW RICHARD WARD
BSC PGCE MA(ED) MRSC
ENDORSED BY
THE ROYAL SOCIETY OF CHEMISTRY AND CAMBRIDGE EXAMINATIONS BOARD.
CONTENTS
[ANDREW RICHARD WARD – ©ALL RIGHTS RESERVED – A WARD TUITION - 2009] Page 1
PRINCIPLES OF CHEMISTRY
1. PARTICULATE NATURE OF MATTER
2. EXPERIMENTAL TECHNIQUES
3. ATOMS, ELEMENTS AND COMPOUNDS
4. STOICHIOMETRY
PHYSICAL CHEMISTRY
5. ELECTRICITY AND CHEMISTRY
6. CHEMICAL CHANGES
7. CHEMICAL REACTIONS
8. ACIDS, BASES AND SALTS
INORGANIC CHEMISTRY
9. THE PERIODIC TABLE
10. METALS
11. AIR AND WATER
12. SULPHUR
13. CARBONATES
ORGANIC CHEMISTRY
14. ORGANIC CHEMISTRY
INTRODUCTION
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THIS STUDY GUIDE IS A REVISION GUIDE
IT IS NOT A TEXTBOOK
IT IS TO BE USED ALONGSIDE A TEXT BOOK AND
CLASSROOM NOTES AS A REFERENCE TEXT TO HELP WITH
EXAM REVISION
THE ESSENTIAL FACTS NEEDED FOR CHEMISTRY AT IGCSE
ARE SUMMARIZED WITH A MINIMUM OF FUSS AND
MAXIMUM EFECT
MR. WARD HAS BEEN A SECONDARY TEACHER OF SCIENCE,
MATHEMATICS AND ICT SINCE 1992.
MR. WARD IS A GRADUATE OF UNIVERSITIES IN THE
NORTH EAST OF ENGLAND WHERE HE OBTAINED HIS
BACHELORS AMD MASTERS DEGREES.
MR. WARD IS CURRENTLY STUDYING FOR HIS DOCTORATE
OF EDUCATION AT LONDON UNIVERSITY, ENGLAND WHERE
HE IS SPECIALIZING IN THE USE OF MIND-MAPPING TO
ENHANCE SCIENCE EDUCATION.
MR. WARD CAN BE CONTACTED ON 66735119
AND BY EMAIL AT
THIS GUIDE CONTAINS NEARLY 300 PAGES AND IS THE
MOST CONCISE AND ONLY ELECTRONIC GUIDE TO
CHEMISTRY CURRENTLY AVAILABLE IN KUWAIT
“MAXIMUM EFFECT – MINIMUM NOTES – MAXIMUM
GRADES”
NON SCHOLAE SED VITAE DISCIMUS
“IT IS NOT FOR SCHOOL – BUT FOR LIFE”
IN MEMORY OF MARY PATTISON 1918 – 1988.
MY GUIDING LIGHT WHO IS ALWAYS LOVED AND NEVER
FORGOTTEN.
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TOPIC 1 – ALL ABOUT MATTER
Chemistry is the study of matter
Matter is all the substances and materials that the universe is made from.
There are many millions of known chemical substances.
All can be classified as solid, liquid or gas.
SOLID
Definite fixed shape and volume
Increase in size when heated – expand
Decrease in size when cooled – contract
LIQUID
Has a fixed volume
Takes up shape of container it is poured into
Liquids slightly expand when heated also
Can be compressed – volume gets smaller when pressure added
GAS
No fixed shape or volume
Takes up shape of container it is placed into and expands evenly within it
Very noticeable change in volume when the temperature is increased.
Gases are much more easy to compress than liquids
KINETIC THEORY OF MATTER
Explains the way in which matter behaves.
The kinetic theory tells us all matter is made from PARTICLES.
Kinetic theory explains the physical properties of matter in terms of the way that
the particles move.
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There are 3 main points to the Kinetic Theory:
All matter is made from invisible tiny particles. The particles can be called
atoms, molecules or ions and can be different sizes.
The particles move all of the time. High temperature = fast movement
At any temperature, heavier particles move slower than lighter ones.
DESCRIPTION OF PARTICLES IN SOLID, LIQUID AND GAS
SOLID- Particles vibrate around fixed positions. Regular structure
LIQUID- Particles have some freedom to move around each other. Many collisions
GAS- Particles move freely and randomly in available space. Collide less than in
liquid – particles as far apart as possible
CHANGES OF STATE
Solid to liquid = melting
Liquid to gas = boiling or evaporation
Gas to liquid = condensation
Liquid to solid = freezing
Sometimes a solid may change directly into a gas – missing out the liquid stage.
This is called SUBLIMATION.
Iodine is a black solid. It sublimes to form a purple gas.
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Here is a table to show the melting point and boiling point of some chemical
substances
SUBSTANCE MELTING BOILING EXPLANATION
POINT(CELSIUS) POINT
(CELSIUS)
Aluminium 661 2467 SOLID – IT HAS
NOT MELTED
YET
Ethanol -117 79 LIQUID –
MELTED AT
LOW
TEMPERATURE
Magnesium oxide 2827 3627 SOLID – NOT
YET MELTED
Mercury -30 357 LIQUID –
ALREADY
MELTED
Methane -182 -164 GAS –
ALREADY
MELTED AND
BOILED
Oxygen -218 -183 GAS –
ALREADY
MELTED AND
BOILED
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HEATNG AND COOLING CURVES
Here is the heating curve for water
(BY KIND PERMISSION OF THE BBC, UK)
At the start, only ice is present.
After a bit, the curve goes flat.
This means that even as we put heat energy in, the temperature stays the same.
In ice, particles are close together and are attracted to one another.
For ice to melt, the particles must get enough energy to overcome the forces of
attraction in the water molecules to allow movement. This is where the heat energy
is going.
The temperature rises again after all of the ice has melted.
The heating curve of a pure solid always stops rising at the melting point.
A sharp melting point means a pure sample.
ADDING IMPURITIES LOWERS MELTING POINT
ICE CAN MELT AT -15 CELSIUS BY ADDING SALT TO IT.
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If we want to boil the water, we have to give it extra energy.
This can be seen on the graph when the curve levels out at 100 Celsius which is the
boiling point of water.
The reverse processes of condensation and freezing occur on COOLING.
Energy is given out when the gas condenses to a liquid and the liquid freezes to a
solid.
DIFFUSION
DIFFUSION IS THE MOVEMENT OF PARTICLES FROM A REGION OF
HIGH CONCENTRATION TO LOW CONCENTRATION DOWN A
DIFFUSION GRADIENT.
The diagram below shows how the diffusion of bromine molecules can be shown.
Within 24 hours, the molecules of bromine spread out from a high concentration at
the bottom of the gas jar and spread evenly throughout the total volume of the two
gas jars.
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Here is a sequence to show how molecules move down a diffusion gradient.
The example chosen is for dissolving sugar in water:
We will now consider Brownian Motion
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