This document provides ALL the content required for the AQA GCSE Chemistry course! Also applicable for other exam boards (i.e. OCR), this includes diagrams, practice questions and more to help you achieve a grade 9 in the exam :)
HOW IT’S ASSESSED:
PAPER 1 PAPER 2:
Topics 1-5 → atomic structure and the Topics 6-10 → the rate and extent of
periodic table; bonding, structure, and the chemical change; organic chemistry;
properties of chemical analysis,
matter
; quantitative chemistry; chemical changes; chemistry of the atmosphere; using
energy changes resources
1 hour 45 minutes (both Foundation + 1 hour 45 minutes (both Foundation +
Higher Tier) Higher Tier)
100 marks 100 marks
50% of GCSE 50% of GCSE
1. ATOMIC STRUCTURE + THE PERIODIC TABLE
GROUP 1 - ALKALI METALS:
PHYSICAL PROPERTIES: REACTIONS OF GROUP 1 METALS:
Soft metals - can be cut 1. METAL + OXYGEN → METAL OXIDE
with a knife.
e.g. sodium + oxygen → sodium oxide
Low melting points.
The metals are very reactive so it gets dull (or
Low density and can float tarnished) because they react with oxygen in the air.
on water.
AQA GCSE CHEMISTRY 1
, TREND IN REACTIVITY: It is stored in oil to prevent it from reacting with
oxygen.
INCREASES down the group
because: 2. METAL + WATER → METAL HYDROXIDE +
HYDROGEN
There are more shells so
there is greater shielding. e.g. potassium + water → potassium hydroxide +
hydrogen
The nuclear attraction on
the last shell electron is Group 1 metals are called ‘alkali’ metals because
weakening, meaning they react with water to form alkaline metal
losing the last shell hydroxides.
electron is easier.
Observations:
e.g. ‘Compare the reactivity
ALL fizz and produce hydrogen gas.
between Lithium and
Potassium’ All float and melt into a ball (ONLY sodium and
potassium) as they move about the water’s surface.
Potassium is more reactive
than lithium because it is a Forms a colourless solution; becomes PURPLE
bigger atom with more shells when universal indicator is added since it is alkali.
and therefore more shielding.
Potassium → gives off a lilac flame; Sodium → gives
The nuclear attraction on the
off an orange/yellow flame.
last shell electron is weaker in
potassium, so it is easier for 3. METAL + HALOGEN → METAL HALIDE
potassium to lose its last shell e.g. lithium + fluorine → sodium fluoride
electron.
Metal halides are white crystalline salts and form
colourless solutions in water.
TRANSITION METALS:
PROPERTIES: DIFFERENCES BETWEEN ALKALI +
TRANSITION METALS:
They form coloured compounds.
They form more than one ion, e.g. Cu(1+) TRANSITION
ALKALI METALS
and Cu(2+). METALS
Coloured
LOW reactivity. White compounds
compounds
HIGH density. Only form 1+ ions Multiple ions
Transition metals and their compounds High reactivity Low reactivity
can be used as catalysts. Low density High density
USES: Soft and low Hard and high
melting point melting point
Gold is used in jewellery because:
It is unreactive, so it doesn’t react with
chemicals in the body and the air.
Malleable and shiny.
Copper is used in electrical wires and
saucepans because:
AQA GCSE CHEMISTRY 2
, High melting point.
Hard and malleable.
Low reactivity and a good conductor of
heat/electricity.
GROUP 7 - HALOGENS:
TREND IN REACTIVITY:
PHYSICAL
Reactivity DECREASES down the PROPERTIES @ COLOUR IN
HALOGEN
group because: ROOM WATER
TEMPERATURE
The atom size is increasing so
Chlorine Pale green gas Pale green
there’s more shielding.
Red-brown
Nuclear attraction on the incoming Bromine Orange-brown
liquid
electron is getting weaker, Grey-black
therefore it is more difficult to Iodine Brown
solid
gain an incoming electron into the
last shell. DISPLACEMENT REACTIONS:
A more reactive halogen will displace a less
PROPERTIES:
reactive halogen from its compound in solution.
They are diatomic molecules.
e.g. chlorine + lithium bromide → lithium
LOW boiling points are due to the chloride + bromine
weak intermolecular forces
Observation: the colour will change from pale
between the molecules, which
green to orange-brown as chlorine displaces
take little energy to overcome.
bromine.
(boiling point INCREASES down
the group as the molecule size e.g. 2 sodium iodide + chlorine → sodium
increases, meaning IMFs are chlorine + iodine
stronger and require more energy Observation: goes from pale green to brown as
to overcome). chlorine displaces iodine.
e.g. ‘Explain why iodine has a higher ‘Describe an experiment to determine the
boiling point than chlorine’ (3) reactivity of chlorine, bromine + iodine’ (6)
Iodine is a larger molecule (1);
HALOGEN NaCl NaBr NaI
therefore it has stronger
Goes from Goes fr
intermolecular forces (2); meaning
Chlorine X pale-green → pale-gr
more energy is required to overcome
orange-brown brown
them than bromine (3).
Goes fr
Bromine X X orange
to brow
Iodine X X X
2. BONDING, STRUCTURE, + THE PROPERTIES OF
MATTER
AQA GCSE CHEMISTRY 3
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