WHAT YOU SHOULD KNOW FROM GCSE CHEMISTRY
States of matter
understand the arrangement, movement and energy of
the particles in each of the three states of matter: solid,
liquid and gas
explain the changes in arrangement, movement and
energy of particles during the interconversions between
solids, liquids and gases.
The three boxes model for
solids, liquids and gases
Atoms
understand the terms atom and molecule
understand the differences between elements,
compounds and mixtures
describe experimental techniques for the separation of
mixtures, including simple distillation, fractional
distillation, filtration, crystallisation and paper
chromatography
Explain and draw diagrams
to show the differences.
Atomic structure
atoms consist of a central nucleus, composed of protons
and neutrons,
surrounded by electrons, orbiting in shells
recall the relative mass and relative charge of a proton,
neutron and electron
understand the terms atomic number, mass number,
isotopes , relative atomic mass.
understand the term relative atomic mass
calculate the relative atomic mass of an element from the
relative abundances of its isotopes
deduce the electronic configurations of the first 20
elements from their
positions in the Periodic Table
deduce the number of outer electrons in a main group
element from its position in the Periodic Table.
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Work out the mass of an
elements if given its
isotopes
Know the first shell holds 2,
second shell 8, then 8 (18)
Relationship between
number of electrons in outer
shell and group number
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Bonding
describe the formation of ions by the gain or loss of
electrons
explain, using dot and cross diagrams, the formation of
ionic compounds by
electron transfer
explain the properties of ionic compounds in terms of
their bonding
describe the formation of a covalent bond by the sharing
of a pair of electrons between two atoms
Draw dot and cross diagrams of hydrogen, chlorine,
hydrogen chloride, water, methane, ammonia, oxygen,
nitrogen, carbon dioxide, ethane and ethene
explain the properties of covalent compounds in terms of
their bonding
Draw diagrams to explain the bonding and properties in
diamond and graphite
explain the properties of metals in terms of their bonding
giant three-dimensional
lattice
structure held together by
the attraction between
oppositely
charged ions
ionic compounds have high
melting and boiling points
because of strong
electrostatic forces
between oppositely
charged ions
low melting and boiling
points in terms of the
relatively weak forces
between the molecules
explain the high melting
and boiling points of
substances with giant
covalent structures in terms
of the breaking of many
strong covalent bonds
metal can be described as a
giant structure of positive
ions surrounded by a sea of
delocalised electrons
The Periodic Table
understand the terms group and period
recall the positions of metals and non-metals in the
Periodic Table
explain the classification of elements as metals or nonmetals on the basis of
their electrical conductivity and the acid-base character of
their oxides
understand why elements in the same group of the
Periodic Table have similar chemical properties
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understand that the noble gases (Group 0) are a family of
inert gases and explain their lack of reactivity in terms of
their electronic configurations.
Group 1 - describe the reactions of Group 1 elements with
water
Group 7 – names, properties, relative reactivities
equations for these
Recall tests for hydrogen, oxygen, carbon dioxide,
ammonia and chlorine.
Recall tests for common anions: chloride, bromide, iodide.
Sulphate and carbonate
Recall the colours of flames given by common cations
during flame tests
Reactivity Series
Recall the reactivity series of metals
Explain displacement reactions between metals and their
oxides, and between metals and their salts in aqueous
solutions
understand oxidation and reduction as the addition and
removal of oxygen respectively
understand the terms redox, oxidising agent, reducing
agent
Acids, Alkalis and Salts
pH scale, from 0–14, can be used to classify solutions as
strongly acidic, weakly acidic, neutral, weakly alkaline or
strongly alkaline
define acids as sources of hydrogen ions, H+, and alkalis as
sources of hydroxide ions, OH¯
Recall the solubility rules
describe experiments to prepare soluble salts from acids
Acid + metal
Acid + base
Acid + carbonate
describe experiments to prepare insoluble salts using
precipitation reactions
Relative formula masses and molar volumes of gases
calculate relative formula masses (Mr) from relative
atomic masses (Ar)
understand the use of the term mole to represent the
amount of substance
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Rates of reaction
Reactions happen when particles collide.
Anything which speeds up
these collisions will make
the reaction go faster.
Explain how the rate of reaction affected by: surface area,
concentration, temperature, catalyst
Activation energy
The minimum energy
needed by particles to react
Reaction profile
A graph representing the
energy changes in a
reaction
Energy changes
chemical reactions in which heat energy is given out are
exothermic
chemical reactions in which heat energy is taken in are
endothermic
You can measure these energy changes in a range of
reactions e.g. Combustion (burning), Neutralising (acid
and alkali), Displacement (more reactive metal kicking out
less reactive metal), Dissolving (this is a physical change)
breaking of bonds is endothermic
Takes energy in
making of bonds is exothermic
Gives energy out
Energy changes in chemistry are called enthalpy changes
and use the symbol ΔH
The enthalpy changes of a reaction can be calculated
using bond energies
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Organic chemistry
Formation of crude oil
Crude oil is a mixture of hydrocarbons
How the industrial process of fractional distillation
separates crude oil into fractions
Recall the names and uses of the main fractions obtained
from crude oil
Describe the trend in boiling point and viscosity of the
main fractions
What cracking is, how to do it and what it does.
Know the meaning of the key words: General formula
Molecular formula, Structural formula, Homologous series
Saturated, Unsaturated, Isomer, alkane, alkene
draw displayed formulae for alkanes with up to five
carbon atoms in a molecule, and name the straight-chain
isomers
recall the products of the complete and incomplete
combustion of alkanes
draw displayed formulae for alkenes with up to four
carbon atoms in a
molecule, and name the straightdescribe the addition reaction of alkenes with bromine,
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What from
What a hydrocarbon is.
How the hydrocarbons
differ and effect on boiling
point
The different fractions,
length of chain, boiling
point and their uses
Viscosity is how
sticky/runny they are
(bigger ones are more
viscous)
Uses of products – alkanes
and alkenes
decolourising of bromine
water as a test for alkenes.
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