understand the arrangement, movement and energy of the
particles in each of the three states of matter: solid, liquid and
gas
understand how the interconversions of solids, liquids and gases
are achieved and recall the names used for these
interconversions
explain the changes in arrangement, movement and energy of
particles during these interconversions.
b) Atoms (Chapter 11, pages 89-91)
Students will be assessed on their ability to:
1.4 describe and explain experiments to investigate the small size of
particles and their movement including:
i dilution of coloured solutions
ii diffusion experiments
. 1.5
. 1.6
. 1.7
. 1.8
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 how information from chromatograms can be used to
identify the composition of a mixture.
c) Atomic structure (Chapter 2, pages 6-12)
Students will be assessed on their ability to:
. 1.9 understand that atoms consist of a central nucleus, composed of
protons and neutrons, surrounded by electrons, orbiting in shells
. 1.10 recall the relative mass and relative charge of a proton,
neutron and electron
. 1.11 understand the terms atomic number, mass number, isotopes
and relative atomic mass (Ar)
. 1.12 calculate the relative atomic mass of an element from the
relative abundances of its isotopes
. 1.13 understand that the Periodic Table is an arrangement of
elements in order of atomic number
. 1.14 deduce the electronic configurations of the first 20 elements
from their positions in the Periodic Table
. 1.15 deduce the number of outer electrons in a main group element
from its position in the Periodic Table.
e) Chemical formulae and chemical equations (Chapter 5, pages
33-39)
Students will be assessed on their ability to:
. 1.21 write word equations and balanced chemical equations to
represent the reactions studied in this specification
. 1.22 use the state symbols (s), (l), (g) and (aq) in chemical
equations to represent solids, liquids, gases and aqueous
solutions respectively
f) Ionic compounds (Chapter 3, pages 17-19)
Students will be assessed on their ability to:
. 1.28 describe the formation of ions by the gain or loss of electrons
. 1.29 understand oxidation as the loss of electrons and reduction as
the gain of electrons
. 1.30 recall the charges of common ions in this specification
. 1.31 deduce the charge of an ion from the electronic configuration
of the atom from which the ion is formed
. 1.32 explain, using dot and cross diagrams, the formation of ionic
compounds by electron transfer, limited to combinations of
elements from Groups 1, 2, 3 and 5, 6, 7
. 1.33 understand ionic bonding as a strong electrostatic attraction
between oppositely charged ions
. 1.34 understand that ionic compounds have high melting and boiling
points because of strong electrostatic forces between oppositely
charged ions
. 1.35 understand the relationship between ionic charge and the
melting point and boiling point of an ionic compound
. 1.36 describe an ionic crystal as a giant three-dimensional lattice
structure held together by the attraction between oppositely
charged ions
. 1.37 draw a diagram to represent the positions of the ions in a
crystal of sodium chloride.
g) Covalent substances (Chapter 3, pages 13-17)
Students will be assessed on their ability to:
. 1.38 describe the formation of a covalent bond by the sharing of a
pair of electrons between two atoms
. 1.39 understand covalent bonding as a strong attraction between
the bonding pair of electrons and the nuclei of the atoms
involved in the bond
. 1.40 explain, using dot and cross diagrams, the formation of
covalent compounds by electron sharing for the following
substances:
. i hydrogen
. ii chlorine
. iii hydrogen chloride
. iv water
. v methane
. vi ammonia
. vii oxygen
. viii nitrogen
. ix carbon dioxide
. x ethane
. xi ethene
(Chapter 4, pages 23-32)
. 1.41 understand that substances with simple molecular structures
are gases or liquids, or solids with low melting points
. 1.42 explain why substances with simple molecular structures have
low melting and boiling points in terms of the relatively weak
forces between the molecules
. 1.43 explain the high melting and boiling points of substances with
giant covalent structures in terms of the breaking of many
strong covalent bonds
. 1.44 draw diagrams representing the positions of the atoms in
diamond and graphite
. 1.45 explain how the uses of diamond and graphite depend on their
structures, limited to graphite as a lubricant and diamond in
cutting.
h) Metallic crystals
Students will be assessed on their ability to:
. 1.46 understand that a metal can be described as a giant structure
of positive ions surrounded by a sea of delocalised electrons
. 1.47 explain the electrical conductivity and malleability of a metal in
terms of its structure and bonding.
Section 2: Chemistry of the elements
a) The Periodic Table (Chapter 12, pages 99 to 106, then page
108 to 111)
Students will be assessed on their ability to:
. 2.1
. 2.2
. 2.3
. 2.4
. 2.5
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 non-metals 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
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.
b) Group 1 elements — lithium, sodium and potassium
Students will be assessed on their ability to:
. 2.6
. 2.7
. 2.8
describe the reactions of these elements with water and
understand that the reactions provide a basis for their
recognition as a family of elements
describe the relative reactivities of the elements in Group 1
explain the relative reactivities of the elements in Group 1 in
terms of distance between the outer electrons and the nucleus.
c) Group 7 elements — chlorine, bromine and iodine
Students will be assessed on their ability to:
. 2.9 recall the colours and physical states of the elements at room
temperature
. 2.10 make predictions about the properties of other halogens in this
group
. 2.11 understand the difference between hydrogen chloride gas and
hydrochloric acid
. 2.12 explain, in terms of dissociation, why hydrogen chloride is
acidic in water but not in methylbenzene
. 2.13 describe the relative reactivities of the elements in Group 7
. 2.14 describe experiments to demonstrate that a more reactive
halogen will displace a less reactive halogen from a solution of
one of its salts
This plus everything new I’ve learnt this year. Note that this
specification does not have everything. New stuff includes:
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