2.1.1: atomic structure and isotopes
- isotopes as atoms of the same element with
different numbers of neutrons and different
masses
- atomic structure in terms of the numbers of
protons, neutrons, and electrons for atoms
and ions, given the atomic number, mass
number, and any ionic charge (including
different models for atomic structure to
explain different phenomena e.g. Bohr model
explains periodic properties, and the
changing accepted models of atomic
structure over time)
- explanation of the terms relative isotopic
mass-mass compared with 1/12th mass of
carbon-12, and relative atomic mass-
weighted mean mass compared with 1/12th
mass of carbon-12, based on the mass of a
12
C atom, the standard of atomic masses
- use of mass spectrometry in the
determination of relative isotopic masses and
relative abundances of the isotope, and
calculation of the relative atomic mass of an
element from the relative abundances of its
isotopes (limited to ions with single charges)
- use of the terms relative molecular mass Mr,
and relative formula mass and their
calculation from relative atomic masses
(simples molecules-relative molecular mass,
compounds with giant structures-relative
formula mass)
,2.1.2: compounds, formulae and equations
- the writing of formulae of ions compounds
from ionic charges including: the prediction of
ionic charges from the position of an element
in the periodic table, and recall the names
and formulae for the following ions: NO3-,
CO32-, SO42-, OH-, NH4+, ZN2+, and Ag+
- construction of balanced chemical equations
including ionic equations, including state
symbols, for reactions studied and for
unfamiliar reactions given appropriate
information.
2.1.3: amount of substance
- explanation and use of the terms: amount of
substance, mole as the unit for amount of
substance, the Avogadro constant NA(the
number of particles per mole, 6.02 x 1023 mol-
1
), molar gas(mass per mole, units g mol-1),
molar gas volume(gas volume per mole, units
dm3 mol-1)
- use of the terms: empirical formula(the
simplest whole number ratio of atoms of each
element present in a compound), molecular
formula(the number and type of atoms of
each element in a molecule)
- calculations of empirical and molecular
formulae, from composition by mass or
percentage compositions by mass and
relative molecular mass
- the terms anhydrous, hydrated and water of
crystallisation and calculation of the formula
, of a hydrated salt from given percentage
composition, mass composition or based on
experimental results (PAG 1)
- calculations, using amount of substance in
mol, involving: mass, gas volume, and
solution volume and concentration
- the ideal gas equation: pV=nRT
- use of stoichiometric relationships in
calculations
- calculations to determine: the percentage
yield of a reaction or related quantities, the
atom economy of a reaction
- the techniques and procedures required
during experiments requiring the
measurement of mass, volumes of solutions
and gas volumes (PAG 1)
- the benefits of sustainability of developing
chemical processes with a high atom
economy
2.1.4: acids
- formulae of HCl, H2SO4, HNO3 and CH3COOH,
NaOH, KOH and NH3, and the explanation
that acids release H+ ions in aqueous solution
and alkalis release OH- ions in aqueous
solution
- qualitative explanation of strong and weak
acids in terms of relative dissociations
- neutralisation as the reaction of: H+ and OH-
to form H2O, and acids with bases, including
carbonates, metal oxides and alkalis(water-
, soluble bases), to form salts, including full
equations
- the techniques and procedures used when
preparing a standard solution of required
concentration and carrying out acid-base
titrations (PAG 2)
- structured and non-structured titration
calculations, based on experimental results
of familiar and non-familiar acids and bases
2.1.5: redox
- rules for assigning and calculating oxidation
number for atoms in elements, compounds
and ions(oxidation numbers of O in peroxides
and H in metal hydrides)
- writing formulae using oxidation numbers
- use of a Roman numeral to indicate the
magnitude of the oxidation number when an
element may have compounds/ions with
different oxidation numbers
- oxidation and reductio in terms of electron
transfer, and changes in oxidation
number(include examples of s-, p-, and d-
block elements)
- redox reactions of metals with acids to form
salts: full equations
- interpretation of redox equations to make
predictions in terms of oxidation numbers
and electron loss/gain
- isotopes as atoms of the same element with
different numbers of neutrons and different
masses
- atomic structure in terms of the numbers of
protons, neutrons, and electrons for atoms
and ions, given the atomic number, mass
number, and any ionic charge (including
different models for atomic structure to
explain different phenomena e.g. Bohr model
explains periodic properties, and the
changing accepted models of atomic
structure over time)
- explanation of the terms relative isotopic
mass-mass compared with 1/12th mass of
carbon-12, and relative atomic mass-
weighted mean mass compared with 1/12th
mass of carbon-12, based on the mass of a
12
C atom, the standard of atomic masses
- use of mass spectrometry in the
determination of relative isotopic masses and
relative abundances of the isotope, and
calculation of the relative atomic mass of an
element from the relative abundances of its
isotopes (limited to ions with single charges)
- use of the terms relative molecular mass Mr,
and relative formula mass and their
calculation from relative atomic masses
(simples molecules-relative molecular mass,
compounds with giant structures-relative
formula mass)
,2.1.2: compounds, formulae and equations
- the writing of formulae of ions compounds
from ionic charges including: the prediction of
ionic charges from the position of an element
in the periodic table, and recall the names
and formulae for the following ions: NO3-,
CO32-, SO42-, OH-, NH4+, ZN2+, and Ag+
- construction of balanced chemical equations
including ionic equations, including state
symbols, for reactions studied and for
unfamiliar reactions given appropriate
information.
2.1.3: amount of substance
- explanation and use of the terms: amount of
substance, mole as the unit for amount of
substance, the Avogadro constant NA(the
number of particles per mole, 6.02 x 1023 mol-
1
), molar gas(mass per mole, units g mol-1),
molar gas volume(gas volume per mole, units
dm3 mol-1)
- use of the terms: empirical formula(the
simplest whole number ratio of atoms of each
element present in a compound), molecular
formula(the number and type of atoms of
each element in a molecule)
- calculations of empirical and molecular
formulae, from composition by mass or
percentage compositions by mass and
relative molecular mass
- the terms anhydrous, hydrated and water of
crystallisation and calculation of the formula
, of a hydrated salt from given percentage
composition, mass composition or based on
experimental results (PAG 1)
- calculations, using amount of substance in
mol, involving: mass, gas volume, and
solution volume and concentration
- the ideal gas equation: pV=nRT
- use of stoichiometric relationships in
calculations
- calculations to determine: the percentage
yield of a reaction or related quantities, the
atom economy of a reaction
- the techniques and procedures required
during experiments requiring the
measurement of mass, volumes of solutions
and gas volumes (PAG 1)
- the benefits of sustainability of developing
chemical processes with a high atom
economy
2.1.4: acids
- formulae of HCl, H2SO4, HNO3 and CH3COOH,
NaOH, KOH and NH3, and the explanation
that acids release H+ ions in aqueous solution
and alkalis release OH- ions in aqueous
solution
- qualitative explanation of strong and weak
acids in terms of relative dissociations
- neutralisation as the reaction of: H+ and OH-
to form H2O, and acids with bases, including
carbonates, metal oxides and alkalis(water-
, soluble bases), to form salts, including full
equations
- the techniques and procedures used when
preparing a standard solution of required
concentration and carrying out acid-base
titrations (PAG 2)
- structured and non-structured titration
calculations, based on experimental results
of familiar and non-familiar acids and bases
2.1.5: redox
- rules for assigning and calculating oxidation
number for atoms in elements, compounds
and ions(oxidation numbers of O in peroxides
and H in metal hydrides)
- writing formulae using oxidation numbers
- use of a Roman numeral to indicate the
magnitude of the oxidation number when an
element may have compounds/ions with
different oxidation numbers
- oxidation and reductio in terms of electron
transfer, and changes in oxidation
number(include examples of s-, p-, and d-
block elements)
- redox reactions of metals with acids to form
salts: full equations
- interpretation of redox equations to make
predictions in terms of oxidation numbers
and electron loss/gain
