Topics / Units
Structure 1.1—Introduction to the particulate nature of matter (1.1.1 – 1.1.3)
Structure 1.2—The nuclear atom (1.2.1 – 1.2.2)
Structure 1.3—Electron configurations (1.3.1 – 1.3.5)
Structure 1.4—Counting particles by mass: The mole (1.4.1 – 1.4.6)
Structure 1.5—Ideal gases (1.5.1 – 1.5.4)
Core Declarative Knowledge
What should students know?
Distinguish between the properties of elements, compounds and mixtures.
Distinguish the different states of matter.
Interpret observable changes in physical properties and temperature during changes of state.
Isotopes are atoms of the same element with different numbers of neutrons.
Mass spectra are used to determine the relative atomic masses of elements from their isotopic composition.
Emission spectra are produced by atoms emitting photons when electrons in
excited states return to lower energy levels.
The line emission spectrum of hydrogen provides evidence for the existence of electrons in discrete energy levels, which converge at higher energies.
The main energy level is given an integer number, n, and can hold a maximum of 2n2 electrons.
A more detailed model of the atom describes the division of the main energy level into s, p, d and f sublevels of successively higher energies.
Each orbital has a defined energy state for a given electron configuration and chemical environment, and can hold two electrons of opposite spin.
Sublevels contain a fixed number of orbitals, regions of space where there is a high probability of finding an electron.
The mole (mol) is the SI unit of amount of substance. One mole contains exactly the number of elementary entities given by the Avogadro constant.
Masses of atoms are compared on a scale relative to 12C and are expressed as relative atomic mass Ar and relative formula mass Mr.
Moles calculations.
The empirical formula of a compound gives the simplest ratio of atoms of each element present in that compound. The molecular formula gives the actual number of atoms of
each element present in a molecule.
The molar concentration is determined by the amount of solute and the volume of solution.
Avogadro’s law states that equal volumes of all gases measured under the same conditions of temperature and pressure contain equal numbers of molecules.
An ideal gas consists of moving particles with negligible volume and no intermolecular forces. All collisions between particles are considered elastic.
Real gases deviate from the ideal gas model, particularly at low temperature and high pressure.
The molar volume of an ideal gas is a constant at a specific temperature and pressure.
The relationship between the pressure, volume, temperature and amount of an ideal gas is shown in the ideal gas equation PV = nRT and the combined gas law P1V1/T1 =
P2V2/T2
Core Procedural Knowledge
What should students be able to do?
Use state symbols (s, , g and aq) in chemical equations.
Different separation techniques like Solvation, filtration, recrystallization, evaporation,
distillation and paper chromatography
Remember different changes of states like melting, freezing, vaporization (evaporation and
boiling), condensation, sublimation and deposition.
Convert between values in the Celsius and Kelvin scales.
Use the nuclear symbol to deduce the number of protons, neutrons and electrons in atoms and ions.
Perform calculations involving non-integer relative atomic masses and abundance of isotopes from given data.
Interpret mass spectra in terms of identity and relative abundance of isotopes.
Qualitatively describe the relationship between colour, wavelength, frequency and energy across the
electromagnetic spectrum.
Distinguish between a continuous and a line spectrum.
Describe the emission spectrum of the hydrogen atom, including the relationships between the lines and energy transitions to the first, second and third energy levels.
Deduce the maximum number of electrons that can occupy each energy level.
Recognize the shape and orientation of an s atomic orbital and the three p atomic orbitals.
Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to deduce electron configurations for atoms and ions up to Z = 36.
Convert the amount of substance, n, to the number of specified elementary entities.
Determine relative formula masses Mr from relative atomic masses Ar.
Solve problems involving the relationships between the number of particles, the amount of substance in moles and the mass in grams.
Interconvert the percentage composition by mass and the empirical formula.
Determine the molecular formula of a compound from its empirical formula and molar mass.
Solve problems involving the molar concentration, amount of solute and volume of solution.
Solve problems involving the mole ratio of reactants and/or products and the volume of gases.
Recognize the key assumptions in the ideal gas model.
Investigate the relationship between temperature, pressure and volume for a fixed mass of an ideal gas and analyse graphs relating these variables.
Solve problems relating to the ideal gas equation.