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Topic 2 Atomic structure 
​Link to YouTube Playlist 
2.1/2.2 Sub-atomic particles and structure of an atom
Understandings:
Atoms contain a positively charged dense nucleus composed of protons and neutrons (nucleons).
Negatively charged electrons occupy the space outside the nucleus.
The main energy level or shell is given an integer number, n, and can hold a maximum number of electrons, 2n2.
A more detailed model of the atom describes the 
division of the main energy level into s, p, d and 
f sub-levels of successively higher energies.
​Structure of an atom worksheet
2.1 Atomic number and mass number
Applications and skills:
Use of the nuclear symbol notation to deduce the number of protons, neutrons and electrons in atoms and ions. 
Atomic number and mass number worksheet 
2.1 Isotopes
This video covers the definition and properties of isotopes. Isotopes are atoms of the same element that have different numbers of neutrons. They have the same atomic number but different mass numbers.
Isotopes worksheet
2.1 Calculating relative atomic mass
Understandings:
The mass spectrometer is used to determine the relative atomic mass of an element from its isotopic composition.
Applications and skills: 
Calculations involving non-integer relative atomic masses and abundance of isotopes from given data, including mass spectra.
Relative atomic mass worksheet 
2.2 Atomic orbitals and sub-levels
Understandings:
Sub-levels contain a fixed number of orbitals, regions of space where there is a high probability of finding an electron.
Applications and skills:
Recognition of the shape of an s atomic orbital and the px, py and pz atomic orbitals.
2.2 Electron configurations and the Aufbau principle (part one and part two) 
Understandings:
Each orbital has a defined energy state for a given electronic configuration and chemical environment and can hold two electrons of opposite spin.
Applications and skills: 
Application of the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 36.
Guidance:
Orbital diagrams should be used to represent the character and relative energy of orbitals.
​Applications and skills:
Application of the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 36.
Guidance:
Orbital diagrams should be used to represent the character and relative energy of orbitals.
The electron configurations of Cr and Cu as exceptions should be covered.
Electron configurations worksheet
2.2 Electron configurations of ions 
This video covers the electron configurations of ions.
2.2 Electromagnetic spectrum
Applications and skills:
Description of the relationship between colour, wavelength, frequency and energy across the electromagnetic spectrum.
Electromagnetic spectrum worksheet
2.2 Line spectra
Applications and skills:
Distinction between a continuous spectrum and a line spectrum.
Line spectra worksheet
2.2 Hydrogen emission spectrum
Understandings:
Emission spectra are produced when photons are emitted from atoms as excited electrons return to a lower energy level.
The line emission spectrum of hydrogen provides evidence for the existence of electrons in discrete energy levels, which converge at higher energies.
Applications and skills:
Description of the emission spectrum of the hydrogen atom, including the relationships between the lines and energy transitions to the first, second and third energy levels.
Hydrogen emission spectrum worksheet 
2.2 Flame tests
This video covers the flame tests.