- Emission Spectra, photons and excited electrons 

- line emission spectra of HYDROGEN

Main energy levels of shells= 2n^2

-s p d and f sub levels and higher energies

- Sub levels and orbitals and probability of finding an electron

-Orbital defined energy state

-relationship between colour wavelength frequency and energy across the electromagnetic spectrum

- Distinction between a line and continuous spectrum

- Emission spectrum of the hydrogen atom + relationships between the lines and energy transitions to the 1st, 2nd and 3rd energy levels

- Recognition of the shape of an s atomic orbital and the px py and pz atomic orbitals

Application of Hund's rule, the Aufbau principle and the Pauli exclusion principle to write electron configurations up to Z = 36