International Baccalaureate IB Chemistry

Qualitatively describe the relationship between colour, wavelength, frequency and energy across the electromagnetic spectrum.

Distinguish between a continuous and a line spectrum. Details of the electromagnetic spectrum are given in the data booklet.

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.

The names of the different series in the hydrogen emission spectrum will not be assessed.

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.

Full electron configurations and condensed electron configurations using the noble gas core should be covered. 
Orbital diagrams should be used to represent the filling and relative energy of orbitals. 

The electron configurations of Cr and Cu as exceptions should be covered.

Explain the trends and discontinuities in first ionisation energy ($IE$) across a period and down a group.

Calculate the value of the first $IE$ from spectral data that gives the wavelength or frequency of the convergence limit. 

The value of the Planck constant $h$ and the equations $E = hf$ and $c = \lambda f$ are given in the data booklet.

Successive ionisation energy and group identification
Deduce the group of an element from its successive ionisation data.