1.3 Electron configurations

• Produced when electrons in excited states return to lower energy levels

• Relationship: colour, wavelength, frequency, energy across electromagnetic spectrum

• Continuous vs. line spectrum

• Evidence for discrete energy levels

• Energy transitions to n=1, n=2, n=3

• Describe convergence at higher energies; series names are not assessed

• Integer n, holds maximum 2n² electrons

• Deduce maximum electrons in each main energy level

• Main energy levels divided into s, p, d, f sublevels

• Shapes: s orbital (spherical), three p orbitals (dumbbell)

• Link sublevels to s, p, d, f blocks in the periodic table

• Each orbital holds 2 electrons of opposite spin

• Aufbau principle, Hund's rule, Pauli exclusion principle

• Electron configurations for atoms and ions up to Z=36

• Use full, condensed, and orbital box diagrams; include Cr and Cu exceptions

• Convergence limit = ionization

• Trends in 1st IE across period and down group

• Calculate 1st IE from spectral data (wavelength/frequency)

• Provide information about electron configuration

• Deduce element's group from successive IE data