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10 Cards in this Set

  • Front
  • Back

Aufbau principle

Electrons enter orbitals of lowest energy first

Pauli exclusion principle

An atomic orbital may hold a maximum of two electrons. Must have opposite spin

Hunds rule

When electrons enter the same orbitals of equal energy, one electron enters each orbital until all are filled with electrons of the same spin.

Writing electron configurations

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6

Crystal Field Theory- d orbitals along or between axes

dxy, dxz, dyz BETWEEN AXES


dx2-y2, dz2 ALONG AXES

Energy of electrons in orbitals

In an isolated metal atom or ion, the five d-orbitals are degenerate- and so all have the same energy level.


- However, under the influence of ligands, this is NOT the case

d-orbital splitting octahedral complex

Crystal Field Theory and Colour

Dimagnetic, Paramagnetic

- If d-orbital splitting energy is low, then there will be a high number of unpaired electrons. This is termed high spin distribution.


High spin=Paramagnetic (attracted into a magnetic field)


- if the d-orbital splitting energy is high, then there will be a high number of paired electrons. This is termed low spin distribution.


Low spin=dimagnetic (not attracted into a magnetic field)

electrons configurations

- Electron distribution for the split d orbitals changes as the d-orbital splitting energy increases.


- If the d-orbital splitting energy is high, it can overcome the pairing energy (repulsion from electrons in the same orbital) and so the electrons will be paired rather than split.


- If the d-orbital splitting energy is low, then it won't overcome the pairing energy, and electrons will be distributed evenly over the five orbitals (both high and low- so promotes, rather than pairs)