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10 Cards in this Set
- Front
- Back
Aufbau principle |
Electrons enter orbitals of lowest energy first |
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Pauli exclusion principle |
An atomic orbital may hold a maximum of two electrons. Must have opposite spin |
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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. |
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Writing electron configurations |
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6 |
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Crystal Field Theory- d orbitals along or between axes |
dxy, dxz, dyz BETWEEN AXES dx2-y2, dz2 ALONG AXES |
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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 |
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d-orbital splitting octahedral complex |
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Crystal Field Theory and Colour |
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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) |
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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)
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