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Spring 2011 |
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| Exercise: Quantum Numbers & Periodicity |
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Discussion Modules |
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| Quantum Number | Symbol | Characteristic specified | Information provided | Possible values |
| Principle quantum number | n | Shell | Average distance from nucleus (r) | 1, 2, 3, 4, ... |
| Angular momentum (Azimuthal) quantum number | l | Subshell | Shape of orbital | 0 (s), 1 (p), 2 (d), 3 (f), ...n - 1 |
| Magnetic quantum number | ml | Orbital | Orientation of orbital | - l ... 0 ... +l |
| Spin quantum number | ms | Electron spin | Spin direction | ± 1/2 |
1. Write sets of quantum numbers for all of the electrons in a ground state Carbon atom.
2. Write sets of quantum numbers for all of the valence electrons in a ground state Phosphorus atom.
3. Write sets of quantum numbers for all of the valence electrons in a ground state Iodine atom.
4. Write sets of quantum numbers for all of the outermost electrons in a ground state Cobalt atom.
5. Using Spectroscopic notation write the electronic configurations for the ground state atoms below:
Be:
Al:
Si:
S:
Ne:
6. Using Spectroscopic notation the Noble Gas Core convention write the electronic configurations for the ground state atoms below:
Hg:
Ta:
Bi:
Am:
Xe:
Mo:
Ag:
7. Using Spectroscopic notation write the electronic configurations for the ground state ions below:
Mg2+:
P3-:
Ni2+:
V3+:
Ag+:
8. Using Orbital Filling Diagrams write the electronic configurations for the ground state atoms below:
B:
Ti:
Fe:
Cr:
As:
Se:
Answers 1-8
In addition to these exercises you should familiarize yourself with the text materials referenced below.
© R A Paselk
Last modified 27 March 2009