Humboldt State University ® Department of Chemistry

Richard A. Paselk

 

General Chemistry

Spring 2009

Exercise: Quantum Numbers & Periodicity

© R. Paselk 2008
 
 

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Quantum Numbers & Periodicity

 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 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.


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© R A Paselk

Last modified 27 March 2009