Difference between revisions of "Pauli exclusion principle"
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* [[Magnetic quantum number]] <i>m<sub>l</sub></i> is the number of orbitals within the subshell. m<sub>l</sub> can be 0,1...all the way to <sup>+</sup>/<sub>-</sub> l | * [[Magnetic quantum number]] <i>m<sub>l</sub></i> is the number of orbitals within the subshell. m<sub>l</sub> can be 0,1...all the way to <sup>+</sup>/<sub>-</sub> l | ||
* [[Spin quantum number]] <i>m<sub>s</sub></i> is the spin of the electron. there are two spins per subshell. they are represented by a +1/2 or -1/2 | * [[Spin quantum number]] <i>m<sub>s</sub></i> is the spin of the electron. there are two spins per subshell. they are represented by a +1/2 or -1/2 | ||
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| + | The Pauli exclusion principle follows from the requirement that fermions must have antisymmetric wavefunctions. | ||
==References== | ==References== | ||
Revision as of 22:25, September 12, 2015
The Pauli Exclusion Principle states that no two electrons in the same atom can have the same set of quantum numbers. This set is made up of
- Principle quantum number n: this is the shell around the atom where the electron exists. The shells are represented by whole numbers. n can be 1,2,3....
- Orbital quantum number l is the number of subshells within a shell. l can be 0,1... to (n-1)
- Magnetic quantum number ml is the number of orbitals within the subshell. ml can be 0,1...all the way to +/- l
- Spin quantum number ms is the spin of the electron. there are two spins per subshell. they are represented by a +1/2 or -1/2
The Pauli exclusion principle follows from the requirement that fermions must have antisymmetric wavefunctions.