Fichas
2.2 Electron Configuration
Fichas del conjunto (11)
- 1Quanta Mechanical Model of Atom1. Electrons are treated as waves
2. The mathematical function that describes the electron wave is called a wave equation ( i.e Schrodinger's wave equation)
3. It is impossible to calculate the exact position and momentum of an e- sumultaneously (i.e Heisenburg Uncertainty Principle)
4. The probability of finding an electron in a given space can be determined and is related to the square of a wave function
5. When analyzed, the wave function gives us regions of space around the nucleus where there is a high probability of finding and e-. These are called atomic orbitals (a.k.a electron clouds)
6. A greater number of characteristics of the electron are quantized in QM model than in Bohr model. Electrons and their orbitals are described by four quantum numbers. - 2n=principle quantum number
- 3l (cursive)=angular momentum quantum #
- 4mlmagnetic quantum number
- 5msspin quantum number
- 6# of orbitals per energy level=n^2
- 7# of e- per energy level=2n(^2)
- 8orbital diagramlines/boxes= orbitals
arrows=electrons
direction of arrow=spin - 9electron configurationsuperscripts
individual orbitals not shown - 10Exceptions in the D blockAtoms naturally adopt lowest energy state
A half-filled (d^s) and fully-filled d orbital (d^10) are very stable and are therefore favored - 11Transition Metal IonsWhen ant d- block elements form ions, the 4s electrons are always lost first
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- Descripción
- IB Chemistry SL 1 (Topic 2.2 Electron configuration & Topic 12.1 ) IB Chemistry SL I Fichas sobre 2.2 Electron Configuration, creado por hollandblumer6 el 16/11/2014.
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- hollandblumer6
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