Ch7 Lec 5
(4/27/20, bes)
Welcome to your afternoon lecture...as opposed to online..."lab"...as always...please take notes (no need to turn anything in), the WA will test your understanding...
Here is a slightly different version of the hydrogen atom energy level diagram. As you will recall, this idea of "quantized" energy levels was a result of some experiments that resulted in the formulation of quantum mechanics. The electron exists in the lowest energy state, the 1s orbital, unless this electron is excited to higher energy levels.
In the following version of the energy level diagram, i have places a few "excited" electrons...complete the following table to identify the quantum numbers with each of these electrons.
| color | n - principal | l -angular | ml - magnetic | 'ms - spin |
| purple | ||||
| orange | ||||
| green | ||||
| red |
Multi-electron Energy Levels
The hydrogen atom is special in that it only contains 1 electron. When a second electron (or more) is added into the atom, there is a BIG change in the energy levels. Below is the energy level diagram for a multi-electron system...note the following:
- 1) relative to the s-orbitals, the p-orbital energy levels is shifted up,
- 2) relative to the p-orbitals, the d-orbital energy levels are shifted up,
- 3) relative to the d-orbitals, the f-orbital energy levels are shifted up,
