1. Important Questions In The Overall Scheme of Life (…or what I learned in chemistry class last Friday!)

2. Give one noteworthy piece of information indicating an electron is a particle and then do the same thing from a wave perspective.

3. When Schroedinger treated the electron as a wave he came up with his famous “wave equation”…what information does psi, Y, stand for?....what about Y 2

4. When considering the size of an electron, what makes us rationalize why it makes sense for Y to have many solutions for the same energy value?

5. Give one noteworthy piece of information indicating an electron is a particle and then do the same thing from a wave perspective.
Particle: electrons have a mass
Wave: electrons produce interference patterns in the double slit experiment.

6. A series of images taken in a double-slit experiment with electrons as the electron current density is increased. Since there is only one
electron in the apparatus at a given time, this figure shows how an
interference pattern can be built up from single-electron events.
(Taken from physicsweb.org/box/world/15/9/1/bologna-image)

7. Y stands for location of the electron
When Schroedinger treated the electron as a wave he came up with his famous “wave equation”…what information does psi, Y, stand for?....what about Y 2
Y stands for location of the electron
Y2 stands for the probability of finding the electron at a specific location

8. When considering the size of an electron, what makes us rationalize why it makes sense for Y to have many solutions for the same energy value?
Heisenberg’s Uncertainty Principle tells us that we can’t predict where an electron will be, only where it will probably be!

9. What we know (about the hydrogen atom):
There is a nucleus
Electron (wave/particle) is around the nucleus
The location of the electron is not absolutely known…but the probable positions can be calculated with the wave equation.
These locations are called orbitals (the wave function, Y)
The orbital depends upon the total energy of the electron

11. This distance matches the distance of the closest orbit for an electron in the Bohr model

12. ◄Boundary Surface Diagrams
Of which of the “s” orbitals is this distribution representative?
◄Boundary Surface Diagrams

13. What we know (about the hydrogen atom):
There is a nucleus
Electron (wave/particle) is around the nucleus
The location of the electron is not absolutely known…but the probable positions can be calculated with the wave equation.
These locations are called orbitals (the wave function, Y)
The orbital depends upon the total energy of the electron
Orbitals can be pictured as boundary surface diagrams.

14. The existance of sublevels!!!!!
Bright-Line Spectrum for Cadmium
The existance of sublevels!!!!!

15. …described as the p sublevel’s “p” type orbitals
Orbitals (pictured as boundary surfaces) that become available once the electron reaches the second energy level.

17. …described as the “d” sublevel’s “d” type orbitals available once n = 3.

18. …described as the “f” sublevel’s “f” type orbitals available once n = 4

19. How many sublevels are “in” the second energy level?2
How many orbitals are “available” in the third energy level? 9
How many nodes does a 3d orbital have?
What’s the difference between a 1s and a 2s orbital?
1s is “smaller” than the 2s and the 2s has one node while the 1s has no nodes.