1. Basic Bohr to Quantum Orbitals KLM to spdf
Orbits and Orbitals
Basic Bohr to Quantum Orbitals
KLM to spdf

2. KLM and spdf???
KLM – Bohr style / old style lettering for the “shells” or “orbits”. K is closest to the nucleus, L is next, M (N,O,P etc)
Now we know that KLM is “really” the “Principle Quantum Number” 1,2,3 for the energy levels
spdf – refers to the shape of the “orbital” –

3. A short deBroglie diversion

6. More rules
No orbital can have more than 2 e- in it. (one spin up, one spin down)
Orbitals are half filled (with spins in the same direction) before they are doubly filled.
Orbitals are filled from lowest energy to highest energy.

7. Confusing? OK
“Quantum Numbers” are the way we can describe locations where electrons can be found.
The “Principle Quantum Number” – n – is the same as the old shells, and is the same as the number of the Period on the table.

8. n, l, m, s n = energy level (old shell / Bohr model)
l = angular momentum => shape
s = 0 , p = 1, d = 2, f = 3
l ≤ n - 1
m = magnetic quantum number => orientation
-l ≤ m ≤ +l
s = spin ( +½, -½ or: up, down)

9. That didn’t Help!!!
In the 1st level – Only an s orbital with 2electrons
In the 2nd level, an s orbital with 2 electrons and a p orbital with 6 electrons
OK, pictures are easier

10. Only 1 S orbital per level, 2 e-
S Orbital – Spherical
Only 1 S orbital per level, 2 e-

11. P orbital – Perpendicular 3 orbitals, 2e- each

12. D Orbitals – “double dumbbells” 5 orbitals, 2e- each, 10e- total

13. F orbital – “dead spiders” 7 orbitals – 2e- in each – 14 total
*late breaking info – the above is correct, however since I went to school, a new shape – the one in the middle, has been added

15. Now, How do you Fill Them
You fill the orbitals from the lowest energy on up – Half filling them first, (with spins the same) then doubly filling them

20. Aufbau principle 1s *we haven’t needed these yet 2s 2p 3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f 5g*
6s 6p 6d 6f*6g*6h*
7s 7p

21. Some practice – Some Questions
Look up the Atomic number, and then determine (not look up) the electron orbital configuration.
H He
O K
Ca Cr
U Ag
Au Pt

22. Compare your configuration for Cr, Ag, Au and Pt with the “official” one. Are they the same? If not, why are they different?

23. Noble Gas Configuration
1s2 He 2s2 2p6 Ne 3s2 3p6 Ar 4s2 3d10 4p6 Kr 5s2 4d10 5p6 Xe 6s2 4f14 5d10 6p6 Rn 7s2 5f14 6d10 7p6 Uuo

25. Olympicene

27. 5 linked carbon rings with hydrogens
Pentacene
5 linked carbon rings with hydrogens

28. Fullerenes

35. Magic Numbers
2 – 8 – 8 –
2 – 6 – 10 – 14 (1,3,5,7)

42. electronegativity

43. Disclaimer
Aloha I put together these power points for use in my science classes. You may use them in your classes. Some images are public domain, some are used under the fair-use provisions of the copyright law, some are mine. Copyright is retained by the owners!
Ted Brattstrom