1. The Quantum Mechanical Model of the Atom

2. Schrodinger The quantum mechanical model determines the energy an electron can have and the PROBABILITY of finding an electron in a certain location. Like a plane propeller –Where we get “electron cloud” phrase

3. Atomic Orbitals Vocab to know: 1.Atomic orbitals: where you’re most likely to find an electron, designated by a letter, s p d or f 2.Energy level: Tells you whether an electron has lots of NRG or just a little. -Low #, Close to nucleus, low NRG 3. Sublevel: consists of a number AND a letter. The number IS the principal energy level / quantum number; the letter IS the orbital—tells you the shape of the orbitals

5. Each orbital can hold a maximum of 2 electrons!

6. Orbitals The letters in the energy levels always occur in this order: s, p, d, f Yes, they are LOWERCASE letters!

7. Orbital Shapes Designated with letters s, p, d, and f s = spherical shaped. There is just one possible orbital. How many electrons can the s orbital hold? p = dumbell shaped. There are 3 possible orbitals. How many electrons can the p orbital hold? d = Shaped like a Rubic’s cube. 5 possible orbitals f = Weirdly shaped. 7 possible orbitals

8. How do principal energy levels, energy sublevels, and orbitals all tie together? Principal NRG level = 1 THEN There is 1 sublevel AND That sublevel is 1s SO It can hold a maximum of 2 electrons

9. Look at this one: If the principal energy level is 2 There are 2 sublevels They are 2s and 2p s indicates 1 orbital, can hold 2 e- p indicates 3 orbitals, can hold 6e- The maximum electrons in energy level 2 is 8 electrons!

10. YOU TRY! If the principal energy level is 3: How many sublevels? What are they? What is the maximum number of electrons?

11. Again! Yea! If the principal energy level is 4: How many sublevels? What are they? Max # of electrons?

12. Electron Configurations Na (11) 1s 2 2s 2 2p 6 3s 1 An electron configuration is a map that tells you where the electrons are located!

13. Aufbau Principle The lowest energy levels fill first!

14. Pauli Exclusion Principle There are 2 electrons in each orbital; they have opposite spins, that are designated by up and down arrows:

15. Hund’s Rule One electron enters each orbital in a sublevel until each one has one, then start adding the second electrons.