1. Electron Configuration I.Introduction (OLD WAY) A. Principal Energy Level –(____)

2. Know that the Bohr Model goes from ___ to _____ _____=tells you what pel you are at. Ex. N=3 means? N=5 means?

3. B. Your number of pel = your number of sublevels C. Ex. N=3 n=5

4. II. Sublevels-(Bohr did not know of their existence) A. Sublevel names (4) are: n=1 n=2n=3n=4

5. B. Maximum number of electrons each sublevel can hold s= p= d= f=

6. II. Try electron configuration 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 7p 3d 4d 5d 6d 7d 4f 5f 6f 7f Ex. Lithium Carbon Magnesium Iron Strontium Silver

7. III. Orbitals- places where electrons are found Sublevels # of orbitals Max. # electrons

8. Pauli Exclusion Principle: Maximum number of electrons per orbital is 2 Hund’s Rule: The first electron must go up (clockwise) and the second electron must go down (counter clock wise). Each p and d sublevels must have 1e- before you double up.

9. Try some examples Nitrogen Fluorine Shapes of the orbitals are: s= p= d=

11. IV New Way(total # of e- in the pel) Ex. Ca Zn Pb

12. What does 2-8-2 mean? Can you identify the element? A. 2-8-9-2 B. 2-8-18-32-12-2 C. 2-8-18-32-18-8

13. V. Valence electrons-outermost electrons How do you find valence electrons? 1.Go to periodic table, look up electron configuration and pick the last # Octet Rule: no more than 8 valence electrons Ex. Mg= F= Au= O=

14. VI Electron Dot diagrams or Lewis Dot structures 1.Place e- in correct sublevel 2.Each p sublevel must have one e- before you double up 3.Most you can have is 8 (Octet Rule) Ex N O C Ar Cl