1. Atomic Structure Quantum Numbers

2.  specify the properties of orbitals and of electrons in orbitals  the first three numbers describe: main energy level (n) main energy level (n) Shape (l) Shape (l) Orientation (m l ) Orientation (m l )  4 th describes spin of electron (m s )

3. 1 st Quantum Number (n)  main energy level occupied by electron  values are all positive whole # integers (1,2,3,…)  As it increases, the electron: has more energy has more energy is farther from nucleus is farther from nucleus  the total number of orbitals in a level is equal to n 2

4. 1 st Quantum Number (n) n# of orbitals n# of orbitals 11 11 24 24 39 39 416 416

5. 2 nd Quantum Number (l)  the shape of the orbital (sublevel)  # possible shapes = energy level 4 th energy level has 4 possible shapes 4 th energy level has 4 possible shapes  possible values: 0 to n-1 s: 0 s: 0 p: 1 p: 1 d: 2 d: 2 f: 3 f: 3

6. 2 nd Quantum Number LevelSublevels 0 1 2 3 0 1 2 0 1 0

7. 3 rd Quantum Number (m l )  the position of an orbital around the nucleus (x, y, or z direction)  has values from +l  -l  each orbital holds maximum of 2 electrons

8. 4 th Quantum Number (m s )  the spin state of the electron  only 2 possible directions  only 2 possible values: +½ and -½  paired electrons must have opposite spins -1/2 +1/2

9. Connection to Configurations 1. Draw out the orbital notation for the last sublevel filled in an atom 2. Circle the last electron inserted in that sublevel 3. Find the four quantum numbers for that electron

10. Example 1 What are the 4 quantum numbers for the electron of highest energy in nitrogen?

11. Example 2 What are the 4 quantum numbers for the electron of highest energy in sulfur?

12. Example 2 What are the 4 quantum numbers for the electron of highest energy in iron?

13. Example 4 What are the 4 quantum numbers for the electron of highest energy in calcium?