1. Aufbau Principle An electron occupies the lowest energy orbital that can receive it.

2. Pauli Exclusion Principle No two electrons in the same atom can have the same set of four quantum numbers.

3. Hund’s Rule Orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin.

4. Heisenberg Uncertainty Principle It is impossible to determine simultaneously both the position and the velocity of an electron or any other particle.

5. Bohr Model of Hydrogen http://science.sbcc.edu/physics/solar/sciencesegment/boh ratom.swf

7.  Symbolized by n  Indicates the energy level  Values are all positive integers  # of orbitals in energy level = n 2

8.  Symbolized by l  Indicates the shape of the orbital  Values of l: 0 and all integers ≤ n-1

9.  Symbolized by m  Indicates the orientation of an orbital around the nucleus

10.  Has only two possible values +1/2, -1/2  Indicates the two fundamental spin states of an electron in an orbital

11.  Chapter 4 Things to Review Vocabulary Electron Configuration Orbital Notation Noble Gas Configuration Bohr’s Model of Hydrogen Wave: crest, trough, amplitude, wavelength Calculations: Energy, Wavelength, Frequency

12.  Chapter 4 Review page 118 1, 3, 4, 6, 8, 9,11,12, 13, 14a&b, 16, 17,18a, 19a, 20, 21, 22, 23, 24,25, 36, 27, 28. 29, 30, 32, 36, 37, 39, 40, 41, 42, 43, 44, 44, 45 1, 3, 4, 6, 8, 9, 11-13, 14a&b, 16, 17,18a, 19a, 20-30, 32, 36, 37, 39- 45