1. 5.1 2nd Half

2. Warm Up #2 What was the problem with Rutherford’s model of the atom?
Describe Bohr’s model of the atom.
Explain the problem with Bohr’s model of the atom.

3. Atomic Orbitals
Energy levels of electrons are designated by principle quantum numbers (n).
These are assigned certain values:
n=1,2,3,4,5,6, etc.

4. Atomic Orbitals Each energy level divides into energy sublevels.
Each sublevel corresponds to a different cloud shape.

5. Atomic Orbitals This cloud space is called an atomic orbital.
An atomic orbital is a region in space with a high probability of finding an electron.

6. Atomic Orbitals Number of sublevels = number of principle energy level
number of orbitals per level = n2

7. Atomic Orbitals There are four types of orbitals: 1. s (1) 2. p (3)
3. d (5)
4. f (7)
The number inside the parenthesis is how many there actually are of that type.

8. Atomic Orbitals
The s orbitals give spherical clouds, and the p orbitals give dumbbell shaped clouds.
The d and f orbitals are far more complex.

10. Atomic Orbitals Places with a high probability of finding an electron.
The maximum number of electrons that can occupy an energy level is given by the formula: 2n2

12. 5.2 Electron Configurations
The ways in which electrons are arranged in various orbitals around the nuclei of atoms are called electron configurations.
Three rules—the aufbau principle, the Pauli exclusion principle, and Hund’s rule—tell you how to find the electron configurations of atoms.