1. Warm Up 9-20-17 Explain why the atom is neutral with no charge.
In the flame test how do we know which element absorb more energy?
If a Bunsen burner doesn’t turn on, what could be the problem?
Agenda Notes Unit 2-6
Turn in Lab Practice worksheet 2-6
Homework
Sept 26 - Test Unit 2
Sept 26 - Notebook check
Sept 26 - Online HW unit 2

2. Unit 2-6 Writing Electron Configuration

3. Writing Electron Configuration
Use energy level and orbitals
Read from left to right & top to bottom

4. Electron Configurations Example
Do electron configuration for the first 13 elements Only record down the ending electron configuration for each orbital
Try doing Ca, S, Ti, Fe

5. Electron Configuration Problems
Try: Ca S Ti Fe
1s22s22p63s23p64s2
1s22s22p63s23p4
1s22s22p63s23p64s23d2
1s22s22p63s23p64s23d6

6. Exception Rules D orbitals are 1 less energy than the S orbital
Cu and Cr electron config. are different

7. Orbital Filling Pauli Exclusion Principle
No more than two electrons can be in the same orbital
Aufbau Principle
Electrons fill orbitals that have the lowest energy first
Hund’s Rule
Orbitals of the same quantum number are occupied by one electron before any pairing occurs

8. Orbital Filling Examples

9. E. Configuration (Short Hand)

10. E. Configuration Short Hand Notation
Using the previous element in the last column as a base (bookmark)
Sulfur =
Ne as a base =
Short hand =
1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6
[Ne] 3s2 3p4
Think of short hand notation as bookmarks. We’re going to start after the designated noble gas. Do more examples

11. Electron Configuration
Exceptions:
Cu = [Ar] 3d10 4s1
Cr = [Ar] 3d5 4s1

12. Check for understanding
Write the short hand notation for: O, Mg, Zn

13. Assignments
Summary: What is the difference between short hand and long hand electron configuration?
Lab flame due before class is over
2-6 WS due next class

14. Homeroom
Digital citizen assessment
Quote of the week