1. Element Quiz #3 Quietly study for your quiz – spelling counts!
Make sure you write “Element Quiz #3” at the top of the paper, portrait layout, and your name & bell.
Number 1 – 11.
Directions: Given the name or symbol, provide the opposite.

2. Element Quiz #3
Lead Mn
Neon Hg
Nickel Mg
Lithium Mo
Nitrogen P
Oxygen

3. Follow along in Text Chapter 3 Section 3 Pgs. 90 - 99
Electron Configuration
Follow along in Text
Chapter 3 Section 3
Pgs

4. Orbitals
Regions around a nucleus where electrons are located that correspond to specific energy levels
Called electron cloud because no definite boundaries

5. Electron States Ground State: Lowest possible energy level
Excited State: Electron gains energy & moves to a higher level
Energy in the form of light is emitted when an electron loses energy & falls to a lower level

6. Aufbau Principle Aufbau means “building up” in German
Electrons fill orbitals that have the lowest energy first
The Diagonal Rule follows the Aufbau Principle

7. Shorthand (Noble Gas) Configuration
The Noble Gases can be used to fill in the first part of the electron configuration of atoms of the following period
S = 1s2 2s2 2p6 3s2 3p4 and
Ne =1s2 2s2 2p6 so
S = [Ne] 3s2 3p4

8. Complete the below nuclear equations on your exit slip.
Closure
Complete the below nuclear equations on your exit slip.
218 84 Po -1 e 1. → +
238 92 U 4 2 He 2. → + 59 27 Co 1 n 3. + → 14 4.
C undergoes beta decay 6

9. Follow along in Text Chapter 3 Section 3 Pgs. 90 - 99
Orbital Diagrams
Follow along in Text
Chapter 3 Section 3
Pgs

10. Orbital Diagrams
Uses arrows to represent each electron and lines to represent each sublevel
Can be determined from Electron Configuration

11. Pauli Exclusion Principle
Wolfgang Pauli discovered that no more than 2 electrons can occupy a single orbital
No two electrons in an atom will have all the same quantum numbers, which tell an electrons location in an atom

12. Orbital Diagrams
Each sublevel is represented by a line above the orbital’s name 1s 2s 2p

13. Sublevels Divisions of orbitals
Each type of orbital has its own amount of sublevels -1 1
s - orbital
p - orbitals -2 -1 1 2
d - orbitals -3 -2 -1 1 2 3
f - orbitals

14. Orbital Diagrams
Electrons are put on each line and the number of electrons for each sublevel is a superscript
1s2
2s2
2p6

15. Hund’s Rule
Each line of a sublevel must have one electron on it before the electrons are paired 1 2 3 4 5 8 6 9 7 10
1s2
2s2
2p6

16. Neon (Ne) Orbital Diagrams
Counting these electrons, you can tell that this element is…
Neon (Ne)
1s2
2s2
2p6

17. Hund’s Rule So for Oxygen, the orbital diagram would be 1s2 2s2 2p4 13 4 5 8 6 7
1s2
2s2
2p4