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Happy Monday!

Electron Configurations!

- Last week of 1stQuarter
- Lab Reports due WEDNESDAY!!
- Chapter 3.3 (Part 2) Test = THURSDAY!

Quantum Number

- A number that specifies the properties of electrons
- Every electron has 4 quantum numbers
- Most importantly, it specifies the orbital in which the electron is located

Energy Levels, Sublevels, and Orbitals

- Energy Levels (represented by principle quantum number - n)
- Higher the n, the farther away from the nucleus

(More Energy)

- Sublevels (s,p,d,f)
- Number of sublevels is related to the energy level
- Orbitals
- Make up sublevels

Sooo….

- Energy levelsare made up of..
- Sublevels which are made up of..
- Orbitals!

Orbitals

- Orbital:
- Most probable location of electrons (90% chance)
- Each orbital can hold a maximum of 2 electrons
- Each region corresponds to a specific energy level (n)
- Sometimes called electron clouds

Orbitals

- Described by both a number and a letter
- Number – tells the energy level in which the orbital is located
- Letter – tells the shape of the orbital
- The higher the energy level, the more different shapes that are possible

Orbitals

- How do these orbitals fit together?
- Watch this…
- And this…

Electron Configurations!

- An electron configuration is the arrangement of electrons in an atom

Orbital Labels:(examples)

- 1s
- 2s
- 2p
- The number tells us the energy level

- 3s
- 3p
- 3d
- The letter tells us the orbital shape!

Happy Tuesday!!

- Talk about Conclusions
- Electron Configurations

Lab Report due tomorrow TYPED

Chapter 3.3 (part2) Test = Thursday

Aufbau Principle

- Electrons fill the lowest-energy orbital first

The order in which orbitals are filled (Aufbau principle) may be also be displayed as an arrow diagram:

1s

2s 2p

3s3p 3d

4s 4p4d 4f

5s 5p5d 5f

6s 6p6d 6f

7s 7p7d 7f

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

7s 7p 7d 7f

Pauli Exclusion Principle

- Two electrons of opposite spins can occupy the same orbital

Hund’s Rule

- The number of unpaired electrons is the maximum possible and these unpaired electrons must have the same spin
- (Must fill each orbital with 1 electron–all with the same spin–before doubling up).

Orbital Diagram:

Lowest Energy Level

- Write configurations out based on section above.

Remember the Arrow Diagram:

1s

2s 2p

3s3p 3d

4s 4p4d 4f

5s 5p5d 5f

6s 6p6d 6f

7s 7p7d 7f

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

7s 7p 7d 7f

Practice using it!

- Follow the arrows to write on the electron configurations on the bottom of p.12

Electron Configuration Practice

- Practice writing configurations based on Periodic Table Method – p.13
- Homework if not finished.

Happy Wednesday!!

- Finish Electron Configurations!
- More Periodic Table Method Practice
- Exceptions
- Noble Gas Simplification/shortcut
- Lab Reports Typed due TODAY!!
- Turn in on front table
- UPDATE: Ch.3 Pt.2 Test FRIDAY!

Exceptions to the Rule

- Cr and Mo
- s1d5
- Cu, Ag, Au
- s1d10

Noble Gas Shortcut

- A noble gas has a full outer shell (s and p orbitals)
- So, we can use the noble gas symbol to represent all of the inner layers of the atom, and then show what we have added to it

Noble Gas Shortcut:

[Noble gas that comes before the element]

+ additional electrons

Ex: Chlorine

instead of… 1s22s22p63s23p5

Noble Gas shortcut Method = [Ne]3s23p5

Ions!!

- Remember how to find your number of electrons in ions!!

K+ = how many electrons?

Cl- = how many electrons?

O2- = how many electrons?

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