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Electron Configurations!

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

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

- Higher the n, the farther away from the nucleus
- Sublevels (s,p,d,f)
- Number of sublevels is related to the energy level

- Orbitals
- Make up sublevels

- There are 4 sublevels
(& types of orbitals):

s, p, d, f

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

- Sublevels which are made up of..

- 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

- 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

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

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

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

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

- Talk about Conclusions
- Electron Configurations
Lab Report due tomorrow TYPED

Chapter 3.3 (part2) Test = Thursday

- Electrons fill the lowest-energy orbital first

1s

2s 2p

3s3p 3d

4s4p4d 4f

5s5p5d5f

6s6p6d6f

7s7p7d7f

1s

2s 2p

3s3p 3d

4s4p 4d 4f

5s5p 5d 5f

6s6p 6d 6f

7s7p 7d 7f

- Two electrons of opposite spins can occupy the same orbital

- 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).

Lowest Energy Level

2p

2s

1s

2p

1s

2s

- Cl:
1s22s22p63s23p5

2p

1s

2s

3p

3s

- Complete bottom of p.11
- Write configurations out based on section above.

1s

2s 2p

3s3p 3d

4s4p4d 4f

5s5p5d5f

6s6p6d6f

7s7p7d7f

1s

2s 2p

3s3p 3d

4s4p 4d 4f

5s5p 5d 5f

6s6p 6d 6f

7s7p 7d 7f

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

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

- 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!

- Cr and Mo
- s1d5

- Cu, Ag, Au
- s1d10

- 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 that comes before the element]

+ additional electrons

Ex: Chlorine

instead of… 1s22s22p63s23p5

Noble Gas shortcut Method = [Ne]3s23p5

- Si
- Br

- Remember how to find your number of electrons in ions!!
K+ = how many electrons?

Cl- = how many electrons?

O2- = how many electrons?