1. BELLWORK 10/27/16

2. QUANTUM MODEL OF THE ATOM – Day 2 Review
Organizes the electrons into 4 orbitals found on different energy levels.
The four orbitals are….s, p,d, f
The “s” orbital can hold a maximum of ____ 2 electrons.
The “p” orbital is made up of _3___ sub-orbitals, and each one holds _2____ electrons.
Which orbital is found on the 1st energy level? “s” 2nd? “s” and “p”

3. Electron Configuration
Gives a detailed description of where the electrons in an atom are located.
Ex: Show where all of the electrons in Al are located within the Aluminum atom.

4. Rules for Writing Electron Configurations
Aufbau Principle- electrons enter the lowest energy level first. All orbitals have to be filled before electrons can be placed in the next energy level

5. Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p
Aufbau Principle – the electrons fill the lowest energy levels first.
Ex:
Show the location of the electrons in the neutral atom. Al13

6. Rules for Writing Electron Configurations
Hund’s Rule – Each suborbital within an orbital is filled with one electron before the 2nd electron is added.

7. Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p
Hunds Rule – one
electron is placed in each orbital before the second electron is placed into the orbital
Ex: Which element does this electron configuration represent?

8. Rules for Writing Electron Configurations
Pauli Exclusion Principle - Electrons within the same orbital must have opposite spins.

9. Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p
Pauli Exclusion Principle – Electrons within the same suborbital must have opposite spins.

10. We use the Periodic Table to determine the order in which the electrons fill the orbitals. Read the periodic table from left to right beginning with the 1st energy level (Period 1)

11. HOW MANY ELECTRONS CAN A “D” ORBITAL HOLD?

12. CHECKPOINT

13. PRACTICE PROBLEM #1
Write the electron configuration and the orbital notation for He.

14. Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p
The 1s orbital is filled first. (Aufbau Principle)
Notice the 2 electrons have opposite spins
(Pauli Exclusion)

15. Helium
1s2

16. Practice Problem #2
Write the electron configuration and the orbital notation for Boron.

17. Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p
The 1s orbital is filled first. (Aufbau Principle)
Notice the 2 electrons have opposite spins (Pauli Exclusion)

18. Boron - 1s22s22p1

19. Practice Problem #3
Write the electron configuration and orbital notation for silicon.

20. Silicon – 1s22s22p63s23p2

21. Practice Problem #4
Write the electron configuration and the orbital notation for Manganese.

22. Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p
Hunds Rule – one
electron is placed in each orbital before the second electron is placed into the orbital

23. Manganese – 1s22s22p63s23p64s23d5

24. Finish working in your cooperative groups on you inquiry packet.
AGENDA
Finish working in your cooperative groups on you inquiry packet.

25. EXIT TICKET
Why do you fill the 3d orbital before the 4p?