1. Happy Monday! GRAB YOUR HW SHEET Take electron configuration
Take out your lab notebook
Ask your partner how they’re feeling about this week…Good? Bad? Stellar?
Happy Monday!

2. Warm-Up 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d5 [Ar] 4s2 3d5
Write the complete and abbreviated electron configurations for Manganese (#25).
How many electrons are in each energy level of Manganese?
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d5
[Ar] 4s2 3d5
Energy Level 1-2 electrons
Energy Level 2-8 electrons
Energy Level 3-13 electrons
Energy Level 4-2 electrons

4. Review Homework!
With your partner take turns answering each others questions.
Explain how YOU solved each type of problem.
Find out what questions still remain for you and your partner
Call over Ms. Bryce for help

5. Learning Targets

6. More Practice!
In the space below, write the unabbreviated electron configurations of the following elements: 1) sodium ________________________________________________ 2) iron __________________________________________________ 3) bromine________________________________________________ 4) barium ________________________________________________ 5) neptunium______________________________________________

7. Answers
1) Sodium 1s22s22p63s1 2) Iron 1s22s22p63s23p64s23d6 3) Bromine 1s22s22p63s23p64s23d104p5 4) Barium 1s22s22p63s23p64s23d104p65s24d105p66s2 5) Neptunium 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f5

8. MORE!
In the space below, write the abbreviated electron configurations of the following elements: 6) cobalt ________________________________________________ 7) silver ________________________________________________ 8) tellurium ________________________________________________ 9) radium ________________________________________________ 10) lawrencium ________________________________________________

9. Answers
6) cobalt [Ar] 4s23d7 7) silver [Kr] 5s24d9 8) tellurium [Kr] 5s24d105p4 9) radium [Rn] 7s2 10) lawrencium [Rn] 7s25f146d1

10. More
Determine what elements are denoted by the following electron configurations: 11) 1s22s22p63s23p4 ____________________ 12) 1s22s22p63s23p64s23d104p65s1 ____________________ 13) [Kr] 5s24d105p3 ____________________ 14) [Xe] 6s24f145d6 ____________________ 15) [Rn] 7s25f11 ____________________

11. Answers
11) 1s22s22p63s23p4 sulfur
12) 1s22s22p63s23p64s23d104p65s1 rubidium
13) [Kr] 5s24d105p3 antimony
14) [Xe] 6s24f145d6 osmium
15) [Rn] 7s25f11 einsteinium

12. MORE!
Determine which of the following electron configurations are not valid: 16) 1s22s22p63s23p64s24d104p5 ____________________ 17) 1s22s22p63s33d5 ____________________ 18) [Ra] 7s25f8 ____________________ 19) [Kr] 5s24d105p5 ____________________ 20) [Xe] ____________________

13. Answers!
16) 1s22s22p63s23p64s24d104p5 not valid (take a look at “4d”) 17) 1s22s22p63s33d5 not valid (3p comes after 3s) 18) [Ra] 7s25f8 not valid (radium isn’t a noble gas) 19) [Kr] 5s24d105p5 valid 20) [Xe] not valid (an element can’t be its own electron configuration)

14. Orbital Diagram Notes

15. How do Electrons Behave Inside Orbitals
How do Electrons Behave Inside Orbitals? - Electrons move in waves and also “spin” - Orbitals must have 2 electrons of opposite spins to be magnetically neutral (physics of matter) - Each orbital needs an electron before a second is added

16. Orbital Diagrams!
Combine electron configurations & spin into one tidy package
Write the e- configuration of each:
1s1
1s2
1s22s1
1s22s22p3
1s22s22p4

17. Orbital Diagram Rules
1. Aufbau Principle: fill lowest orbitals first 2. Hund’s Rule: All up, before 1 down Ex: In p orbitals, put 1 electron per orbital until all of the orbitals contain electrons with parallel spins. 3. Pauli Exclusion Principle: only 2 electrons per orbital and in opposite directions

18. Practice With Me!
Fluorine
Neon

19. Practice Without Me!
Phosphorus
Sulfur

20. ClEvR Scientific Explanations– Three Parts
English Class
Chemistry Class
Claim-Thesis
Evidence-Quote from a book
Reasoning-An explanation as to why that quote supports your thesis
Claim- Statement answering the question
Evidence- Data, diagrams, or models
Reasoning- An explanation using theory, scientific “rules”, or definitions

21. Example- Explain why we no longer use the “plum pudding” model.
Claim- The “plum pudding” model is not longer used because it is not longer scientifically accurate.
Evidence- Rutherford performed the gold foil experiment observing that some, not all alpha particles bounced back when shot at a layer of gold foil. This proved that the atom was mostly empty space and that there was a dense center (nucleus) in an atom.
Reasoning- Since Rutherford provided evidence that disproved the “plum pudding” model, we not longer use it. Science is constantly providing new evidence that requires us to revise, edit, and create better models.

22. What ion would Aluminum form
What ion would Aluminum form? Explain using the octet rule and orbital diagrams.
Claim- An aluminum would form an ______ ion.
Evidence-
Al0
Al3+
Reasoning- Aluminum wants to have 8 electrons in its outer most energy level to satisfy the octet rule. It is easier for Aluminum to lose 3 electrons than to gain 5 electrons to having 8 electrons in the outer most energy level, because of it’s low ionization energy and electroneg.
Al3+
1s 2s p s p
1s 2s p s p

23. Exit Task
The abbreviated electron configuration of Silver is [Kr] 5s2, 4d9. Create an orbital diagram that illustrates this abbreviated configuration.