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

Warm-Up Write the complete and abbreviated electron configurations for Manganese (#25). How many electrons are in each energy level? 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 5 [Ar] 4s 2 3d 5 Energy Level 1-2 electrons Energy Level 2-8 electrons Energy Level 3-13 electrons Energy Level 4-2 electrons

Review Homework! 1.With your partner take turns answering each others questions. 2.Explain how YOU solved each type of problem. 3.Find out what questions still remain for you and your partner 4.Call over Ms. Bryce for help

Learning Targets

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______________________________________________

Answers 1)Sodium1s 2 2s 2 2p 6 3s 1 2)Iron 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 3)Bromine 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 4)Barium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 5)Neptunium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 5

MORE! In the space below, write the abbreviated electron configurations of the following elements: 6)cobalt________________________________________________ 7)silver________________________________________________ 8)tellurium________________________________________________ 9)radium________________________________________________ 10)lawrencium________________________________________________

Answers 6)cobalt[Ar] 4s 2 3d 7 7)silver[Kr] 5s 2 4d 9 8)tellurium[Kr] 5s 2 4d 10 5p 4 9)radium[Rn] 7s 2 10)lawrencium[Rn] 7s 2 5f 14 6d 1

More Determine what elements are denoted by the following electron configurations: 11) 1s 2 2s 2 2p 6 3s 2 3p 4 ____________________ 12) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 ____________________ 13) [Kr] 5s 2 4d 10 5p 3 ____________________ 14) [Xe] 6s 2 4f 14 5d 6 ____________________ 15) [Rn] 7s 2 5f 11 ____________________

Answers 11) 1s 2 2s 2 2p 6 3s 2 3p 4 sulfur 12) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 1 rubidium 13) [Kr] 5s 2 4d 10 5p 3 antimony 14) [Xe] 6s 2 4f 14 5d 6 osmium 15) [Rn] 7s 2 5f 11 einsteinium

MORE! Determine which of the following electron configurations are not valid: 16) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 10 4p 5 ____________________ 17) 1s 2 2s 2 2p 6 3s 3 3d 5 ____________________ 18) [Ra] 7s 2 5f 8 ____________________ 19) [Kr] 5s 2 4d 10 5p 5 ____________________ 20) [Xe] ____________________

Answers! 16) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d 10 4p 5 not valid (take a look at “4d”) 17) 1s 2 2s 2 2p 6 3s 3 3d 5 not valid (3p comes after 3s) 18) [Ra] 7s 2 5f 8 not valid (radium isn’t a noble gas) 19) [Kr] 5s 2 4d 10 5p 5 valid 20) [Xe] not valid (an element can’t be its own electron configuration)

Orbital Diagram Notes

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

Orbital Diagrams! Combine electron configurations & spin into one tidy package Write the e - configuration of each: 1s 1 1s 2 1s 2 2s 1 1s 2 2s 2 2p 3 1s 2 2s 2 2p 4

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

Practice With Me! Fluorine Neon

Practice Without Me! Phosphorus Sulfur

ClEvR Scientific Explanations– Three Parts English ClassChemistry Class 1.Claim-Thesis 2.Evidence-Quote from a book 3.Reasoning-An explanation as to why that quote supports your thesis 1.Claim- Statement answering the question 2.Evidence- Data, diagrams, or models 3.Reasoning- An explanation using theory, scientific “rules”, or definitions

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.

Claim- An aluminum would form an ______ ion. Evidence- Al 0 Al 3+ 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. What ion would Aluminum form? Explain using the octet rule and orbital diagrams. Al 3+ 1s 2s 2p 3s 3p

Exit Task The abbreviated electron configuration of Silver is [Kr] 5s 2, 4d 9. Create an orbital diagram that illustrates this abbreviated configuration.