1. AP Chem Catalyst AP Chem Catalyst Catalyst Questions To Do & Homework Name the following compounds or write the formulas: ① CuSO 4 ② N 2 Cl 6 ③ Iron (II) Phosphate ④ Copper (III) Nitrate ⑤ Hydrochloric Acid Name the following compounds or write the formulas: ① CuSO 4 ② N 2 Cl 6 ③ Iron (II) Phosphate ④ Copper (III) Nitrate ⑤ Hydrochloric Acid HW: Outline this by tomorrow: http://electronconfiguration.info http://electronconfiguration.info Read up to the overlap of orbital sublevels. Lecture will make sense if you read this! Unit 1 and Unit 2 Test on Thurday! Lessons 1.1-1.7 Tutoring Friday (or form study groups Thursday) HW: Outline this by tomorrow: http://electronconfiguration.info http://electronconfiguration.info Read up to the overlap of orbital sublevels. Lecture will make sense if you read this! Unit 1 and Unit 2 Test on Thurday! Lessons 1.1-1.7 Tutoring Friday (or form study groups Thursday) You will have 6 tabs: (Use sticky notes if you don’t have dividers) 1.In Class Notes 3. Tests/Quizzes/Study Guides 5. Classwork 2.Outlines 4. Problem Sets 6. Homework (Place In Class Notes in Tab 1) You will have 6 tabs: (Use sticky notes if you don’t have dividers) 1.In Class Notes 3. Tests/Quizzes/Study Guides 5. Classwork 2.Outlines 4. Problem Sets 6. Homework (Place In Class Notes in Tab 1) Binder

2. Atomic Emission Spectra When a gaseous element is excited, a color is observed. The wavelengths being emitted can be detected A spectrum is not detected, only 4 specific wavelengths. So what?

3. Bohr’s Solution Since only specific wavelengths are seen, he concluded that electrons had specific energy levels! He proposed that electrons moved in circular orbitals around the nucleus (wrong) at certain “allowed” energy states (correct)

4. What does this mean? E λ

6. Shorter Formula, but be careful Consider a transition of the electron in the hydrogen atom from n = 4 to n = 9 as a photon is absorbed by the atom. What is the energy for this transition?

10. Save this for tomorrow!

11. Peer Feedback: Go over CELs for Einstein’s application of Max Planck’s hypothesis on quantized energy of photons. Peer Editing Provide Feedback Use the rubric to score. If you’d like to resubmit do so by tonight. CELs will be graded over the next few days. Pull them out on your ipad, swap ipad with elbow partner

12. AP Chem Catalyst AP Chem Catalyst Catalyst Questions To Do & Homework ① What did Schrodinger contribute to the structure of the atom? ② What did Rutherford’s Gold foil contribute to the structure of the atom? ③ What did Neils Bohr accurately contribute to the structure of the atom? ④ What did Einstein call packets (“quantized”) of energy? ① What did Schrodinger contribute to the structure of the atom? ② What did Rutherford’s Gold foil contribute to the structure of the atom? ③ What did Neils Bohr accurately contribute to the structure of the atom? ④ What did Einstein call packets (“quantized”) of energy? HW: Unit 1 and Unit 2 Test on Thurday! Lessons 1.1-1.7 Tutoring Friday (or form study groups Thursday) Quiz on 1.6-1.7 on Monday! HW: Unit 1 and Unit 2 Test on Thurday! Lessons 1.1-1.7 Tutoring Friday (or form study groups Thursday) Quiz on 1.6-1.7 on Monday! You will have 6 tabs: (Use sticky notes if you don’t have dividers) 1.In Class Notes 3. Tests/Quizzes/Study Guides 5. Classwork 2.Outlines 4. Problem Sets 6. Homework (Place In Class Notes in Tab 1) You will have 6 tabs: (Use sticky notes if you don’t have dividers) 1.In Class Notes 3. Tests/Quizzes/Study Guides 5. Classwork 2.Outlines 4. Problem Sets 6. Homework (Place In Class Notes in Tab 1) Binder

13. Lesson 1.7 Topics  Orbitals  Electron Configurations  Orbital diagrams  Condensed Noble Gas Configuration

14. Principal Quantum # Is “n” which is positive # from n=1, 2, 3….infinity. As n increases, the orbital gets larger. As n increase, the electron separates more from the nucleus. As n increases, the electron has a higher energy and less tightly bound to the nucleus What happens when n = ∞ ?

15. Those are your energy levels defined by “n” Orbital shape

20. Socrative (Check for Understanding)

21. Quickwrite Come up to the board and jot down your thoughts

22. Electron Configurations (EC) The way electrons are distributed among orbitals. The most stable EC is that in the ground state. Orbitals are filled in order of increasing energy with no more than two electrons per subshell. o S-orbitals have 1 subshell o P-orbitals have 3 subshells o d-orbitals have 5 subshells.

23. Electron Configurations We write a number showing, n (principal quant #) Then the orbital (s, p, d, f) Lastly a superscript showing the electrons in that orbital. ORBITAL DIAGRAMS We draw boxes representing subshell in that orbital. Upward arrow (electrons) in each subshell and then pair up with a downwards arrow ( Hund’s Rule )

25. Example 1: Electron Configuration and orbital diagram for Boron: You try: Beryllium

26. Example 2: Write electron configuration and orbital diagram for nitrogen You try: Neon

27. Think Pair Share Why do you think we don’t pair up electrons at first? Why must we place one electron in each subshell first and then pair up as stated by Hund’s Rule? Think about what you know about electrons?

28. What’s unusual about this? Beyond the scope of this class Assigning quantum #’s to e - s

29. Example 3: Write the electron configuration for silver (Ag) (Note: Ag = silver; Au = gold) You try: Write EC for gold (Au)

30. Condensed version Another way to write these in a shorter way is to use the noble gas configuration. Look at the element you’re writing the EC for, and look for the noble gas prior to that element on the periodic table. Start with that and then continue the orbital process. Example: Write both the EC and Noble Gas EC for Sulfur What if it were S -2 ? How would the EC above change?

31. You Try: Write the EC and Condensed Noble Gas form for: 1.Selenium EC: Condensed: 2. Barium EC: Condensed:

32. Placed among energy levels BROMINE’S ENERGY DIAGRAM

33. Done. Done.