1. Honors Chemistry Chapter 3 and 4 Review “Electron Configuration”

2. Electron Configurations Rules and Principles Energy Levels, Sublevels, and Orbitals Famous Chemists 1 point 1 point 1 point 1 point 1 point 1 point 1 point 1 point 2 points 2 points 2 points 2 points 2 points 2 points 2 points 2 points 3 points 3 points 3 points 3 points 3 points 3 points 3 points 3 points 4 points 4 points 4 points 4 points 4 points 4 points 4 points 4 points 5 points 5 points 5 points 5 points 5 points 5 points 5 points 5 points

3. Sulfur 1 pointCheck

4. What is 1s 2 2s 2 2p 6 3s 2 3p 4 ? 1 point Back to Category Slide

5. The abbreviated electron configuration for I. 2 pointsCheck

6. What is [Kr] 5s 2 4d 10 5p 5 ? 2 points Back to Category Slide

7. Lutetium 3 pointsCheck

8. What is 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 1 ? 3 points Back to Category Slide

9. The abbreviated electron configuration for neon. 4 pointsCheck

10. What is [He] 2s 2 2p 6 ? 4 points Back to Category Slide

11. Copper 5 pointsCheck

12. 5 points Back to Category Slide What is 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 10 ? (yes this is right!!! Look in your book at Exceptions pg. 153)

13. Two electrons must spin in opposite directions. 1 pointCheck

14. What is the Pauli Exclusion Principle? 1 point Back to Category Slide

15. Electrons are assigned to the lowest energy levels first. 2 pointsCheck

16. What is the Aufbau Principle? 2 points Back to Category Slide

17. Electrons must be added to orbitals one at a time with parallel spin. 3 pointsCheck

18. What is Hund’s Rule? 3 points Back to Category Slide

19. The rule/principle that is broken… 4 pointsCheck 3d 6

20. What is the Pauli Exclusion Principle? 4 points Back to Category Slide

21. Draw the orbital notation for O. 5 pointsCheck 1s 2 2s 2 2p 4

22. 5 points Back to Category Slide 1s 2 2s 2 2p 4

23. The number of sublevels in the 3 rd energy level. 1 pointCheck

24. What is 3 (3s, 3p, 3d)? 1 point Back to Category Slide

25. The number of electrons that can be held in the 2 nd energy level. 2 pointsCheck

26. What is 8? 2 points Back to Category Slide

27. The shape of the “d” orbitals. (4 out of 5) 3 pointsCheck

28. 3 points Back to Category Slide What is a cloverleaf shape?

29. The model that uses energy levels, sublevels and orbitals. (Hint: Schrodinger) 4 pointsCheck

30. 4 points Back to Category Slide What is the Quantum Mechanical Model?

31. The number of orbitals found in the 4 th energy level. 5 pointsCheck

32. What is 16? 5 points Back to Category Slide

33. Chemist who had four basic postulates…1) elements are composed of atoms 2) atoms of the same element are identical 3) atom are neither created nor destroyed in a reaction 4) a given compound has the same numbers and kinds of atoms 1 pointCheck

34. Who was Dalton? 1 point Back to Category Slide

35. Energy levels or orbits. 2 pointsCheck

36. Who was Bohr? 2 points Back to Category Slide

37. Photoelectric Effect 3 pointsCheck

38. Who was Einstein? 3 points Back to Category Slide

39. Quantum or quanta 4 pointsCheck

40. Who was Planck? 4 points Back to Category Slide

41. Teacher of Bohr 5 pointsCheck

42. Who was Rutherford? 5 points Back to Category Slide