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5. Orbitals & electrons Misc.Calculations 10 Point 20 Points 30 Points 40 Points 50 Points 10 Point 20 Points 30 Points 40 Points 50 Points 30 Points 40 Points 50 Points Electron Configuration Scientists

6. Created the “planetary” model of the atom

7. Bohr

8. Told us that you cannot know, with any degree of certainty, both the location of an electron as well as its velocity at any given instant.

9. Heisenberg

10. Developed an equation that allows us to predict the energy either admitted or absorbed by an electron if we know the final and initial energy levels for the electron’s jump.

11. Rydberg

12. Assumed that energy can either be absorbed or released by atoms in discrete “chunks” which he called quantums

13. Planck

14. Developed a wave equation which allows us to predict the likelihood (probability) of finding an electron in a general region of space around the nucleus

15. Schrodinger

16. How many orbitals are required in each subshell- s? p? d? f?

17. s-1, p-3, d-5, f-7

18. What family has an electron configuration that ends with s 2 ?

19. Alkaline earth metals

20. Describe the shape of the 5 th d orbital (the one that no one likes to talk about)

21. 2 lobes and a donut

22. How many electrons can each energy level hold in total? n=1? n=2? n=3? n=4?

23. n=1 – 2 e- n=2 – 8e- n=3 – 18 e- n=4 – 32 e-

24. What is the vocab word used to describe orbitals of equal energy?

25. Degenerate

26. Give the standard configuration for sulfur.

27. 1s 2 2s 2 2p 6 3s 2 3p 4

28. Give the Noble gas configuration for antimony

29. [Kr]5s 2 4d 10 5p 3

30. Draw an orbital diagram for strontium

31. See board

32. Give the Noble gas configuration for tungsten

33. [Xe]6s 1 4f 14 5d 5

34. Write the standard configuration for uranium

35. 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 4

36. Color in the visible spectrum with the shortest wavelength

37. violet

38. Type of electromagnetic radiation with waves the length of a football field

39. Radio waves

40. Relationship between frequency and wavelength

41. inverse or indirect

42. The transition below with the lowest energy photon EMISSION n= 1  n = 6 n = 6  n = 3 n = 1  n = 4 n = 6  n = 2

43. n = 6  n = 3

44. The name for the phenomena that says every metal has a minimum frequency of light below which no electrons are emitted, and that the intensity of this light is not a crucial factor

45. Photoelectric effect

46. Convert 588 nm to meters.

47. 5.88x10 -7 m

48. Your favorite radio station broadcasts at a frequency of 1.15x10 6 Hz or s -1. What is this wavelength in centimeters?

49. 26,087 cm

50. Calculate the frequency of a photon with an energy of 1.66x10 -17 J.

51. 2.5x10 16 s -1 or Hz

52. Calculate the change in energy when an electron jumps from n=4 to n=1 in a hydrogen atom.

53. -2.04x10 -18 J

54. Calculate the wavelength of a photon absorbed in a hydrogen atom when an electron jumps from n=3 to n=6.

55. 1.09x10 -6 m

56. Make your wager

57. Draw an orbital diagram, and fill in the position of the electron with the following quantum numbers n = 3, l = 2, m l = -1, m s = +1/2

58. 3d __ ↑_ __ __ __