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5. 100 200 300 400 500 Vocabulary Electron Configurati on Periodic Trends The Periodic Table Electroma gnetic Radiation Isoelectric ions and miscellane ous

6. Wavelength, frequency A 100

7. Distance between two wave peaks The number of waves that pass a given point per unit of time A 100

8. Photon, excited state A 200

9. Tiny packet of energy Contains an electron with excess energy A 200

10. Ground state, orbital A 300

11. Lowest possible energy state for an atom Region where an electron resides in an atom A 300

12. Pauli Exclusion Principle, Valence electrons A 400

13. An atomic orbital can hold no more than two electrons, and they must be of opposite spin Electrons in outermost (highest) occupied principal energy level A 400

14. Core electrons, Ionization energy A 500

15. Inner electrons of an atom Energy required to remove an electron from an atom in the gas phase A 500

16. Write the electron configuration for Al B 100

17. 1s 2 2s 2 2p 6 3s 2 3p 1 B 100

18. Write the electron configuration for Ge B 200

19. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 2 B 200

20. Br, Bromine B 300

21. [Ar]4s 2 3d 10 4p 5 B 300

22. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 B 400

23. Fe, Iron B 400

24. Write the electron configuration for astatine B 500

25. [Xe] 6s 2 4f 14 5d 10 6p 5 B 500

26. Which of the following is the smallest atom? K, Ge, Si, O C 100

27. Oxygen, O C 100

28. Which of the following has the highest ionization energy? K, Ge, Si, O C 200

29. O

30. Which neutral atom has six 3d electrons? Fe, Co, Ru, Rh C 300

31. Fe C 300

32. Which one of the following elements has five valence electrons? B, C, N, F C 400

33. N

34. Use atomic structure to explain the trends of atomic size C 500

35. Atoms get bigger going down the periodic table and smaller going across the periodic table (across to the right). As you go down the periodic table the energy level increases, increasing the distance from the nucleus. Across the p.t., the energy level stays the same but the larger charge attracts the electrons making the distance smaller from the nucleus. C 500

36. What group are the alkali metals? D 100

37. Group 1 D 100

38. Where are the alkaline earth metals? D 200

39. Group 2 D 200

40. Where are the transition metal? D 300

41. Middle block on the periodic table; groups 3-12 D 300

42. Where are the halogens? D 400

43. Group 7 or 17 D 400

44. Where are the noble gases? D 500

45. Group 8 or 18 D 500

46. What would be the amount of energy contained by a photon whose frequency is 2.17 x 10 19 Hz? E 100

47. 1.44 x 10 -14 J E 100

48. What would be the wavelength of electromagnetic radiation (X- ray) if its frequency is 2.5 x 10 18 Hz? E 200

49. 1.2 x 10 -10 m E 200

50. What would be the energy of an FM radio signal if the wavelength is 1.5 m? E 300

51. 1.33 x 10 -25 J E 300

52. As the wavelength of light increases, its frequency and energy do what? E 400

53. decrease E 400

54. What are the units of energy, frequency, wavelength and speed of light, respectively? E 500

55. J·s; Hz or s -1 ; m; m/s E 500

56. SOPHOMORES ONLY-What would be the electron configuration for the calcium ion, Ca +2 F 100

57. 1s 2 2s 2 2p 6 3s 2 3p 6 F 100

58. What is the maximum number of electrons that can be in the third principal energy level? F 200

59. 18 F 200

60. When an electron in an atom absorbs energy, it does what? F 300

61. Moves to a higher energy level F 300

62. In a hydrogen atom, an electron undergoing which of the following transitions would emit light of the shortest wavelength? from n=5 to n=1 From n=5 to n=2 From n=4 to n=1 From n=1 to n=5 F 400

63. From n=5 to n=1 Emitting energy means going from a higher energy level to lower energy level; shortest wavelength corresponds to highest energy change F 400

64. The 4 th energy level contains how many orbitals? F 500

65. 4 or 16; 4 if you are talking s, p, d and f; 16 if you are thinking how many pairs of electrons total F 500

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