3. Let’s Play Sit in teams of 4.

5. Periodic Table- History and Organization

6. Periodic Families

7. What is my size?

8. Giving up electrons

9. I love electrons!

10. Potpourri

11. 200 300 400 500 Periodic Table- History and Organization Periodic Families What is my size? Giving up electrons I love electrons! Potpourri 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100 200 300 400 500 100

12. $100 He is sometimes called the “father of the Periodic Table”

13. Mendeleev

14. $200 On the original periodic table, elements were organized by similar properties and this

15. Atomic mass (or weight)

16. $300 These are the two ways elements on the modern periodic table are organized

17. Similar properties and atomic number

18. $400 The names given to rows and columns on the periodic table

19. Periods (rows) and groups (columns)

20. $500 These elements tend to lose electrons and are found on the left side of the periodic table

21. Metals

22. $100 Lithium is a member of this family of highly reactive metals

23. Alkali metals

24. $200 Chlorine is a member of this family

25. Halogens

26. $300 Xenon is a member of this family

27. Noble Gases

28. $400 Atoms of elements in this family tend to lose two electrons

29. Alkaline Earth Metals

30. $500 Thorium is a member of this family

31. Actinide Family

32. $100 Which has a smaller ionic radius, cesium or potassium?

33. Potassium

34. $200 How does a neutral atom compare in size to its cation?

35. The neutral atom is larger; the cation is smaller

36. $300 Why is an anion larger than its neutral atom?

37. The anion has more electrons that repel each other and cause the electron cloud to expand

38. $400 What is the general trend for atomic radii as you move from left to right across a row on the periodic table and why?

39. Atomic radius decreases; increasing nuclear charge pulls electrons is closer

40. $500 What is the reason for the difference in size between a neutral atom and its cation?

41. The cation has lost (electrons) an entire energy level

42. $100 What is the general trend in ionization energy as you move down a group on the periodic table?

43. Ionization energy decreases

44. $200 What is the general trend in ionization energy as you move across a period from left to right?

45. IE increases

46. $300 What is the difference between first, second, and third ionization energies?

47. 1 st IE<2 nd IE<3 rd IE Or 1 st IE= energy to remove the first electron, 2 nd is to remove the second, etc.

48. $400 Why is the first ionization energy for sodium so much lower than the first ionization energy for magnesium?

49. Sodium has 1 valence electron in the 3s sublevel, and it wants to lose this electron. Magnesium has two electrons in the 3s sublevel so this sublevel is completely filled. It requires a lot more energy to remove an electron from a full sublevel.

50. Daily Double!

51. Daily Double! Why is the third ionization energy for beryllium significantly higher than its second ionization energy?

52. Beryllium has 2 valence electrons in a 2s subshell. Once it has lost two electrons (2 nd IE), it has lost an entire energy level and has a noble gas electron configuration. The 3 rd IE involves removing one of the core electrons from a stable noble gas configuration which requires significantly more energy. Also the protons have a much stronger pull on the remaining electrons.

53. $100 The measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound is called this.

54. Electronegativity

55. $200 Why does electronegativity increase as you move from left to right on the periodic table?

56. Effective nuclear charge increases and radius decreases, increasing the force/pull of the nucleus on electrons

57. $300 What is the name for the energy released when an electron is added to an atom?

58. Electron affinity

59. $400 What is the most electronegative element?

60. Fluorine

61. $500 Why are valence electrons of larger atoms less atttracted to the nucleus?

62. Shielding effect (more core electrons blocking their “view”) or greater distance = lower Coulombic force

63. $100 These are the most reactive metals

64. Alkali metals

65. $200 The outer shell electrons involved in bonding are called this.

66. Valence electrons

67. $300 Metals tend to ___________ electrons to become ___________

68. Lose, cations

69. $400 Put the following atoms in order from lowest to highest ionization energy (first IE) Ba, Cu, Ne

70. Ba<Cu<Ne

71. $500 Put the following atoms in order from smallest to the largest ionic radii. K, Mg, P

72. P<Mg<K

73. FinalJeopardy

74. Periodicity

75. The shielding effect is one of the three primary factors that affect the periodic trends. Name or describe the other two.

76. 1. Nuclear charge (number of protons in the nucleus) 2. Highest energy level (or number of energy levels)

77. Daily Double!