3. Regions

4. Scientists

5. Families

6. Vocab

7. Trends

8. Grab Bag

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10. Name 4 characteristics of metals.

11. Shiny, malleable, ductile, and conductive

12. What region of the periodic table do metals react with in order to become stable?

13. The nonmetals

14. Walk up to the periodic table and point out ALL the metals.

16. Potassium has properties most similar to calcium, argon, or rubidium

17. Rubidium because elements are most similar to those in the same group.

18. Write a noble gas configuration for a d-block element of your choice

19. Use a noble gas in brackets, then read the next line on the periodic table until you get to the element.

20. Name the 3 scientists who contributed to the periodic table, in order.

21. Newlands, Mendeleev, and Moseley

22. Who arranged the periodic table by atomic number?

23. Henry Moseley

24. Who was the first scientist to arrange the periodic table by properties and the Law of Octaves?

25. John Newlands

26. Whose contribution was significant because he had better technology available to him?

27. Henry Moseley

28. Who left gaps in the periodic table and predicted properties of elements?

29. Dmitri Mendeleev

30. Walk up & point to the families on the periodic table in order from left to right & top to bottom.

31. alkali metals, alkali-earth, transitions, halogens, noble gases, lanthanides, actinides

32. Which family is slightly harder, denser and less reactive than the alkali metals?

33. Alkaline earth metals

34. Which group has a small peak on an ionization energy graph due to a half full orbital?

35. Group 15

36. Which 2 families are the most reactive?

37. Alkali metals and halogens

38. Which family has 7 valence electrons? Give a noble gas configuration of any one of them to demonstrate.

39. halogens

40. Define Octet Rule.

41. The tendency of atoms to gain or lose electrons in order to become stable (refers mainly to filling the s and p orbitals.

42. Define ionization energy.

43. The energy required to remove an electron.

44. Define electron affinity.

45. The amount of energy released when an atom gains an electron.

46. Define nuclear charge.

47. The charge/strength of the protons in the nucleus.

48. Shielding effect

49. The reduction in attraction between the valence e and the nucleus due to the interference of the core e

50. Where on the periodic table is ionization energy the greatest?

51. Top right.

52. Which trend increases down a group but has no change across a period?

53. The shielding effect. (electron shielding)

54. Explain why atomic radius decreases across a period.

55. The nuclear charge increases, and electrons are added to the same energy level, so the attraction is greater.

56. Why does electron shielding increase down a group?

57. Core electrons are added and the valence electrons are further from the nucleus.

59. Which atom has a lower ionization energy: silver (Ag), arsenic (As), or strontium (Sr)? Explain your answer.

60. Strontium, b/c it has more e - shielding than arsenic, and a greater desire to lose an e - than silver because it wants to acquire a noble gas config.

61. Which family tends to have a +2 charge?

62. Alkaline-Earth Metals

63. Why does group 16 have a -2 charge?

64. Group 16 wants to gain 2 e - to fill it’s octet.

65. Draw arrows on the board to represent the increase in the trend of atomic radii.

66. Should look like 9:30 on a clock higher on the right and higher at the bottom

67. Which family has the most negative electron affinity values?

68. halogens

69. Although Xenon is a noble gas, it has reacted with other nonmetals. He, Ne, and Ar have not. How is this possible?

70. Because it is so far down the group, electron shielding has permitted highly electronegative atoms to take a valence electron.

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