1. Test Review – Periodic Table Unit 2 Section A

2. Use your periodic table to enter the symbol of the element for each of the following questions.

4. The name given to all the elements on the left side of the periodic table which have from 1 to 3 valence electrons, conduct electricity and heat, are malleable and ductile.

5. Metals

7. The name given to all the elements on the right side of the periodic table which have from 5 to 7 valence electrons, do not conduct electricity or heat, and are brittle in texture.

8. Nonmetals

9. The name given to all the elements on the border of metals and nonmetals which are not malleable or ductile, and sometimes can conduct electricity (semiconductors)

10. Metalloids

11. The vertical columns of the periodic table. These groups share common characteristics and are placed in these columns by their number of valence electrons.

12. Families (groups)

13. The horizontal rows of the periodic table. These tell the number of electron shells or energy levels for each element.

14. Periods

15. The name given to the electrons found in the outside shell of each atom.

16. Valence electrons

17. These are the group IA elements with 1 valence electron in their outside shell.

18. Alkali metals

19. These are the group IIA elements with 2 valence electrons in their outside shell.

20. Alkali Earth Metals

21. These are the group VII A elements with 7 valence electrons in their outside shell.

22. Halogens

23. These are the group VIII A or group 0 elements with 8 valence electrons in their outside shell. They have filled outside shells and are inert.

24. Noble Gases

25. These are the Group B metals. They are not very reactive and their valence electrons can change from 1 to 3. They resist corrosion and are used for coins and jewelry.

26. Transition metals

27. These groups include large elements which are sometimes radioactive and some are synthetically made.

28. Rare earth metals

29. The family of most reactive metals.

30. Alkali metals

31. The family of most reactive nonmetals

32. Halogens

33. The family of least reactive elements all of which are gases.

34. Noble gases

35. Examples of this family include Be, Mg, and Ca.

36. Alkali earth metals

37. Examples of this family include Cl, Br, F, and I

38. Halogens

39. Examples of this family include Cu, Ag, Au, Fe, and Zn.

40. Transition metals

41. Examples of this family include He, Ne, Ar, and Kr.

42. Noble gases

43. Examples of this family include Li, Na, and K

44. Alkali metals

45. Examples of this family include Uranium, Plutonium, and Curium.

46. Rare earth metals

47. Examples of this family include B, Si, As, and Ge,

48. Metalloids

49. Name the halogen in period 4.

52. Br

53. Name the alkali metal in period 2.

56. Li

57. Name an element with properties similar to Neon.

60. He, Ar, Kr, Xe, or Rn

61. Which element has 8 protons?

64. O

65. Which element has 20 electrons?

68. Ca

69. Which element has 24 neutrons?

71. 44.956 = 45 45 – 21 = 24

72. Sc - Scandium 44.956 = 45 45 – 21 = 24

73. Which element has an atomic mass (weight) closest to 56?

76. Fe

77. Name the alkaline earth metal in period 3.

80. Mg

81. Which period 3 element is the most reactive metal?

84. Na

85. Which period 2 element is the most reactive nonmetal?

88. F

89. Which element has 2 more protons than Iron?

91. Iron = Fe = 26 26 + 2 = 28

92. Ni Iron = Fe = 26 26 + 2 = 28

93. What is the least reactive period 4 element?

96. Kr

97. Which two elements are in the same family and have properties most similar to Zinc?

100. Cd and Hg

101. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Alkali Metals: 1) 2) 3) 4)

102. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Alkali Metals: 1)1 2) IA 3)Most reactive metals; combine with Halogens 4)Na, K 5)Outer e- config: *s 1

103. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Alkali Earth Metals: 1) 2) 3) 4)

104. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Alkali Earth Metals: 1)2 2) IIA 3)+2 charge 4)Ca, Mg 5)Outer e- config: *s 2

105. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Transition Metals: 1) 2) 3) 4)

106. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Transition Metals: 1)1-3 2)Group B 3)Valence varies, resist corrosion 4)Cu, Ag, Au, Zn, Fe 5)Sublevel orbital block = d

107. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Rare Earth Metals: 1) 2) 3) 4)

108. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Rare Earth Metals: 1)1-3 2)Group B 3)Large, synthetic, radioactive 4)U, La, Ac 5)Sublevel orbital block = f

109. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Metalloids: 1) 2) 3) 4)

110. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Metalloids: 1)3-7 2) IIIA-VIIA 3)Semi-metals, Semiconductors 4)Si, B, As 5)Outer e- config: *s 2 *p 1 - *s 2 *p 5

111. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Halogens: 1) 2) 3) 4)

112. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Halogens: 1) 7 2) VIIA 3)Most reactive nonmetals 4)Cl, Br 5)Outer e- config: *s 2 *p 5

113. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Noble Gases: 1) 2) 3) 4)

114. For each of the following Groups (Families) state; 1) The # of valence e-, 2) The Group #, 3) Defining characteristics, 4) Example Noble Gases : 1)8 2) VIIIA or 0 3)Inert, least reactive 4)Ne, Kr 5)Outer e- config: *s 2 *p 6

115. Explain how the sizes of atomic radii change as you travel down and across the periodic table:

116. Sizes increase going down table Sizes decrease going left to right

117. Size increases going down table Size decreases going left to right Largest Smallest

118. Place these elements in order of increasing atomic radii size: P, Cl, Fr, Mg, K =

119. Place these elements in order of increasing atomic radii size: P, Cl, Fr, Mg, K = Cl, P, Mg, K, Fr

120. Explain how the electronegativity of atom change as you travel down and across the periodic table:

121. Electronegativity decreases going down table Electronegativity increases going left to right

122. Electronegativity decreases going down table Electronegativity increases going left to right Lowest Highest

123. Place these elements in order of decreasing electronegativity: Ca, Br, As, Cl, Rb =

124. Place these elements in order of decreasing electronegativity: Ca, Br, As, Cl, Rb = Cl, Br, As, Ca, Rb

125. Which two Groups (families) are most reactive and why?

126. 1) Alkali metals – Group 1A – only 1 valence electron 2) Halogens – Group VII A – 7 valence electrons

127. What is the main property of noble gases and why?

128. Inert – Don’t react 8 valence electrons (octet) in outside shell, filled outer shells.

129. Why do all elements in a group (or family) have similar properties?

130. Same number of outside or valence electrons, so same reactivity.