The Periodic Table. 4. Plutonium was not discovered until 1940 (see Figure 3.7).
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1 CHAPTER The Periodic Table 5 Section 5.1 Classification of Elements 2. Krypton was not discovered until 1898 (see Figure 3.7). 4. Plutonium was not discovered until 1940 (see Figure 3.7). Section 5.2 The Periodic Law Concept 6. After Moseley s discovery in 1913, the periodic law states that physical and chemical properties tend to repeat periodically when elements are arranged according to increasing atomic number. 8. Note that Te precedes I in the periodic table, even though the atomic mass of Te (127.60) is greater than I (126.90). Section 5.3 Groups and Periods of Elements 10. Horizontal rows in the periodic table are referred to as periods or series. 12. The term for the elements that belong to Groups 3 12 is the transition elements. 14. The elements in the series that follow element 89 are called the actinides. 16. The elements Sc, Y, and La are rare earth elements, but not lanthanides. 18. The elements on the right side of the periodic table are nonmetals. 20. The appearance of B, Si, Ge, As, Sb, and Te resembles that of metals, and these nonradioactive elements are referred to as semimetals, or metalloids Pearson Education, Inc. The Periodic Table 27
2 22. Family Group Number (a) boron group IIIA/13 (b) oxygen group VIA/16 (c) nickel group VIII/10 (d) copper group IB/ IUPAC American IUPAC American (a) Group 2 IIA (b) Group 4 IVB (c) Group 6 VIB (d) Group 8 VIII (e) Group 11 IB (f) Group 12 IIB (g) Group 16 VIA (h) Group 18 VIIIA 26. Element Element (a) Ge (b) Na (c) I (d) Pm 28. Element Element (a) Se (b) Pt (c) Sc (d) Rn Section 5.4 Periodic Trends 30. Proceeding up a group in the periodic table, the metallic character of an element generally decreases. 32. Proceeding up a group of elements in the periodic table, the metallic character of an element generally decreases. 34. Metallic Character Metallic Character (a) K > Ca (b) Mg > Al (c) Fe > Cu (d) S > Ar (Note: The element with the greater metallic character is in bold.) 36. Atomic Radius Atomic Radius (a) Rb > Sr (b) As > Se (c) Pb > Bi (d) I > Xe (Note: The element with the larger atomic radius is in bold.) 28 Chapter Pearson Education, Inc.
3 Section 5.5 Properties of Elements 38. Predicted melting point of Cr: 2617 C (3410 C 2617 C) = 1824 C Predicted atomic radius of Mo: nm nm 2 = nm Predicted density of W: g/ml + (10.28 g/ml 7.14 g/ml) = g/ml 40. Predicted boiling point of Ar: 152 C + [ 152 C ( 107 C)] = 197 C Predicted atomic radius of Kr: nm nm 2 = nm Predicted density of Xe: 3.74 g/l + (3.74 g/l 1.78 g/l) = 5.70 g/l 42. Compound Formula Compound Formula (a) lithium oxide Li 2 O (b) barium oxide BaO (c) gallium oxide Ga 2 O 3 (d) tin oxide SnO Compound Formula Compound Formula (a) cadmium oxide CdO (b) cadmium sulfide CdS (c) cadmium selenide CdSe (d) cadmium telluride CdTe 46. Compound Formulas Compound Formulas (a) arsenic sulfide As 2 S 3 (b) antimony sulfide Sb 2 S 3 and As 2 S 5 and Sb 2 S 5 Section 5.6 Blocks of Elements 48. The elements in Groups IIIA/3 through VIIIA/18 are filling p sublevels. 50. The inner transition elements are filling f sublevels. 52. The elements in the actinide series are filling a 5f sublevel. 54. Element Highest Sublevel Element Highest Sublevel (a) He 1s (b) K 4s (c) U 5f (d) Pd 4d (e) Be 2s (f) Co 3d (g) Si 3p (h) Pt 5d 2014 Pearson Education, Inc. The Periodic Table 29
4 56. Element Electron Configuration Core Notation (a) B 1s 2 2s 2 2p 1 [He] 2s 2 2p 1 (b) Ti 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2 [Ar] 4s 2 3d 2 (c) Na 1s 2 2s 2 2p 6 3s 1 [Ne] 3s 1 (d) O 1s 2 2s 2 2p 4 [He] 2s 2 2p 4 (e) Ge 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 2 [Ar] 4s 2 3d 10 4p 2 (f) Ba 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 [Xe] 6s 2 5p 6 6s 2 (g) Pd 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 8 [Kr] 5s 2 4d 8 (h) Kr 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 [Ar] 4s 2 3d 10 4p 6 Section 5.7 Valence Electrons 58. Group Valence Electrons Group Valence Electrons (a) IIA/2 2 (b) IVA/14 4 (c) VIA/16 6 (d) VIIIA/ Element Valence Electrons Element Valence Electrons (a) He 2 (b) Pb 4 (c) Se 6 (d) Ne 8 (e) Cs 1 (f) Ga 3 (g) Sb 5 (h) Br 7 Section 5.8 Electron Dot Formulas 62. Element Electron Dot Formula Element Electron Dot Formula (a) He He (b) Pb Pb (c) Se Se (d) Ne Ne (e) Cs Cs (f) Ga Ga (g) Sb Sb (h) Br Br Section 5.9 Ionization Energy 64. Proceeding from left to right in the periodic table, the ionization energy increases. 66. The Group VIIIA/18 elements have the highest ionization energy. 30 Chapter Pearson Education, Inc.
5 68. Ionization Energy Ionization Energy (a) Ga < Ge (b) Si < P (c) Br < Cl (d) As > Sb (Note: The element with the higher ionization energy is in bold.) 70. Ionization Energy Ionization Energy (a) Mg < Si (b) Pb < Bi (c) Ca < Ga (d) P < Cl (Note: The element with the lower ionization energy is in bold.) Section 5.10 Ionic Charges 72. Group Ionic Charge Group Ionic Charge (a) IVA/14 4 (b) VA/15 3 (c) VIA/16 2 (d) VIIA/ Ion Ionic Charge Ion Ionic Charge (a) Be ion 2+ (b) Sn ion 4+ (c) P ion 3 (d) S ion Ion Isoelectronic Ion Isoelectronic (a) K + Ar (b) Sr 2+ Kr (c) Cl Ar (d) Se 2 Kr 78. Ion Electron Configuration Core Notation (a) Ti 2+ [Ar] 3d 2 (b) Zn 2+ [Ar] 3d 10 (c) Y 3+ [Kr] (d) Cs + [Xe] 80. Ion Electron Configuration Core Notation (a) Br [Ar] 4s 2 3d 10 4p 6, or [Kr] (b) Te 2 [Kr] 5s 2 4d 10 5p 6, or [Xe] (c) As 3 [Ar] 4s 2 3d 10 4p 6, or [Kr] (d) O 2 [He] 2s 2 2p 6, or [Ne] 2014 Pearson Education, Inc. The Periodic Table 31
6 General Exercises 82. European IUPAC European IUPAC (a) Group IIA Group 2 (b) Group IIB Group 12 (c) Group IVA Group 14 (d) Group IVB Group Predicted atomic radius of Ra: nm + ( ) nm = nm Predicted density of Ra: 3.65 g/ml + ( ) g/ml = 4.67 g/ml Predicted melting point of Ra: 725 C ( ) C = 681 C 86. Element Electron Configuration (a) W [Xe] 6s 2 4f 14 5d 4 (b) Bi [Xe] 6s 2 4f 14 5d 10 6p 3 (c) Ra [Rn] 7s 2 (d) Ac [Rn] 7s 2 6d Ionic Charges of Hydrogen Ions H + Hydrogen loses an electron similar to the Group IA/1 elements. H Hydrogen gains an electron similar to the Group VIIA/17 elements. Challenge Exercises 90. Mendeleev predicted the element gallium (Ga), which was not discovered until Magnesium has two valence electrons in a filled s sublevel. Aluminum has one electron in an unfilled p sublevel. The ionization energy for aluminum is less than that of magnesium because of the single electron in a p sublevel. Online Exercises 94. Element 104 was named rutherfordium (Rf) for an English physicist. 96. Soluble compounds containing barium are poisonous to humans. Barium sulfate is highly insoluble, thus elemental barium is not free to enter the blood. 32 Chapter Pearson Education, Inc.
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