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Chapter 3: Electronic Structure and the Periodic Law

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Chapter 3: Electronic Structure and the Periodic Law Chapter 3: Electronic Structure and the Periodic Law CHAPTER OUTLINE 3.1 The Periodic Law and Table 3.4 Electronic Configurations 3.2 Electronic Arrangements in Atoms 3.5 Another Look at the Periodic Table 3.3 The Shell Model and Chemical Properties 3.6 Property Trends within the Periodic Table LEARNING OBJECTIVES/ASSESSMENT When you have completed your study of this chapter, you should be able to: 1. Locate elements in the periodic table on the basis of group and period designations. (Section 3.1; Exercise 3.4) 2. Determine the number of electrons in designated atomic orbitals, subshells, or shells. (Section 3.2; Exercise 3.12) 3. Determine the number of valence shell electrons and the electronic structure for atoms, and relate this information to the location of elements in the periodic table. (Section 3.3; Exercises 3.18 and 3.22) 4. Determine the following for elements: the electronic configuration of atoms, the number of unpaired electrons in atoms, and the identity of atoms based on provided electronic configurations. (Section 3.4; Exercises 3.24 and 3.28) 5. Determine the shell and subshell locations of the distinguishing electrons in elements, and based on their location in the periodic table, classify elements into the categories given in Figures 3.10 (representative element, transition element, inner‐transition element, noble gas) and 3.12. (metal, metalloid, nonmetal). (Section 3.5; Exercises 3.34 and 3.36) 6. Recognize property trends of elements within the periodic table, and use the trends to predict selected properties of the elements. (Section 3.6; Exercises 3.40 and 3.42) LECTURE HINTS AND SUGGESTIONS 1. Extend the concept of chemical change and chemical properties to the atomic level. Chemical changes cause a change in the constituent particles. The atoms are rearranged to make different constituent particles. This rearrangement involves the electrons of the atoms. Thus, atoms with similar chemical properties must have similar electronic arrangements. 2. Relate the arrangement of the periodic table with groups and periods to the electronic structure of the atom, and the filling order of the orbitals. This facilitates the understanding of the ʺouter electronsʺ determining the chemical combinations. 3. Avoid bringing in any detailed discussion about nuclear changes (covered in Chapter 10) into this chapter. Mention that isotopes are either stable or radioactive (unstable) as well as the facts that only nuclear reactions involve nuclear changes and that all other chemical reactions involve electrons, but defer any further discussion of radioactivity until the later chapter. 4. If samples of some of the elements are available, showing them may benefit the discussion of the periodic table as it relates to metals, non‐metals, similarity within groups, etc. SOLUTIONS FOR THE END OF CHAPTER EXERCISES THE PERIODIC LAW AND TABLE (SECTION 3.1) 3.1 Group Period a. Ca II A (2) 4 b. element number 22 IV B (4) 4 53 54 Chapter 3 Group Period c. nickel VIII B (10) 4 d. tin IV A (14) 5 3.2 Group Period a. element number 27 VIII B (9) 4 b. Pb IV A (14) 6 c. arsenic V A (15) 4 d. Ba II A (2) 6 3.3 Symbol Name a. Belongs to group VIA(16) and period 3 S sulfur b. The first element (reading down) in group VIB(6) Cr chromium c. The fourth element (reading left to right) in period 3 Si silicon d. Belongs to group IB(11) and period 5 Ag silver ;3.4 Symbol Name a. The noble gas belonging to period 4 Kr krypton b. The fourth element (reading down) in group IV A (14) Sn tin c. Belongs to group VI B (6) and period 5 Mo molybdenum d. The sixth element (reading left to right) in period 6 Nd neodymium 3.5 a. How many elements are located in group VIIIB(8,9,10) of the periodic table? 12 b. How many elements are found in period 2 of the periodic table? 8 c. How many total elements are in group IIA(2) and VIA(16) of the periodic 11 table? 3.6 a. How many elements are located in group VII A (17) of the periodic table? 5 b. How many total elements are found in periods 2 and 3 of the periodic table? 16 c. How many elements are found in period 6 of the periodic table? 32 3.7 a. This is a vertical arrangement of elements in the periodic table group b. The chemical properties of the elements repeat in a regular way as periodic law the atomic numbers increase c. The chemical properties of elements 11, 19, and 37 demonstrate this periodic law principle d. Elements 4 and 12 belong to this arrangement group 3.8 a. This is a horizontal arrangement of elements in the periodic table. period b. Element 11 begins this arrangement in the periodic table. period c. The element nitrogen is the first member of this arrangement. group d. Elements 9, 17, 35, and 53 belong to this arrangement. group ELECTRONIC ARRANGEMENTS IN ATOMS (SECTION 3.2) 3.9 According to Bohr theory, an electron in an orbit located farther from the nucleus would have higher energy than an electron in an orbit close to the nucleus. 3.10 Protons are subatomic particles with a positive charge that are located in the nucleus. Electronic Structure and the Periodic Law 55 3.11 a. A 2s orbital 2 electrons b. A 2s subshell 2 electrons c. The first shell 2 electrons ;3.12 a. A 2p orbital 2 electrons b. A 2p subshell 6 electrons c. The second shell 8 electrons 3.13 Nine (9) orbitals are found in the third shell: one 3s orbital, three 3p orbitals, and five 3d orbitals. 3.14 Sixteen (16) orbitals are found in the second shell: one 4s orbital, three 4p orbitals, five 4d orbitals, and seven 4f orbitals. 3.15 Five (5) orbitals are found in the 3d subshell. The maximum number of electrons that can be located in this subshell is 10 because each of the five orbitals can hold two electrons. 3.16 Seven (7) orbitals are found in a 4f subshell. The maximum number of electrons that can be located in this subshell is 14 because each of the seven orbitals can hold two electrons. 3.17 The subshells in the fourth shell are 4s, 4p, 4d, 4f. The maximum number of electrons in each subshell are 2 (4s), 6 (4p), 10 (4d), and 14 (4f). The total number of electrons that can occupy the fourth shell is 32. THE SHELL MODEL AND CHEMICAL PROPERTIES (SECTION 3.3) ;3.18 a. element number 54 8 electrons b. The first element (reading down) in group V A (15) 5 electrons c. Sn 4 electrons d. The fourth element (reading left to right) in period 3 4 electrons 3.19 a. element number 35 7 electrons b. Zn 2 electrons c. strontium 2 electrons d. The second element in group VA(15) 5 electrons 3.20 Cesium is the period 6 element with chemical properties most like sodium. Cesium has 1 valence‐shell electron. Sodium also has only 1 valence‐shell electron. 3.21 The period 5 element with chemical properties most like silicon is tin (Sn). Tin has four valence‐shell electrons. Silicon also has four valence‐shell electrons. ;3.22 I would expect to find silver and gold in addition to the copper because these elements are all in the same group on the periodic table. Elements that are in the same group have similar chemical properties; therefore, if copper is part of this ore, then the other elements that are most similar to it are also likely to be part of the ore. 3.23 Strontium would be likely to be deposited in bones because it is in group IIA(2), just like calcium (a major component of bone). 56 Chapter 3 ELECTRONIC CONFIGURATIONS (SECTION 3.4) ;3.24 Electron Configuration Unpaired Electrons a. element number 37 1s22s22p63s23p64s23d104p65s1 1 b. Si 1s22s22p63s23p2 2 Electron Configuration Unpaired Electrons c. titanium 1s22s22p63s23p64s23d2 2 d. Ar 1s22s22p63s23p6 0 3.25 Electron Configuration Unpaired Electrons a. Br 1s22s22p63s23p64s23d104p5 1 b. element number 36 1s22s22p63s23p64s23d104p6 0 c. cadmium 1s22s22p63s23p64s23d104p65s24d10 0 d. Sb 1s22s22p63s23p64s23d104p65s24d105p3 3 3.26 Electron Configuration Solutions a. s electrons in magnesium 1s22s22p63s2 6 b. unpaired electrons in nitrogen 1s22s22p3 3 c. filled subshells in Al 1s22s22p63s23p1 4 3.27 Electron Configuration Solutions a. total electrons in Ge have a number designation (before the letters) of 4 1s22s22p63s23p64s23d104p2 4 b. unpaired p electrons in sulfur, 2 electrons, number designation of the number unpaired electrons 1s22s22p63s23p4 designation = 3 c. 3d electrons in tin 1s22s22p63s23p64s23d104p65s24d105p2 10 ;3.28 Symbol Name a. Contains only two 2p electrons C carbon b. Contains an unpaired 3s electron Na sodium c. Contains two unpaired 3p electrons Si or S silicon or sulfur d. Contains three 4d electrons Nb niobium e. Contains three unpaired 3d V or Co vanadium or cobalt electrons 3.29 Symbol Name a. Contains one unpaired 5p electron In or I indium or iodine b. Contains a half‐filled 5s subshell Rb rubidium c. Contains a half‐filled 6p subshell Bi bismuth d. The last electron completes the 4d Cd cadmium subshell e. The last electron half fills the 4f Eu europium subshell 3.30 a. selenium [Ar]4s23d104p4 c. Ca [Ar]4s2 b. element number 23 [Ar]4s23d3 d. carbon [He]2s22p2 Electronic Structure and the Periodic Law 57 3.31 a. lead [Xe]6s24f145d106p2 c. An element [Ar]4s23d4 that contains 24 electrons b.
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