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Chapter 8
Electron Configurations, Atomic Properties, and the Periodic Table
8.1
Title
 Orbital energy diagrams
Caption
 Some orbital energies of the first four principal shells are compared for a hydrogen atom and a typical multielectron atom. The energies are not plotted to scale.
Keywords
 orbital, energy, effective nuclear charge, hydrogen, principle quantum number, shielding, electron
8.2
Title
 Order in which subshells are filled w/electrons
Caption
 To determine the order of filling of orbitals in a multi-electron system, tart at the upper left of the grid and follow the arrows. The order in which the arrows slice through the subshell designations is the order in which the subshells fill. The blank space at the upper right corresponds to nonexistent orbitals (1p, 1d, 2d, and so on). The blank space at the bottom corresponds to orbitals that are not filled in the known elements (7p, 8s, and so on).
Keywords
 aufbau, electron, subshell, electron configuration, orbital
8.3.1T.2
Title
 Electron configurations of the first transition series elements
Caption
 The electron configurations of the first transition series elements show that these elements generally follow the predicted sequence of filling of subshells. For those that violate the rules, the energy of the subshells must be different for these particular cases because electrons fill the lowest energy orbitals first.
Keywords
 orbital, subshell, transition metal, half-filled orbital, electron configuration
8.3
Title
 Electron configurations & the periodic table
Caption
 Subshells that lie at lower energies than those listed are filled with electrons. For example, the electron configuration of arsenic is [Ar]3d104s24p3, that of iodine is [Kr]4d105s25p5, that of lead is [Xe]4f145d106s26p2, and that of uranium is [Rn]5f36d17s2.
Keywords
 electron configuration, periodic table, noble gas
8.6
Title
 Periodic table & order of filling of subshells
Caption
 Read through this periodic table, starting at the upper left, and you will discover the same order of filling of subshells as shown in Figure 8.2. Note that helium (ZÊ=Ê2) is an s-block element, but it is grouped with the p-block elements because we place it in Group 8A with the other noble gas elements that it so strongly resembles.
Keywords
 periodic table, electron configuration, orbital
8.7ab
Title
 Paramagnetism illustrated
Caption
 (a) A sample (left side of balance) is weighed in the absence of a magnetic field. (b) When the field is turned on, the balanced condition is upset. The sample appears to gain weight. This is because it is now subjected to two attractive forces, the force of gravity and the force exerted by the magnetic field.
Keywords
 paramagnetism, magnetic field, electron spin
8.8
Title
 Atomic radius illustrated.
Caption
 The covalent radius is half the distance between the nuclei of the two I atoms in the I2 molecule. The atomic radius is the distance between the nucleus and the outside of the atom.
Keywords
 atomic radius, covalent radius, bonding, diatomic, internuclear distance
8.9
Title
 Atomic radii of the elements
Caption
 The values shown here, in picometers (pm), are metallic radii for metals and covalent radii for nonmetals. Data are not included for the noble gases because it is difficult to assess their covalent radii (only Kr and Xe compounds are known). Explanations have been offered for the small peaks in the middle of some periods and for other irregularities, but they are beyond the scope of this book.
Keywords
 effective nuclear charge, atomic radius, periodic trends
8.10
Title
 Shielding effect & effective nuclear charge
Caption
 This simplified sketch of a magnesium atom shows the two valence electrons and one core electron as discrete particles. The remaining 9 core electrons are shown as a circular cloud of negative electric charge. Interactions (discussed in the text) between valence electrons, core electrons, and the atomic nucleus determine an effective nuclear charge. Attractions are indicated in red and repulsions in blue.
Keywords
 effective nuclear charge, shielding, valence electron, core electron
8.11
Title
 Ionic radii
Caption
 The distance between the centers of the two ions (205 pm) is apportioned between the Mg2+ (65 pm) and O2- (140 pm) ions. The sizes of other cations can be related to their internuclear distance to the oxide ion.
Keywords
 internuclear distance, bonding radius, ionic radius
8.12
Title
 Comparison of atomic & cationic radii
Caption
 Metallic radii are shown for Na and Mg, and ionic radii for Na+ and Mg2+. The radius for Ne is for a nonbonded atom.
Keywords
 effective nuclear charge, atomic radius, ionic radius
8.13
Title
 Atomic and anionic radii compared
Caption
 The two chlorine atoms in a Cl2 molecule gain one electron each to form two chloride ions (2 Cl-).
Keywords
 atomic radius, effective nuclear charge, ionic radii
8.14
Title
 Some representative atomic & ionic radii
Caption
 Some representative atomic & ionic radii are shown.
Keywords
 atomic radius, ionic radius, periodic trends
8.15
Title
 First ionization energy as function of atomic number
Caption
 The first ionization energy is shown as function of atomic number. Explanations have been offered for the small peaks in the middle of some periods and for other irregularities, but they are beyond the scope of this book.
Keywords
 ionization energy, periodic trends
8.16
Title
 Metal, nonmetals, metalloids, & noble gases
Caption
 The grouping of metals, nonmetals, metalloids, and noble gases are shown within the periodic table.
Keywords
 periodic trends, periodic table, metal
8.17
Title
 Atomic properties- summary of trends inthe periodic table
Caption
 This figure summarizes the trends noted in the margins of some of the preceding pages. Vertical arrows point in the direction of a trend within a group. Horizontal arrows point in the direction of a trend within a period.
Keywords
 periodic trends, effective nuclear charge, ionization energy, atomic radius
8.22
Title
 Acidic, basic, & amphoteric oxides of the main group elements
Caption
 Similar valence electron configuration of the main group elements has further implications than just size or ionization energy. The oxides of these elements can be acidic, basic or amphoteric.
Keywords
 periodic trends, oxides
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