chapter 7(a) atomic structure and periodicity. figure 7.1: the nature of waves. note that the...
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Chapter 7(a)
Atomic StructureAtomic Structureand Periodicityand Periodicity
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Figure 7.1: The nature of waves. Note that the radiation with the shortest wavelength has the highest frequency.
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Copyright © Houghton Mifflin Company. All rights reserved. 7a–3
Figure 7.2: Classification of electromagnetic radiation.
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When a strontium salt is dissolved in methanol (with a little water) and ignited, it gives a brilliant red flame. The red color is produced by emission of light when electrons,
excited by the energy of the burning methanol, fall back to their ground states.
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Figure 7.4: Electromagnetic radiation exhibits wave properties and particulate
properties.
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Figure 7.5: (a) Diffraction occurs when electromagnetic radiation is scattered from a regular array of objects, such as the ions in a crystal of sodium chloride. The large spot in the center is from the main incident beam of X rays. (b) Bright spots in the diffraction pattern result from constructive interference of waves. The waves are in phase; that is, their peaks match. (c) Dark areas result from destructive interference of waves. The waves are out of phase; the peaks of one wave coincide with the troughs of another wave.
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Figure 7.6: (a) A continuous spectrum containing all wavelengths of visible light. (b) The hydrogen line spectrum contains only a few discrete wavelengths.
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Figure 7.7: A change between two discrete energy levels emits a photon of light.
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Figure 7.8: Electronic transitions in the Bohr model for the hydrogen atom.
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Figure 7.9: The standing waves caused by the vibration of a guitar string fastened at both ends. Each dot represents a node (a point of zero displacement).
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Wave-generating apparatus.
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Figure 7.10: The hydrogen electron visualized as a standing wave around the nucleus.
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Chapter 7(b)
Atomic StructureAtomic Structureand Periodicity and Periodicity (cont’d)(cont’d)
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Figure 7.11: (a) The probability distribution for the hydrogen 1s orbital in three dimensional space. (b) The probability of finding the electron at points along a line drawn from the nucleus outward in any direction for the hydrogen 1s orbital.
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Figure 7.12: (a) Cross section of the hydrogen 1s orbital probability distribution divided into successive thin spherical
shells. (b) The radial probability distribution.
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Copyright © Houghton Mifflin Company. All rights reserved. 7a–16
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Figure 7.13: Two representations of the hydrogen 1s, 2s, and 3s orbitals.
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Figure 7.14: Representation of the 2p orbitals. (a) The electron probability distributed for a 2p orbital.
(b) The boundary surface representations of all three 2p orbitals.
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Figure 7.15: A cross section of the electron probability distribution for a 3p orbital.
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Figure 7.16: Representation of the 3d orbitals.
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Figure 7.17: Representation of the 4f orbitals in terms of their boundary surface.
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Figure 7.18: Orbital energy levels for the hydrogen atom.
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Figure 7.19: A picture of the spinning electron.
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Chapter 7(c)
Atomic StructureAtomic Structureand Periodicity and Periodicity (cont’d)(cont’d)
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Figure 7.20: A comparison of the radial probability distributions of the 2s and 2p
orbitals.
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Figure 7.21: (a) The radial probability distribution for an electron in a 3s orbital. (b) The radial
probability distribution for the 3s, 3p, and 3d orbitals.
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Figure 7.22: The orders of the energies of the orbitals in the first three levels of
polyelectronic atoms.
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Figure 7.24: Mendeleev's early periodic table, published in 1872. Note the spaces left for missing
elements with atomic masses 44, 68, 72, 100.
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Copyright © Houghton Mifflin Company. All rights reserved. 7a–30
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Sodium metal is so reactive that it is stored under kerosene to protect it from the oxygen in the air.
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A vial containing potassium metal. The sealed vial contains an inert gas to protect the potassium from
reacting with oxygen.
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Figure 7.25: The electron configurations in the type of orbital occupied last for the first
18 elements.
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Figure 7.26: Electron configurations for potassium through krypton.
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Figure 7.27: The orbitals being filled for elements in various parts of the periodic
table.
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Chapter 7(c)
Atomic StructureAtomic Structureand Periodicity and Periodicity (cont’d)(cont’d)
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Figure 7.20: A comparison of the radial probability distributions of the 2s and 2p
orbitals.
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Figure 7.21: (a) The radial probability distribution for an electron in a 3s orbital. (b) The radial
probability distribution for the 3s, 3p, and 3d orbitals.
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Figure 7.22: The orders of the energies of the orbitals in the first three levels of
polyelectronic atoms.
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Figure 7.24: Mendeleev's early periodic table, published in 1872. Note the spaces left for missing
elements with atomic masses 44, 68, 72, 100.
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Copyright © Houghton Mifflin Company. All rights reserved. 7a–42
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Copyright © Houghton Mifflin Company. All rights reserved. 7a–43
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Sodium metal is so reactive that it is stored under kerosene to protect it from the oxygen in the air.
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Copyright © Houghton Mifflin Company. All rights reserved. 7a–45
A vial containing potassium metal. The sealed vial contains an inert gas to protect the potassium from
reacting with oxygen.
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Figure 7.25: The electron configurations in the type of orbital occupied last for the first
18 elements.
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Figure 7.26: Electron configurations for potassium through krypton.
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Figure 7.27: The orbitals being filled for elements in various parts of the periodic
table.
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Chapter 7(d)
Atomic StructureAtomic Structureand Periodicity and Periodicity (cont’d)(cont’d)
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Figure 7.28: The periodic table with atomic symbols, atomic numbers, and partial electron configurations.
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Figure 7.29: A diagram that summarizes the order in which the orbitals fill in polyelectronic
atoms.
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Figure 7.30: The positions of the elements considered in Sample Exercise 7.7
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Figure 7.31: The values of first ionization energy for the elements in the first six
periods.
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Figure 7.32: Trends in ionization energies (kJ/mol) for the representative elements.
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Figure 7.33: The electron affinity values for atoms among the first 20 elements that form
stable, isolated X- ions.
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Liquid bromine in equilibrium with its vapor.
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Figure 7.34: The radius of an atom (r) is defined as half the distance between the
nuclei in a molecule consisting of identical atoms.
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Figure 7.35: Atomic radii (in picometers) for selected atoms.
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Figure 7.36: Special names for groups in the periodic table.
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Potassium reacts violently with water.
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