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Chapter 10
The Periodic Table and Some Atomic Properties
 
 
 
Movie
Title
 p 357-3
Caption
 This animation illustrates the arrangement of elements in the periodic table.
Notes
 Periodic properties. Elements are arranged in the periodic table in order of increasing atomic number (number of protons). The horizontal rows are called periods and the columns are called groups. Elements in groups have similar chemicalchemical and physical properties. The metallic character of the elements increases to the left and down the periodic table. Nonmetallic character increases to the right and up the periodic table.
Movie
Title
 p 952-3
Caption
 Animation illustrating the periodic trend in oxidation states
Notes
 Periodic trends: common oxidation states. Elements in group IA and group IIA have oxidation numbers of +1 and +2, respectively. The maximum oxidation state increases from left to right across the periodic table. In the first row, O and F have negative oxidation numbers. In the second row S and Cl have positive oxidation numbers when they combine with O or F. In the third row the maximum oxidation number is +7 for Mn.
Movie
Title
 p 951-3
Caption
 Animation illustrating the periodic trends in atomic radii
Notes
 Periodic trends: atomic radii. As we move down a group in the periodic table the effective nuclear charge is essentially unchanged while the principal quantum number increases, resulting in an increase in the atomic radius. From left to right across a period the shielding by the inner electrons remains nearly constant while the number of protons in the nucleus increases, causing the atomic radii to decrease.
Movie
Title
 p 370-3
Caption
 Ionization energy of atoms and ions
Notes
 Ionization energy. Ionization energy is the energy required to remove an electron from the ground state of a gaseous atom or ion. I1 is the energy required to remove an electron from an uncharged atom. I2 is the energy required toremove the second electron. The removal of an electron results in less electron-electron repulsion and a greater effective nuclear charge, causing each successive ionization energy to increase.
Movie
Title
 p 370-3a
Caption
 Animation illustrating the periodic trends in ionization energies
Notes
 Periodic trends: ionization energies. The first ionization energy is the energy required to remove an electron from the ground state of an uncharged atom. The first ionization energies of the elements generally increase from right to left across a row as a result of the increasing nuclear charge and decreasing atomic radius. The ionization energies decrease down a group since the effective nuclear charge remains essentially the same and the atomic radius increases.
Movie
Title
 p 373-3
Caption
 Electron affinity is defined in this animation.
Notes
 Electron affinity. Electron affinity is the energy change that occurs when an electron is added to a gaseous atom or ion. Energy is usually released when an uncharged atom gains an electron, so the process is exothermic. Addition of an ion with a 1- charge results in an increased electron-electron repulsion, so work is required to add a second electron.
Movie
Title
 p 373-3a
Caption
  
Notes
 Periodic Trends: electron afinity. Electron affinity is the energy change that occurs when an electron is added to a gaseous atom or ion. Electron affinity is usually an endothermic process. Electron affinities generally decrease from top to bottom within a group and vary irregularly across a row of the periodic table. The halogens have the most negative electron affinities since the addition of one electron gives them an octet of electrons.
Movie
Title
 P 694-3
Caption
 Illustration of the periodic trends in the acid-base behavior of oxides
Notes
 Periodic trends: Acid-Base behaviour of oxides. Representative metal oxides are ionic and form basic aqueous solutions. Nonmetal oxides are usually covalent and most are acidic in aqueous solution with strength of the acid increasing as the oxidation state of the nonmetal increases. SO2 (oxidation state of S = 4) dissolves in water to give H2SO3 while SO3 (oxidation state of S = 6) produces H2SO4 in aqueous solution. Metalloids have oxides which are amphoteric.
10.1
Title
 10-1
Caption
  
Notes
 An illustration of the periodic law„variation of atomic volume with atomic number.
10.1.1UN2
Title
 p 358-1
Caption
  
Notes
 Dmitri Mendeleev (1834_1907) stamp
10.1.1UN
Title
 p 358-1a
Caption
  
Notes
 Dmitri Mendeleev (1834_1907) periodic table
10.1.2UN
Title
 p 359-1
Caption
  
Notes
 Henry G. J. Moseley (1887_1915)
10.2
Title
 10-2
Caption
  
Notes
 MoseleyÍs X-ray spectra of several elements
10.2.1UN
Title
 p 361-1
Caption
 Partial periodic table - metals tend to lose electrons to attain noble gas electronic configuration
Notes
 Partial periodic table - metals tend to lose electrons to attain noble gas electronic configuration
10.2.2UN
Title
 p 362-1
Caption
 Partial periodic table - Non-metals tend to gain electrons to attain noble gas electronic configuration
Notes
 Partial periodic table - Non-metals tend to gain electrons to attain noble gas electronic configuration
10.3
Title
 10-3
Caption
  
Notes
 Covalent, metallic, and ionic radii compared.
10.4
Title
 10-4
Caption
  
Notes
 Atomic radii
10.5
Title
 10-5
Caption
  
Notes
 The shielding effect and effective nuclear charge, Zeff
10.6
Title
 10-6
Caption
  
Notes
 A comparison of atomic and ionic sizes
10.7
Title
 10-7
Caption
  
Notes
 Covalent and anionic radii compared
10.8
Title
 10-8
Caption
  
Notes
 A comparison of some atomic and ionic radii
10.9
Title
 10-9
Caption
  
Notes
 First ionization energies as a function of atomic number
10.10
Title
 10-10
Caption
  
Notes
 Electron affinities of representative elements.
10.10.1UN
Title
 p 375-1
Caption
 3d and 4s boxes with arrows for Mn
Notes
 3d and 4s boxes with arrows for Mn
10.10.2UN
Title
 p 375-1a
Caption
 3d and 4s boxes with arrows for Mn2+
Notes
 3d and 4s boxes with arrows for Mn2+
10.10.3UN
Title
 p 375-1b
Caption
 3d and 4s boxes with arrows for Mn3+
Notes
 3d and 4s boxes with arrows for Mn3+
10.11
Title
 10-11
Caption
 Atomic properties and the periodic table
Notes
 Atomic properties and the periodic table
10.12
Title
 10-12
Caption
  
Notes
 Three halogen elements
10.13
Title
 10-13
Caption
  
Notes
 Melting points of the third-period elements
10.14
Title
 10-14
Caption
 composite of two photos - potassium reaction, calcium reaction
Notes
 composite of two photos - potassium reaction, calcium reaction
10.14a
Title
 p 378-1a
Caption
 Potassium, a Group 1A metal, reacts so rapidly that the hydrogen evolved bursts into flame. Notice that the metal is less dense than water
Notes
 Potassium, a Group 1A metal, reacts so rapidly that the hydrogen evolved bursts into flame. Notice that the metal is less dense than water
10.14b
Title
 p 378-1b
Caption
  
Notes
 Calcium, a Group 2A metal, reacts more slowly than does potassium
10.15
Title
 10-15
Caption
  
Notes
 Reaction of sodium metal and chlorine gas.
10.16
Title
 10-16
Caption
 composite of two photos - colorless solution, purple solution
Notes
 composite of two photos - colorless solution, purple solution
10.16a
Title
 p 379-1a
Caption
  
Notes
 Cl2(g) is bubbled through a colorless, dilute solution containing iodide ion, I2(aq)
10.16b
Title
 p 379-1b
Caption
  
Notes
 I2 produced in the aqueous solution is extracted into CCl4(l), in which it is much more soluble (purple layer)
10.17.3UN
Title
 p 380-1
Caption
 Mercury is a liquid at room temperature
Notes
 Mercury is a liquid at room temperature
10.17
Title
 10-17
Caption
 Acid Basic and Amphoteric Oxides
Notes
 Acid Basic and Amphoteric Oxides
10.17.1UN
Title
 p 381-1
Caption
 Melting point versus period number of Li, Na, K, Rb, Cs, and Fr
Notes
 Melting point versus period number of Li, Na, K, Rb, Cs, and Fr
10.17.2UN
Title
 p 382-1
Caption
 Molar Volume versus period number of Li, Na, K, Rb, Cs, and Fr
Notes
 Molar Volume versus period number of Li, Na, K, Rb, Cs, and Fr
10.17.4UN
Title
 p 385-1
Caption
 Four different size spheres for exercise 55
Notes
 Four different size spheres for exercise 55
Table 10.1
Title
 Table 10.1
Caption
  
Notes
 Properties of germanium: predicted and observed
Table 10.2
Title
 Table 10.2
Caption
  
Notes
 Electron configurations of some metal ions
Table 10.3
Title
 Table 10.3
Caption
  
Notes
 Atomic Radii and first ionization energies of the alkali metal elements
Table 10.4
Title
 Table 10.4
Caption
  
Notes
 ionization energies of the third period elements
Table 10.5
Title
 Table 10.5
Caption
  
Notes
 Some properties of three halogen elements
Table 10.6
Title
 Table 10.6
Caption
  
Notes
 Melting points of two series of compounds