General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 10: The Periodic Table and Some Atomic Properties Philip Dutton University of Windsor, Canada N9B 3P4 Prentice-Hall 2002
Contents 10-1 Classifying the Elements: The Periodic Law and the Periodic Table 10-2 Metals and Nonmetals and Their Ions 10-3 The Sizes of Atoms and Ions 10-4 Ionization Energy 10-5 Electron Affinity 10-6 Magnetic Properties 10-7 Periodic Properties of the Elements Focus on The Periodic Law and Mercury Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 2 of 35
10-1 Classifying the Elements: The Periodic Law and the Periodic Table 1869, Dimitri Mendeleev Lother Meyer When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically. Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 3 of 35
Periodic Law Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 4 of 35
Mendeleev s Periodic Table 1871 = 44 = 68 = 72 = 100 Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 5 of 35
Predicted Elements were Found Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 6 of 35
X-Ray Spectra Moseley 1913 X-ray emission is explained in terms of transitions in which e - drop into orbits close to the atomic nucleus. Correlated frequencies to nuclear charges. ν = A (Z b) 2 Used to predict new elements (43, 61, 75) later discovered. Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 7 of 35
Alkali Metals The Periodic table Alkaline Earths Halogens Main Group Transition Metals Noble Gases Main Group Lanthanides and Actinides Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 8 of 35
10-2 Metals and Nonmetals and Their Ions Metals Good conductors of heat and electricity. Malleable and ductile. Moderate to high melting points. Nonmetals Nonconductors of heat and electricity. Brittle solids. Some are gases at room temperature. Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 9 of 35
Metals Tend to Lose Electrons Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 10 of 35
Nonmetals Tend to Gain Electrons Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 11 of 35
Electron Configuration of Some Ions Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 12 of 35
10-3 The Sizes of Atoms and Ions Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 13 of 35
Atomic Radius Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 14 of 35
Screening and Penetration Z eff = Z S Z 2 E n = - R eff H n 2 Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 15 of 35
Cationic Radii Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 16 of 35
Anionic Radii Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 17 of 35
Atomic and Ionic Radii Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 18 of 35
10-4 Ionization Energy Mg(g) Mg + (g) + e - I 1 = 738 kj Mg + (g) Mg 2+ (g) + e - I 2 = 1451 kj Z 2 I = R eff H n 2 Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 19 of 35
First Ionization Energy Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 20 of 35
Table 10.4 Ionization Energies of the Third-Period Elements (in kj/mol) 737.7 577.6 1451 7733 1012 999.6 I 2 (Mg) vs. I 3 (Mg) I 1 (Mg) vs. I 1 (Al) I 1 (P) vs. I 1 (S) Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 21 of 35
10-5 Electron Affinity F(g) + e - F - (g) EA = -328 kj F(1s 2 2s 2 2p 5 ) + e - F - (1s 2 2s 2 2p 5 ) Li(g) + e - Li - (g) EA = -59.6 kj Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 22 of 35
First Electron Affinities Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 23 of 35
Second Electron Affinities O(g) + e - O - (g) EA = -141 kj O - (g) + e - O 2- (g) EA = +744 kj Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 24 of 35
10-6 Magnetic Properties Diamagnetic atoms or ions: All e - are paired. Weakly repelled by a magnetic field. Paramagnetic atoms or ions: Unpaired e -. Attracted to an external magnetic field. Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 25 of 35
Paramagnetism Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 26 of 35
10-7 Periodic Properties of the Elements Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 27 of 35
Boiling Point 266? 332? Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 28 of 35
Melting Points of Elements Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 29 of 35
Melting Points of Compounds Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 30 of 35
Reducing Ability of Group 1 and 2 Metals 2 K(s) + 2 H 2 O(l) 2 K + + 2 OH - + H 2 (g) I 1 = 419 kj I 1 = 590 kj I 2 = 1145 kj Ca(s) + 2 H 2 O(l) Ca 2+ + 2 OH - + H 2 (g) Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 31 of 35
Oxidizing Abilities of the Halogens 2 Na + Cl 2 2 NaCl Cl 2 + 2 I - 2 Cl - + I 2 Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 32 of 35
Acid Base Nature of Element Oxides Basic oxides or base anhydrides: Li 2 O(s) + H 2 O(l) 2 Li + (aq) + 2 OH - (aq) Acidic oxides or acid anhyhydrides: SO 2 (g) + H 2 O(l) H 2 SO 3 (aq) Na 2 O and MgO yield basic solutions Cl 2 O, SO 2 and P 4 O 10 yield acidic solutions SiO 2 dissolves in strong base, acidic oxide. Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 33 of 35
Focus on The Periodic Law and Mercury Should be a solid. Relativistic shrinking of s-orbitals affects all heavy metals but is maximum with Hg. Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 34 of 35
Chapter 10 Questions 1, 2, 18, 21, 27, 33, 39, 43, 51, 55 Prentice-Hall 2002 General Chemistry: Chapter 10 Slide 35 of 35