philip dutton university of windsor, canada prentice-hall © 2002 general chemistry principles and...
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Philip DuttonUniversity of Windsor, Canada
Prentice-Hall © 2002
General ChemistryPrinciples and Modern Applications
Petrucci • Harwood • Herring
8th Edition
Chapter 9: The Periodic Table and Some Atomic Properties
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 2 of 35
Contents
9-1 Classifying the Elements: The Periodic Law and the Periodic Table
9-2 Metals and Nonmetals and Their Ions
9-3 The Sizes of Atoms and Ions
9-4 Ionization Energy
9-5 Electron Affinity
9-6 Magnetic Properties
9-7 Periodic Properties of the Elements
Focus on The Periodic Law and Mercury
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 3 of 35
9-1 Classifying the Elements: The Periodic Law and the Periodic Table
• 1869, Dimitri Mendeleev Lothar Meyer
When the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically.
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 4 of 35
Periodic Law
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 5 of 35
Mendeleev’s Periodic Table
1871
— = 44
— = 72— = 68— = 100
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 6 of 35
Predicted Elements were Found
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 7 of 35
X-Ray Spectra
• H.G.J. Moseley 1913–X-ray emission is explained
in terms of transitions in which e- drop into orbits close to the atomic nucleus.
–Correlated (Ka) frequencies to atomic number Z: (Ka) = a (Z – 1)2
–Used to predict new elements (43, 61, 75) later discovered.
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Bohr atom and Moseley empirical formula
• Bohr:• 1913: Z-1 because one 1s electron is there.
• Moseley’s empirical formula:• 199-14
General ChemistryG. I. Csonka
Slide 8 of 35
22
221 2
111
1)( ZREEhKE H
HzZZh
RH 2152 11047.243
1
HzZK 215 11048.2
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 9 of 35
The Periodic tableAlkali Metals
Alkaline Earths
Transition Metals
Halogens
Noble Gases
Lanthanides and Actinides
Main Group
Main Group
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 10 of 35
9-2 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.
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 11 of 35
Metals Tend to Lose Electrons
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 12 of 35
Nonmetals Tend to Gain Electrons
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 13 of 35
Electron Configuration of Some Ions
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 14 of 35
9-3 The Sizes of Atoms and Ions
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 15 of 35
Atomic Radius
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 16 of 35
Screening and Penetration
Zeff = Z – S
En = - RH n2
Zeff2
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Prentice-Hall © 2002 General Chemistry: Chapter 9 Slide 17 of 50
Penetration and Shielding
Slater rules: For a 1s electron, S = 0.3.
For electrons in an s or p orbital with n > 1, the screening constant is given by
S = 1.00·N2 + 0.85·N1 + 0.35·N0N0 represents the number of other electrons in the same shell, N1 represents the number of electrons in the next smaller shell (n-1), and N2 is the number of electrons in other smaller shells
(n-2 and smaller).
The effective nuclear charge is
Zeff = Z - S
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 18 of 35
Cationic Radii
Ne 131 pm
13]Ne[ s23]Ne[ s
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 19 of 35
Anionic Radii
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 20 of 35
Atomic and Ionic Radii
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 21 of 35
9-4 Ionization Energy
Mg(g) → Mg+(g) + e-I1 = 738 kJ
Mg+(g) → Mg2+(g) + e- I2 = 1451 kJ
I1 = RH n2
Zeff12 S1 = 2 + 8·0.85 + 0.35 = 9.15
Zeff1 = 2.85
S2 = 2 + 8·0.85 = 8.80Zeff2 = 3.2 I2 = RH n2
Zeff22
Where n is the main quantum number, here it is 3. (3s2)
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 22 of 35
First Ionization Energy
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 23 of 35
Table 10.4 Ionization Energies of the Third-Period Elements (in kJ/mol)
I2 (Mg) vs. I3 (Mg)
7733
1451
I1 (Mg) vs. I1 (Al)
737.7 577.6
I1 (P) vs. I1 (S)
1012 999.6
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 24 of 35
9-5 Electron Affinity
F(g) + e- → F-(g) EA = -328 kJ
F(1s22s22p5) + e- → F-(1s22s22p6)
Li(g) + e- → Li-(g) EA = -59.6 kJ
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 25 of 35
First Electron Affinities
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 26 of 35
Second Electron Affinities
O(g) + e- → O-(g) EA = -141 kJ
O-(g) + e- → O2-(g) EA = +744 kJ
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 27 of 35
9-6 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.
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 28 of 35
Paramagnetism
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 29 of 35
9-7 Periodic Properties of the Elements
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 30 of 35
332266
Boiling Point
??
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 31 of 35
Melting Points of Elements
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 32 of 35
Melting Points of Compounds
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 33 of 35
Reducing Ability of Group 1 and 2 Metals
2 K(s) + 2 H2O(l) → 2 K+ + 2 OH- + H2(g)
Ca(s) + 2 H2O(l) → Ca2+ + 2 OH- + H2(g)
I1 = 419 kJ
I1 = 590 kJ
I2 = 1145 kJ
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 34 of 35
Oxidizing Abilities of the Halogens
2 Na + Cl2 → 2 NaCl
Cl2 + 2 I- → 2 Cl- + I2
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 35 of 35
Acid Base Nature of Element Oxides
• Basic oxides or base anhydrides:Li2O(s) + H2O(l) → 2 Li+(aq) + 2 OH-(aq)
• Acidic oxides or acid anhydrides:SO2 (g) + H2O(l) → H2SO3(aq)
• Na2O and MgO yield basic solutions
• Cl2O, SO2 and P4O10 yield acidic solutions
• SiO2 dissolves in strong base, acidic oxide.
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 36 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.
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Prentice-Hall © 2002 General Chemistry: Chapter 10 Slide 37 of 35
Chapter 10 Questions
1, 2, 18, 21, 27, 33, 39, 43, 51, 55