chapter 6 ionic compounds: periodic trends and bonding theory
TRANSCRIPT
![Page 1: Chapter 6 Ionic Compounds: Periodic Trends and Bonding Theory](https://reader034.vdocument.in/reader034/viewer/2022042620/62645d940ec3f6507456f8bc/html5/thumbnails/1.jpg)
© 2016 Pearson Education, Inc.Instructor’s Resource Materials (Download only) for Chemistry, 7e
John E. McMurry, Robert C. Fay, Jill Robinson
John E. McMurry
Robert C. Fay
Lecture Presentation
Chapter 6
Ionic Compounds:
Periodic Trends
and Bonding
Theory
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Group 1a ion+: [Noble gas]
Group 2a ion2+: [Noble gas]
Electron Configurations of Ions
–1 e–
–2 e–
Na:
Cl:
1s2 2s2 2p6 3s1
1s2 2s2 2p6 3s2 3p5
Na+:
Cl–:
1s2 2s2 2p6
1s2 2s2 2p6 3s2 3p6
Group 1a atom: [Noble gas] ns1
Group 2a atom: [Noble gas] ns2
–1 e–
+1 e–
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© 2016 Pearson Education, Inc.Instructor’s Resource Materials (Download only) for Chemistry, 7e
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Electron Configurations of Ions
Group 6a ion2–: [Noble gas] ns2 np6
Group 7a ion–: [Noble gas] ns2 np6
+2 e–
+1 e–
Na:
Cl:
1s2 2s2 2p6 3s1
1s2 2s2 2p6 3s2 3p5
Na+:
Cl–:
1s2 2s2 2p6
1s2 2s2 2p6 3s2 3p6
Group 6a atom: [Noble gas] ns2 np4
Group 7a atom: [Noble gas] ns2 np5
–1 e–
+1 e–
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© 2016 Pearson Education, Inc.Instructor’s Resource Materials (Download only) for Chemistry, 7e
John E. McMurry, Robert C. Fay, Jill Robinson
Electron Configurations of Ions
![Page 5: Chapter 6 Ionic Compounds: Periodic Trends and Bonding Theory](https://reader034.vdocument.in/reader034/viewer/2022042620/62645d940ec3f6507456f8bc/html5/thumbnails/5.jpg)
© 2016 Pearson Education, Inc.Instructor’s Resource Materials (Download only) for Chemistry, 7e
John E. McMurry, Robert C. Fay, Jill Robinson
Electron Configurations of Ions
–2 e–
–3 e–
Fe:
Fe:
[Ar] 4s2 3d6
[Ar] 4s2 3d6
Fe2+:
Fe3+:
[Ar] 3d6
[Ar] 3d5
IonsAtoms
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John E. McMurry, Robert C. Fay, Jill Robinson
Ionic Radii
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© 2016 Pearson Education, Inc.Instructor’s Resource Materials (Download only) for Chemistry, 7e
John E. McMurry, Robert C. Fay, Jill Robinson
Ionic Radii
![Page 8: Chapter 6 Ionic Compounds: Periodic Trends and Bonding Theory](https://reader034.vdocument.in/reader034/viewer/2022042620/62645d940ec3f6507456f8bc/html5/thumbnails/8.jpg)
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John E. McMurry, Robert C. Fay, Jill Robinson
Ionization Energy
Ionization Energy (Ei): The amount of energy
necessary to remove the highest-energy electron
from an isolated neutral atom in the gaseous state
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© 2016 Pearson Education, Inc.Instructor’s Resource Materials (Download only) for Chemistry, 7e
John E. McMurry, Robert C. Fay, Jill Robinson
Ionization Energy
![Page 10: Chapter 6 Ionic Compounds: Periodic Trends and Bonding Theory](https://reader034.vdocument.in/reader034/viewer/2022042620/62645d940ec3f6507456f8bc/html5/thumbnails/10.jpg)
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Ionization Energy
Boron has a lower Ei due to a smaller Zeff
(shielding by the 2s electrons).
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Ionization Energy
Oxygen has a lower Ei, since the first electron is
removed from a filled orbital.
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Higher Ionization Energies
M3+ + e–M2+ + energy
M+ + e–M + energy
M2+ + e–M+ + energy
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Electron Affinity
Electron Affinity (Eea): The energy change that
occurs when an electron is added to an isolated
atom in the gaseous state
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John E. McMurry, Robert C. Fay, Jill Robinson
Octet Rule
Octet rule: Main-group elements tend to undergo
reactions that leave them with eight outer-shell
electrons. That is, main-group elements react so that
they attain a noble-gas electron configuration with
filled s and p sublevels in their valence electron shell.
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© 2016 Pearson Education, Inc.Instructor’s Resource Materials (Download only) for Chemistry, 7e
John E. McMurry, Robert C. Fay, Jill Robinson
Octet Rule
Octet rule: Main-group elements tend to undergo
reactions that leave them with eight outer-shell
electrons. That is, main-group elements react so that
they attain a noble-gas electron configuration with
filled s and p sublevels in their valence electron shell.
Metals tend to have low Ei and low Eea.
They tend to lose one or more electrons.
Nonmetals tend to have high Ei and high Eea.
They tend to gain one or more electrons.
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John E. McMurry, Robert C. Fay, Jill Robinson
Ionic Bonds and the Formation of Ionic
Solids
Na+ + Cl–Na
1s2 2s2 2p6
Cl+
1s2 2s2 2p6 3s2 3p6
3s1 3p51s2 2s2 2p6 1s2 2s2 2p6 3s2
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Ionic Bonds and the Formation of
Ionic Solids
Born-Haber Cycle
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John E. McMurry, Robert C. Fay, Jill Robinson
Ionic Bonds and the Formation of
Ionic Solids
Born-Haber Cycle
Step 2: Cl(g)Cl2(g) +122 kJ/mol
Step 5:
NaCl(s)Na(s) + Cl2(g) –411 kJ/mol
Step 1: Na(g)Na(s) +107.3 kJ/mol
Step 3: Na+(g) + e–Na(g) +495.8 kJ/mol
Step 4: Cl–(g)Cl(g) + e– –348.6 kJ/mol
NaCl(s)Na+(g) + Cl–(g) –787 kJ/mol
2
1
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Lattice Energies in Ionic Solids
Lattice Energy (U): The amount of energy that must
be supplied to break up an ionic solid into individual
gaseous ions