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Chapter 8 Study Guide
Chapter 8 is the second half of the "theory of atoms" presentation
(following chapter 7.) The principle focus of Chapter 8 is using
the solution of the hydrogen atom and other
concepts to chart the electronic structure of all the other
elements in the Periodic Table, and thus to explain the
shape of the Table and the similarities in Chemistry between
atoms in each column of the table.
Suggested Problems
The following problems (in the textbook) are illustrative of the
important concepts covered in this chapter, and are of comparable
(or greater!) difficulty with what you might see on homeworks or exams:
Chapter 8, problems: 29, 30, 31, 35, 36, 41, 43, 47, 48, 50,
51, 52, 57, 58, 60,61, 64, 66, 73, 74, 77, 80, 84, 86, 87, 89.
You should be able to:
- Apply the Bohr model to one-electron atoms.
- Write the electronic configuration of most any common atom
or ion.
- Explain the electronic configuration of most any
common atom or ion.
- Give the standard ordering of orbital energies.
- Explain and apply the Pauli Exclusion Principle, the aufbau principle,
and Hund's Rule.
- Identify the different blocks of the Periodic Table.
- Identify paramagnetic and diamagnetic species, and
count unpaired spins.
- Manipulate and apply ionization energies and electron affinities.
- Explain and apply trends in the periodic table.
- Identify acidic, basic and amphoteric oxides.
Important topics and Concepts
- The Bohr model and one-electron atoms; effects of Z
on orbital sizes and energies
- Orbitals in multi-electron atoms
- l-dependence of the energy
- degeneracy of the p orbitals, etc.
- Ordering of the orbital energies
- Electronic configurations
- Standard notation
- Energy level diagrams
- Aufbau principle
- Pauli Exclusion Principle
- Hund's Rule
- Exceptions
- Electronic configurations determine the "block structure"
of the Periodic table.
- Valence vs. Core electrons
- Electronic structure of ions
- Ionization energies and Electron affinities; energy level
diagrams and their interpretation.
- Diamagnetism and Paramagnetism
- Trends in the Periodic Table:
- Ionization energy
- Electron affinity
- Atomic size
- Metallic character
- Strength as a Reducing or Oxidizing Agent.
- Acidity or Basicity of Oxides.
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