Chapter 8 Notes
Chem201A
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Dr. Baxley
Chapter 8 Notes: Periodic Properties of the Elements
I. Development of the Periodic Table
II.
Characteristics of Many-Electron Atoms
A. Energy-Level Splitting
B. Orbital Energies
Chapter 8 Notes
Chem201A
III.
Electron Configurations
A. Atomic Orbitals and the Periodic Table
B. Electron configuration
1 a. Write the electron configuration of fluorine.
b. Write the abbreviated electron configuration of Zr.
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Dr. Baxley
Chapter 8 Notes
Chem201A
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Dr. Baxley
C. Exceptions to electron configurations
D. Orbital Diagram
2. a. Draw the orbital diagram for oxygen.
2. a. Draw the orbital diagram for molybdenum.
E. Categories of Electrons
Examples:
Si: 1s22s22p63s23p2
Ti: 1s22s22p63s23p64s23d2
Chapter 8 Notes
Chem201A
page 4
Dr. Baxley
F. Quantum Numbers
Principle quantum number
n = 1, 2, 3….
Angular momentum quantum number
l = 0, 1, …, n-1
Magnetic quantum number
ml = 0, ±1,±2, …, ± l
Spin quantum number (spin of e–)
ms = ± ½
Example: What are the four quantum numbers for the last electron in each of the following
elements.
• oxygen
•
zinc
Chapter 8 Notes
Chem201A
The Pauli Exclusion Principle
IV.
Trends in Atomic Properties
A. Effective Nuclear Charge
B. Atomic Radius
How does radius size vary down a group? Why?
How does radius size vary across a period? Why?
C. Ionic Radii
What happens to the size when a metal becomes a cation? Why?
What happens to the size when a nonmetal becomes an anion ? Why?
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Dr. Baxley
Chapter 8 Notes
Chem201A
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Dr. Baxley
D. Isoelectronic Series
Isoelectronic:
Rank this isoelectronic series from smallest to largest.
Mg2+ Na+ O2- F- Al3+ Ne
E. Ionization Energy
F. Successive Ionization Energies
Na
Mg
Chapter 8 Notes
Chem201A
G. Electron Affinity
V. Properties of Ions
A Electron configurations Ions
3. Write the abbreviated electron configurations for Cu2+ and Sn4+.
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Dr. Baxley
Chapter 8 Notes
Chem201A
B. Magnetic Properties
4. Are each of the following diamagnetic or paramagnetic?
Cu+
Cu2+
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Dr. Baxley