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Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch.17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
The Electron Configuration
The Electron Configuration: Condensed
The Electron Configurations: Exceptions
The Electron Configuration: Ions
Paramagnetism and Diamagnetism
The Electron Configuration: Quantum Numbers
Valence Electrons of Elements
Periodic Trend: Metallic Character
Periodic Trend: Atomic Radius
Periodic Trend: Ionic Radius
Periodic Trend: Ionization Energy
Periodic Trend: Successive Ionization Energies
Periodic Trend: Electron Affinity
Periodic Trend: Electronegativity
Periodic Trend: Effective Nuclear Charge
Periodic Trend: Cumulative

Most Electron Configuration Exceptions are the result of elements drive to obtain half filled or totally filled d orbitals

Electron Configuration Exceptions

Concept #1: Electron Orbital Stability

p and d subshells are most stable when either half filled or totally filled with electrons.

Concept #2: Exceptions to Electron Configurations

Concept #3: Half-filled Orbitals

When electron configuration ends with d4, an s orbital electron is promoted to d orbital to create half filled orbital: d5.

Concept #4: Completely-filled Orbitals

When electron configuration ends with d9, an s orbital electron is promoted to d orbital to create completely filled orbital: d10.

Example #1: Based on the exceptions, provide the condensed electron configuration for the silver atom.

Practice: Illustrate the exception to the electron configuration of molybdenum.

Practice: Which of the following is the correct electron configuration of gold? 

Practice: A comparison of the electron configurations of palladium (Pd) and silver (Ag) indicates that: