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Ch.2 Atoms and the Periodic TableWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
The Atom (Simplified)
Subatomic Particles (Simplified)
Ions (Simplified)
Atomic Mass (Simplified)
Atomic Mass (Conceptual)
Periodic Table: Element Symbols
Periodic Table: Classifications
Periodic Table: Group Names
Periodic Table: Representative Elements & Transition Metals
Periodic Table: Elemental Forms (Simplified)
Periodic Table: Phases (Simplified)
Law of Definite Proportions
Atomic Theory
Rutherford Gold Foil Experiment
Wavelength and Frequency (Simplified)
Electromagnetic Spectrum (Simplified)
Bohr Model (Simplified)
Emission Spectrum (Simplified)
Electronic Structure
Electronic Structure: Shells
Electronic Structure: Subshells
Electronic Structure: Orbitals
Electronic Structure: Electron Spin
Electronic Structure: Number of Electrons
The Electron Configuration (Simplified)
Electron Arrangements
The Electron Configuration: Condensed
The Electron Configuration: Exceptions (Simplified)
Ions and the Octet Rule
Ions and the Octet Rule (Simplified)
Valence Electrons of Elements (Simplified)
Lewis Dot Symbols (Simplified)
Periodic Trend: Metallic Character
Periodic Trend: Atomic Radius (Simplified)

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: