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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.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Sections
The Atom (Simplified)
Subatomic Particles (Simplified)
Isotopes
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)

The electron configuration of an element is the distribution of its electrons within atomic orbitals.

The Electron Configuration

Concept #1: Electron Orbital Diagrams

Example #1: Properly fill in the orbitals of an atom that possesses 8 electrons within its d set of orbitals.

Practice: Which electron configuration represents a violation of Hund’s Rule? 

Concept #2: Ground State Electron Configurations

Concept #3: Auf Bau Principle

Example #2: Write the ground state electron configuration for the following element: Fluorine (Z = 9)

Practice: Which electron configuration represents a violation of the Auf Bau Principle? 

Practice: Identify the element with the given electron orbital diagram. 

Practice: Write the electron configuration and electron orbital diagram for the following element:

Sulfur   (Z = 16)

Practice: Write the ground state electron configuration for the following element:

Magnesium   (Z = 12)  

Concept #4: Unpaired vs Paired Electrons

Example #3: Determine the number of unpaired electrons in vanadium.

Practice: Which of the following atoms has no unpaired electrons?

Practice: Which of the following atoms has the most unpaired electrons?