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
Additional Guides
Atomic Radius
Ionization Energy

Effective Nuclear Charge (Zeff) measures the force exerted onto an electron by the nucleus. 

Effective Nuclear Charge

Concept #1: Periodic Trend: Effective Nuclear Charge

Concept #2: Periodic Trends

Moving towards the top right corner of the Periodic Table causes effective nuclear charge to increase.

Example #1: Which of the following represents a chalcogen with the greatest effective nuclear charge?

Concept #3: Calculate without Slater’s Rules

Example #2: What is the effective nuclear charge felt by an electron in the third shell of an aluminum atom?

Practice: What is the identity of an element when the effective nuclear charge of its valence electrons is 18 while its shielding constant is 5?

Example #3: Using Slater’s Rules, calculate the effective nuclear charge of a 3p orbital electron in calcium.

Practice: In which orbital does an electron in a sulfur atom experience the greatest shielding?

Practice: Rank the following elements by effective nuclear charge, ZEff, for a valence electron: Kr, Se, Ca, K, Ge

Practice: Using Slater’s Rules calculate the effective nuclear charge of the 4d orbital electron in iodine.