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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
Sections
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 (IGNORE)
Ionization Energy (IGNORE)

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

Effective Nuclear Charge

Concept #1: Periodic Trend: Effective Nuclear Charge

Higher the Effective Nuclear Charge (ZEff), greater the attractive force, which results in electrons being pulled closer to the nucleus.

Higher the Shielding Constant (S), greater the repulsive force between valence and inner core electrons, which results in valence electrons pushed away from the nucleus.

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.