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

Solution: Arrange these elements in order of decreasing radius: S, Ca, F, Rb, and Si.

Solution: Arrange these elements in order of decreasing radius: S, Ca, F, Rb, and Si.

Problem

Arrange these elements in order of decreasing radius: S, Ca, F, Rb, and Si.

Solution
  • For a diatomic molecule, atomic radius is defined as half the distance between the nuclei in a molecule of two identical elements
  • In general, atomic radius decreases from left to right across a period. Reason is as protons (atomic number) are added in a period, electrons also increases in the same principal energy level. 
  • More protons will cause more positive charge which attract electrons closer to the nucleus.


  • Another trend is that atomic radius decreases from bottom to top. Reason is that as it goes down a group, new valence shell is added. 
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