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 the following in order of increasing radius:O2-, F- , Ne, Rb+, Br-

Solution: Arrange the following in order of increasing radius:O2-, F- , Ne, Rb+, Br-

Problem

Arrange the following in order of increasing radius:

O2-, F- , Ne, Rb+, Br-

Solution

We are being asked to rank the given species in order of increasing radius


The given species are ions and a neutral atom. When ranking compounds based on their ionic radius, we have the following rules:

The more electrons that an atom/ion possess, the bigger it is.

Cations (positively charged ions) tend to be smaller than their parent atoms

            Positive charge → lost electrons

Anions (negatively charged ions) tend to be bigger than their parent atoms

            Negative charge → gained electrons

Comparing atoms and ions that are isoelectronic or with the same number of electrons:

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