Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
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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: Place the following ions in order from smallest to largest ionic radii: Note that < means less than. K+, Ca2+, S2-, and Cl-.a. S2- < Cl- < Ca2+ < K+b. Ca2+ <  K+ < Cl-  < S2- c. S2-  <  Cl- < K+ < Ca2+d. K+ <  Cl-  < S2-  < Ca2+e. Ca2+ <  K+ <  S2-  < Cl- 

Problem

Place the following ions in order from smallest to largest ionic radii: Note that < means less than. K+, Ca2+, S2-, and Cl-.

a. S2- < Cl- < Ca2+ < K+

b. Ca2+ <  K+ < Cl-  < S2- 

c. S2-  <  Cl- < K+ < Ca2+

d. K+ <  Cl-  < S2-  < Ca2+

e. Ca2+ <  K+ <  S2-  < Cl- 

Solution

Establish the trend for ionic radius and rank the following ions and element to increasing ionic radius


Recall that ionic radius is the size of an ion. The trend for ionic radius is as follows: it increases from right to left and down a period in the periodic table. Ionic radius also increases with increasing number of electrons.


For this problem, we need to do the following:

Step 1: Determine the electrons in each species.

Step 2: Compare the charges if they are isoelectronic.


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