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- 

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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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Problem Details

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- 

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