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homework 2.59

Posted: Wed May 02, 2018 8:47 pm
by tatianatumbling_1J
I am confused on the answer to 2.59.
the question says to rank the ions from smallest to largest ionic radius. S2-, Cl-, and P3-
I thought the answer would be the all have the same ionization energy because they all end up on Ar on the periodic table after adding electrons. but the solution is P3-,S2-,Cl-

can someone explain what I am misunderstanding?

Re: homework 2.59

Posted: Wed May 02, 2018 8:53 pm
by annie_finneran_1K
go to the chem website and click solution manual errors. but also they do not have the same ionic radius, because ionic radius decreases across a period and those elements are all in the same period

Re: homework 2.59

Posted: Wed May 02, 2018 8:57 pm
by Adela Henry 1I
Atomic radii decrease across a period and since P3- appears first it has the greatest atomic radii and S2- and Cl- appear after it respectively on the periodic table meaning that their atomic radii are less than it. Therefore, since it asks for increasing atomic order it would be Cl- < S2- < P3-
I don't think for the distance of atomic radii you take into account the electron configuration only where it is on the periodic table.
Hope this helps

Re: homework 2.59

Posted: Wed May 02, 2018 9:20 pm
by tatianatumbling_1J
Adela Henry 1I wrote:Atomic radii decrease across a period and since P3- appears first it has the greatest atomic radii and S2- and Cl- appear after it respectively on the periodic table meaning that their atomic radii are less than it. Therefore, since it asks for increasing atomic order it would be Cl- < S2- < P3-
I don't think for the distance of atomic radii you take into account the electron configuration only where it is on the periodic table.
Hope this helps

that makes more sense, thank you!