If they were atoms, $\ce{Mg}$ should have a smaller radii. How does this change?
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$\begingroup$ Can you point to a source that says calcium ion is smaller than magnesium ion? $\endgroup$– Brinn BelyeaCommented Feb 16, 2015 at 3:59
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$\begingroup$ An exercise book.Also look here: answers.yahoo.com/question/index?qid=20071216145936AAgZZnv "To answer your question: (out of Ca2+ and Mg2+ )Mg2+ is larger because it they are cations and Mg is above Ca;" $\endgroup$– user13411Commented Feb 16, 2015 at 4:08
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3 Answers
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Ca2+ is bigger than Mg2+
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as shown in the above pic Mg2+has more smaller size then Ca2+... I'm sorry but your question is wrong, Why Ca2+ has bigger Ionic Radii then Mg2+? because
No of Shells increases down the group
-Property of Periodic table
therefore ->
As you move down a group in the periodic table , additional layers of electrons are being added, which naturally causes the ionic radius to increase as you move down the periodic table.
you can check reference this for more information
Image source : http://searchpp.com/ionic-radii-periodic-table/
answered Feb 16, 2015 at 19:15
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Mg is smaller the Ca because it is above it in the periodic table, magnesium being a period above it shows that it has one less electron shell so it's smaller, calcium has another ring of electrons, as to say, that are around it so it's radius would be bigger. Your question is wrong.
