![]() If we move down any of the columns, ionic sizes increase due to the increasing principal quantum number of the outermost electrons. Each row in the figure corresponds to an isoelectronic series involving a different noble-gas electron configuration.Īs we move from the more negative to the more positive ions in each row, there is a steady decrease in size. For any electronic series, such as H –, He, Li +, Be 2 +, in which the nuclear charge increases by 1 each time, we find a progressive decrease in size due to the increasingly strong attraction of the nucleus for the electron cloud. Species which have the same electronic structure but different charges are said to be isoelectronic. As we move across each row, the radius of each circle decreases. The final row has T e superscript 2 negative to T l superscript 3 positive. Fourth row has S e superscript 2 negative to I n superscript 3 positive. ![]() Third row has S superscript 2 negative to G a superscript 3 positive. ![]() The second row is N superscript 3 negative to Al superscript 3 positive. The first row is H negative to B e superscript 2 positive. Each row consists of elements as well as ions which have the same number of electrons. ![]() The elements of the periodic table are shown as circles with different radius. Ions in the first row of this figure, H –, Li +, and Be 2 +, all have the same 1 s 2 electronic structure as the helium (He) atom, but differ in size due to the different number of protons each has in their nucleus. This relationship is evident in the following figure comparing ionic radii. The size of an ion is governed not only by its electronic structure but also by its charge. Periodic Table of Elements - Sorted by Ionic Radius. If you need to cite this page, you can copy this text:
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