Down a Group of the Periodic Table from top to bottom, comparing ions with a similar charge, the ionic radius increases as the number of completed energy levels increases.Anions are larger than their respective atoms as electrons are added to the highest energy level (valence shell) the repulsion between the negatively charged electrons increases the ionic radius.Cations are smaller than their respective atoms as electrons are removed from the highest energy level (valence shell) while the positive nuclear charge remains the same thereby increasing the attraction between the remaining electrons and the nucleus resulting in a reduction in the size of the radius of the cation.
Use the data given in the table below to find patterns (trends) in (B) Trends in the Atomic Radius of Elements in Period 3
ATOMIC RADIUS TREND PERIODIC TABLE FREE
No ads = no money for us = no free stuff for you! Trends in Atomic Radius in Groups of the Periodic TableĪs you go down a Group in the Periodic Table from top to bottom, the number of energy levels or electron shells increases so the atomic radius of the elements increases.Ĭompare the number of occupied energy levels (electron shells) and the radius of the atom of elements in Group 1 and in Group 17 as given in each section below: ionic radii of group 17 anions increases down the group.ionic radii of group 1 cations increases down the group.ionic radius of an anion is greater than atomic radius of the atom.ionic radius of a cation is less than atomic radius of the atom.Atomic radius decreases across a period from left to right
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