![]() ![]() Why does radius increase with higher atomic numbers in a group? 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. While the atomic radius follows a similar trend, ions may be larger or smaller than neutral atoms.But for the nonmetallic elements, the ionic radius increases because there are more electrons than protons. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly. As we begin our summary of periodic trends, recall that the single most important unifying principle in understanding the chemistry of the elements is the systematic increase in atomic number, accompanied by the orderly filling of atomic orbitals by electrons, which leads to periodicity in such properties as atomic and ionic size, ionization ene. This is because in periods, the valence electrons are in the same outermost shell. In general, the atomic radius decreases as we move from left to right in a period, and it increases when we go down a group. Ionic radius decreases moving from left to right across a row or period. Summary Atomic radius The atomic radius is the distance from the atomic nucleus to the outermost electron orbital in an atom.This is because each row adds a new electron shell. As you move down a column or group, the ionic radius increases.Number of shells increases atomic radius increases. The size of an element's ionic radius follows a predictable trend on the periodic table. Number of protons increases nuclear charge increases atomic size decreases.To find the value, ions are treated as if they were hard spheres. The ionic radius is half the distance between atomic ions in a crystal lattice. ![]()
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