Atomic radius is one of the periodic properties of the elements. If you look at the table, you can see there is a clear trend in atomic radius. While the atomic radius follows a similar trend, ions may be larger or smaller than neutral atoms. Atomic Radius Trend on the Periodic Table The size of neutral atoms is drawn from the atomic radius, which is half the distance between two atoms that are just touching each other.But for the nonmetallic elements, the ionic radius increases because there are more electrons than protons. Consequently, the size of the atom (and its covalent radius) must increase as we increase the distance of the outermost electrons from the nucleus. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly. Ionic radius decreases moving from left to right across a row or period.This trend in atomic radius is best understood in terms of the effective nuclear. Atomic size gradually decreases from left to right across a period of elements. Atomic radius increases right to left across a period on the periodic table. The electron cloud size determines the atomic radius for an atom. Atomic radius patterns are observed throughout the periodic table. This is because each row adds a new electron shell. To find atomic radius, atoms are assumed to be spheres. As you move down a column or group, the ionic radius increases.The size of an element's ionic radius follows a predictable trend on the periodic table.

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. Periodic Trends Last updated Periodic Properties of the Elements Periodic Trends in Ionic Radii Periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of a certain element, including its size and its electronic properties.

Atomic size trend on periodic table