Atomic Radius In Periodic Table

Moving down a group or across a column or row in the modern periodic table, we can observe a lot of trends in the properties (physical and chemical) of elements in basic chemistry. For example: When we move down a group of non-metals, the reactivity of the elements decreases while it increases with moving down the group in case of representative metals.


In basic chemistry, atomic radius is defined as the shortest distance between the atom’s nuclei and the outermost shell of the atom. Measuring the atomic radii of chemical elements is a complicated task as the size of an atom is of the order of 1.2×10-10 m. The electron cloud forming the shell of an atom does not have any fixed shape which makes it difficult to determine the atomic size of an atom. So we can say that practically we cannot determine the size of an individual atom.

Atomic Radius Trends in the Periodic Table

Atomic Radius Trends in the Periodic Table

When two atoms are combined, then we can estimate their atomic size by checking the distance between the atoms. The other method by which we can measure the atomic size of a non-metallic element is by forming a single covalent bond between two atoms and checking the distance between the two atoms. The radius found by this method is known as the covalent radii of the element. In the case of metal, it is termed as a metallic radius. It is defined as half of the total distance between the nuclei of two adjoining metal ions joined by a metallic bond.

The Atomic radius of an atom is measured by X-ray or other spectroscopy methods. The atomic radii of elements vary in the periodic table in a fixed pattern. We can explain this trend by considering the nuclear charge and energy level. In general, atomic radius decreases as we move from left to right in a period and it increases when we go down a group. This is because in periods the valence electrons are in the same outermost shell. The atomic number increases within the same period while moving from left to right which in turn increases the effective nuclear charge. The increase in attractive forces reduces the atomic radius of elements.

It was interesting to see how the force of attraction between electrons and protons plays a major role in increasing or decreasing the atomic radius. To know more about the periodic trends in the properties of elements. Please visit Byju’s.

Practise This Question

Which of the following observations are incorrect for the noble gases - He, Ne, Ar, Kr, and Xe?