Ions are formed when an atom loses or gains electrons.It is defined as the distance from the centre of the nucleus of the ion up to which it exerts its influence on the electron cloud of the ion.Again, this is because the atomic radius decreases in the same direction. The Covalent radius decreases as you move across the periodic table, from left to right.This is because the atomic radius increases in the same direction. The covalent radius increases when we move from top to bottom in a group of the periodic table.Therefore the covalent radius is always shorter than the actual atomic radius.The formation of covalent bonds involves the overlapping of atomic orbitals and it reduces the expected inter-nuclear distance.It is one-half of the inter-nuclear distance between two identical atoms linked together by a single covalent bond.Read more about the Position of Hydrogen in Periodic Table, here. Along with the group, the atomic radius increases from top to bottom as the electron is added to the next principal energy level.Due to this the attraction between nucleus and electrons increases leading to contraction of the atomic radius.At the same time, the number of protons in the nucleus increases i.e. ![]()
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