Vander Waal's radius : This is one-half of the distance between the nuclei of two adjacent atoms belonging to two neighbouring molecules of an element in the solid state.
The covalent radius is always smaller than the corresponding vander Waal's radius. This is due to the fact that in the formation of the chemical bond, two atoms should come near each other. It also explains why the covalent bonds are stronger than the vander Waal's forces. It is significant to note that since the noble gases ordinarily do not form any covalent bond, in crystals of noble gases, no chemical forces are operating among the atoms. Therefore the vander Waal's forces are the only attractive forces in these cases. Or we can say that, the vander Waal's radii constitute the atomic radii of noble gases and as vander Waal's radii are larger than the covalent radii, atomic radii of the noble gases are largest in their respective periods (anomaly).
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