If an element 'X' is assumed to have the types of radii, then their order is

Covalent radius is of an atom is about 20% shorter, because the formation of covalent bond involves overlapping of atomic orbitals.

The metallic radius is 10% larger.

The van der waals radius of an atom is usually 40% larger than the atomic radius, because the non-bonded atoms of the molecules are held together by weak attractive forces.

Hence, Van der waals radius > Crystal radius > Covalent radius.