Question

Atomic radii of fluorine and neon are given as:
$$\begin{gathered} (a)\text{ 72pm,160pm} \\ (b)\text{ 160pm,160pm} \\ (c)\text{ 72pm,72pm} \\ (d)\text{ none of these} \end{gathered}$$

Answer 1

Hint – Using the idea of the neon having low van der waals in this problem, and the atomic radii decreases from left to right as we shift in a periodic table. This will help to get the right answer for the fluorine and neon atomic radii.

Complete answer:
As we know, neon has low van der waals force, and in neon the electrons are more concentrated, and therefore the attraction force from the nucleus decreases, resulting in greater neon size than fluorine.
And we all know that when we move in the periodic table in the periods the atomic radii decreases from left to right.
Now because we know fluorine and neon are in the same period and the neon is extreme left in the periodic table and the neon atomic radii is smaller than the fluorine.
And the fluorine atomic radius is 160 pm, and the fluorine is 72 pm.

Hence option (D), None of these is the required answer.

Note – Forces of Van der Waals involve attraction and repulsion between atoms , molecules, and surfaces as well as other intermolecular forces. They differ from covalent and ionic bonding, as they are caused by similarities in the fluctuating polarizations of neighboring particles.