Question

Which of the following is the correct statement?
A.\[{F_2}\] has higher dissociation energy than $C{l_2}$
B.\[F\] has higher electron affinity than $Cl$
C.$HF$ is stronger acid than $HCl$
D.Boiling point increases down the group in halogens

Answer 1

Hint: We need to know and understand a certain group of elements of the periodic table known as halogens. The halogens are a set of five chemically related elements in the periodic table: fluorine, chlorine, bromine, iodine, and astatine. Tennessine, an artificially produced element, may also be a halogen. This group is designated as group 17 in modern IUPAC nomenclature.

Complete answer:
The halogens are a group of non-metal elements in Periodic Table Group 17 of the periodic table. As more electron shells are filled, atoms grow larger as they move down the group. The F–F bond is very weak when fluorine occurs as a diatomic molecule. This is due to the fact that fluorine atoms are the smallest of the halogens—the atoms are linked close together, resulting in repulsion between free electrons in the two fluorine atoms. Because the strength of Van der Waals forces increases with atomic size and relative atomic mass, the boiling temperatures of halogens rise along the group.

Hence, the correct option is option (D).

Note:
It must be noted that \[{F_2}\] has higher dissociation energy than $C{l_2}$; $Cl$ has higher electron affinity than \[F\] and $HF$ is weaker acid than $HCl$ due to higher bond energy. Electronegativity decreases down the group. One of the most reactive elements is fluorine. It interacts with inert materials such as glass and creates compounds with heavier noble gases. It is a very caustic and poisonous gas. Fluorine's reactivity implies that when it reacts with anything, it forms such strong bonds that the resultant molecule is inert and non-reactive.