Question

The reaction of the type $2{{X}_{2}}+S\to S{{X}_{4}}$ is shown by sulphur when X is
A. Fluorine or chlorine
B. Chlorine only
C. Chlorine and bromine only
D. F, Cl, Br all

Answer 1

Hint: In this question, we are to answer which of the atoms undergoes reaction with the sulphur. On the basis of electronegativity and the size of the atom, we are able to answer this question and choose the correct option.

Complete Step by Step Solution:
We know group 17 are referred as halogens and are known as halogen groups. This group consists of fluorine, chlorine, bromine, iodine and a radioactive element astatine.

Electronegativity is the tendency of an atom to attract the pair of electrons towards itself. As we go down the group, size of the atom goes on increasing and hence electronegativity goes on decreasing. The size of chlorine is smaller and it needs only one electron to have stable noble gas configuration. So the fluorine and chlorine have greater attraction for electrons than that of sulphur.

Fluorine and chlorine are more electronegative than sulphur and are small in size which undergoes the following reaction :
$2{{X}_{2}}+S\to S{{X}_{4}}$
So fluorine and chlorine undergo reaction with the sulphur.
Thus, Option (A) is correct.

Note: We know in a periodic table, bromine is to the right of sulphur and sulphur is further up than bromine. So the sulphur is closer to the fluorine and chlorine. That’s why sulphur undergoes reaction with only fluorine or chlorine.