Question

Which of the following does not truly represent the property indicated against it?
A.$B{r_2} < C{l_2} < {F_2}:$oxidizing power
B.$Br < Cl < F:$electronegativity
C.$Br < F < Cl:$electron affinity
D.$B{r_2} < C{l_2} < {F_2}:$Bond energy

Answer 1

We have to know that the oxidizing power can be defined on the bases of capacity to oxidize another species. And if the compound undergoes reduction, that compound is known as an oxidizing agent. Electronegativity is the ability to attract the bonding electrons by participating in a covalent bond. And the electron affinity is the change in potential energy of an atom by adding an electron. The bond energy is used to measure the strength of a bond. And the bond strength increases with increasing bond energy.

Complete answer:
The order of oxidizing power of halogen is $B{r_2} < C{l_2} < {F_2}:$. Among the halogens, fluorine has more oxidizing power due to its smaller size. So it can easily accept the electrons. Hence, option (A) is incorrect.
$Br < Cl < F:$is the correct order of electronegativity. The fluorine is more electronegative from the halogen. Because, the atomic radius of fluorine is very small. Therefore, it has more tendency to attract the bond pair of electrons. Hence, the option (B) is incorrect.
The increasing order of electron affinity of halogen is $Br < F < Cl:$. Here, the electron affinity of Cl is more than the F atom. Because, the chlorine size of chlorine is greater than fluorine. And it has more space to accommodate the electrons. Hence, option (C) is incorrect.
Among the options,$B{r_2} < C{l_2} < {F_2}:$is not the correct order of bond energy. And the correct order is ${F_2} < B{r_2} < C{l_2}$. The chlorine has the highest bond energy and fluorine has the least bond energy.

Hence, the option (D) is correct.

Note:
We need to know that Fluorine, chlorine, bromine and iodine are the halogen elements. It has high melting and boiling points. And these are increased when down the group. The atomic radius also increases when down the group due to increasing the number of shells. The electronegativity and oxidizing power also decreases down the group due to increasing the size of atoms.