Question

Which of the following options are not in accordace with the property mentioned against them?

• A. $HI<HBr<HCl<HF$
  Hydrogen halogen bond strength
• B. $F_2>C{l}_2>B{r}_2>I_2$
  Bond dissociation
• C. $MI>MBr>MCl>MF$
  Ionic character of metal halide.
• D. $F_2>C{l}_2>B{r}_2>I_2$
  Oxidizing power

Answer 1

Answer: (B), (C)

$MI>MBr>MCl>MF$

Ionic character of metal halide.
Option (A):

oxidizing power decreases down the group as the tendecy to accept the electrons decreases down the group.

Therefore, order $F_2>C{l}_2>B{r}_2>I_2$
Oxidizing power is true.
Therefore, it matches against the property mentioned and hence incorrect option for the given quetion.

Option (B)

Ionic character of metal halide decreases down the group since the size of halide io $X^{-}$ increases down the group as per fajan's rule

$MI>MBr>MCl>MF$ for ionic character is incorrect, the correct order is:

$MI>MBr>MCl>MF$
Therefore, it dose not match against the property mentioned and hence correct option for the given question.

Option(C):

Generally the bond dissociation energy decreases down the group as bond length increases down the group.

$F_2>C{l}_2>B{r}_2>I_2$ for the bond dissociation is incorrect. The correct order is:
$C{l}_2>B{r}_2>F_2>I_2$

Due to smaller size of florine and more number of lone pairs, it experiences more inter electronic repulsion and hence bond between fluorine atoms weakens.
Therefore,it dose not match against the property mentioned and hence correct option for given question.

Option (D):

Hydrogen-Halogen bond strength decreases down the group as the bond lenght between HX increase down the group

$HI<HBr<HCl<HF$ for Hydrogen - Halogen bond strenght is correct because down the group atomic size increases and therefore bond lenght increases thus bond strenght decreases.
Therefore,it matches against the property mentioned and hence incorrect option for the given question.