Question

Which of the following is correct regarding $H-X$ bond polarity?

• A. $H-F>H-Cl>H-Br>H-I$
• B. $H-I>H-Cl>H-Br>H-F$
• C. $H-I>H-F>H-Br>H-Cl$
• D. $H-F>H-Br>H-Cl>H-I$

Answer 1

The correct option is A $H-F>H-Cl>H-Br>H-I$

$H-X$ bonds are between a hydrogen and a halogen.

Polarisation :- When electronegative difference between the atoms is high, the more electronegative atoms tends to attracts the electrons of the less electronegative atom iducing partial positive ${\delta }^{+}$ and partial negative ${\delta }^{-}$ charge to the less electronegative atom respectively.

Among the halogens the electronegativity of halogen is as follows

$F^{-}>{Cl}^{-}>{Br}^{-}>I^{-}$

Fluorine, being the most electronegative atom will attract the electrons of hydrogen atom mole.

So, the $H-X$ bond polarity is as follows.

$H-F>H-Cl>H-Br>H-I$.