How can the charge distribution in iodine mon | vedclass

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(B) Iodine $(I)$ has a lower electronegativity $(2.66)$ compared to Chlorine ($Cl$,$3.16$). Due to this difference in electronegativity,the shared pai

Vedclass · Accepted Answer

$I^{\delta+}Cl^{\delta-}$

Vedclass · Answer

(B) Iodine $(I)$ has a lower electronegativity $(2.66)$ compared to Chlorine ($Cl$,$3.16$). Due to this difference in electronegativity,the shared pair of electrons in the $I-Cl$ bond is shifted towards the more electronegative Chlorine atom. This results in the development of a partial negative charge $(\delta-)$ on the Chlorine atom and a partial positive charge $(\delta+)$ on the Iodine atom. Therefore,the charge distribution is represented as $I^{\delta+}Cl^{\delta-}$.

List-$I$ (Molecules)	List-$II$ (Dipole moment)
$A$. $HBr$	$I$. $1.04$
$B$. $H_2S$	$II$. $0$
$C$. $NH_3$	$III$. $0.79$
$D$. $CHCl_3$	$IV$. $0.95$
	$V$. $1.47$

How can the charge distribution in iodine monochloride $(ICl)$ be represented?

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Which of the following molecules does not possess a permanent dipole moment?

Match the following molecules in List-$I$ with their respective dipole moments in List-$II$.
List-$I$ (Molecules) List-$II$ (Dipole moment)
$A$. $HBr$ $I$. $1.04$
$B$. $H_2S$ $II$. $0$
$C$. $NH_3$ $III$. $0.79$
$D$. $CHCl_3$ $IV$. $0.95$
$V$. $1.47$

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