Which of the following molecules can be repre | vedclass

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(C) To determine the $AB_nE_m$ type for a molecule,we identify the central atom $(A)$,the number of atoms bonded to it $(B)$,and the number of lone pa

Vedclass · Accepted Answer

$H_2O$

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(C) To determine the $AB_nE_m$ type for a molecule,we identify the central atom $(A)$,the number of atoms bonded to it $(B)$,and the number of lone pairs on the central atom $(E)$:$1$. For $SO_2$: The central atom $S$ has $2$ bond pairs and $1$ lone pair,so it is $AB_2E$.$2$. For $H_2O_2$: The structure is $H-O-O-H$. Each oxygen atom is bonded to $2$ atoms and has $2$ lone pairs,but it is not a simple $AB_2E_2$ system due to the $O-O$ bond.$3$. For $H_2O$: The central oxygen atom is bonded to $2$ hydrogen atoms $(B=2)$ and has $2$ lone pairs $(E=2)$. Thus,it is $AB_2E_2$.$4$. For $XeF_2$: The central xenon atom is bonded to $2$ fluorine atoms $(B=2)$ and has $3$ lone pairs $(E=3)$. Thus,it is $AB_2E_3$.Therefore,the correct molecule is $H_2O$.

List-$I$	List-$II$
$a. NH_3$	$i$. Square pyramidal
$b. ClF_3$	$ii$. Trigonal bipyramidal
$c. PCl_5$	$iii$. Trigonal pyramidal
$d. BrF_5$	$iv$. $T$-shape

Which of the following molecules can be represented as $AB_2E_2$,where $A$ is the central atom,$B$ represents bond pairs of electrons,and $E$ represents lone pairs of electrons?

Similar Questions

The increasing order of the number of lone pairs of electrons on the central atom of the following molecules is:
$I) \ ClF_3$
$II) \ XeF_2$
$III) \ SF_4$
$IV) \ SiH_4$

Match List-$I$ with List-$II$ :
List-$I$ List-$II$
$a. NH_3$ $i$. Square pyramidal
$b. ClF_3$ $ii$. Trigonal bipyramidal
$c. PCl_5$ $iii$. Trigonal pyramidal
$d. BrF_5$ $iv$. $T$-shape

Choose the correct answer from the options given below :

The shape of $O_2F_2$ is similar to which of the following?

What is the $H-S-H$ bond angle in $H_2S$ (in $^{\circ}$)?

Which of the following molecules possesses a three-fold axis of symmetry?

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