Which of the following has the smallest bond | vedclass

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(B) To determine the bond angle,we look at the hybridization and the number of lone pairs on the central atom: $1$. $BeF_2$: $sp$ hybridization,linear

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$H_2O$

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(B) To determine the bond angle,we look at the hybridization and the number of lone pairs on the central atom: $1$. $BeF_2$: $sp$ hybridization,linear geometry,bond angle = $180^{\circ}$. $2$. $CH_4$: $sp^3$ hybridization,tetrahedral geometry,bond angle = $109.5^{\circ}$. $3$. $NH_3$: $sp^3$ hybridization,one lone pair,bond angle = $107^{\circ}$. $4$. $H_2O$: $sp^3$ hybridization,two lone pairs,bond angle = $104.5^{\circ}$. Due to the presence of two lone pairs on the oxygen atom in $H_2O$,the lone pair-lone pair repulsion is greater than the lone pair-bond pair repulsion,which compresses the bond angle to $104.5^{\circ}$,the smallest among the given options.

List-$I$ (Molecule)	List-$II$ (Shape)
$A$. $BrF_5$	$I$. $T$-shape
$B$. $H_2O$	$II$. See-saw
$C$. $ClF_3$	$III$. Bent
$D$. $SF_4$	$IV$. Square pyramidal

Which of the following has the smallest bond angle?

Similar Questions

Match List-$I$ with List-$II$:

List-$I$ (Molecule) List-$II$ (Shape)

$A$. $BrF_5$ $I$. $T$-shape

$B$. $H_2O$ $II$. See-saw

$C$. $ClF_3$ $III$. Bent

$D$. $SF_4$ $IV$. Square pyramidal

Which of the following orders cannot be explained by back bonding?

According to $VSEPR$ theory,in which species do all the atoms lie in the same plane?
$1.$ $CH^{+}_3$
$2.$ $CH^{-}_3$

Statement $I$ : $SO_2$ and $H_2O$ both possess $V$-shaped structure.
Statement $II$ : The bond angle of $SO_2$ is less than that of $H_2O$.
In the light of the above statements,choose the most appropriate answer from the options given below:

In a $AX_2L_n$ compound,if $X$ is a bond pair and $n$ is the number of lone pairs of electrons,which of the following options is incorrect?

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