Which of the following has the least bond ang | vedclass

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Question

(C) The bond angles for the given molecules are as follows:$BeF_2$: $180^o$ ($sp$ hybridization,linear geometry).$CH_4$: $109^o 28'$ ($sp^3$ hybridiza

Vedclass · Accepted Answer

$H_2O$

Vedclass · Answer

(C) The bond angles for the given molecules are as follows:$BeF_2$: $180^o$ ($sp$ hybridization,linear geometry).$CH_4$: $109^o 28'$ ($sp^3$ hybridization,tetrahedral geometry).$NH_3$: $107^o$ ($sp^3$ hybridization,one lone pair,pyramidal geometry).$H_2O$: $104.5^o$ ($sp^3$ hybridization,two lone pairs,bent geometry).Due to the presence of two lone pairs on the oxygen atom in $H_2O$,the $lp-lp$ repulsion is greater than the $lp-bp$ repulsion in $NH_3$,resulting in the smallest bond angle among the given options. Thus,the correct option is $(C)$.

List-$I$ (Molecule)	List-$II$ (Shape)
$A. SF_4$	$I. T\text{-shaped}$
$B. ClF_3$	$II. \text{Square planar}$
$C. BrF_5$	$III. \text{See-saw}$
$D. XeF_4$	$IV. \text{Square pyramidal}$

Which of the following has the least bond angle?

Similar Questions

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Here $X$ is a gas and $Y$ is a liquid and both are triatomic molecules. The number of electron lone pairs present on the central atoms of $X$ and $Y$ are respectively.

Which molecule is linear?

In which of the following is the bond angle maximum?

The shape of $O_2F_2$ is similar to that of:

Match the molecules in List-$I$ with their respective shapes in List-$II$.
List-$I$ (Molecule) List-$II$ (Shape)
$A. SF_4$ $I. T\text{-shaped}$
$B. ClF_3$ $II. \text{Square planar}$
$C. BrF_5$ $III. \text{See-saw}$
$D. XeF_4$ $IV. \text{Square pyramidal}$

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