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.

Molecule	$P-X$ (axial) bond length / $P-X$ (equatorial) bond length
$PF_5$	$a / b$
$PF_4CH_3$	$c / d$
$PF_3(CH_3)_2$	$e / f$
$PCl_5$	$g / h$

Which of the following has the smallest bond angle?

Similar Questions

Which of the following contains the maximum number of lone pairs on the central atom?

Consider the following information $(X = F$ or $Cl)$:

Molecule $P-X$ (axial) bond length / $P-X$ (equatorial) bond length

$PF_5$ $a / b$

$PF_4CH_3$ $c / d$

$PF_3(CH_3)_2$ $e / f$

$PCl_5$ $g / h$

According to the given information,choose the incorrect order of bond lengths.

Which set of the following molecules has only one lone pair of electrons on their respective central atoms?
$(i)$ $SO_2$
$(ii)$ $XeF_4$
$(iii)$ $PbCl_2$
$(iv)$ $SF_4$
$(v)$ $ClF_3$

The correct pair of species which are not isostructural is

Which of the following pairs of compounds is isoelectronic and isostructural?

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