In which of the following,are the molecules a | vedclass

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Question

(A) The bond angles for the given molecules are as follows:$H_2O$: The bond angle is $104.5^{\circ}$ due to two lone pairs on the oxygen atom.$NH_3$:

Vedclass · Accepted Answer

$H_2O < NH_3 < SO_2$

Vedclass · Answer

(A) The bond angles for the given molecules are as follows:$H_2O$: The bond angle is $104.5^{\circ}$ due to two lone pairs on the oxygen atom.$NH_3$: The bond angle is $107^{\circ}$ due to one lone pair on the nitrogen atom.$SO_2$: The bond angle is $119.5^{\circ}$ due to the $sp^2$ hybridization of the sulfur atom.Comparing these values,the increasing order of bond angles is $H_2O Therefore,the correct option is $A$.

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

In which of the following,are the molecules arranged in the increasing order of their bond angles?

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The molecular shapes of $SF_4$,$CF_4$,and $XeF_4$ are:

Which of the following is the correct decreasing order of bond angles?

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.

Identify the pair in which the geometry of the species is $T$-shape and square pyramidal,respectively.

Bond angle is minimum for

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