In the following reaction,how do the Cl-P-Cl | vedclass

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(D) In $PCl_5$,the geometry is trigonal bipyramidal with bond angles of $120^\circ$ (equatorial) and $90^\circ$ (axial).In the product $PCl_4^+$,the p

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Some increase and some decrease

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(D) In $PCl_5$,the geometry is trigonal bipyramidal with bond angles of $120^\circ$ (equatorial) and $90^\circ$ (axial).In the product $PCl_4^+$,the phosphorus atom undergoes $sp^3$ hybridization,resulting in a tetrahedral geometry with bond angles of $109.5^\circ$.Comparing the angles: The $120^\circ$ angles decrease to $109.5^\circ$,while the $90^\circ$ angles increase to $109.5^\circ$.Therefore,some angles increase and some decrease.

List-$I$ (Molecule)	List-$II$ (Shape)
$A$. $NH_3$	$I$. Square pyramid
$B$. $BrF_5$	$II$. Tetrahedral
$C$. $PCl_5$	$III$. Trigonal pyramidal
$D$. $CH_4$	$IV$. Trigonal bipyramidal

In the following reaction,how do the $Cl-P-Cl$ bond angles change?
$PCl_5 \longrightarrow PCl_4^+ + Cl^-$

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

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

$A$. $NH_3$ $I$. Square pyramid

$B$. $BrF_5$ $II$. Tetrahedral

$C$. $PCl_5$ $III$. Trigonal pyramidal

$D$. $CH_4$ $IV$. Trigonal bipyramidal

Choose the correct answer from the options below:

Consider the molecules $CH_4$,$NH_3$ and $H_2O$. Which of the given statements is false?

The group having triangular planar structures is

Which is the $CORRECT$ relation of bond angles?

The group of molecules having identical shape is

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In the following reaction,how do the $Cl-P-Cl$ bond angles change?$PCl_5 \longrightarrow PCl_4^+ + Cl^-$