Which of the following pairs is isostructural?

Give the correct order of initials $T$ or $F$ for following statements. Use $T$ if statement is true and $F$ if it is false:
$(I)$ The order of repulsion between different pair of electrons is $lp-lp > lp-bp > bp-bp$.
$(II)$ In general,as the number of lone pair of electrons on the central atom increases,the deviation of the bond angle from the normal bond angle increases.
$(III)$ The number of lone pairs on $O$ in $H_2O$ is $2$,while on $N$ in $NH_3$ is $1$.
$(IV)$ The structures of xenon fluorides and xenon oxyfluorides could not be explained on the basis of $VSEPR$ theory.

The shape of $O_2F_2$ is similar to that of

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.

Compare the $x$ and $y$ bond angles for the given molecules.

Match the following:
$($Molecule$/$Ion$)$  $($Shape$)$
$A. I_3^- \rightarrow  4.$ Linear  
$B. ClF_3 \rightarrow  1.$ $T-$shaped  
$C. H_2O \rightarrow  3.$ Angular  
$D. SF_4 \rightarrow  2.$ See$-$Saw