Which of the following statements are true?

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(A) $1$. $PH_5, NCl_5$ and $OF_6$ do not exist because $P$ cannot expand its octet to $5$ bonds due to steric hindrance,$N$ lacks $d$-orbitals to form

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$PH_5, NCl_5$ and $OF_6$ do not exist

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(A) $1$. $PH_5, NCl_5$ and $OF_6$ do not exist because $P$ cannot expand its octet to $5$ bonds due to steric hindrance,$N$ lacks $d$-orbitals to form $5$ bonds,and $O$ cannot form $6$ bonds due to its small size and lack of $d$-orbitals. Thus,this statement is true.$2$. $I_3^{-}$ has a linear geometry ($sp^3d$ hybridization with $3$ lone pairs on the central $I$ atom). Thus,this statement is false.$3$. $XeF_4$ has a square planar geometry,which is symmetric,making it non-polar. Thus,this statement is false.$4$. The bond order of $O_2$ is $2.0$ and the bond order of $O_2^{2-}$ (peroxide ion) is $1.0$. Thus,this statement is false.

Order	Property
$(A)$ $NO_2 > O_3 > H_2O$	Bond angle
$(B)$ $H_2O > HF > NH_3$	Dipole moment
$(C)$ $I_2 > F_2 > N_2$	Bond length

Similar Questions

The correct order as indicated in each option is

The correct order for $O-O$ bond length in the given substances is:
$I.$ $H_2O_2$
$II.$ $O_2$
$III.$ $O_3$

Consider the following pairs:
Order Property
$(A)$ $NO_2 > O_3 > H_2O$ Bond angle
$(B)$ $H_2O > HF > NH_3$ Dipole moment
$(C)$ $I_2 > F_2 > N_2$ Bond length

Which of the above pairs are correctly matched?

The angular shape of the ozone molecule consists of

Some of the properties of the two species,$NO_{3}^{-}$ and $H_{3}O^{+}$ are described below. Which one of them is correct?

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