Amongst the following,the linear species is:

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(D) To determine the shape of the given species,we analyze their structures based on $VSEPR$ theory:$1$. $NO_2$: The nitrogen atom has one unpaired el

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$N_3^-$

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(D) To determine the shape of the given species,we analyze their structures based on $VSEPR$ theory:$1$. $NO_2$: The nitrogen atom has one unpaired electron and two oxygen atoms attached,resulting in a bent shape due to the lone electron and repulsion.$2$. $Cl_2O$: The central oxygen atom has two lone pairs and two bonded chlorine atoms,resulting in a bent shape (similar to $H_2O$).$3$. $O_3$: The central oxygen atom has one lone pair and is bonded to two other oxygen atoms,resulting in a bent shape.$4$. $N_3^-$ (Azide ion): The central nitrogen atom is $sp$ hybridized and bonded to two other nitrogen atoms with no lone pairs on the central atom,resulting in a linear shape.Thus,the linear species is $N_3^-$.

Similar Questions

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

What do you understand by bond pairs and lone pairs of electrons? Illustrate by giving one example of each type.

Identify the number of molecules in which the central atom has one lone pair of electrons from the following list:
$PbCl_2, PH_3, ClF_3, SF_4, BF_3, SnCl_2$

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$i$. $SnCl_2, NH_3, SF_4$
$ii$. $HgCl_2, SO_3, SF_6$
$iii$. $BeCl_2, BF_3, PCl_5$
$iv$. $ClF_3, BrF_5, XeF_6$

The $O-N-O$ bond angle is maximum in:

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