Which of the following is not linear?

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(C) To determine the geometry,we calculate the hybridization and number of lone pairs using the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is

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$I_3^+$

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(C) To determine the geometry,we calculate the hybridization and number of lone pairs using the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is valence electrons,$M$ is monovalent atoms,$C$ is cationic charge,and $A$ is anionic charge.$1$. For $IBrF^-$: $H = \frac{1}{2}(7 + 2 + 1) = 5$ ($sp^3d$ hybridization). With $2$ bonding pairs and $3$ lone pairs in equatorial positions,the shape is linear.$2$. For $ICl_2^-$: $H = \frac{1}{2}(7 + 2 + 1) = 5$ ($sp^3d$ hybridization). With $2$ bonding pairs and $3$ lone pairs,the shape is linear.$3$. For $I_3^+$: $H = \frac{1}{2}(7 + 2 - 1) = 4$ ($sp^3$ hybridization). With $2$ bonding pairs and $2$ lone pairs,the shape is bent (angular).$4$. For $I_3^-$: $H = \frac{1}{2}(7 + 2 + 1) = 5$ ($sp^3d$ hybridization). With $2$ bonding pairs and $3$ lone pairs,the shape is linear.Therefore,$I_3^+$ is not linear.

$X = x$	$1$	$2$	$3$	$4$	$5$	$6$	$7$	$8$
$P(X = x)$	$0.15$	$0.23$	$K$	$0.10$	$0.20$	$0.08$	$0.07$	$0.05$

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