How many of the following molecules / ions ha | vedclass

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(B) To determine the geometry,we look at the hybridization and lone pairs of each species:$1$. $BO_3^{3-}$: Central atom $B$ has $3$ bonding pairs and

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$2$

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(B) To determine the geometry,we look at the hybridization and lone pairs of each species:$1$. $BO_3^{3-}$: Central atom $B$ has $3$ bonding pairs and $0$ lone pairs ($sp^2$ hybridization). Geometry: Trigonal planar.$2$. $NH_3$: Central atom $N$ has $3$ bonding pairs and $1$ lone pair ($sp^3$ hybridization). Geometry: Trigonal pyramidal.$3$. $PCl_3$: Central atom $P$ has $3$ bonding pairs and $1$ lone pair ($sp^3$ hybridization). Geometry: Trigonal pyramidal.$4$. $BCl_3$: Central atom $B$ has $3$ bonding pairs and $0$ lone pairs ($sp^2$ hybridization). Geometry: Trigonal planar.$5$. $ClF_3$: Central atom $Cl$ has $3$ bonding pairs and $2$ lone pairs ($sp^3d$ hybridization). Geometry: $T$-shaped.$6$. $XeO_3$: Central atom $Xe$ has $3$ bonding pairs and $1$ lone pair ($sp^3$ hybridization). Geometry: Trigonal pyramidal.Thus,only $BO_3^{3-}$ and $BCl_3$ have a trigonal planar structure. The total count is $2$.

How many of the following molecules / ions have trigonal planar structure?
$BO_3^{3-}, NH_3, PCl_3, BCl_3, ClF_3, XeO_3$

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How many of the following molecules / ions have trigonal planar structure?$BO_3^{3-}, NH_3, PCl_3, BCl_3, ClF_3, XeO_3$