Observe the following molecules: PCl_5, BrF_5 | vedclass

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(C) To determine the geometry,we calculate the hybridization and the number of lone pairs for each molecule:$1$. $PCl_5$: $sp^3d$ hybridization,trigon

Vedclass · Accepted Answer

$3$

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(C) To determine the geometry,we calculate the hybridization and the number of lone pairs for each molecule:$1$. $PCl_5$: $sp^3d$ hybridization,trigonal bipyramidal geometry.$2$. $BrF_5$: $sp^3d^2$ hybridization with $1$ lone pair,square pyramidal geometry.$3$. $ClF_5$: $sp^3d^2$ hybridization with $1$ lone pair,square pyramidal geometry.$4$. $PF_5$: $sp^3d$ hybridization,trigonal bipyramidal geometry.$5$. $ClF_3$: $sp^3d$ hybridization with $2$ lone pairs,$T$-shaped geometry.$6$. $XeF_4$: $sp^3d^2$ hybridization with $2$ lone pairs,square planar geometry.$7$. $XeF_2$: $sp^3d$ hybridization with $3$ lone pairs,linear geometry.$8$. $IF_5$: $sp^3d^2$ hybridization with $1$ lone pair,square pyramidal geometry.Thus,the molecules with square pyramidal geometry are $BrF_5, ClF_5$,and $IF_5$.The total count is $3$.

Observe the following molecules: $PCl_5, BrF_5, ClF_5, PF_5, ClF_3, XeF_4, XeF_2, IF_5$. The number of molecules having square pyramidal geometry from the above is:

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