The species in which the central atom uses sp | vedclass

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(C) To determine the hybridization,we use the formula: $	ext{Steric Number} = 	ext{Number of sigma bonds} + 	ext{Number of lone pairs}$.For $H_3C^{

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$H_3C^{+}$

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(C) To determine the hybridization,we use the formula: $	ext{Steric Number} = 	ext{Number of sigma bonds} + 	ext{Number of lone pairs}$.For $H_3C^{+}$,the carbon atom is bonded to $3$ hydrogen atoms and has $0$ lone pairs. $	ext{Steric Number} = 3 + 0 = 3$,which corresponds to $sp^2$ hybridization.For $NH_3$,$PH_3$,and $SbH_3$,the central atoms are bonded to $3$ atoms and have $1$ lone pair. $	ext{Steric Number} = 3 + 1 = 4$,which corresponds to $sp^3$ hybridization (though in $PH_3$ and $SbH_3$,the bond angles are close to $90^{\circ}$ due to the lack of significant hybridization,often described as using pure $p$-orbitals).

The species in which the central atom uses $sp^2$ hybrid orbitals in its bonding is

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The number of species from the following in which the central atom uses $sp^3$ hybrid orbitals in its bonding is . . . . . . .
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