A tetrahedral shape corresponds to sp3 hybridization.

The carbon atoms in benzene are sp2 hybridized, forming a planar structure with 120-degree bond angles.

The nitrogen in a primary amine is sp3 hybridized.

Nitrogen in amines is sp3 hybridized due to the presence of three substituents and a lone pair.

In acetylene, each carbon atom is sp hybridized, forming a triple bond between them.

In CO2, the carbon atom forms two double bonds with oxygen atoms, indicating sp hybridization.

In ethylene, each carbon atom is sp2 hybridized, forming a double bond with the other carbon.

The carbon atoms in ethyne (C2H2) are sp hybridized due to the triple bond between them.

The carbon atoms in alkenes are sp2 hybridized due to the presence of a double bond.

In alkynes, the carbon atoms involved in the triple bond are sp hybridized.

The carbon atoms in benzene are sp2 hybridized, forming a planar structure with 120-degree bond angles.

The carbon atoms in ethylene (C2H4) are sp2 hybridized due to the presence of a double bond.

In ethyne, the carbon atoms are sp hybridized due to the presence of a triple bond.

The carbon atoms in the double bond of alkenes are sp2 hybridized.

A tetrahedral shape corresponds to sp3 hybridization.

In CH4, the central carbon atom forms four equivalent bonds with hydrogen atoms, indicating sp3 hybridization.

The carbon atom in CO2 is sp hybridized, forming two double bonds with oxygen atoms.

Oxygen in H2O is sp3 hybridized, forming two bonds and two lone pairs.

The central nitrogen atom in N2O is sp hybridized, leading to a linear arrangement.

The central nitrogen atom in NH3 is sp3 hybridized due to three bonding pairs and one lone pair.

The central atom nitrogen in NH4+ undergoes sp3 hybridization to form four equivalent bonds with hydrogen.

The central oxygen atom in O3 is sp2 hybridized, leading to a bent molecular shape.

In ozone (O3), the central oxygen atom is sp2 hybridized, resulting in a bent molecular shape.

In PCl5, phosphorus is sp3d hybridized, allowing for five bonding pairs.

The central sulfur atom in SF6 is surrounded by six fluorine atoms, leading to an octahedral geometry and sp3d2 hybridization.

The sulfur atom in SO2 is sp2 hybridized, forming one double bond and one single bond.

The xenon atom in XeF4 is dsp3 hybridized, resulting in a square planar geometry.

In [Ni(CN)4]2-, nickel is in the +2 oxidation state and undergoes dsp2 hybridization to accommodate the four cyanide ligands.

In [Cu(NH3)4]2+, the copper ion undergoes dsp2 hybridization to accommodate four ligands.

In [Ni(CO)4], the nickel ion undergoes sp3 hybridization to accommodate four CO ligands.