Final answer:
Carbon dioxide contains an sp hybridized atom. The central carbon in CO2 exhibits sp hybridization because it is surrounded by two regions of valence electron density, which correspond to the two double bonds with oxygen, creating a linear molecule.
Step-by-step explanation:
The molecule that contains an sp hybridized atom among the options given is Carbon dioxide (CO2). In Carbon dioxide, each oxygen atom forms a double bond with the carbon atom, creating a linear molecule, which means that the carbon atom is surrounded by just two regions of valence electron density. Such an arrangement exhibits sp hybridization. Consequently, the carbon atom in CO2 has two sp hybrid orbitals that form sigma bonds with the oxygen atoms, and it retains two unhybridized p orbitals that form pi bonds with oxygen. Other examples of sp hybridization include acetylene (H-C≡C-H) and the mercury atom in linear HgCl2.