Select the single best answer. Which of the following describes the bonding in the hydrogen cyanide molecule, HCN? As N is \( s p \)-hybridized. C uses \( s p \) hybridized orbitals in bonding. C uses \( s p^{2} \) hybridized orbitals in bonding. C uses \( s p^{3} \) hybridized orbitals in bonding. C uses \( s p^{3} d \) hybridized orbitals in bonding.

In the hydrogen cyanide (HCN) molecule, carbon is indeed \( sp \)-hybridized. This is because carbon forms a triple bond with nitrogen while also bonding with hydrogen, resulting in a linear shape. The hybridization leads to one \( s \) orbital mixing with one \( p \) orbital, creating two \( sp \) hybrid orbitals for that linear geometry, which best supports the bonding arrangement in HCN. Furthermore, the overall geometry of the HCN molecule is linear due to the arrangement of the \( sp \)-hybridized orbitals. This bonding structure is crucial for understanding the chemical behavior of HCN, including its reactivity and interactions with other molecules, making it an essential concept in organic and inorganic chemistry.