Final Answer:
For the molecule C2H5NO, with four carbon atoms, one nitrogen, and one oxygen, the total number of hybrid orbitals used to describe the molecule is 32.
Step-by-step explanation:
To determine the number of hybrid orbitals used to describe a molecule, we can employ the concept of hybridization, which involves the combination of atomic orbitals to form new hybrid orbitals. In the case of organic compounds like C2H5NO, we need to focus on the central atom(s) and the surrounding atoms to identify the hybridization state.
In C2H5NO, the central atom is nitrogen (N), surrounded by two carbon (C) atoms, five hydrogen (H) atoms, and one oxygen (O) atom. Nitrogen typically forms three sigma (σ) bonds with other atoms. Carbon forms four sigma bonds, and oxygen usually forms two sigma bonds.
For nitrogen in C2H5NO, we can consider its three sigma bonds to be formed by hybridizing its 2s and two 2p orbitals. Therefore, nitrogen undergoes sp2 hybridization.
Each carbon in C2H5NO forms four sigma bonds, suggesting sp3 hybridization for each carbon atom. The oxygen forms two sigma bonds, indicating sp3 hybridization.
So, for the four carbon atoms in C2H5NO, the total number of hybrid orbitals used is 4 (carbons) * 4 (sigma bonds per carbon) = 16 hybrid orbitals.
For the nitrogen atom, the number of hybrid orbitals used is 3 (nitrogen) * 4 (sigma bonds per nitrogen) = 12 hybrid orbitals.
The oxygen atom contributes 4 hybrid orbitals (since it forms two sigma bonds).
Summing up these contributions: 16 (from carbon) + 12 (from nitrogen) + 4 (from oxygen) = 32 hybrid orbitals.
Therefore, C2H5NO can be described using a total of 32 hybrid orbitals.