Question

predict the type of hybrid orbitals used by each of the indicated inner atoms.
part 1

1. 2. 3.

1 = sp; 2 = sp²; 3 = sp²
1 = sp²; 2 = sp; 3 = sp³
1 = sp³; 2 = sp²; 3 = sp³
1 = sp²; 2 = sp²; 3 = sp³
1 = sp; 2 = sp; 3 = sp²

Explanation:

Step1: Determine hybridization for atom 1

Atom 1 is part of a double - bond. In \(sp^{2}\) hybridization, an atom has three equivalent hybrid orbitals and one un - hybridized p orbital. A double - bonded carbon (assuming these are carbon atoms in a hydrocarbon chain) has \(sp^{2}\) hybridization.

Step2: Determine hybridization for atom 2

Atom 2 is also part of a double - bond. Using the same logic as for atom 1 (carbon in a double - bond), it has \(sp^{2}\) hybridization.

Step3: Determine hybridization for atom 3

Atom 3 is part of a single - bond (assuming it is bonded to two hydrogens and one carbon). In \(sp^{3}\) hybridization, an atom has four equivalent hybrid orbitals. A carbon in a single - bonded (saturated) environment has \(sp^{3}\) hybridization.

Answer:

\(1 = sp^{2};2 = sp^{2};3 = sp^{3}\) (the fourth option in the given choices)