Question

consider the molecule below. determine the hybridization at each of the 2 labeled carbons.

○ c1 = sp², c2 = sp³d
○ c1 = sp², c2 = sp²
○ c1 = sp³d², c2 = sp³d²
○ c1 = sp², c2 = sp³
○ c1 = sp³, c2 = sp²

Explanation:

• For \(C1\):
• Carbon \(C1\) is double - bonded to another carbon. In a double - bonded carbon, the hybridization is \(sp^{2}\). The double - bonded carbon has three regions of electron density (two single bonds and one double bond). According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, when the number of electron - pair domains (\(n\)) around an atom is \(3\), the hybridization is \(sp^{2}\) (\(n = 3\), and the formula for hybridization is \(sp^{n - 1}\)).
• For \(C2\):
• Carbon \(C2\) is single - bonded to three hydrogen atoms and one carbon atom. So, it has four regions of electron density. When the number of electron - pair domains (\(n\)) around an atom is \(4\), according to the VSEPR theory, the hybridization is \(sp^{3}\) (\(n=4\), and using the formula \(sp^{n - 1}\)).

Answer:

C1 = \(sp^{2}\), C2 = \(sp^{3}\) (the fourth option in the given multiple - choice list)