Question

draw the lewis structure of ch₃cch and then choose the appropriate set of hybridization states for the three central atoms. your answer choice is independent of the orientation of your drawn structure.

Explanation:

Step1: Determine the structure of \(CH_3CCH\)

The formula \(CH_3CCH\) can be written as \(H_3C - C\equiv C - H\).

Step2: Analyze the hybridization of the first \(C\) atom (\(CH_3 - C\))

The first \(C\) atom (connected to \(CH_3\)) has 4 regions of electron density (4 single bonds). According to the VSEPR theory, when an atom has 4 regions of electron density, it is \(sp^3\) hybridized.

Step3: Analyze the hybridization of the middle \(C\) atom (\(C\equiv C\))

The middle \(C\) atom (in the triple bond) has 2 regions of electron density (one triple bond and one single bond). When an atom has 2 regions of electron density, it is \(sp\) hybridized.

Step4: Analyze the hybridization of the last \(C\) atom (\(C\equiv C\))

The last \(C\) atom (in the triple bond) also has 2 regions of electron density (one triple bond and one single bond). So, it is \(sp\) hybridized.

Answer:

The Lewis structure of \(CH_3CCH\) is \(H - C - C\equiv C - H\) with the first \(C\) (connected to \(CH_3\)) being \(sp^3\) hybridized, the middle \(C\) (in the triple bond) being \(sp\) hybridized, and the last \(C\) (in the triple bond) being \(sp\) hybridized.