See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Analysis of Hybridization in n-Allene ($C_3H_4$) **Structure of n-allene:** n-Allene has the structure: $H_2C=C=CH_2$ The three carbon atoms are arranged linearly with two double bonds. **Determine hybridization of each carbon:** 1. **Terminal carbons (C1 and C3):** - Each forms 2 σ-bonds with hydrogen atoms and 1 π-bond with the central carbon - Total: 3 electron groups around each terminal carbon - Hybridization: $sp^2$ 2. **Central carbon (C2):** - Forms 2 π-bonds (one with each terminal carbon) and 0 σ-bonds with other carbons - The two π-bonds lie in perpendicular planes - Total: 2 electron groups around central carbon - Hybridization: $sp$ **Conclusion:** The carbon atoms exhibit both $sp$ (central carbon) and $sp^2$ (terminal carbons) hybridization. **The answer is (B): sp and $sp^2$** --- *Why others are wrong:* - **(A)** includes $sp^3$, which requires 4 electron groups—not present here - **(C)** ignores the central carbon's $sp$ hybridization - **(D)** incorrectly suggests only $sp^2$ hybridization exists