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$\text{Hint: Double-bond carbon is sp}^2 \text{ hybridized, triple-bond carbon is sp hybridized and single-bond carbon is sp}^3 \text{ hybridized.}$ $\text{Step 1: Draw the structure of the compound}$ $\text{CH}_3 - \text{CH} = \text{CH}_2$ $\text{sp}^3 \quad \text{sp}^2 \quad \text{sp}^2$ $\text{When carbon is bonded to four other atoms (with no lone electron pairs), the hybridization is sp}^3 \text{ and the arrangement is tetrahedral. Carbon is sp hybridization which occurs when carbon is bound to two other atoms (two double bonds or one single + one triple bond)}$ $\text{Step 2: A carbon atom bound to three atoms (two single bonds, one double bond) is sp2 hybridized and forms a flat trigonal or triangular arrangement with 120° angles between bonds.}$ $\text{Carbon - sp}^2 \text{ hybridization: A carbon atom bound to three atoms (two single bonds, one double bond) is sp}^2 \text{ hybridized and forms a flat trigonal or triangular arrangement with 120° angles between bonds. Notice that acetic acid contains one sp}^2 \text{ carbon atom and one sp}^3 \text{ carbon atom.}$ $\text{Hence the correct option is 3.}$ $\text{CH}_3 - \text{CH} = \text{CH}_2$ $\text{sp}^3 \quad \text{sp}^2 \quad \text{sp}^2$