For each of the following molecules, indicate the...

For each of the following molecules, indicate the hybridization of each carbon atom and give the approximate values of all the bond angles: a. $\quad \mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{CH}$ b. $\quad \mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}$ c. $\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}$

For each of the following molecules, indicate the hybridization of each carbon atom and give the approximate values of all the bond angles:
a. $\quad \mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{CH}$
b. $\quad \mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}$
c. $\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}$

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Key Concepts

Orbital Hybridization

Orbital hybridization refers to the process in which atomic orbitals mix to create new hybrid orbitals that define the geometry of covalent bonding. In organic molecules, carbon commonly adopts sp, sp2, or sp3 hybridization states, which correspond respectively to linear (180° bond angles), trigonal planar (120° bond angles), and tetrahedral (approximately 109.5° bond angles) arrangements. This concept is crucial for understanding molecular shapes and reactivities.

Molecular Geometry and Bond Angles

The overall shape of a molecule is determined by the hybridization of its atoms, which in turn dictates the bond angles. For instance, a carbon atom in a triple bond (sp hybridization) will have a linear geometry with bond angles of 180°, while in a double bond (sp2 hybridization) the geometry is trigonal planar with bond angles around 120°, and in a single bond (sp3 hybridization) the geometry is tetrahedral with bond angles near 109.5°. This understanding helps predict the three-dimensional configuration of organic molecules.

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