Question

Predict the ideal values for the bond angles about each carbon atom in the following molecule. Indicate the hybridization of orbitals for each carbon. $${\mathrm{CH}}_3{\mathrm{CCCH}}_2\mathrm{COOH}$$

Short answer

The ideal bond angles around each carbon atom in the given molecule are: 1. C1: 109.5° (sp³) 2. C2: 120° (sp²) 3. C3: 120° (sp²) 4. C4: 109.5° (sp³) 5. C5: 120° (sp²)

Step-by-step solution

(Step 1: Drawing the Lewis Structure)

Draw the complete Lewis structure of the given molecule: ${\mathrm{CH}}_3{\mathrm{CCCH}}_2\mathrm{COOH}$. The lewis structure of the given molecule is: ``` H O O | | // H-C-CH=CH-CH2-C | | H H ```

(Step 2: Identify Hybridization and Bond Types)

Examine each carbon atom and its bonding pattern to determine the hybridization. 1. The first carbon (C1) is bonded to three hydrogen atoms through single bonds and one carbon through a single bond; this indicates sp³ hybridization. 2. The second carbon (C2) is bonded to one hydrogen atom through a single bond, one carbon through a single bond, and a double bond with another carbon; this indicates sp² hybridization. 3. The third carbon (C3) is bonded to two hydrogen atoms through single bonds and has a double bond with another carbon; this indicates sp² hybridization. 4. The fourth carbon (C4) is bonded to two hydrogen atoms through single bonds and one carbon through a single bond, thus sp³ hybridization. 5. The fifth carbon (C5) has a single bond with an oxygen, a single bond with a carbon, and a double bond with an oxygen, indicating sp² hybridization.

(Step 3: Predicting Ideal Bond Angles)

Using the information on hybridization, we can predict the ideal bond angles for each carbon. 1. For sp³ hybridized carbon (C1 and C4), the ideal bond angle is 109.5°. 2. For sp² hybridized carbon (C2, C3, and C5), the ideal bond angle is 120°. So, the ideal bond angles around each carbon are: 1. C1: 109.5° (sp³) 2. C2: 120° (sp²) 3. C3: 120° (sp²) 4. C4: 109.5° (sp³) 5. C5: 120° (sp²)