91Ó°ÊÓ

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 ```

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.

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)