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Chapter 10: Problem 78

Levulinic acid has the formula $\mathrm{CH}_{3}(\mathrm{CO}) \mathrm{CH}_{2} \mathrm{CH}_{2}$ COOH. Sketch the levulinic acid molecule, and indicate the various bond angles.

Short Answer

Expert verified
Levulinic acid is a chain of 5 carbon atoms: begins with a CH3 group, has a CO group followed by two CH2 groups and ends with a COOH group. The bond angles are approximately 109.5° for C-H, 120° for C=C and O=C, and 104.5° for O-H.

Step by step solution

01

Identify the elements in the molecule and their bonds

The levulinic acid molecule is comprised of Carbon (C), Hydrogen (H), and Oxygen (O) atoms. The compound contains single and double bonds, where single bonds are represented by a single line (-) and double bonds are represented by a double line (=). Identify and list down all the atomic symbols that we are going to use.
02

Sketch the structural formula of the levulinic acid molecule

Draw the Structural formula according to the formula of levulinic acid. It is CH3(CO)CH2CH2COOH. Carbon atom in methyl group (CH3) will have bond angles of 109.5°. Carbon atoms in (CO), (CH2) and (CH2) should form a straight chain having 120° angle with double bonded Oxygen and the rest two bonds with the hydrogen atoms or Carbon atoms will be 109.5°. And the carbon atom that bound with hydroxyl group (-COOH) will have 120° bond angle with oxygen atom of hydroxyl group.
03

Indicate the bond angles

Label the bond angles on your drawn structure. Atom in the center holds the bond angles. The bond angles for C-H bonds is 109.5°, for C=C is 120° and for O-H in COOH group is approximately 104.5°

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Most popular questions from this chapter

Sketch the propene molecule, \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

Write a plausible Lewis structure for \(\mathrm{C}_{3} \mathrm{O}_{2},\) a substance known as carbon suboxide.

Suggest reasons why the following do not exist as stable molecules: (a) \(\mathrm{H}_{3} ;\) (b) \(\mathrm{HHe} ;\) (c) \(\mathrm{He}_{2}\); (d) \(\mathrm{H}_{3} \mathrm{O}\).

Briefly describe each of the following ideas: (a) formal charge; (b) resonance; (c) expanded valence shell; (d) bond energy.

Use the VSEPR theory to predict the shape of (a) the molecule OSF \(_{2} ;\) (b) the molecule \(\mathrm{O}_{2} \mathrm{SF}_{2} ;\) (c) the ion \(\mathrm{SF}_{5}^{-} ;\) (d) the ion \(\mathrm{ClO}_{4}^{-} ;\) (e) the ion \(\mathrm{ClO}_{3}^{-}\).
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