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Chapter 25: Problem 3

Individually, provide the Lewis structure for 1 -propanol and then predict which bond will be the shortest and what the \(\mathrm{C}-\mathrm{O}-\mathrm{H}\) bond angle will be. When all team members are done, compare answers and reach consensus.

Short Answer

Expert verified
The Lewis structure of 1-propanol has the hydrogen and oxygen forming a single bond. The shortest bond in 1-propanol is the O-H bond due to hydrogen's small atomic size. The \(C-O-H\) bond angle is approximately 104.5 degrees due to the bent shape of the molecule.

Step by step solution

01

Draw Lewis Structure of 1-Propanol

The molecular formula of 1-propanol is \(C_3H_7OH\). Lewis structure is drawn, starting with the central atom and moving outward, arranging atoms to fill the octet of each atom efficiently. The structure of 1-propanol has an oxygen atom connected to the last carbon atom, and a hydrogen atom connected to the oxygen. Since hydrogen can accommodate 2 electrons, oxygen and hydrogen atoms will form a single bond. Remaining hydrogen atoms will form single bonds with the carbon atoms.
02

Predict the Shortest Bond

In order to determine the shortest bond, we look at the bond length. Bond length depends on the atomic size, and since there is a direct bond between hydrogen and oxygen in 1-propanol (O-H), this will be the shortest bond as hydrogen is the smallest atom in this molecule.
03

Predict \(C-O-H\) Bond Angle

The bond angle is determined by the shape of the molecule. In 1-propanol, the central atom is oxygen which forms two sigma bonds with one lone pair, giving it a bent (V-shaped) molecular geometry. According to the VSEPR theory, the lone pair pushes the two hydrogen atoms downward, making a \(C-O-H\) bond angle of approximately 104.5 degrees.

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Most popular questions from this chapter

Find an alkane, a ketone, and an alcohol with roughly the same MW (within \(5 \mathrm{~g} / \mathrm{mole}\) ). Rank these compounds in terms of relative boiling points.

Recall that the electronegativity of \(\mathrm{C}\) and \(\mathrm{H}\) are roughly the same, but that \(\mathrm{O}\) has a significantly higher electronegativity. For each type of compound (alkane, ketone, alcohol) predict whether or not the compound is expected to be polar or nonpolar.

For each type of compound below, indicate how the boiling point changes as the molecular weight of the compound increases: a) alkane b) ketone c) alcohol

Is the strength of intermolecular forces determined by the bond strengths within the individual molecules? Explain your reasoning.
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