What is the predominant intermolecular force responsible for the dissolution of the hydrophilic end of
soap in water? Using dashed lines, illustrate where the intermolecular force occurs between atoms in
adjacent molecules? Lone pair electrons have been omitted in the molecules drawn below. Add lone
pair electrons to all atoms as needed. Indicate bond polarity, if the molecules contain polar bonds,
using ä+ and ä-� symbols where appropriate.
H2 H2 H2 H2 H2 H2
H3C-C-C-C-C-C-C-C-C-C-C-C-C=O H-O-H
H2 H2 H2 H2 H2 H2-O^- H-O-H
You can see that spacing is a problem.
The intermolecular force responsible for the dissolution of the hydrophilic end of soap in water is hydrogen bonding.
To identify hydrogen bonding and illustrate where it occurs between atoms in adjacent molecules, we need to consider the bonding structure and the presence of lone pair electrons.
In the given illustration, we have a molecule of soap with a hydrophilic end and a hydrophobic end.
First, let's focus on the hydrophilic end of soap, which is the part of the molecule that will interact with water.
Here is the breakdown of the hydrophilic end of soap molecule:
H3C-C-C-C-C-C-C-C-C-C-C-C-C=O
To determine where hydrogen bonding occurs, we need to identify the atoms that are capable of forming hydrogen bonds. In this case, we have an oxygen atom bonded to a hydrogen atom (H-O) in water, and this is where hydrogen bonding can occur.
To represent the hydrogen bonding, we use dashed lines between the oxygen in water (H2O) and the hydrogen in the hydrophilic end of soap (H-O-H).
The hydrogen bonding can be depicted as follows:
H2 H2 H2 H2 H2 H2
H3C-C-C-C-C-C-C-C-C-C-C-C-C=O H-O-H
H2 H2 H2 H2 H2 H2-O^- H-O-H
In this illustration, the dashed lines represent the hydrogen bonds that form between the oxygen atom in water and the hydrogen atoms in the soap molecule.
Moreover, it's important to note that the oxygen atom in water has lone pair electrons, which are not explicitly shown in the given illustration. These lone pair electrons are crucial for the formation of hydrogen bonds.
Remember that hydrogen bonds are a specific type of dipole-dipole interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and is attracted to another electronegative atom nearby.
The predominant intermolecular force responsible for the dissolution of the hydrophilic end of soap in water is hydrogen bonding.
Hydrogen bonding occurs between the hydrogen atom of one molecule and the electronegative atom (oxygen or nitrogen) of another molecule. In this case, the hydrogen bonding occurs between the oxygen atoms in water (H-O-H) and the oxygen atom in the hydrophilic end of soap (C=O).
The dashed lines in the diagram illustrate the hydrogen bonding interactions between the atoms in adjacent molecules.
Here's an updated diagram:
H
|
H2 H2 H2 H2 H2 H2
H3C-C-C-C-C-C-C-C-C-C-C-C-C=O
H2 H2 H2 H2 H2 H2-O^-
|
H-O-H
In the soap molecule, the oxygen atom in the carbonyl group (C=O) has a partial negative charge (δ-) due to its higher electronegativity compared to carbon and hydrogen atoms. The oxygen atoms in water have a partial positive charge (δ+) due to the hydrogen atoms being slightly positively charged (δ+). The interaction between δ- and δ+ results in the formation of hydrogen bonds.