Use the References to access important values if needed for this question. What type(s) of intermolecular forces are expected between
molecules? H H H H H-C-C-C-C-C-C-O-H H H H H H H Indicate with a Y (yes) or an N (no) which apply. dipoles forces induced dipole forces Y hydrogen bonding N
The Correct Answer and Explanation is:
The correct answer is:
- Dipole forces: Y (yes)
- Induced dipole forces: Y (yes)
- Hydrogen bonding: Y (yes)
Explanation:
The given molecular structure represents hexanol, an alcohol with six carbon atoms and a hydroxyl (-OH) functional group. The intermolecular forces present in hexanol molecules include dipole-dipole interactions, induced dipole forces, and hydrogen bonding.
Dipole-dipole interactions occur due to the hydroxyl group, which is polar because of the significant difference in electronegativity between oxygen and hydrogen. This creates a permanent dipole where the oxygen atom attracts electron density, making it partially negative, while the hydrogen becomes partially positive. These interactions lead to electrostatic attraction between adjacent molecules, contributing to hexanol’s relatively high boiling point.
Induced dipole forces, also known as London dispersion forces, are present because hexanol contains a long hydrocarbon chain. These forces arise due to temporary shifts in electron density within the molecules, causing weak attraction between nonpolar regions. Although London dispersion forces are weaker than dipole-dipole interactions, they become more significant as the molecular size increases, affecting properties like solubility and volatility.
Hydrogen bonding is another major intermolecular force in hexanol. This type of interaction occurs when hydrogen is directly bonded to highly electronegative atoms such as oxygen. The hydroxyl group allows hydrogen bonds to form between molecules, significantly increasing the boiling point compared to hydrocarbons of similar molecular weight.
All three types of intermolecular forces contribute to hexanol’s physical properties. The presence of hydrogen bonding makes it more soluble in water than nonpolar compounds, while London dispersion forces influence interactions within nonpolar solvents. These forces collectively determine hexanol’s behavior in different environments, from solubility patterns to phase transitions and boiling point trends.
