Identify the predominant intermolecular forces between molecules of each of the following compounds:
a. CCl4
b. HF
c. SO2
d. CH3COOH
e. HI
Do you have thoughts. Would b and d be hydrogen bonding? And a would be dispersion forces?
To identify the predominant intermolecular forces between molecules of each of the compounds, we need to consider their molecular structures and the types of bonding present.
a. CCl4 (carbon tetrachloride):
CCl4 is a nonpolar molecule with a tetrahedral shape. The predominant intermolecular force between CCl4 molecules is London dispersion forces. These forces arise due to temporary fluctuations in electron distribution, resulting in temporary dipoles.
b. HF (hydrogen fluoride):
HF is a polar molecule with a linear shape. The predominant intermolecular force between HF molecules is hydrogen bonding. Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom, such as fluorine in this case. The partially positive hydrogen atom of one HF molecule is attracted to the partially negative fluorine atom of another HF molecule, leading to a stronger intermolecular force.
c. SO2 (sulfur dioxide):
SO2 is a polar molecule with a bent shape. The predominant intermolecular force between SO2 molecules is dipole-dipole interactions. The electronegative sulfur atom and the two oxygen atoms create a polar bond, resulting in a partial positive charge on sulfur and partial negative charges on the oxygen atoms. These partial charges attract neighboring molecules, creating dipole-dipole interactions.
d. CH3COOH (acetic acid):
CH3COOH is a polar molecule with a bent shape. The predominant intermolecular forces between CH3COOH molecules are hydrogen bonding and dipole-dipole interactions. The carboxylic acid functional group (-COOH) contains both a polar C=O bond and an -OH group, allowing for both types of intermolecular forces.
e. HI (hydrogen iodide):
HI is a polar molecule with a linear shape. The predominant intermolecular forces between HI molecules are dipole-dipole interactions. The electronegative iodine atom creates a polar bond with the hydrogen atom, resulting in a partial positive charge on hydrogen and a partial negative charge on iodine. These partial charges attract neighboring molecules, leading to dipole-dipole interactions.