what intermolecular forces are present in each: Potassium nitrate, Naphthalene, and benzoic Acid?
To determine the intermolecular forces present in each compound, we need to consider the types of chemical bonds and the molecular structure of the compounds.
1. Potassium Nitrate (KNO3):
Potassium nitrate consists of potassium ions (K+) and nitrate ions (NO3−). The ions are held together by ionic bonds, which are the strongest type of chemical bond. In the solid state, potassium nitrate forms a crystal lattice structure in which the ions are held together by electrostatic attractions. Therefore, the dominant intermolecular force in potassium nitrate is the ionic bond.
2. Naphthalene (C10H8):
Naphthalene is an organic compound composed of carbon and hydrogen atoms. Its molecular structure consists of two benzene rings fused together. Within each benzene ring, there are delocalized electrons that create a temporary dipole. These temporary dipoles induce dipole-dipole forces between adjacent naphthalene molecules. Additionally, naphthalene molecules can also experience London dispersion forces. These forces arise from temporary fluctuations in electron density, resulting in temporary dipoles. Overall, the dominant intermolecular forces in naphthalene are dipole-dipole forces and London dispersion forces.
3. Benzoic Acid (C6H5COOH):
Benzoic acid is a carboxylic acid with a benzene ring and a carboxyl group (-COOH). The carboxyl group contains a highly polarized carbon-oxygen double bond (C=O) and a polar O-H bond. The polar nature of these bonds allows for the formation of hydrogen bonds between neighboring benzoic acid molecules. In addition to hydrogen bonding, benzoic acid can also experience dipole-dipole forces and London dispersion forces. However, hydrogen bonding is the dominant intermolecular force in benzoic acid.
In summary, the dominant intermolecular forces in potassium nitrate are ionic bonds, while naphthalene exhibits dipole-dipole forces and London dispersion forces. Benzoic acid, on the other hand, demonstrates hydrogen bonding along with dipole-dipole forces and London dispersion forces.