(c) Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?

Key Concepts

Hydrogen Bonding

Hydrogen bonding is a specific type of intermolecular force that occurs when a hydrogen atom, covalently bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine, interacts with another electronegative atom. This interaction is characterized by a strong dipole-dipole attraction due to the significant difference in electronegativity, leading to a partial positive charge on the hydrogen and a partial negative charge on the electronegative atom.

Polar Bonds

Polar bonds form when there is a significant difference in electronegativity between two atoms, resulting in an uneven distribution of electron density. This creates a dipole moment, where one end of the bond becomes partially negative and the other partially positive. In the context of hydrogen bonding, the polar bond is crucial as it allows the hydrogen atom to participate in attractive interactions with other electronegative atoms.

Intermolecular Forces

Intermolecular forces are the forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions). These forces are weaker than covalent or ionic bonds and play a significant role in determining the physical properties of substances, such as boiling and melting points. Understanding the different types of intermolecular forces, including hydrogen bonds, dipole-dipole interactions, and London dispersion forces, is essential for predicting the behavior of substances in various states.