What is a dipole moment?

A dipole moment is a quantitative measure of the separation of positive and negative charges in a molecule. It reflects how much the electron density is unevenly distributed within the molecule due to differences in electronegativity between bonded atoms. The dipole moment can be calculated as the product of the magnitude of the charge and the distance between the centers of positive and negative charge. This is why the correct choice is the product of charge and distance between charge centers. It is this very concept that allows chemists to predict the polarity of molecules, which has implications in molecular interactions, solubility, and reactivity.

In contrast, other options do not accurately describe what a dipole moment represents. The distance between two bonded atoms pertains to bond length, which is different from the idea of charge distribution. Bond energy refers to the strength of the bond between atoms, not the charge separation. Lastly, hybridization is a concept related to the mixing of atomic orbitals to form new hybrid orbitals, and it is not directly related to the dipole moment. Understanding the nature and significance of dipole moments is crucial for interpreting chemical behavior in polarity and intermolecular forces.