Molecular polarity

Molecular polarity is an uneven distribution of electrical charge across a molecule. It arises from polar bonds and their three-dimensional arrangement, producing a net molecular dipole.

Electronegativity: A measure of an atom’s tendency to attract shared electrons in a chemical bond. Electronegativity differences create the uneven electron sharing that makes bonds polar.
Chemical bond: An attraction that holds atoms or ions together through shared or transferred electrons. Molecular polarity depends on how electrons are distributed across chemical bonds.
Solubility: The ability of a substance to dissolve in a specified solvent under defined conditions. Polarity helps predict which solutes interact favorably with a solvent.
Nonpolar molecule: A molecule with no net permanent electric dipole moment. Symmetric arrangements can make a molecule nonpolar despite its polar bonds.
Bond dipole moment: A vector describing charge separation across a chemical bond. Each bond dipole contributes to the molecule’s overall polarity.
Covalent bond: A chemical bond in which atoms share one or more pairs of electrons. Unequal sharing in covalent bonds is a common source of molecular polarity.
Hydrogen bond: An attractive interaction involving hydrogen bonded to an electronegative atom and another electronegative site. Polar bonds enable the strong directional attractions that form hydrogen bonds.
Carbon dioxide: A linear molecule with one carbon atom between two oxygen atoms. Its polar carbon–oxygen bonds cancel because they point in opposite directions.
Molecular geometry: The three-dimensional arrangement of atoms in a molecule. Geometry determines whether bond dipoles reinforce or cancel one another.
Partial charge: A fractional positive or negative charge assigned to an atom within a molecule. Partial charges describe the local charge differences behind molecular dipoles.

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