Question

To recognize what intermolecular forces are present in a given compound and which of those forces is predominant. Chemists use the term intermolecular forces to describe the attractions between two or more molecules. Dipole-dipole forces result from the attraction of the positive end of one polar molecule to the negative end of another polar molecule. Compounds consisting of atoms with different electronegativities may have a dipole moment, or partial charge, caused by an asymmetry of electrons.

A) London dispersion forces
B) Dipole-dipole forces
C) Hydrogen bonding
D) Ionic forces

Answer 1

The predominant intermolecular forces can include dipole-dipole forces, London dispersion forces, hydrogen bonding, and ionic forces.

Step-by-step explanation:

The intermolecular forces that can be present in a compound include dipole-dipole forces, London dispersion forces, hydrogen bonding, and ionic forces.

Dipole-dipole forces occur between polar molecules and result from the attraction of the positive end of one polar molecule to the negative end of another polar molecule.

London dispersion forces, also known as van der Waals forces, occur between all molecules and are caused by temporary fluctuations in electron charge distribution.

Hydrogen bonding is a strong type of dipole-dipole interaction that occurs between molecules with a hydrogen atom bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine.

Ionic forces result from the electrostatic attraction between ions in a compound. The predominant intermolecular force in a given compound depends on its molecular structure and the types of atoms or ions present.