Author name: tirta

Intermolecular forces in NaCl involve strong electrostatic interactions between the positively charged sodium ions (Na+) and negatively charged chloride ions […]

Butanol’s intermolecular forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. These forces influence physical properties such as boiling

Hydrogen bromide (HBr) exhibits intermolecular forces primarily through dipole-dipole interactions. The polar nature of HBr arises from the electronegativity difference

Carbonyl sulfide (COS) exhibits intermolecular forces that influence its physical properties. Its polarity stems from a dipole moment due to

n-Pentane, a five-carbon alkane, exhibits nonpolar intermolecular forces primarily governed by weak van der Waals interactions. These forces, comprising London

Intermolecular forces (IMFs) are the attractive forces that hold neighboring molecules together. There are three main types of IMFs: dipole-dipole

Carbon monoxide, a nonpolar molecule, experiences only weak intermolecular forces known as van der Waals forces. These forces arise from

In polar molecules, permanent dipole-permanent dipole forces (Keesom forces) arise from the alignment and attraction of permanent dipoles. These intermolecular

Carbon disulfide is a nonpolar molecule with weak intermolecular forces. These forces are primarily London dispersion forces, which are due

Carbon tetrafluoride (CF4) is a nonpolar molecule with a tetrahedral molecular structure. The strong covalent bonds between carbon and fluorine

NaCl’s intermolecular forces arise from electrostatic interactions between positively charged sodium (Na+) and negatively charged chloride (Cl-) ions. The strength

Methane, a nonpolar molecule, primarily experiences London dispersion forces, which arise from temporary fluctuations in electron distribution. These weak intermolecular