Molecular Interactions and Properties Quiz

Atoms in a molecule are held together by the electrostatic force of attraction between positively charged protons and negatively charged electrons.

Solubility is the ability of a substance (solvent) to dissolve in another substance (solute) to form a homogeneous mixture.

Viscosity is the measure of a liquid's resistance to flow; higher viscosity indicates slower flow.

Covalent bonding involves the sharing of electrons between atoms, leading to the formation of molecules.

Sublimation is the process where a solid transforms directly into a gas without undergoing the liquid phase.

Methane (CH4) is a nonpolar molecule, as it has a symmetrical tetrahedral shape with equal sharing of electrons.

Hydrogen bonding involves the attraction between a hydrogen atom and a highly electronegative atom, such as oxygen or nitrogen.

The high boiling point of water is due to the strong hydrogen bonding between water molecules.

Hexane, with a larger number of electrons, exhibits stronger London dispersion forces among nonpolar molecules.

Ionic compounds conduct electricity in the solid state due to the movement of ions.

Dipole-dipole interactions involve the attraction between molecules with permanent dipoles.

The boiling point is reached when the vapor pressure of a liquid matches the external pressure, leading to the liquid turning into vapor.

Van der Waals forces encompass London dispersion forces, which result from temporary dipoles, and dipole-dipole interactions between molecules.

Water has the highest boiling point among the given substances due to its strong hydrogen bonding.

Bond dissociation energy is the energy needed to break one mole of bonds in a gaseous substance.

Ammonia (NH3) experiences strong hydrogen bonding due to the presence of a highly electronegative nitrogen atom.

Water has the highest surface tension among the given substances due to its strong cohesive forces.