Lecture 24 – Partial Pressures, Solids, Liquids, and Changing States

These flashcards cover key vocabulary and concepts related to partial pressures, states of matter, and the properties of solids and liquids as discussed in Lecture 24.

Partial pressure

The contribution of a given gas in a mixture to the total pressure.

Dalton’s law

The total pressure exerted by a gas is the sum of the partial pressures of the components in the mixture.

Atmospheric pressure

The sum of the partial pressures of all the gases in the atmosphere, typically 1 atm.

Viscosity

The measure of a liquid’s resistance to flowing; increases with stronger intermolecular forces.

Surface tension

The energy required to increase the surface area of a liquid due to intermolecular forces.

Crystalline solids

Solids in which the atoms, molecules, or ions are rigidly held in an ordered arrangement.

Ionic solids

Solids composed of ions held together by ionic bonds in a regular three-dimensional arrangement.

Molecular solids

Crystalline solids made of molecules held together by intermolecular forces.

Covalent Networks

Solids where individual atoms are held together by covalent bonds in giant three-dimensional arrays.

Metallic solids

Solids where metal atoms are held together by metallic bonds, allowing for free movement of valence electrons.

Amorphous solids

Solids whose constituent particles are randomly arranged with no long-range structure.

Vapor pressure

The partial pressure of vapor molecules in equilibrium with a liquid.

Heat of Fusion (Hfus)

The quantity of heat required to completely melt one gram of a substance at its melting point.

Heat of Vaporization (Hvap)

The quantity of heat needed to completely vaporize a liquid at its boiling point.

Normal boiling point

The temperature at which boiling occurs at a pressure of exactly 1 atmosphere.