Chapter 11: Solutions and Their Properties

Vocabulary flashcards derived from Chapter 11 lecture notes on liquid properties, intermolecular forces, and phase change dynamics.

Liquid

A phase of matter where substances take the shape of their container while maintaining a constant volume.

Viscosity

A property of liquids representing the resistance to flow; substances with high viscosity flow slowly (like honey), while those with low viscosity flow easily (like water).

Surface Tension

The result of attractive forces on molecules at the surface of a liquid being drawn inward toward the liquid, measured in $J/m^2$.

Intermolecular Forces

Noncovalent attractions between molecules that are electrical in origin, resulting from the mutual attraction of unlike charges.

Ion-Dipole Forces

Electrical interactions between an ion (solute) and the partial charges on a polar molecule (solvent).

Hydrogen Bonding

An attractive force between a hydrogen atom bonded to a very electronegative atom ($O$, $N$, or $F$) and an unshared electron pair on another electronegative atom.

Dipole-Dipole Forces

Electrical interactions among dipoles on neighboring molecules; as the dipole moment increases, the intermolecular forces and boiling points increase.

London Dispersion Forces

Intermolecular forces present in all molecules resulting from the motion of electrons that creates short-lived, temporary dipoles.

Polarizability

The ease with which the electron cloud of a molecule can be distorted; it increases with size, which in turn increases London dispersion forces and boiling/melting points.

Vapor Pressure

The amount of gas (pressure) created by a liquid in a closed container due to its ability to spontaneously vaporize.

Clausius-Clapeyron Equation

An equation relating the vapor pressure of a liquid to its temperature: $\ln(P_{vap}) = -\frac{\Delta H_{vap}}{R} \left(\frac{1}{T}\right) + C$.

Heat of Vaporization ($\Delta H_{vap}$)

The amount of energy required to convert one mole of a liquid into a gas at a constant temperature.

Fusion

The phase change from a solid to a liquid, also known as melting.

Sublimation

The phase change process where a substance transitions directly from a solid to a gas.

Deposition

The phase change process where a substance transitions directly from a gas to a solid.

Boiling Point

The specific temperature where a liquid's vapor pressure is equal to the external or atmospheric pressure surrounding it.

Phase Diagram

A plot showing the effects of pressure and temperature on a substance, with lines representing combinations where two phases coexist in equilibrium.

Triple Point

The specific point on a phase diagram where solid, liquid, and gas phases all coexist in equilibrium.

Liquid Crystal

An intermediate phase of matter that is ordered like a solid but flows like a liquid.

Nematic Liquid Crystal

A liquid crystal phase where the long axes of the molecules are approximately parallel, similar to the arrangement of bricks.

Smectic Liquid Crystal

The most ordered liquid crystal phase where the long axes of molecules are parallel and their ends are aligned in rows.

Cholesteric Liquid Crystal

A liquid crystal phase where sheets of molecules align parallel in layers that are rotated relative to one another.