OpenStax Chemistry 2e - Chapter 10: Liquids and Solids

Vocabulary practice flashcards covering intermolecular forces, liquid properties, phase transitions, phase diagrams, crystalline/amorphous solids, and unit cell lattice structures from Chapter 10 of OpenStax Chemistry 2e.

Intermolecular Forces (IMFs)

The various noncovalent attractive electrostatic forces that exist between the atoms or molecules of a substance.

Intramolecular Forces

The forces, such as covalent bonds, that hold atoms together within an individual molecule.

Dispersion Forces

Fleeting, weak electrostatic forces resulting from the formation of temporary, instantaneous dipoles and induced dipoles in atoms and molecules (also called London dispersion forces).

Polarizability

The measure of how easy or difficult it is for an external electrostatic charge to distort an atom's or molecule's electron charge distribution.

Dipole-Dipole Attractions

Electrostatic attractive forces present only in polar molecules, where adjacent molecules align such that the partial negative pole of one is near the partial positive pole of another.

Hydrogen Bonding

An unusually strong type of dipole-dipole attraction occurring in polar molecules where hydrogen is covalently bonded to a highly electronegative element ($\text{N}$, $\text{O}$, or $\text{F}$).

Viscosity

The measure of a fluid's resistance to gradual deformation or flow.

Cohesive Forces

Intermolecular forces of attraction that bind identical molecules of the same substance to one another.

Adhesive Forces

Forces of attraction between different molecules, such as between liquid molecules and the molecules of a container's surface.

Surface Tension

The energy required to increase the surface area of a liquid, resulting from unbalanced inward cohesive forces acting on surface molecules.

Capillary Action

The spontaneous rise or depression of a liquid inside a narrow tube resulting from the balance between cohesive forces within the liquid and adhesive forces between the liquid and tube walls.

Dynamic Equilibrium (Liquid-Vapor)

The condition reached in a closed container when the rate of vaporization of a liquid equals the rate of condensation of its vapor.

Vapor Pressure

The pressure exerted by a vapor in dynamic equilibrium with its liquid phase in a closed container at a given temperature.

Boiling Point

The temperature at which the equilibrium vapor pressure of a liquid equals the surrounding external atmospheric pressure.

Normal Boiling Point

The temperature at which a liquid's equilibrium vapor pressure equals exactly $1\,\text{atm}$ ($101.3\,\text{kPa}$).

Clausius-Clapeyron Equation

A mathematical equation relating a substance's temperature and vapor pressure: $\ln\left(\frac{P_2}{P_1}\right) = \frac{\Delta H_{\text{vap}}}{R}\left[\frac{1}{T_1} - \frac{1}{T_2}\right]$.

Sublimation

A phase transition directly from the solid state to the gaseous state without passing through an intermediate liquid state.

Deposition

A phase transition directly from the gaseous state to the solid state without passing through an intermediate liquid state.

Triple Point

The unique combination of temperature and pressure at which the solid, liquid, and gas phases of a substance coexist simultaneously in thermodynamic equilibrium.

Critical Point

The temperature and pressure condition on a phase diagram above which distinct liquid and gas phases cease to exist.

Supercritical Fluid (SCF)

A physical state of matter existing at temperatures and pressures beyond the critical point, possessing properties intermediate between those of a liquid and a gas.

Crystalline Solid

A solid substance whose constituent atoms, ions, or molecules are arranged in a regular, repeating, three-dimensional geometric pattern.

Amorphous Solid

A noncrystalline solid (such as glass or fused silica) whose constituent particles lack an ordered, repeating, long-range geometric structure.

Unit Cell

The simplest repeating structural unit that displays the full three-dimensional symmetry and generates an entire crystal lattice when translated in space.

Coordination Number

The number of neighboring atoms or ions in direct contact with a specific central atom or ion within a crystal lattice.

Simple Cubic Structure

A cubic lattice arrangement with atoms located only at the eight corners of the unit cell, characterized by a coordination number of $6$ and containing a net total of $1$ atom per unit cell.

Body-Centered Cubic (BCC) Structure

A cubic unit cell containing atoms at each of the eight corners and one central atom, characterized by a coordination number of $8$ and containing a net total of $2$ atoms per unit cell.

Face-Centered Cubic (FCC) Structure

A cubic unit cell containing atoms at all eight corners and at the center of each of the six faces, characterized by a coordination number of $12$ and containing a net total of $4$ atoms per unit cell.

Cubic Closest Packing (CCP)

A closest-packed crystalline arrangement consisting of three alternating repeating layers ($\text{ABCABC}\dots$) with a coordination number of $12$, which is structurally equivalent to a face-centered cubic unit cell.

Hexagonal Closest Packing (HCP)

A closest-packed crystalline arrangement consisting of two alternating repeating layers ($\text{ABABAB}\dots$) with a coordination number of $12$.

Vacancy Defect

A crystal defect characterized by an unoccupied position where an atom or ion is missing from its normal lattice site.

Interstitial Impurity

A crystallographic defect occurring when an atom occupies an empty space (interstice) between regular lattice points in a crystal.

Substitution Impurity

A crystallographic defect occurring when a regular host atom or ion in a crystal lattice is replaced by an atom or ion of a different element.

X-Ray Diffraction (XRD)

An experimental technique that measures the interference patterns of scattered X-rays passing through a crystalline substance to determine interatomic distances and 3D crystal structure.