Chapter 11: Liquids and Chapter 12: Solids

Flashcards covering key concepts from Chapters 11 and 12 on liquids and solids, including properties, behaviors, and types of substances.

Viscosity

The resistance of a liquid to flow, related to the ease with which molecules can move past each other.

Surface Tension

The force that causes the surface of a liquid to behave like a stretched elastic membrane, influenced by intermolecular forces.

Capillary Action

The ability of a liquid to flow in narrow spaces without the assistance of external forces, resulting from the balance of cohesive and adhesive forces.

Phase Change

The conversion of a substance from one state of matter to another, involving energy changes.

Heat of Fusion

The energy required to change a solid into a liquid at its melting point.

Heat of Vaporization

The energy required to convert a liquid into a gas at its boiling point.

Critical Temperature

The temperature above which a gas cannot be liquefied regardless of the pressure applied.

Supercritical Fluid

A state of matter that occurs when a substance is above its critical temperature and pressure, exhibiting properties of both gas and liquid.

Intermolecular Forces

Forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions), crucial for determining the physical properties of substances.

Cohesive Forces

Intermolecular forces that cause similar molecules to attract each other.

Adhesive Forces

Intermolecular forces that cause a substance to be attracted to a surface.

Crystalline Solids

Solids with a regular, repeating arrangement of atoms or molecules.

Amorphous Solids

Solids that lack a long-range order in the arrangement of atoms.

Metallic Bonding

The bonding that occurs in metallic solids, characterized by the sharing of a 'sea' of delocalized electrons among positively charged metal ions.

Electron-Sea Model

A model describing metallic bonding where electrons are not associated with any specific atom and are free to move around.

Phase Diagram

A graphical representation of the states of a substance as a function of temperature and pressure, showing phase changes.

Clausius Clapeyron Equation

An equation describing the relationship between pressure and temperature during phase transitions.

Heating Curve

A graph depicting temperature changes of a substance as heat is added or removed, showing phase changes.

Alloy

A mixture of two or more elements, where at least one is a metal, with properties distinct from those of its individual components.

Physical characteristics of gases

Composed of nonmetallic laments, expand to fill their container, highly compressible, have extremely low densities

Atmospheric pressure

Weight of air per unit of area

Manometer

Measure the difference in pressure between atmospheric pressure and that of a gas in a vessel

Boyles law

The volume of fixed quantity of gas at constant temp is inversely proportional to pressure

Charles law

The volume of a fixed amount of gas at constant pressure is directly proportional to its absolute temp

Avogadro law

The volume of a gas at a constant temp and pressure is directly proportional to the number of moles of gas

STP

one mol of any gas occupies 22.4 L

average kinetic energy of mol

At any given temp it is the same , if a gas has a low mass the speed with be greater than for a heavier molecule

Ump

Most probable speed

Uav

Average speed of the molecules

Urms

Root mean square speed, associated with their kinetic energy

Effusion

The escape of gas molecules through a tiny hole into evacuated space

Diffusion

The spread of one substance throughout a space or second substance

Mean free path

The average distance a particle travels between collisions

Grahams law

The molar mass of two gases to their rate of speed of travel

The lighter gas always has a

Faster rate of speed

liquid properties

Assumes shape of portion of container it occupies

Does not expand to fill its container, flows, virtually incompressible, diffuses slowly

Solid

Does not flow, virtually incompressible, does not expand, diffusion occurs very slow

Vapor pressure

Having enough energy to escape the surface and become a gas