Honors Chemistry: Liquids, Solids, Changes of State, and Solutions

Flashcards based on lecture notes for Honors Chemistry, covering liquids, solids, changes of state, and solutions.

liquid

The least common state of matter is the __ state.

narrow

Liquids can exist only within a relatively __ range of temperature and pressure.

Attractive

__ forces between liquid particles are significant.

ordered

Particles in a liquid are more __ than particles in a gas.

lower

The average kinetic energy of particles in the liquid state is generally __ than the average kinetic energy of those particles in the gas state.

Temperature

__ is a measure of the average kinetic energy of the particles in a sample of matter.

definite

Liquids have a __ volume.

shape

Liquids take the __ of their container.

fluids

Liquids (and gases) are __.

high

Liquids have a relatively __ density compared to gases.

incompressible

Liquids are relatively __.

diffuse

Liquids will __ through other liquids (if they will dissolve).

slower

Diffusion is __ between liquids than between gases.

faster

Diffusion is __ at higher temperatures.

surface

All liquids exhibit __ tension to varying degrees.

hydrogen

Water has a high surface tension due to __ bonds.

capillary action

The tendency of a liquid to rise up a narrow tube is called __.

meniscus

The curve a liquid forms in such items as test tubes or graduated cylinders is called __.

Viscosity

__ is the resistance of a liquid to flow.

Solid

__ particles are closely packed.

Attractive forces

__ exert stronger effects in the solid state than in the liquid state.

fixed

Solid particles are in relatively __ positions but they do move in place

less

Ice is __ dense than liquid water

low

There is an extremely __ rate of diffusion between solids

crystalline

The majority of solids are __ solids.

Crystalline

__ solids have defined melting points.

Crystal

_ = a substance in which the particles are arranged in an orderly, geometric, repeating pattern

Unit cell

= simplest repeating unit of a crystal

Crystal lattice

= unit cells repeated over and over in a definite geometric arrangement (similar to bricks or blocks)

rare

A perfect crystal is __.

hydrates

Some ionic crystals can form __

Hydrate

= a solid ionic compound containing water molecules incorporated into its solid crystal structure

Anhydrous salt

_= an ionic compound that remains after the water has been removed from a hydrate (usually by heating)

Amorphous

__ solids have No defined melting point

Amorphous

__ solids are Without shape; no crystal form

Vapor

_ = gas phase of a substance that is normally a solid or liquid at room temperature

matter

Closed system = system in which __ cannot enter and leave the system (but energy can enter and leave)

Vaporization

= a general term for the process by which a liquid changes to a gas

Evaporation

= the process by which particles escape from the surface of a non-boiling liquid and enter the gas state (evaporation is a type of vaporization)

Volatile Liquid

_ = a liquid that will evaporate readily

Nonvolatile Liquid

_ = a liquid that will evaporate slowly

Equilibrium

_ a dynamic condition in which two opposing physical or chemical changes occur at equal rates in a given closed system

equilibrium

If the system is at __, vaporization and condensation will occur at equal rates but there will be no net change

Equilibrium Vapor Pressure

= the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature

increase

Equilibrium vapor pressure will __ as temperature increases

Le Châtelier’s Principle

__ - When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress

Boiling

- the conversion of a liquid to a vapor within the liquid as well as at its surface

Boiling

__- Boiling occurs when a liquid’s equilibrium vapor pressure is equal to the external pressure on the liquid (often atmospheric pressure).

Boiling Point

the temperature at which the equilibrium vapor pressure of a liquid is equal to the external pressure on the liquid (often atmospheric pressure)

Normal Boiling Point

__ of water = 100C

Triple Point

- indicates the temperature and pressure conditions at which the solid, liquid, and gas (vapor) of a substance can coexist at equilibrium

Critical Point

- indicates the critical temperature and critical pressure of a substance

Critical Temperature

the temperature above which a substance cannot exist in the liquid state no matter how high the pressure exerted

Mixture

__= matter that can be separated into two or more pure substances by physical changes

Homogeneous

mixture = a mixture that is uniform in composition throughout an entire sample

Heterogeneous

_mixture = a mixture that is not uniform in composition throughout an entire sample

Suspension

__= a heterogeneous mixture that separates on standing

Colloid

= a heterogeneous mixture that does not separates on standing

Solution

__= a homogeneous mixture

Tyndall Effect

__= visible pattern caused by the reflection of light from dispersed particles in a colloid

Sol

= solid dispersed in liquid

Gel

= solid network extending throughout liquid

Liquid emulsion

= liquid dispersed in liquid

Foam

= gas dispersed in liquid

Smoke

= solid dispersed in gas

Fog

= liquid dispersed in gas

Brownian Motion

= the random continuous motions of colloidal particles

Solvent

= the substance that does the dissolving in a solution

Solute

= the substance being dissolved in a solution

Aqueous Solution

= a solution in which water is the solvent

Alloy

_= a solid solution in which the atoms of two or more metals are uniformly mixed

Solution Concentration

= a measure of the amount of solute in a given amount of solvent or solution

Molarity

= the number of moles of solute per one liter of solution