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Solids, Liquids, and Gases Terms
Solids, Liquids, and Gases Terms
Adhesive Forces
The attractive forces between unlike molecules.
Amorphous Solids
A solid that does not have a repeating, regular three-dimensional arrangement of particles.
Aqueous
Water, made up of water
Avogadro's Law
Equal volumes of an ideal gas contain equal numbers of molecules if both volumes are at the same temperature and pressure.
Boiling Point (or Vaporization)
The temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure.
Boiling Point Elevation
The boiling point of a solution is higher than the boiling point of the pure solvent (colligative property).
Boyle's Law
The pressure of an ideal gas is inversely proportional to its volume if the temperature and amount of gas is held constant.
Capillary Action
The movement of a liquid along the surface of a solid caused by the attraction of molecules of the liquid to the molecules of the solid.
Charles' Law
The volume of a gas is directly proportional to its temperature if pressure and amount of gas remain constant.
Chemical Process
A method of changing one or more chemicals or chemical compounds.
Cohesive Forces
The intermolecular forces which cause a tendency in liquids to resist separation.
Colligative Properties
Properties of a solution that depend on the number of solute molecules present but not on the identity of the solute.
Combined Gas Law
The gas law that combines Boyle's Law, Charles' Law, and Gay-Lussac's Law.
Compound
A substance that is formed from more than one kind of atom chemically bound together. For example, carbon dioxide (CO2) and sodium chloride (NaCl) are compounds because each one has two kinds of atoms that are bound by covalent or ionic bonds. Oxygen (O2) is not a compound, however, because it has one single kind of atom (O). Oxygen is referred to a diatomic molecule.
Compressibility
A measure of the volume change of a fluid or solid as a response to a pressure.
Condensation
Change water from gas to liquid, act of making something denser
Condensed Phase
Either the solid or liquid phase of a substance.
Covalent Bond
A very strong attraction between two or more atoms that are sharing their electrons.
Covalent Crystal
A crystal in which the structure is maintained by covalent bonds.
Crystal Lattice
A three-dimensional array of points that embodies the pattern of repetition in a crystalline solid.
Crystalline Solid
A solid that possesses long-range order at the atomic or molecular level in its structure.
Dalton's Law of Partial Pressures
The total pressure exerted by a mixture of gases is the sum of the partial pressure of the individual gases.
Density
Density is a measure of an object's mass in comparison to its volume (density= mass/volume). Density can increase either by increased mass or by decreased volume. Picture a jar of raisins and a jar of peanut butter. If both jars are the same size, the peanut butter would have a higher mass and consequently a higher density. To increase the density of the raisins you would have to either increase the mass of the raisins (squash more and more raisins into the original jar) or decrease the volume (take the same amount of raisins from the original jar and squash them into a smaller jar).
Deposition
The transition from a gas to a solid.
Dissociation
When ionic substances dissolve their ions while surrounded by solvent molecules and separated from each other.
Effusion
Gas molecules in a container escape from tiny pinholes into a vacuum with the same average velocity they have inside the container.
Electrostatic Force
A phenomenon resulting from slow-moving electrical charges.
Element
An element is a substance composed of atoms with identical atomic number.
Evaporation
Vaporization of a liquid below its boiling point.
Filtration
The act of passing a liquid or gas through a filter to remove solid particles.
Fluid
Substances (gases and liquids) that flow freely.
Freezing
The conversion of a liquid into a gas.
Freezing Point
The temperature at which the vapor pressure of a liquid is equal to the vapor pressure of the corresponding solid.
Freezing Point Depression
The freezing point of a solution is lower than the freezing point of the pure solvent (colligative property).
Gas
Matter in a form that has low density, is easily compressible, expands spontaneously when placed in a larger container, and has particles that are far apart and move freely
Graham's Law
The rates of effusion of gases are inversely proportional to the square roots of their molecular weights or densities.
Heat
A means by which energy is transferred from a hot body to a colder body when the two are placed in thermal contact with one another.
Heterogeneous
Diverse, different, not all alike
Homogeneous
Alike, "homo" is together/similar/the same
Hydrogen Bond
Strong dipole-dipole forces between molecules X-H … Y, where X and Y are small electronegative atoms and H denotes the hydrogen bond.
Hydrostatic Pressure
The pressure exerted by a liquid when it is at rest.
Ideal Gas
A gas whose pressure P, volume V, and temperature T are related by PV = nRT, where n is the number of moles of gas and R is the ideal gas law constant.
Ideal Gas Law
The product of pressure and the volume of an ideal gas is directly proportional to the number of moles of the gas and the temperature.
Intermolecular Force
An attraction or repulsion between molecules.
Ionic Crystal
A crystal held together by Coulomb attractions.
Kinetic Energy
The energy an object possesses as a result of its motion.
Kinetic Molecular Theory
A collection of postulates that describe the behavior of molecules in a gas.
Liquid
A state of matter that has a high density, low compressibility, takes the shape of their container, and possesses particles that are close together but are still able to flow.
Mass
The quantity of matter in a body.
Matter
Anything that has mass and volume.
Melting
The process of a solid becoming a liquid.
Melting Point
The temperature at which liquid and solid coexist in equilibrium.
Metallic Crystal
A crystal in which the atoms are linked by electrons shared in delocalized valence orbitals.
Mixture
A sample of matter composed of two or more substances each of which retains its own identity and properties.
Molality
Concentration of a solution measured as moles of solute per kilogram of solvent.
Molarity
Concentration measured as the number of moles of solute per liter of solution.
Mole Fraction
Concentration of a substance in a mixture measured as moles of the substance per mole of mixture.
Molecular Crystal
A crystal in which groups of strongly linked atoms or molecules are held in position by weak intermolecular interactions.
Osmotic Pressure
The pressure that develops in a solution separated from a solvent by a membrane permeable only to the solvent.
Partial Pressure
The independent pressure exerted by different gases in a mixture.
Particle
The building block of matter usually in the form of atoms, molecules, or ions.
Phase
A sample of matter that is uniform throughout both in its chemical composition and in its physical state.
Phase Diagram
A map that shows which phases of a substance are most stable for a given set of pressure and volume conditions.
Physical Change
A change where the identity of the chemical does not change, but the phase does. For example, melting ice is an example of physical change because frozen H2O and liquid H2O are both still just H2O.
Pressure
Force per unit area.
Raoult's Law
Applies to a gas-liquid mixture when a gas is highly soluble in a liquid and relates the mole fractions of the species in the liquid and gas phases.
Saturated Solution
A solution in equilibrium with a solid state.
Solid
A dense rigid state of matter with a definite volume and shape whose particles are packed close together.
Solubility
The solubility of a substance is its concentration in a saturated solution.
Soluble
Able to be dissolved or able to be solved (depending on the context in which you see the word).
Solute
A substance dissolved in a solvent to make a solution.
Solution
The solutions of quadratic equations are the same as the roots of quadratic equations. The solutions of a quadratic equation are the values of x for which the equation equals zero. They are also the x-intercepts of the function.
Solvent
A solid, liquid, or gas that causes another substance to dissolve. Water is a top-notch solvent.
Standard Pressure
Standard pressure has a pressure of 1 atmosphere (atm).
Standard Temperature
Standard temperature is a temperature of 0ºC.
Standard Temperature and Pressure (STP)
Conditions in which pressure is 1 atm and temperature is 0ºC
Sublimation
The process of a solid becoming a gas.
Substance
A sample of matter that has the same chemical composition and physical properties.
Surface Tension
The force per unit length used to overcome the microscopic forces between molecules at the liquid-air interface.
Suspension
A heterogeneous mixture in which solute particles settle out of a solvent after some time has passed.
Temperature
A property associated with the hotness or coldness of an object.
Triple Point
The state at which all three phases coexist in equilibrium.
Unit Cell
The simplest arrangement of atoms or molecules that regularly repeat in a crystal structure.
Universal Gas Constant
The constant in the Ideal Gas Law, equal to 8.3145 J mol-1 K-1 or 0.082058 L atm mol-1 K-1.
Van der Waals Force
A force acting between non-bonded atoms or molecules.
Vapor Pressure
The pressure of the vapor coexisting with a confined liquid or solid at any specified temperature.
Vaporization (or Boiling Point)
The temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure.