Second semester exam vocab
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| Kinetic-molecular theory | Based in the idea that particles of matter are always in motion
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| Ideal gas | A hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory.
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| Elastic collision | One in which there is no net loss of total kinetic energy
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| Diffusion | Spontaneous mixing of the particles of two substances caused by their random motion
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| Effusion | A process by which gas particles pass through a tiny opening
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| Real gas | A gas that does not behave completely according to the assumptions of the kinetic-molecular theory
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| Fluid | A substance that can flow and therefore take the shape of it's container
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| Surface tension | A force that tends to pull adjacent parts of a liquids surface together, thereby decreasing surface tension
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| Capillary action | The attraction of the surface of a liquid to the surface of a solid
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| Vaporization | The process by which a liquid or solid changes to a gas
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| Evaporation | The process by which particles escape from the surface of a non boiling liquid and enter the gas state
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| Freezing | The physical change of a liquid to a solid by removal of energy as heat
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| Crystalline solids | They consist of crystals
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| Crystal | A substance in which the particles are arranged in an orderly, geometric, repeating pattern
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| Amorphous solid | One in which the particles are arranged randomly
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| Melting | The physical change of a solid to a liquid by the addition of energy as heat
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| Melting point | The temperature at which a solid becomes a liquid
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| Supercooled liquids | Substances that retain certain liquid properties even at temperatures at which they appear to be solid
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| Crystal structure | The total three dimensional arrangement of particles of a crystal
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| Unit cell | The smallest portion of a crystal lattice that shows the 3D pattern of the entire lattice
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| Phase | Any part of a system that has uniform composition and properties
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| Condensation | The process by which a gas changes to a liquid
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| Equilibrium | A dynamic condition in which two opposing changes occur at equal rates in a closed system
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| Equilibrium vapor | The pressure exerted by a vapor in equilibrium with it's corresponding liquid at a given temperature
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| Volatile liquids | Liquids that evaporate readily
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| Boiling | The conversion of a liquid to a vapor within the liquid as well as it's surface
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| Boiling point | The temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure
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| Molar enthalpy of vaporization | The amount of energy as heat that is needed to vaporize one mole of liquid at the liquid's boiling point at constant pressure
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| Freezing | The physical change of a liquid to a solid
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| Freezing point | The temperature at which the solid and liquid are in equilibrium at 1 atm pressure
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| Molar enthalpy of fusion | The amount of energy as heat required to melt one mole of solid at the solid's melting point
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| Sublimation | The change of state from a solid directly to a gas
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| Deposition | The change of state from a gas directly to a solid
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| Phase diagram | A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
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| Triple Point | The temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium
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| Critical Point | The critical temperature and critical pressure
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| Critical Temperature | The temperature above which the substance cannot exist in the liquid state
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| Critical Pressure | The lowest pressure at which the substance can exist as a liquid at the critical temperature
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| Pressure | The force per unit area on a surface
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| Newton | The force that will increase the speed of a one-kilogram mass by one meter per second each second that the force is applied
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| Barometer | A device used to measure atmospheric pressure
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| Millimeters of mercury | The common unit of pressure symbolized mm Hg
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| Atmosphere of pressure | Exactly equivalent to 760 mm Hg
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| Pascal | The pressure exerted by a force of one newton acting on an area of one square meter
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| Partial Pressure | The pressure of each gas in a mixture
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| Dalton's law of partial pressure | The total pressure of a gas mixture is the sum of the partial pressure of the component gases
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| Boyle's law | Pressure and volume at a constant temperature are inversely proportional
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| Absolute zero | The temperature -273.15 C is given a value of zero in the Kelvin scale
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| Charles's law | Temperature and volume at a constant pressure are directly proportional
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| Gay-Lussac's law | Pressure and temperature at a constant volume are directly proportional
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| Combined gas law | The relationship between pressure, volume, and temperature of a fixed amount of gas
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| Avogradro's law | equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
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| Gay-Lussac's law of combining volumes of gases | At constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers
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| Standard molar volume of a gas | The volume occupied by one mole of a gas at STP 22.414 10 L
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| Ideal Gas Law | The mathematical relationship among pressure, volume, termperature, and the number of moles of a gas
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| Ideal gas constant | The constant R
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| Graham's law of effusion | The rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses
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| Soluble | Capable of being dissolved
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| Solution | A homogenous mixture of two or more substances in a single phase
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| Solvent | The solution that dissolves a substance
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| Solute | The substance dissolved in a solution
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| Suspension | When the particles in a solvent are so large that they settle out unless the mixture id constantly stirred or agitated
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| Colloids | Particles that are intermediate in size between those in solutions and suspensions form mixtures called:
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| Electrolyte | A substance that dissolves in water to give a solution that conducts eletric current
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| Nonelectrolyte | A substance that dissolves in water to give a solution that does not conduct an electric current
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| Solution Equilibrium | The physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates
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| Saturated Solution | A solution that contains the maximum amount of dissolved solute
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| Unsaturated solution | A solution that contains less solute than a saturated solution under the existing conditions
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| Supersaturated solution | A solution that contains more dissolve solute than a saturated solution contains under the same condition
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| Solubility | The amount of that substance required to form a saturated solution with a specific amount of solvent at a specified temperature
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| Hydration | The solution process with water as the solvent
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| Immiscible | Liquids that are not soluble in each other
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| Miscible | Liquids that dissolve freely in one another in any proportion
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| Henry's law | The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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| Effervescence | The rapid escape of a gas from a liquid in which it is dissolved
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| Solvate | A solute particle that is surrounded by solvent molecules
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| Enthalpy of solution | The net amount of evergy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent
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| Concentration | A measure of the amount of solute in a given amount of solvent or solution
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| Molarity | The number of moles of solute in one liter of solution
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| Molality | The concentration of a solution expressed in moled of solute perkilogram of solvent
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| Dissociation | The separation of ions that occurs when an ionic compound dissolves
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| Net ionic equation | The compounds and ions that undergo a chemical change in a reaction in an aqueous solution
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| Spectator ions | Ions that do not take part in a chemical reaction and are found in solution both before and after the reaction
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| Ionization | When ions are formed from solute molecules by the action of the solvent
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| Hydronium ion | The H3O+ ion
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| Strong electrolyte | An aqueous solution that conducts electricity well
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| Weak electrolyte | An aqueous solution that conducts electricity poorly
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| Colligative Properties | Properties that depend on the concentration of solute particles but not on their identity
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| Nonvolatile substance | A substance that has little tendency to become a gas
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| Molal freezing point | The freezing-points of the pure solvent and a solution of a nonelectrolyte in that solvent, and is directly proportional to the molal concentration of the solution
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| Molal boiling point constant | The boiling point elevation of the solvent in a 1-molal solution of a nonvolatile, nonelectroylte solute
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| Boiling-point elevation | The difference between the boiling points of the pure solvent and a nonelectrolyte solution of that solvent
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| Semipermeable membrane | Allows the passage of some particles while blocking others
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| Osmosis | The movement of solvent through a semipermeable membrane from the side of lower solute concentration to the side of higher solute concentration
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| Osmotic pressure | The external pressure that must be applied to stop osmosis
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| Binary acid | An acid that contains only two different elements: hydrogen and one of the more electronegative elements
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| Oxyacid | An acid that is a compound of hydrogen, oxygen, and a third element usually nonmetal
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| Arrhenius acid | A water solution containing the hydronium ion (H3O+)
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| Arrhenious base | A water solution containing the hydroxide ion (OH-)
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| Strong acid | One that contains a large number of hydronium ions (H3O+)
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| Weak acid | One that contains a large number of hydroxide ions (OH-)
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| Bronstead acid | A proton donor
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| Bronstead base | A proton acceptor
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| Bonstead acid-base reaction | The process in which protons are transferred from one reactant to another
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| Monoprotic acid | An acid that can donate only one proton per molecule
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| Polyprotic acid | An acid that can donate more than one proton per molecule
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| Diprotic acid | An acid that can donate two protons per molecule
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| Triprotic acid | An acid that can donate three protons per molecule
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| Lewis acid | An electron pair acceptor
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| Lewis base | An electron pair donor
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| Lewis acid-base reaction | The formation of one ormore covalent bonds between an electron-pair donor and an electron-pair acceptor
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| Conjugate acid | What is formed when a base accepts a proton
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| Conjugate base | What is left over when an acid donates a proton
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| Amphoteric | Any substance that can react as either an acid or a base
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| Neutralization | The reaction of hydronium ions and hydroxide ions to form water molecules
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| Salt | An ionic compound composed of a cation from a base and an anion from an acid
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| Self-ionization of water | The process that occurs when two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton
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| pH | The negative of the common logarithm of the hydronium ion concentration
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| pOH | The negative common logarithm of the hydroxide ion concentration
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| Acid-base indicators | Compounds whose colors are sensitive to pH
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| Transition interval | The pH range over which an indicator changes color
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| pH meter | A device used to measure the pH of a solution
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| Titration | The controlled addition and measurement of the amount of solution of known concetration required to react completely with a measure amount of a solution of unknown concentration
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| Equivalence point | The point at which the two solution used in a titration are presen in chemically equivalent amounts
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| End point | The point in titration at which an indicator changes color
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| Standard solution | The solution that contains the precisely known concentration of a solute
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| Primary standard | A highly purified solid compound used to check the concentration of the known solution in titration
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| Thermochemistry | The study of the transfers of energy as heat that accompany chemical reactions and physical changes
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| Calorimeter | The energy absorbe or released as heat in a chemical or physical change
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| Temperature | A measure of the average kineitc energy of the particles in a sample of matter
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| Joule | The SI unit of heat as well as all other forms of energy
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| Heat | The energt transferred between samples of matter because of a difference in their temperatures
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| Specific heat | The amount of energy required to raise the temperature of one gram of a sybstance by one degree Celsius of one kelvin
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| Enthalpy change | The amount of energy absorbed by a system as heat during a process at constant pressure
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| Enthalpy of reaction | The quantity of energy transferred as heat during a chemical reaction
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| Thermochemical equation | An equation that includes the quantity of energy released or absorbed as heat during the reaction as written
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| Molar enthalpy of formation | The enthalpy change that occurs when one mole of a compound is formed from its elements in their standard state at 25 C and 1 atm
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| Enthalpy of combustion | The enthalpy change that occurs during the complete combustion of one mole of a substance
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| Hess's law | The overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process
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| Entropy | A measure of the degree of randomness of the particles
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| Free energy | The combined enthalpy-entropy function
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| Free-energy change | The difference between the change in ethalpy and the product of the Kelvin temperature and the entropy change
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| Reaction mechanism | The step-by-step process by which a reaction takes place
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| Intermediates | A substance that appears in some steps but not in the net equation
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| Homogenous reactoin | A reaction whose reactants and prducts exist in single phase
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| Collision theory | The set of assumptions regarding collisions and reactions
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| Acivation energy | The energy require to start/begin a reaction
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| Activated complex | A transitional structure that results from an effective collision and that persists while old bonds are breaking and new bonds are forming
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| Reaction rate | The change in concentration of reactants per unit of time
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| Chemical kinetics | The area of chemistry that is concerned with reaction rates and reaction mechanisms
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| Heterogenoud reactions | Reactions that involve reactants in two different phases
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| Catalyst | A substance that speeds up the rate of a reaction without taking place in the reaction
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| Catalysis | The action of a catalyst
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| Homogenous catalyst | A catalyst that is in the same phase as all the reactants anf products in a reaction system
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| Heterogenous catalyst | A catalyst that is in a differenc phase from that of the reactants
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| Composition Stoichiometry | The mass relationships of elements in compounds
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| Reaction Stoichiometry | The mass relationships between reactants and products in a chemical reaction
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| Mole ratio | A conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction
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| Limiting reactant | The reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction
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| Excess reactant | The substance that is not used up completely in a reaction
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| Theortical yield | The maximum amount of product that can be produced from a given amount of reactant
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| Actual yield | The measure anount of a product obtained from a reaction
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| Percentage yield | The ratio of the actual yield to the theoretical yield, multiplied by 100
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