set 1
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172 terms
Terms | Definitions |
|---|---|
 Empirical formula | Tells us which elements are present in the smallest whole number ratio |
| Compound | Pure substance that has a fixed propotrtion of two or more elements |
| Combustion reaction | Substaance + oxygen --> oxides of that substance; Hydrocarbon + oxygen --> carbon dioxide + water |
| Cation | Positively charged ion |
| Anion | Negatively charged ion |
| Binary compound | A compound that contains two elements |
| Avogadros number | The number of particles present in one mole of a substance |
| Atomic number | Indicates the number of protons in an atom |
| Atomic mass | Indicates the number of protons + the number of neutrons in an atom |
| Alkanes | CnH2n+2 |
| Alkenes | CnH2n |
| Alkynes | CnH2n-2 |
| Molecular formula | Formula that shows which elements are in the compound and the actual number of atoms of each element; (simplest formula)x |
| Molar mass | Aka. Molecular weight or atomic mass; the number of grams per mol |
| Limiting reactant | The reactant that runs out first; limits the amount of product that can be made |
| Hydrocarbon | A compound containing only hydrogen and carbon |
| Treatment for an acid splash on the skin | A paste of a weak base. (Sodium bicarbonate aka baking soda) |
| Treatment for a base splash on the skin | Vinegar |
| Hydrates | Solid compounds that have water trapped in the crystals- can be driven off by heating the solid |
| always soluble | nitrates, chlorates, perchlorates, acetates, ammonium, and group 1 compounds |
| insoluble (unless combined with an always soluble) | carbonates, phosphates, sulfites, sulfides |
| soluble with exceptions | halides EXCEPT mercury, silver, and lead |
| soluble with exceptions | sulfates EXCEPT mercury, lead, and barium |
| soluble with exceptions | only soluble hydroxides are strong bases |
| saturated solution | a solution containing the maximum amount of solute that will dissolve under a given set of pressure and temeprature conditions |
| unsaturated solution | a solution containing less than the maximum amount of solute that will dissolve under a given set of conditions |
| supersaturated solution | a solution that has been prepared at an elevated temperature and then slowly cooled so that it holds more than the maximum amount of solute under a given set of conditions |
| colligative properties | properties that depend only on the amount of solute particles in solution, not the identity |
| molarity | moles of solute per liter of solution |
| molality | moles of solute per kg of solvent |
| mass % | grams of solute per grams of solution x 100 |
| mol fraction | moles of solute per moles of solution |
| solute | substance being dissolved in solution |
| solvent | dissolving medium of a solution |
| solution | solute + solvent |
| conditions for highest solublity of a gas/liquid solution | high pressures and low temperatures |
| PbI2 | yellow precipitate |
| AgCl | white precipitate |
| BaSO4 | white precipitate |
| copper solutions | blue |
| nickel solutions | green |
| miscible | when two or more liquids mix |
| immiscible | when two or more liquids don't mix |
| addition of a non volatile solute | raises boiling point, lowers freezing point, increases surface tension, decreases vapor pressure |
| product of decomposition of carbonic acid | carbon dioxide and water |
| product of decomposition of sulfurous acid | sulfur dioxide and water |
| product of decomposition of ammonium hydroxide | ammonia and water |
| product of decomposition of a metal carbonate | metal oxide and carbon dioxde |
| product of decomposition of a metal hydroxide | metal oxide and water |
| product of decomposition of hydrogen peroxide | water and oxygen |
| alkali metals | group 1 elements; highly reactive with water |
| alkaline earth metals | group 2 elements |
| tranisition metals | elements in groups 3-12; tend to form colored compounds |
| halogens | group 17 elements; most reactive non metals |
| noble gases | group 18 elements; all inert |
| color of permanganate solutions | purple |
| test for the evolution of hydrogen, oxygen, and carbon dioxide gas | oxygen- glowing splint ignites carbon dioxide- flaming splint goes out hydrogen- flaming splint "pops" |
| oxidation | process of losing electrons |
| reduction | process of gaining electrons |
| oxidizing agent | substance being reduced |
| reducing agent | substance being oxidized |
| galvanic cell | a spontaneous cell; battery |
| electrolytic cell | a non spontaneous cell; requires an energy source |
| anode | electrode where oxidation occurs |
| cathode | electrode where reduction occurs |
| salt bridge | device used to maintain elecrical neutrality in a galvanic cell; anions flow through the salt bridge |
| cell potential | E cell; electromotive force; the "pull" of electrons as they travel; measured in volts |
| direction of electron travel in an electrochemical cell | from anode to cathode |
| standard conditions | 1 atm, 1.0 M, 25 C |
| faraday | the charge on one mole of electrons; 96500 coulombs |
| negative E cell | non spontaneous reaction |
| positive E cell | spontaneous reaction |
| electrolysis | the use of electricity to bring about chemical change |
| 1 amp | coulomb/second |
| 1 volt | joule/coulomb |
| dilution | M1V1= M2V2 |
| aqueous solution | solutions in which water is the solvent |
| energy | the ability to do work or produce heat |
| potential energy | energy of position or composition |
| kinetic energy | energy of motion |
| first law of thermodynamics | energy cannot be created or destroyed |
| enthalpy | heat content at constant pressure |
| enthalpy of formation | the heat absorbed or released when one mole of a compound is formed from the elements in their standard state |
| enthalpy of fusion | heat absorbed to melt one mole of a solid to a liquid at its melting point |
| enthalpy of vaporization | heat absorbed to change one mole of a liquid to a gas at its boiling point |
| endothermic | reaction in which energy is absorbed; + H |
| exothermic | reaction in which energy is released; - H |
| entropy | a measure of disorder |
| positive S | system is becoming more disordered |
| negative S | system is becoming more ordered (losing disorder) |
| gibbs free energy | G; -G is always spontaneous |
| standard conditions | 1atm, 1M, 25 C |
| +w | work is being done to the system |
| -w | work is being done on the system |
| calorimetry | the process of measuring heat based on observing the temperature change when a body absorbs or discharges heat |
| specific heat capacity | energy required to raise the temp of 1 gram of a substance by 1 degree celsius |
| specific heat of water | 4.184 J/g C |
| Hess's law | energy is a state function |
| Heat of formation | Hrxn= Hproducts- H reactants |
| bond energy | "backwards equation" Hrxn= bonds broken - bonds formed |
| units for entropy | J/mol K |
| units for enthalpy and free energy | kJ/mol |
| value for G at a phase change | zero |
| thermodynamically favored conditions | negative G (always spontaneous) positive S negative H |
| differential rate law | rate is dependent on concentration |
| integrated rate law | rate is dependent on time |
| plot of concentration vs time gives a straight line | zero order |
| plot of ln(concentration) vs time gives a straight line | 1st order |
| plot of 1/concentration vs time gives a straight line | 2nd order |
| catalyst | lowers activation energy; found in the reactants first, then products |
| intermediate | found in the product first, then the reactants |
| elementary step | a reaction whose rate law can be written from its molecularity |
| reaction mechanism | a series of steps in a chemical reaction |
| molecularity | the number of species that must collide to produce the reaction indicated by that step |
| Arrhenius equation | k depends on temperature |
| half life stays constant | 1st order |
| half life increases over time | 2nd order |
| half life decreases over time | zero order |
| unit for rate | mol / L s |
| unit for zero order rate constant | mol / L s |
| unit for 1st order rate constant | 1 / s |
| unit for 2nd order rate constant | L/ mol s |
| unit for 3rd order rate constant | L2/ mol2 s |
| rate determining step | slow step |
| chemical equilibrium | a dynamic state where the concentrations of all reactants and products remain constant over time |
| always include in equilibrium expressions | solutions (aq) and gases (g) |
| never include in equilibrium expressions | solids and pure liquids |
| when given molarities of reactants and products use | K, Keq, Kc |
| when given pressures (atm) | Kp |
| when dealing with the equilibrium of bases | Kb |
| when dealing with the equilibrium of acids | Ka |
| when dealing with solubility | Ksp |
| relationship between K and the equilibrium position | K>1: products are favored K<1; reactants are favored |
| Relationship between K and Kp | Kp=Kc(RT)^delta n |
| relationship between Q and the equilibrium position | Q=K: at equlibrium Q>K shifts left Q<K shifts right |
| What does RICE stand for | reaction, initial, change, equilibrium |
| adding more reactant causes the equilibrium position to | shift right |
| adding more product causes the equilibrium position to | shift left |
| removing reactant causes the equilibrium position to | shift left |
| removing product causes the equilibrium position to | shift right |
| adding an inert gas causes the equilibrium position to | have no change |
| adding a catalyst to a system causes the equilibrium position | have no change |
| increasing the temperature of an exothermic reaction causes the equilibrium position | shift left |
| increasing the temperature of an endothermic reaction causes the equilibrium position to | shift right |
| increasing the pressure by decreasing the volume causes the equilibrium position to | shift from the most moles of gas to the least |
| adding a common ion to a solution | decreases solubility |
| relationship between Q and precipitates | Q>Ksp; a precipitate will form Q <Ksp; no precipitate will form |
| color of litmus in an acidic solution | red |
| color of litmus in a basic solution | blue |
| color of phenolphthalein in an acidic solution | colorless |
| color of phenolphthalein in a basic solution | pink |
| donate protons in water | acid |
| accept protons in water | base |
| electron pair donors | Lewis base |
| electron pair acceptors | Lewis acid |
| 6 strong acids | HCl, HI, HBr, HNO3, HClO4, H2SO4 |
| 9 strong bases | NaOH, KOH, LiOH, CsOH, RbOH, FrOH, Ba(OH)2, Sr(OH)2, Ca(OH)2 |
| indicates an organic acid | carboxyl group, COOH |
| substance that can act as an acid or a base | amphoteric |
| how to solve a strong acid or strong base problems | stoichiometry |
| how to solve a weak acid or weak base problem | equilibrium |
| Large Ka values indicate | stronger acids |
| Larger Kb values indicate | stronger bases |
| the only acids/bases that are weaker than water | conjugates of strong acids or bases |
| pH>7, [OH-] > [H+] | basic solution |
| pH<7, [H+] >[OH-] | acidic solution |
| pH=7, [H+]=[OH-] | neutral solution |
| contains more than one acidic hydrogen | polyprotic acid |
| the only polyprotic acid that has a strong acid in one dissociation, and a weak in the next | sulfuric acid, H2SO4 |
| a salt whose cation is from a strong acid in one dissociation, and a weak in the next | neutral salt |
| a salt whose cation is from a strong base and the anion is from a weak acid | basic salt |
| a salt whose cation is from a weak base and its anion is from a strong acid | acidic salt |
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