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chem exam 2
| Question | Answer |
|---|---|
| chemical equation | symbolic representation of a chemical reaction in terms of chemical formulas |
| reactants | starting materials written on left of eqn what actually undergo change |
| products | the materials at the end of the reaction written on right of equation |
| strong electrolyte | an electrolyte that exists in solution almost entirely as ions (completely) dissolve to produce ions lightbulb would shine strong |
| electrolytes | are why water dissociates and whatnot |
| battery electrolyte example (prob dont need to know just cool) | if you dissolve a strong electrolyte in water, the ions, as moving charges, complete the circuit with a battery! when a light bulb is attached to the circuit it shines! |
| weak electrolyte | an electrolyte that dissolves in water to give a relatively small percentage of ions in this example, lightbulb would shine weakly |
| soluble | compounds that dissolve readily (giving strong electrolyte vibes) |
| insoluble | compounds that dissolve very little (giving weak electrolyte vibes) |
| types of chemical reactions | precipitation, acid-base, oxidation-reduction |
| precipitation reactions | when a solid ionic substance forms from the mixture of two solutions of ionic substances |
| acid-base reactions | reactions that involve the transfer of a proton (H+) between reactants (usually produce water?) but not always |
| oxidation-reduction reactions | reactions that involve the transfer of electrons between reactants |
| precipitate | an insoluble solid compound formed during a chemical reaction in a solution |
| arrhenius acid | a substance that produces hydrogen ions (H+) when it dissolves in water (limited to aqueous solutions) |
| arrhenius base | a subastance that produces hydroxide ions, (OH-) when it dissolves in water (limited to aqueous solutions) |
| brønsted-Lowry acid | the species (molecule or ion) that DONATES a proton to another species in a proton-transfer reaction (not aqueous limited) |
| brønsted-Lowry Base | the species (molecule or ion) that ACCEPTS a proton form another species in a proton-transfer reaction (not aqueous limited) |
| strong acid | an acid that ionizes completely in water present entirely as ions strong electrolyte (common=HNO3, H2SO4, HClO4, HCl, HBr, HI ex: HCl --> H+ + Cl- |
| weak acid | an acid that only PARTLY ionizes in water present primarily as molecules and partly as ions; it is a weak electrolyte CH3COOH-->CH3COO- (aq) + H+(aq) 98.7 <-- 1.3% 1.3% *if an acid isnt strong, its weak* |
| strong base | a base that ionizes completely in water present entirely as ions strong electrolyte common: LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 |
| weak base | a base that is only partly ionized in water present primarily as molecules and partly as ions weak electrolyte often nitrogen bases such as NH3 NH3(aq)+H2O(l) -->NH4+(aq) + OH- (aq) <-- |
| polyprotic acid | acid that results in two or more acidic hydrogens per molecule example: H2SO4 -----> H+ + HSO4- (strong electrolyte, strong acid) HSO4- ------> H+ + SO42- (weak electrolyte weak acid) <----- |
| neutralization reaction | a reaction of an acid and a base that results in an ionic compound (a salt) and possibly water |
| compounds are always | aqueous or solid |
| oxidation number | for a monatomic ion, the actual charge of the atom or a hypothetical charge assigned to the atom in the substance using simple rules |
| half reaction | one of two parts of an oxidation reduction reaction (o or r) one part of which involves a loss of electrons (therefore an increase in oxidation number) and the other part which involves a gain of electrons (therefore a decrease in oxidation number) |
| oxidation | the half reaction in which there is a LOSS OF ELECTRONS by a species (or an increase in oxidation number) get more positive if you undergo oxidation ex: Ag--> Ag+ |
| reduction | the half reaction in which there is a gain of electrons by a species (or a decrease in oxidation number) get more negative if youre reduced ex: Ag --> Ag- |
| oxidizing agent | a species that oxidizes another species it itself is reduced *electron has to come from somewhere!* |
| reducing agent | a species that reduces another species it itself is oxidized *electron has to go somewhere!* |
| common oxidation-reduction reactions | 1. combination reaction 2. decomposition reaction 3. displacement reaction 4. combustion reaction |
| combination reaction | type of redox reaction a reaction in which 2 substances combine to form a third substance ex: 2Na (s) + Cl2(g) --> 2NaCl (s) charges : 0 0 +1 -1 |
| decomposition reaction | redox reaction type reaction in which a single compound reacts to give two more substances ex: 2HgO(s)---> 2Hg(l) + O2(g) |
| displacement reaction | type of redox reaction can have single or double displacement reaction a reaction in which an element reacts with a compound, displacing another element from it ex: Zn (s) + 2HCl (aq)-->H2 (g) + ZnCl2 (aq) |
| combustion reaction | a reaction in which a substance reacts with oxygen, usually with the rapid release of heat to produce a flame ex: 4Fe(s) + 3O2(g) --> 2Fe2O3 this is rusting, so rusting is an example of a combustion reaction |
| stoichiometry | the calculation of quantities of reactants and products involved in a chemical reaction it is also how we can interperate a chemical equation |
| limiting reactant | the reactant that is entirely consumed when a reaction goes to completion once this is used up the reaction stops |
| how to tell if its a limiting reactant problem | if it gives the starting amount for MORE THAN ONE reactant, its a limiting reactant problem |
| theoretical yield | the max amount of a product that can be obtained by a reaction from a given amount of reactants gonna be the amount produced by limiting reactant calculated (as opposed to measured) |
| actual yield | the amount of product that is actually obtained this is a measured amount (as opposed to calculated) |
| percentage yield | actual yield/theoretical yield x 100 |
| quantitative analysis | the determination of the amount of a substance or species present in a material |
| gravimetric analysis | a type of quantitative analysis in which the amount of a species in a material is determined by converting the species to a product that can be isolated completely and weighed "really just taking advantage of solubility rules" |
| titration | a procedure for determining the amount of substance A by adding a carefully measured volume with a known concentration of B until reaction of A and B is just complete |
| indicators | in titration added to the analyte solution to impart a change in color at or very near the equivalence point of titration |
| end point | in titration, the volume of titrant actually measured (difference between this and equivalence should be negligable) |
| volumetric analysis | a type of quantitative analysis based on titration |
| potential energy | the energy an object has because of its relative position, composition, or condition energy stored |
| kinetic energy | the energy that an object possesses because of its motion energy spent ex: throwing a baseball, a moving car, thermal energy (movement of molecules) |
| law of conservation of energy | energy may be converted from one form to another, but the total quantity of energy remains constant |
| thermal energy | a type of kinetic energy (KE) associated with the random motion of atoms and molecules (side note: temperature is telling you how fast the molecules and atoms are moving) |
| temperature | a quantitative measure of "hot" or "cold" -fast moving molecules --> high thermal energy --> "hot" -slow moving molecules --> low thermal energy--> "cold" |
| heat | (q) the transfer of thermal energy between two bodies at different temperatures |
| heat flow | a redundant term lowkey increases the thermal energy of one body and decreases the thermal energy of the other |
| exothermic process | a change that releases heat heat comes out of it; heat is a product |
| endothermic process | a change that absorbs heat heat is going into it; heat is a reactant |
| how many joules in 1 calorie | 4.184 J |
| joule | the SI unit of heat, work and energy |
| heat capacity | (C) the heat capacity of a body of matter is the quantity of heat (q) it absorbs or releases when it experiences a temperature change of 1 degree C, or 1 K its an extensive property |
| extensive property | a property that depends on the amount of substance mass and volume are extensive properties ex: the heat capacity of a large cast iron pan is greater than the heat capacity of a small cast iron pan |
| specific heat capacity | (c) specific heat capacity of a substance, commonly called its 'specific heat', is the quantity of heat required to raise the temp of 1 gram of a substance by 1 degree C (or 1 K) c=q/(m)(deltaT) intensive property |
| intensive property | only depends on the identity of the substance, not the amount ex: the specific heat capacity of a large and small cast iron pan are identical but if one was made of iron and the other of copper, then itd be different |
| specific heat of water at 25 degrees Celsius and 1 bar | 4.184 J/g |
| specific heat of air at 25 degrees celcius and 1 bar | 1.007 J/g (basically 1) |
| when is q positive | in q = mc deltaT if a substance GAINS thermal energy (Tfinal>Tinitial) |
| when is q negative | if a substance loses thermal energy Tfinal<Tinitial |
| thermochemistry | a branch of chemical thermodynamics, the science that deals with the relationships between heat, work, and other forms of energy |
| first law of thermodynamics | change in internal energy = heat + work delta U = q+w |
| enthalpy | the sum of a system's internal energy (U) and the mathematical product of its pressure (P) and volume (V) so H=U+PV |
| thermochemical equation | the chemical equation for a reaction (including phase labels) in which the equation is given a molar interpretation, and the enthalpy of a reaction for these molar amounts is written directly after the equation |
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