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| 13722069404 | atomic number | number of electrons/protons in the atom | 0 | |
| 13722069405 | molar mass | average mass of a single atom measured in amus; also the average mass for one mole of the atom in grams | 1 | |
| 13722069406 | periods | horizontal rows | 2 | |
| 13722069407 | groups | vertical rows | 3 | |
| 13722069408 | alkali metals | G1 elements | 4 | |
| 13722069409 | alkaline earth metals | G2 elements | 5 | |
| 13722069410 | transition metals | G3 through G12 | 6 | |
| 13722069411 | halogens | G17 | 7 | |
| 13722069412 | noble gases | G18 | 8 | |
| 13722069413 | lanthanides and actinides | rare earth elements; inner transition metals | 9 | |
| 13722069414 | proton | positively charged particle in the nucleus; # of which determines the properties of an element | 10 | |
| 13722069415 | neutron | neutral particles in the nucleus of an atom | 11 | |
| 13722069416 | electron | small, negatively charged particle surrounding an atom in orbitals | 12 | |
| 13722069417 | mass number | sum of protons and neutrons | 13 | |
| 13722069418 | isotope | element with a different number of neutrons | 14 | |
| 13722069419 | mass spectrometry | mass of various isotopic elements to create a mass spectrum graph | 15 | |
| 13722069420 | mole | unit used to represent large numbers of small particles such as atoms, molecules, electrons, or ions | 16 | |
| 13722069421 | avogadros number | 6.022 E23 | 17 | |
| 13722069422 | ideal gas law | pv=nrt | 18 | |
| 13722069423 | ? L/mol | 22.4 L | 19 | |
| 13722069424 | percent composition | percent by mass of each element that makes up a compound; mass part/mass whole | 20 | |
| 13722069425 | empirical formula | simplest ratio of the molecules making up a compound | 21 | |
| 13722069426 | molecular formula | actual formula for a substance | 22 | |
| 13722069427 | aufbau principle | e- are placed in orbitals, subshells, and shells in order of increasing energy | 23 | |
| 13722069428 | quantized | e- can only exist at specific energy levels separated by specific intervals | 24 | |
| 13722069429 | pauli exclusion principle | two electrons who share an orbital cannot have the same spin (must be clockwise and counterclockwise); magnetic moment | 25 | |
| 13722069430 | hunds rule | when an electron is added to a subshell it will always occupy an empty orbital if one is available | 26 | |
| 13722069431 | coulombs law | the amount of energy that an electron has depends on its distance from the nucleus of an atom; e=k(q1*q20)/r | 27 | |
| 13722069432 | quantum theory | electromagnetic energy is quantized; for a given frequency of light or radiation, all possible energies are multiples of a certain unit (a quantum) | 28 | |
| 13722069433 | quantum energy equation | e=hv | 29 | |
| 13722069434 | bohr model | each energy level is represented by a row in the periodic table |  | 30 |
| 13722069435 | electromagnetic radiation | the form in which atoms absorb energy | 31 | |
| 13722069436 | when electron drops to a lower energy level | then electromagnetic radiation is released (energy) | 32 | |
| 13722069437 | frequency and wavelength are | inversely proportional; c=hv | 33 | |
| 13722069438 | ionization energy | amount of energy necessary to remove electrons from an atom (electromagnetic energy exceeds binding energy) | 34 | |
| 13722069439 | unit for binding energy | kj/mol or Mj/mol | 35 | |
| 13722069440 | kinetic energy | energy of motion | 36 | |
| 13722069441 | photoelectron spectra (pes) | charted amounts of ionizations energies for electrons ejected from a nucleus; can be used to identify elements |  | 37 |
| 13722069442 | ion | an atom which has either gained or lost electrons | 38 | |
| 13722069443 | anion | particle with more electrons than protons; negatively charged | 39 | |
| 13722069444 | cation | particle with less electrons than protons; positively charged | 40 | |
| 13722069445 | dalton | modern atomic theory; elements combined in different ratios; are never created nor destroyed in chemical reactions | 41 | |
| 13722069446 | mendeleev & meyer | independent proposals of early periodic tables | 42 | |
| 13722069447 | thomsons experiment | cathode ray tube; deflection of charges that concluded atoms are composed of positive and negative particles | 43 | |
| 13722069638 | plum pudding model |  | 44 | |
| 13722069448 | millikans experiment | calculated charge on an electron by examining the behavior of charged oil drops in an electric field | 45 | |
| 13722069449 | rutherfords experiment | fired alpha particles at gold foil and observed how they scattered; concluded that all of the positive charge was concentrated in the center and that an atom is mostly empty space | 46 | |
| 13722069450 | heisenberg uncertainty principle | it is impossible to know both the position and momentum of an electron at a particular instant; means electron orbitals do NOT represent specific orbits | 47 | |
| 13722069451 | shielding electrons | electrons between a valence electron and the nucleus that decreases the attraction between the nucleus and the valence electron | 48 | |
| 13722069452 | stable atoms have | ... completed shells | 49 | |
| 13722069639 | metalloids |  | 50 | |
| 13722069453 | atomic radius | approximate distance from the nucleus of an atom to its valence electrons | 51 | |
| 13722069454 | periodic trend: left to right | periodic trend: atomic radius decreases; protons are added to the nucleus so valence electrons are more strongly attracted ionization energy increases (protons are added to the nucleus) | 52 | |
| 13722069455 | periodic trend: down a group | periodic trend: atomic radius increases; shells of electrons are added which shield the more distant shells and valence e- get farther away ionization energy decreases (shells of e- added, each inner shell shields more and reduces the pull on valence e- so they are easier to remove) | 53 | |
| 13722069456 | periodic trend: cations | periodic trend: ... are smaller than atoms; e- is removed and a shell is lost and electron-electron repulsions are reduced | 54 | |
| 13722069457 | periodic trend: anions | periodic trend: ... are larger than atoms; e- is added, electron-electron repulsions increase and valence electrons move farther apart | 55 | |
| 13722069458 | ionization energy magnitudes | subsequent energies are larger because the e-e repulsion decreases and the remaining valence e- are closer to the nucleus; once a shell is empty the energy required to remove an e- from a full shell is significantly greater than previous energies | 56 | |
| 13722069459 | electronegativity | how strongly the nucleus of an atom attracts the electrons of other atoms in a bond | 57 | |
| 13722069460 | factors that affect electronegativity | smaller atom; greater EN closer the element is to having a full energy level; higher EN | 58 | |
| 13722069461 | EN trends | left to right; EN increases down a group; EN decreases | 59 | |
| 13722069462 | bonding | transfer or sharing of electrons | 60 | |
| 13722069463 | ionic solid | compound held together by electrostatic attractions that are in a lattice structure; weak conductors (e- are localized around a single atom); no IMFs | 61 | |
| 13722069464 | ionic bond | bond between metal and nonmetal; electrons are NOT shared: the cation gives an e- up to the anion |  | 62 |
| 13722069465 | properties of ionic solids | are solid at room temperature; high melting and boiling points | 63 | |
| 13722069466 | 2 factors that affect melting points in ionic substances | primary factor: charge on the ions (greater charges, greater Coulombic attraction) secondary factor: smaller atoms (greater Coulombic attraction) | 64 | |
| 13722069467 | salts have __________ bonding | ionic bonding | 65 | |
| 13722069468 | metallic bonding | bond between two metals; sea of electrons that make metals such good conductors; delocalized structure allows for malleability and ductility | 66 | |
| 13722069469 | interstitial alloy | metal atoms with vastly different radii combine; ex. steel |  | 67 |
| 13722069470 | substitutional alloy | metal atoms with similar radii combine; ex. brass |  | 68 |
| 13722069471 | covalent bonds | bond in which two atoms share electrons; each atom counts the e- as a part of its valence shell |  | 69 |
| 13722069472 | single bonds | one sigma bond, one e- pair; longest bond, least energy | 70 | |
| 13722069473 | double bonds | one sigma bond, one pi bond; two e- pairs | 71 | |
| 13722069474 | triple bonds | one sigma bond, two pi bonds; 3 e- pairs; shortest bond, most energy | 72 | |
| 13722069475 | network covalent bonds | lattice of covalent bonds; network solid (acts similar to one molecule); very hard, high melting/boiling points; poor conductors | 73 | |
| 13722069476 | the common network solids | SiO2, | 74 | |
| 13722069477 | doping | the addition of an impurity to an existing lattice | 75 | |
| 13722069478 | p-doping | create a hole (positively charged) that draws electrons through the substance (add a substance with one LESS valence e-) i.e. si + al | 76 | |
| 13722069479 | n-doping | add a substance with one MORE valence e- which leaves a free e- to travel freely i.e. si + p | 77 | |
| 13722069480 | polarity | exists when a molecule has a clustering of negative charge on one side due to unequal sharing of electrons (e- are pulled to the more electronegative side); creates dipoles in molecules | 78 | |
| 13722069481 | dipole moment | the measurement of the polarity of a molecule; the unit of measurement is a debye (D) |  | 79 |
| 13722069482 | more polar molecule.... | .... larger dipole moment | 80 | |
| 13722069483 | intermolecular forces (IMFs) | forces that exist between molecules in a covalently bonded substance; not bonds | 81 | |
| 13722069484 | dipole-dipole forces | the positive end of one polar molecule is attracted to the negative end of another molecule; relatively weak attraction force |  | 82 |
| 13722069485 | hydrogen bonding | strong IMF between two moelcules; F, O, N; have higher melting and boiling points than molecules with other IMFs |  | 83 |
| 13722069486 | london dispersion forces | IMFs that occur between all molecules; occur because of the random motions of electrons on atoms within molecules to create instantaneous polarities; molecules with more e- will have greater _________________ forces | 84 | |
| 13722069487 | substances with only london dispersion forces usually... | ... are gases at room temp, and boil/melt at extremely low temps | 85 | |
| 13722069488 | melting & boiling points of a covalent substance is almost always _____________ than that of ionic substances | lower | 86 | |
| 13722069489 | vapor pressure | the pressure exerted by a vapor over a liquid | 87 | |
| 13722069490 | vaporization | the process by which molecules with enough KE inside a liquid break the surface of the liquid and transition into the gaseous phase; no outside energy is needed i.e. no heating | 88 | |
| 13722069491 | vapor pressure is primarily dependent on | dependent on IMFs | 89 | |
| 13722069492 | resonance structures | structures that occur when it is possible to draw two or more valid lewis electron dot diagrams that have the same number of electron pairs for a molecule or ion | 90 | |
| 13722069493 | formal charge | used to find which structure is most likely to occur; valence - assigned | 91 | |
| 13722069494 | assigned e- | lone pairs of e- count as two and bonds count as one | 92 | |
| 13722069495 | valence shell electron-pair repulsion model (VSEPR) | model used to predict molecular geometry based on the principle that electrons repel each other and therefore are as far apart as possible in a structure | 93 | |
| 13722069496 | hybrid orbitals | orbitals that have the properties to explain the geometry of bonds between atoms | 94 | |
| 13722069497 | linear geometry | sp hybridization 0 lone pairs ex. BeCl2 & CO2 |  | 95 |
| 13722069498 | trigonal planar geometry | sp2 hybridization bond angles 120 0 lone pairs: trigonal planar (three bonds) 1 lone pair: bent (two bonds) |  | 96 |
| 13722069499 | tetrahedral geometry | 4 e- pairs, sp3 hybridization angles 109.5 0 lone pairs: tetrahedral (four bonds) [CH4, NH4+, ClO4-, SO4 2-, PO4 3-] 1 lone pair: trigonal pyramidal (3 bonds) [NH3, PCl3, SO3 2-] 2 lone pairs: bent (2 bonds) [H2O, OF2, NH2-] |  | 97 |
| 13722069500 | trigonal bipyramidal geometry | 5 e- pairs, sp4 hybridization 0 lone pairs: trigonal bipyramidal (5 bonds) [PCl5, PF5] 1 lone pair: seesaw (4 bonds) [SF4, IF4+] 2 lone pairs: t-shaped (3 bonds) [ClF3, ICl3] 3 lone pairs: linear (2 bonds) [XeF2, I3-] |  | 98 |
| 13722069501 | octahedral geometry | 6 e- pairs, sp5 hybridization 0 lone pairs: octahedral (6 bonds) [SF6] 1 lone pair: square pyramidal (5 bonds) [BrF5, IF5] 2 lone pairs: square planar (4 bonds) [XeF4] |  | 99 |
| 13722069502 | kinetic molecular theory | the theory that all matter is composed of particles (atoms and molecules) moving constantly in random directions | 100 | |
| 13722069503 | KE=0.5mv^2 | average kinetic energy of a single gas molecule (ideal gas) | 101 | |
| 13722069504 | ideal gas | (gas) high temperature, low pressure, no attractive forces, in constant motion without losing energy | 102 | |
| 13722069505 | maxwell-boltzmann diagrams | shows the range of velocities for molecules of a gas | 103 | |
| 13722069506 | effusion | the rate at which a gas will escape from a container through microscopic holes in the surface of the container | 104 | |
| 13722069507 | factors that affect rate of effusion | speed of gas molecules (so ________ increases with higher temperature and lower mass) | 105 | |
| 13722069508 | combined gas law | (P1*V1)/T1=(P2*V2)/T2 | 106 | |
| 13722069509 | boyles law | if temperature is constant: as pressure increases, volume decreases as volume increases, pressure decreases | 107 | |
| 13722069510 | charles law | if pressure is constant: as temp increases, volume increases | 108 | |
| 13722069511 | if volume is constant: | as pressure increases, temperature increases | 109 | |
| 13722069512 | daltons law | the total pressure of a mixture of gases is just the sum of all the partial pressures of the individual gases in the mixture |  | 110 |
| 13722069513 | partial pressure | the pressure of each gas in a mixture; is directly proportional to the number of moles of gas in the mixture Pa = (Ptotal) (moles of A/total moles) | 111 | |
| 13722069514 | molarity | the concentration of a solution in terms of moles of solution/volume (L) | 112 | |
| 13722069515 | mole fraction | moles of substance/total moles in solution | 113 | |
| 13722069516 | solute | substance being dissolved | 114 | |
| 13722069517 | solvent | a liquid substance capable of dissolving other substances | 115 | |
| 13722069518 | dissociation | when ionic substances break up into ions into solution | 116 | |
| 13722069519 | electrolytes | free ions in solution that conduct electricity | 117 | |
| 13722069520 | paper chromatography | the separation of a mixture by passing it through a medium in which the components of the solution move at different rates | 118 | |
| 13722069521 | retention factor | stronger the attraction between the solute and the solvent front is, the larger the Rf value will be |  | 119 |
| 13722069522 | column chromatography | a column is packed with stationary substance, then the solution to be separated (analyte) is injected into the column where it adheres to the stationary phase, then the eluent solution is injected into the column. as the eluent solution passes through the stationary phase the analyte molecules will be attracted to it with varying degrees of strength based on polarity | 120 | |
| 13722069523 | distillation | the process that separates the substances in a solution based on their boiling points |  | 121 |
| 13722069524 | salt | an ionic compound made from the neutralization of an acid with a base | 122 | |
| 13722069525 | synthesis reaction | when elements or simple compounds are combined to form a single, more complex compound | 123 | |
| 13722069526 | decomposition reaction | a reaction where a single compound os split into two or more elements or simple compounds, usually in the presence of heat; opposite of a synthesis | 124 | |
| 13722069527 | acid-base reaction | a reaction when an acid reacts with a base to form water and a salt | 125 | |
| 13722069528 | oxidation-reduction reaction | a reaction that results in the change of the oxidation states of some participating species | 126 | |
| 13722069529 | hydrocarbon combustion | hydrocarbon + oxygen --> carbon dioxide + water a substance is ignited (usually a hydrocarbon) and it reacts with oxygen in the atmosphere; products are always CO2 and H2O | 127 | |
| 13722069530 | precipitation reaction | a reaction in which an insoluble substance (salt) forms and separates from the solution | 128 | |
| 13722069531 | net ionic equation | an equation for a reaction in solution showing only those particles that are directly involved in the chemical change |  | 129 |
| 13722069532 | limiting reactant | the substance that controls the quantity of product that can form in a chemical reaction; moles of each reactant divided by moles used in reaction | 130 | |
| 13722069533 | hydrocarbon | an organic compound composed only of carbon and hydrogen | 131 | |
| 13722069534 | law of conservation of mass | matter can be neither created nor destroyed during a chemical reaction | 132 | |
| 13722069535 | 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 precipitate that can be isolated completely and weighed | 133 | |
| 13722069536 | when bonds are formed | ...energy is released | 134 | |
| 13722069537 | when bonds are broken | ...energy is absorbed | 135 | |
| 13722069538 | exothermic | products have stronger bonds than the reactants; heat is released, - ΔH | 136 | |
| 13722069539 | endothermic | reactants have stronger bonds than the products; heat is absorbed, + ΔH | 137 | |
| 13722069540 | activation energy | the minimum amount of energy required to start a chemical reaction | 138 | |
| 13722069541 | catalyst | substance that speeds up a reaction by reducing the activation energy required by the reaction; provides an alternate reaction pathway; no effect on equilibrium conditions | 139 | |
| 13722069542 | oxidation number: H | +1 | 140 | |
| 13722069543 | oxidation number: alkali metals | +1 | 141 | |
| 13722069544 | oxidation number: alkaline earth metals | +2 | 142 | |
| 13722069545 | oxidation number: oxygen | -2 | 143 | |
| 13722069546 | oxidation number: halogens | -1 | 144 | |
| 13722069547 | hydroxide | OH- | 145 | |
| 13722069548 | nitrate | NO3- | 146 | |
| 13722069549 | acetate | C2H3O2- | 147 | |
| 13722069550 | cyanide | CN- | 148 | |
| 13722069551 | permanganate | MnO4- | 149 | |
| 13722069552 | carbonate | CO3 2- | 150 | |
| 13722069553 | sulfate | SO4 2- | 151 | |
| 13722069554 | dichromate | Cr2O7 2- | 152 | |
| 13722069555 | phosphate | PO4 3- | 153 | |
| 13722069556 | ammonium | NH4+ | 154 | |
| 13722069557 | half-reactions | the two parts of an oxidation-reduction reaction, one representing oxidation, the other reduction | 155 | |
| 13722069558 | titration | the slow addition of a solution at a known concentration to another solution in order to determine the concentration of the unknown solution; color change is often used as an end point | 156 | |
| 13722069559 | galvanic (voltaic) cell | a favored redox reaction in a cell is used to generate an electric current |  | 157 |
| 13722069560 | current | unit: amperes (amps); the flow of electrons from one place to another | 158 | |
| 13722069561 | anode | where oxidation takes place | 159 | |
| 13722069562 | cathode | where reduction takes place | 160 | |
| 13722069563 | electrolyctic cell | an outside source id used to force an unfavored redox rxn to take place | 161 | |
| 13722069564 | purpose of a salt bridge | maintains electrical neutrality in the cell | 162 | |
| 13722069565 | favored redox reaction | +E | 163 | |
| 13722069566 | unfavored redox reaction | -E | 164 | |
| 13722069567 | elecroplating | a process that uses electric current to reduce dissolved metal cations so that they form a thin metal coating on an electrode | 165 | |
| 13722069568 | rate law | an expression relating the rate of a reaction to the concentration of the reactants | 166 | |
| 13722069569 | first order rate law | y= ln[a] subscript (t) m= -k x= time b= ln[a] subscript (0) |  | 167 |
| 13722069570 | half-life | the amount of time it takes for half of a sample to disappear; t1/2=0.693/k | 168 | |
| 13722069571 | second order rate law | [a] sub. (t) = concentration of reactant A at time (t) [a] sub. (0) = initial conc. of A k = rate constant t = time elapsed |  | 169 |
| 13722069572 | zero order rate laws | rate does not depend on the concentration of the reactants at all therefore rate is always the same at a given temperature; rate=k | 170 | |
| 13722069573 | collision theory | theory that collisions occur because reactants are constantly moving around and colliding with one another | 171 | |
| 13722069574 | effective collisions | collisions in which the conditions of the collision theory are met (and therefore the reaction occurs) | 172 | |
| 13722069575 | ineffective collisions | collisions in which the conditions of the collision theory are not met (and therefore reaction does not occur) | 173 | |
| 13722069576 | spectrophotometer | an instrument that measures the proportions of light of different wavelengths absorbed and transmitted by a pigment solution | 174 | |
| 13722069577 | beer's law | A=abc A=absorbance a=molar absorptivity b=path length; the distance the light is traveling through the solution c=concentration of the solution | 175 | |
| 13722069578 | rate-determining step | the slowest step in a reaction mechanism that determines the overall rate of the reaction | 176 | |
| 13722069579 | elementary steps | a series of simple reactions that represent the progress of the overall reaction at the molecular level | 177 | |
| 13722069580 | work | force exerted on an object that causes it to move | 178 | |
| 13722069581 | first law of thermodynamics | the energy of the universe is constant | 179 | |
| 13722069582 | second law of thermodynamics | if a process is favored in one direction, then it cannot be favored in the reverse reaction; and an increase in entropy promotes favored reactions | 180 | |
| 13722069583 | entropy | ΔS; a measure of the randomness or disorder of the system | 181 | |
| 13722069584 | enthalpy | ΔH; heat of a system at constant pressure | 182 | |
| 13722069585 | Gibbs free-energy | ΔG; a measure of whether or not a process will proceed without the input of outside energy ∆G=∆H-T∆S (T in degrees Kelvin) when ΔG=0, the reaction is at equilibrium | 183 | |
| 13722069586 | state functions | functions that depend only on the change between the initial and final states of a system and therefore independent of the reaction pathway (catalyst has no effect) ΔS, ΔH, ΔG | 184 | |
| 13722069587 | standard state conditions | all gases are 1 atm all liquids are pure all solids are pure all solutions are 1 molar the energy of formation of an element in its normal state is defined as zero the temperature used is 25C or 273K | 185 | |
| 13722069588 | ΔH°f (heat of formation) | the change in energy that takes place when one mole of a compound is formed from its pure components under STP |  | 186 |
| 13722069589 | STP | standard temp. and pressure | 187 | |
| 13722069590 | bond energy | the energy required to break a bond; endothermic process (add energy) |  | 188 |
| 13722069591 | hess's law | if a reaction can be described by a series of steps, then ΔH for the overall reaction is the sum of the ΔH values for all the steps | 189 | |
| 13722069592 | rules of hess's law | 1. if you flip the equation, flip the sign on ΔH 2. if you multiply or divide an equation by a #, multiply ΔH by the same # 3. if several equations in summation create a new equation, you can also add the ΔH values of those component equations to get the ΔH value for the new equation | 190 | |
| 13722069593 | enthalpy of solution | the amount of energy released or absorbed as heat when a specific amount of solute dissolves in a solvent | 191 | |
| 13722069594 | solid to liquid | melting | 192 | |
| 13722069595 | liquid to solid | freezing | 193 | |
| 13722069596 | liquid to gas | vaporization | 194 | |
| 13722069597 | gas to liquid | condensation | 195 | |
| 13722069598 | solid to gas | sublimation | 196 | |
| 13722069599 | gas to solid | deposition | 197 | |
| 13722069600 | heat of fusion | the energy that must be absorbed by a solid to melt it | 198 | |
| 13722069601 | heat of vaporization | the energy that must be put into a liquid to turn it into a gas | 199 | |
| 13722069640 | phase diagram (water) |  | 200 | |
| 13722069602 | calorimetry | the measurement of heat changes during chemical reactions | 201 | |
| 13722069603 | specific heat | the amount of heat required to the temperature of one gram of a substance by one degree celsius |  | 202 |
| 13722069604 | heating/cooling curves | curves that display what happens to the temperature of a substance as heat is added |  | 203 |
| 13722069605 | spontaneous | thermodynamically favored; -ΔG | 204 | |
| 13722069606 | nonspontaneous | thermodynamically unfavored; +ΔG | 205 | |
| 13722069607 | at low temperature | enthalpy is dominant; ΔH | 206 | |
| 13722069608 | at high temperature | entropy is dominant; ΔS | 207 | |
| 13722069609 | voltage vs favorability | a redox reaction is favored if voltage is (+) | 208 | |
| 13722069610 | hydration energy | the energy required to break hydrogen bonds | 209 | |
| 13722069611 | law of mass action | the rate of a chemical reaction is proportional to the product of the concentrations of the reactants | 210 | |
| 13722069612 | a solution is at equilibrium when | the rate of the forward reaction is equal to the rate of the reverse reaction | 211 | |
| 13722069613 | large k eq value | products are favored at equilibrium | 212 | |
| 13722069614 | small k eq value | reactants are favored at equilibrium | 213 | |
| 13722069615 | le chateliers principle | states that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves that stress | 214 | |
| 13722069616 | reaction quotient | Q | 215 | |
| 13722069617 | Q > K | precipitate forms; reaction shifts left | 216 | |
| 13722069618 | Q < K | precipitate does not form; reaction shifts right | 217 | |
| 13722069619 | Q = K | the reaction is at equilibrium; voltage in a voltaic cell reaches zero | 218 | |
| 13722069620 | common ion effect | a decrease in the solubility of an ionic compound caused by the addition of a common ion | 219 | |
| 13722069621 | Arrhenius acids | a substance that ionizes in water and produces hydrogen ions | 220 | |
| 13722069622 | Arrhenius bases | a substance that ionizes in water and produces hydroxide ions | 221 | |
| 13722069623 | Brønsted-Lowry acids | a substance that is capable of donating a proton | 222 | |
| 13722069624 | Brønsted-Lowry bases | a substance that is capable of accepting a proton | 223 | |
| 13722069625 | pH | -log [H+] | 224 | |
| 13722069626 | pOH | -log [OH-] | 225 | |
| 13722069627 | pKa | -log [Ka] | 226 | |
| 13722069628 | pKb | -log [Kb] | 227 | |
| 13722069629 | amphoteric | a substance that can act as both an acid and a base; ex. H2O | 228 | |
| 13722069630 | strong acids | dissociate completely in water; reaction goes to completion and never reaches equilibrium | 229 | |
| 13722069631 | weak acid | most of the acid molecules remain in solution and very few dissociate | 230 | |
| 13722069632 | percent dissociation | the ratio of the amount of a substance that is dissociated at equilibrium to the initial concentration of the substance in a solution, multiplied by 100 | 231 | |
| 13722069633 | oxoacids | acids that contain oxygen; the more oxygens, the stronger the acid | 232 | |
| 13722069634 | polyprotic acids | acids that can donate more than one H+ |  | 233 |
| 13722069635 | Kw | 1.0x10^-14 | 234 | |
| 13722069636 | henderson hasselbach | pH = pKa + log([A-]/[HA]) | 235 | |
| 13722069637 | buffers | weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH | 236 |
