Terms : Hide Images
| 13906489454 | Oxidation | loss of electrons | 0 | |
| 13906489455 | Reduction | gain of electrons | 1 | |
| 13906498904 | Oxide | a binary compound of oxygen with another element or group. | 2 | |
| 13906504333 | Oxidizing agent | electron acceptor | 3 | |
| 13906507347 | Reducing agent | electron donor | 4 | |
| 13906516611 | Strong Acids | HCl, HBr, HI, HNO3, H2SO4, HClO4 | 5 | |
| 13906520013 | Strong bases | 1A and heavy 2A hydroxides | 6 | |
| 13906546900 | gas forming reactions | H2CO3 -> H2O + CO2 S + H2 -> H2S(g) | 7 | |
| 13906557366 | Electrolyte | dissociates | 8 | |
| 13906562144 | strong electrolyte | dissociates completely | 9 | |
| 13906566466 | weak electrolyte | partially dissociate | 10 | |
| 13906577040 | Periodicity | the repeating pattern of chemical and physical properties of the elements | 11 | |
| 13906577042 | Coulombs Law | F=K q₁*q₂/r² | 12 | |
| 13906585298 | Zeff (effective nuclear charge) | Z (Atomic #) - S (Screening constant = #inner electrons) | 13 | |
| 13906602440 | Size of Atom trend | Increases down and left (Zeff increases) | 14 | |
| 13906614909 | Size of ions | - Cations are smaller than original atom - Anions are larger - Ion size increases down a group - From left to right they get smaller (because nuclear charge increases), then suddenly larger (once it changes from cations to anions) | 15 | |
| 13906620512 | Ionization energy | The amount of energy required to remove an electron from an atom | 16 | |
| 13906625198 | Ionization energy trend | increases up and to the right | 17 | |
| 13906635480 | Smaller atoms have ___ ionization energies | higher | 18 | |
| 13906642143 | electron affinity | the energy change that occurs when an electron is acquired by a neutral atom | 19 | |
| 13906646192 | electron affinity trend | increases to the right and up | 20 | |
| 13906655655 | lattice energy | the energy released when one mole of an ionic crystalline compound is formed from gaseous ions | 21 | |
| 13906657346 | Lattice energy trend | increases up and to the right | 22 | |
| 13906660713 | Electronegativity | A measure of the ability of an atom in a chemical compound to attract electrons | 23 | |
| 13906660715 | electronegativity trend | increases up and to the right | 24 | |
| 13906667326 | Lewis dot structure steps | 25 | ||
| 13906698255 | free radicals | chemical particles with an odd number of electrons | 26 | |
| 13906700408 | Hypervalent | molecules and ions with more than an octet of electrons around the central atom | 27 | |
| 13906702753 | electron domain | in the VSEPR model, a region about a central atom in which an electron pair is concentrated | 28 | |
| 13906706501 | Kinetic Molecular Theory of Gases | 1. gases made up of negligible volume 2. no intermolecular attractions/repulsions 3. elastical collisions 4. constant random motion 5. kinetic energy of gas is related to T 6. same moles of gas=same kinetic energy | 29 | |
| 13906738308 | Celcius to Kelvin | K=C+273 | 30 | |
| 13906742475 | van der Waals equation | [P+(an^2)/(V^2)][V-nb]=nRT a = strength of attraction b = Size of molecule | 31 | |
| 13906756410 | Real Gas Law | Real gasses only conform to PV=nRT at Low pressures High temps | 32 | |
| 13906774475 | Effusion | A process by which gas particles pass through a tiny opening | 33 | |
| 13906776273 | Diffusion | Movement of molecules from an area of higher concentration to an area of lower concentration. | 34 | |
| 13906780719 | Kinetic energy of gas | KE=1/2mv^2 Same Temp - KE = KE | 35 | |
| 13906789700 | Grams law of effusion |  | 36 | |
| 13906803854 | van der Waals forces | a slight attraction that develops between the oppositely charged regions of nearby molecules | 37 | |
| 13906808402 | London dispersion forces | - Attractions between momentary dipole - All molecules - Polarizability |  | 38 |
| 13906823114 | London Dispersion forces are effected by... | Usually Weak Shape - Long skinny have stronger Weight - Increases with molecular weight. Larger clouds are easier to polarize | 39 | |
| 13906832748 | dipole-dipole forces | attractions between oppositely charged regions of polar molecules | 40 | |
| 13906837310 | dipole-dipole forces are effected by... | Polarity - Increases with increase in polarity | 41 | |
| 13906856563 | Hydrogen Bonding | Very Strong Dipole-Dipole interaction with H + N, O, or F | 42 | |
| 13906867447 | Viscosity | resistance to flow | 43 | |
| 13906868963 | surface tension | A measure of how difficult it is to stretch or break the surface of a liquid | 44 | |
| 13906868964 | Vapor Pressure | - As temp rises, the fraction of molecules having enough energy to escape increases - Pressure increase | 45 | |
| 13906905665 | Boiling poing | When its Vapor pressure = Atmospheric Pressure | 46 | |
| 13906908591 | Normal Boiling Point | The T that VP is 760 torr or 1 ATM | 47 | |
| 13906914380 | Heat of fusion | Amount of energy required to change a substance from the solid phase to the liquid phase. | 48 | |
| 13906914381 | heat of vaporization | The amount of energy required for the liquid at its boiling point to become a gas | 49 | |
| 13906916823 | Triple Point | 3 phases coexist | 50 | |
| 13906923821 | rate of reaction depends on | Catalyst Higher Temp Concentration Homogeneous mixture | 51 | |
| 13906933541 | Reaction rate equation (change in concentration | -Δ[A]/Δt = Δ[B]/Δt | 52 | |
| 13906942699 | steric factor | Size + Orientation | 53 | |
| 13906950394 | Rate Equation | rate = K[A]^a[B]^b | 54 | |
| 13923106378 | Activated complex | a transitional structure that results from an effective collision and that persists while old bonds are breaking and new bonds are forming | 55 | |
| 13923112000 | Maxwell-Boltzmann distribution | The distribution of energies (and therefore speeds) of the molecules in a gas or liquid. | 56 | |
| 13923138907 | Arrhenius equation | K=Ae^(-Ea/RT) k is the rate constant A is pre-exponential factor: how often particles collide in correct orientation. | 57 | |
| 13923212924 | reaction mechanism | the step-by-step sequence of reactions by which the overall chemical change occurs | 58 | |
| 13923222789 | elementary reaction | a reaction in which reactants are converted to products in a single step | 59 | |
| 13923240000 | molecularity | the number of molecules that participate as reactants in an elementary reaction | 60 | |
| 13923245948 | rate law and order for elementary reactions is determined by | Coefficients | 61 | |
| 13923295642 | Kp to Kc | Kp = Kc(RT)^delta n | 62 | |
| 13923303754 | Kp = Kc when | there are the same number of moles of gas on each side of the equation | 63 | |
| 13923308986 | Keq > 1 | products are favored | 64 | |
| 13923311526 | Keq < 1 | reactants favored | 65 | |
| 13923330309 | k = q when | System is in equilibrium | 66 | |
| 13923339118 | Equilibrium Quotient | Q = [Products]/[Reactants] | 67 | |
| 13923905469 | Q > K | shift left | 68 | |
| 13923908069 | Q < K | shift right | 69 | |
| 13923917227 | Amphiprotic | A species that can either accept or donate a proton. | 70 | |
| 13923917228 | Amphoteric | a substance that can act as both an acid and a base | 71 | |
| 13923930504 | Kw | 1.0 x 10^-14 | 72 | |
| 13923930505 | pH | = -log[H+] | 73 | |
| 13923944849 | % Ionization | [H3O+eq]/[HAinitial] x 100 | 74 | |
| 13923964716 | Ka | acid dissociation constant | 75 | |
| 13923964717 | Kb | base dissociation constant | 76 | |
| 13923972850 | Higher Kb | stronger base | 77 | |
| 13923972851 | Lower Ka | weaker acid | 78 | |
| 13923975356 | Higher Ka | stronger acid | 79 | |
| 13923975357 | Lower Kb | weaker base | 80 | |
| 13923981939 | polyprotic acid | an acid that can donate more than one proton per molecule | 81 | |
| 13923987418 | Ka * Kb | Kw | 82 | |
| 13923991850 | pH + pOH = | 14 | 83 | |
| 13923991852 | pKa + pKb = | pKw = 14 | 84 | |
| 13924011211 | Factors affecting acid strenght | - Polarization of Hx bond - Stronger bond = weaker acid - Less stability = weaker acid | 85 | |
| 13924023595 | If x is in same group bond strenght is _ important | more | 86 | |
| 13924048284 | If x is in the same period, bond polarity is _ important | more | 87 | |
| 13924059537 | Carboxilic Acid | COOH | 88 | |
| 13924078269 | Carboxilic Acids draw ___ from ___ Increase ___ of bond Increases ____ | - Electron density, OH bond - Polarity - Acidity | 89 | |
| 13924094001 | Bottom Line of acid strenght | Anything that pulls electrons away from the ionizable hydrogen (making a weaker bond) makes the acid more acidic | 90 | |
| 13924113626 | common ion effect | a decrease in the solubility of an ionic compound caused by the addition of a common ion | 91 | |
| 13924116202 | Buffer | compound that prevents sharp, sudden changes in pH | 92 | |
| 13924119509 | Henderson-Hasselbalch equation | pH = pKa + log [A-]/[HA] | 93 | |
| 13924124516 | Strong acid-strong base titration curve | equivalence point: pH=7 |  | 94 |
| 13924134039 | Weak acid-strong base titration curve | Equivalence point is greater than 7, has a halfway equivalence point |  | 95 |
| 13924144006 | strong acid weak base titration | Slow decline in pH followed by a rapid decrease at equivalence point. End point of indicator should be < 7. |  | 96 |
| 13924196420 | Ksp = | [prodA][prodB] (the bigger, the more soluble) | 97 | |
| 13924207529 | Heat up and cool down | q = mc{delta}t | 98 | |
| 13924216368 | Phase Change | q = n{delta}h fus/vap | 99 | |
| 13924230060 | 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 | 100 | |
| 13924238421 | calorimetry equation | mcdeltaT=mcdeltaT | 101 | |
| 13924286760 | deltaSsurr= | -deltaH/T | 102 | |
| 13924300068 | Oxidation occurs at the | anode | 103 | |
| 13924302664 | Reduction occurs at the | cathode | 104 | |
| 13924307321 | electromotive force (emf) | The power supplied by the supply per unit current. | 105 | |
| 13924328654 | A stronger oxidizing agent exhibits more _______ | Positive reduction potential | 106 |
