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| 9734384835 | atomic radius | distance between nuclei of adjacent atoms in an element | 0 | |
| 9734403486 | atomic radius increases going ___ and ____ when on the periodic table | down and left | 1 | |
| 9734405475 | ionization energy | the energy required to remove an electron from a gaseous atom | 2 | |
| 9734418188 | ionization energy increases going ___ and ___ when on the periodic table | up and right | 3 | |
| 9734427357 | electronegativity | the relative ability of an atom in a bond to attract electrons (excludes noble gases) | 4 | |
| 9734441713 | electronegativity increases going ___ and ___ when on the periodic table | up and right | 5 | |
| 9734475585 | isotope | same element with different amount of neutrons | 6 | |
| 9734479643 | ion | charged particle/atom | 7 | |
| 9734490112 | -ate -> | -ic | 8 | |
| 9734490113 | -ite -> | -ous | 9 | |
| 9734492387 | -ide -> | hydro___ic acid | 10 | |
| 9734501637 | pauli exclusion principle | electrons of the same spin can not occupy the same orbital | 11 | |
| 9734505210 | aufbau principle | electrons fill orbitals in a sequence of most stability | 12 | |
| 9734513447 | hund's rule | electrons must occupy each sub-orbital by one pairing up | 13 | |
| 9734521047 | octet rule | all atoms like to have 8 valance electrons | 14 | |
| 9734540574 | principle quantum number (n) | orbital in which the electron is located. higher n is higher energy of the electron because it is less tightly bonded to the nucleus | 15 | |
| 9734553601 | angular momentum quantum number (l) | shows the shape of the atomic orbital - l=0 (s orbital) - l=1 (p orbital) - l=2 (d orbital) - l=3 (f orbital) | 16 | |
| 9734577098 | magnetic quantum number (m) | shows the orientation of the orbital - can be -l to l | 17 | |
| 9734581312 | electron spin number (s) | shows the spin state of the electron in an orbital - can be -1/2 or 1/2 | 18 | |
| 9734592299 | polar covalent bond | covalent bond where electrons spend more time around a more electronegative atom | 19 | |
| 9734603594 | lattice energy | the energy released when an ionic compound is formed | 20 | |
| 9734630969 | Enthalpy of formation (ΔH°f) | the overall enthalpy of the formation of ONE mole of a compound. it is the summation of all the steps involved in the formation of the compound | 21 | |
| 9734672958 | bond polarity | measure of how equally the electrons in a bond are shared between the two atoms of the bond | 22 | |
| 9734693075 | sigma bond (σ) | -electron density is along the bond axis -end to end overlap of orbitals | 23 | |
| 9734707284 | pi bonds | -electron density is above and below the bond axis | 24 | |
| 9734713878 | single bonds are.... | sigma bonds (σ) | 25 | |
| 9734720056 | double bonds are... | 1 sigma bond and 1 pi bond | 26 | |
| 9734723560 | triple bonds are... | 1 sigma bond and 2 pi bonds | 27 | |
| 9734731343 | strong electrolyte | when a compound 100% dissociates in a solvent | 28 | |
| 9734738366 | strong acid | 100% dissociates in water -H+ donor -OH acceptor | 29 | |
| 9734741257 | strong base | 100% dissociates in water -OH donor -H+ acceptor | 30 | |
| 9734755468 | oxidation | when an electron loses electrons (oxidation numbers increase) | 31 | |
| 9734760987 | reduction | when an element gains electrons (oxidation number decreases) | 32 | |
| 9734771560 | dipole-dipole attraction | attraction between polar particles | 33 | |
| 9734774671 | ion-dipole attraction | attraction between cation or anion with a dipole | 34 | |
| 9734783549 | dipole induced dipole attraction | when a polar molecule causes an instantaneous dipole in a nonpolar molecule | 35 | |
| 9734791838 | hydrogen bonding | strongest intermolecular force, when Hydrogen bonds with Oxygen or Nitrogen or Fluorine | 36 | |
| 9734797281 | london dispersion forces | weakest intermolecular force, temporary dipoles that occur due to unsymmetrical distribution of electrons | 37 | |
| 9734835303 | heat of fusion | energy from solid to liquid | 38 | |
| 9734848111 | heat of vaporization | energy from liquid to gas | 39 | |
| 9734854080 | heat of sublimation | energy from solid to gas (skipping liquid) | 40 | |
| 9734863350 | triple point | conditions where solid,liquid,gas phases coexist | 41 | |
| 9734865725 | critical point | critical temperature and pressure, beyond this point gas cannot be condensed into liquid | 42 | |
| 9734875303 | boiling point | the point at which vapor pressure is equal to atmospheric pressure | 43 | |
| 9734885198 | molality | mols of solute per kg of solvent | 44 | |
| 9734888228 | mol fraction | mols of solute / mols of all parts of solution | 45 | |
| 9734904691 | monatomic gases | noble gases | 46 | |
| 9734918134 | dalton's law of partial pressures | the total pressure of a mixture of gases equals the sum of the pressures that each gas would exert if it were present alone | 47 | |
| 9734945790 | bond enthalpy | H= E breaking - E forming -breaking = reactants -forming = products | 48 | |
| 9734968093 | reaction rate | the change in concentration of reactants or products per unit time (mol/L*s) | 49 | |
| 9734995575 | rate law | links reaction rate with concentrations of reactants at constant temperatures and order perameters rate=k(A)^x * (B)^y for A+B->C | 50 | |
| 9735017601 | reaction order | (x , y) 0=zero order 1=1st order 2=second order | 51 | |
| 9735027014 | zero order | when the rate of a reaction is independent of reactant concentration -rate=k | 52 | |
| 9735036448 | first order | when the rate of reactant depends on the concentration of one reactant -linearly graphed | 53 | |
| 9735043112 | second order | when a rate depends of either 1 second order reactant or 2 first order reactants | 54 | |
| 9735060892 | activation energy | the minimum amount of energy required for reactants to undergo a reaction | 55 | |
| 9735066855 | chemical equilibrium | when the forward and reverse reaction proceeds at equal rates | 56 | |
| 9735072078 | law of mass action | rate of any reaction is proportional to the product(s) of the reacting substances raised to the power of its coefficients | 57 | |
| 9735081392 | k>1 | product favored | 58 | |
| 9735083734 | k<1 | reactant favored | 59 | |
| 9735083735 | k=1 | equilibrium position | 60 | |
| 9735092741 | k= | concentration of products / concentration of reactants | 61 | |
| 9735110213 | reactant quotient (Q) | when the law of mass action is applied to initial concentrations and compared to the Keq to determine the equilibrium shift -the ratio of products to reactants | 62 | |
| 9735123979 | Q=k | equilibrium position | 63 | |
| 9735127020 | Q>k | equilibrium shifts left to reactants | 64 | |
| 9735128856 | Q| equilibrium shifts right to products | 65 | | |
| 9735148452 | when you increase the concentration of reactants... | equilibrium goes to the products | 66 | |
| 9735159201 | when you decrease the concentration of the reactants... | equilibrium goes to the reactants | 67 | |
| 9735164176 | when you increase the concentration of the products... | equilibrium goes to the reactants | 68 | |
| 9735168962 | when you decrease the concentrations of products... | equilibrium goes to the products | 69 | |
| 9735173206 | when you increase pressure... | equilibrium goes to the least amount of mols of gas | 70 | |
| 9735176333 | when you decrease pressure... | equilibrium goes to the most amount of mols of gas | 71 | |
| 9735189544 | endothermic rxn : temp increase = | equilibrium goes to the products -delta H needed | 72 | |
| 9735196196 | endothermic rxn : temp decrease = | equilibrium goes to the reactants -delta H needed | 73 | |
| 9735202928 | exothermic rxn : temp increase = | equilibrium goes to the reactants -delta H needed | 74 | |
| 9735207288 | exothermic rxn : temp decrease = | equilibrium goes to the products -delta H needed | 75 | |
| 9735211929 | negative delta H | exothermic rxn | 76 | |
| 9735214491 | positive delta H | endothermic rxn | 77 | |
| 9735227238 | solubility product | ksp . concentration of product ions times the concentration of the reactant ions that are present in a saturated solution of an ionic compound | 78 | |
| 9735238899 | Q>ksp | super-saturated solution, precipitation is favored | 79 | |
| 9735243900 | Q| unsaturated solution, dissolved state is favored | 80 | | |
| 9735248626 | common ion effect | when the concentration of an ion is increased, more solid will precipitate (solubility lowers) | 81 | |
| 9735263909 | conjugate acid | compound that results after an H+ is accepted | 82 | |
| 9735271053 | conjugate base | compound that results after an H+ is donated | 83 | |
| 9735304816 | a buffer system includes... | a weak acid or base with a salt containing its conjugate base | 84 | |
| 9735311597 | buffer solution | a solution that resists changes in pH | 85 | |
| 9735317004 | strong acid with a strong base pH curve |  | 86 | |
| 9735323196 | weak acid with a strong base pH curve |  | 87 | |
| 9735328279 | weak base with a strong acid pH curve |  | 88 | |
| 9735332481 | diprotic acid pH curve |  | 89 | |
| 9735343102 | entropy | calculation of disorder / randomness within the universe (S) | 90 | |
| 9735353259 | free energy | the amount of useful work that can be obtained from a process at constant temp (298 k) and pressure (1 atm) (G) | 91 | |
| 9735361702 | positive delta G | non-spontaneous | 92 | |
| 9735366186 | negative delta G | spontaneous | 93 | |
| 9735370273 | cathode | reduction occurs, accepting electrons | 94 | |
| 9735372755 | anode | oxidation occurs, donating electrons -the half rxn with the lowest E value is reversed | 95 | |
| 9735386921 | line notations | anode components on the left, cathode on the right. divide by a double line | 96 | |
| 9735393892 | dead battery | a redox rxn at equilibrium | 97 | |
| 9777614485 | viscosity | resistance of a liquid to flow | 98 | |
| 9777624009 | crystalline solid | contain highly ordered structures, with a regular pattern | 99 | |
| 9777629491 | amorphous solids | structures are not completely regular | 100 | |
| 9777669441 | cohesive forces | inter-molecular forces that bind similar molecules to one another | 101 | |
| 9777682946 | adhesive forces | inter-molecular attractions that bind a substance to a surface | 102 | |
| 9777695661 | vapor pressure | the pressure exerted by the vapor when at equilibrium | 103 | |
| 9777699486 | volatile liquid | a liquid that evaporates readily | 104 | |
| 9777723370 | boyle's law | P1V1=P2V2 -graph of V vs. P inverse relationship curve | 105 | |
| 9777732820 | charle's law | V1/T1=V2/T2 -graph of V vs. T is linear | 106 | |
| 9777745143 | Gay Lussac's Law | P1/T1=P2/T2 | 107 | |
| 9777750603 | ideal gas law | PV=nRT | 108 | |
| 9777756271 | avogadro's law | the volume of gas maintained at constant temperature and pressure is directly proportional to the number of moles of the gas | 109 | |
| 9777770331 | partial pressure | the pressure exerted by a particular component of a mixture | 110 | |
| 9777803502 | graham's law of diffusion | rate1/rate2= square root of (molar mass2/molar mass1) | 111 | |
| 9777856353 | arrhenius equation | relates activation energy, number of collisions, and fraction of effective collisions k=Ae^-Ea/RT | 112 | |
| 9777905096 | catalysts | increases the rate at which equilibrium is achieved | 113 | |
| 9777974696 | reducing agent | the species that is oxidized | 114 | |
| 9777977324 | oxidizing agent | the species that is reduced | 115 | |
| 9777985201 | salt bridge | allows ions to move to maintain charge neutrality in both half-cells | 116 |
