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| 9784083401 | STP Conditions | 0 degrees Celsius/273 K, 22.4 L, 1 atm | 0 | |
| 9784083402 | Density | mass / volume | 1 | |
| 9784083403 | Molarity | moles / L | 2 | |
| 9784083404 | Distillation | Depends on differences in boiling point | 3 | |
| 9784083405 | Filtration | Separating a solid from a liquid | 4 | |
| 9784083406 | Chromatography | Separating substances through differences in rates based on polarity | 5 | |
| 9784083407 | Law of conservation of mass | Mass is neither created nor destroyed | 6 | |
| 9784083408 | Dalton's Atomic Theory | Each element is made up of tiny particles called atoms. The atoms of a given element are identical. Chemical compounds are forms when atoms of different elements combine with each other. Chemical reactions involve reorganization of the atoms (changes in the way they are bound together.) | 7 | |
| 9784083409 | JJ Thomson | Cathode Ray, discovered the electron | 8 | |
| 9784083410 | Millikan | Oil Drop Experiment, determined mass and magnitude of the electron | 9 | |
| 9784083411 | Rutherford | Gold Foil Experiment, discovered nuclei, atoms have a lot of space | 10 | |
| 9784083412 | Solubility Rules | Always soluble: Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA | 11 | |
| 9784083413 | Solubility Rules Exceptions | Insoluble: Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Insol: Mercury, Silver, Lead (Halogens) | 12 | |
| 9784083414 | Strong Electrolytes | Good conductors WHEN DISSOLVED IN WATER, easily ionized (strong acids/bases and soluble salts) | 13 | |
| 9784083415 | Weak Electrolytes | Conduct currents very weakly WHEN DISSOLVED IN WATER (weak acids bases & poorly soluble salts) | 14 | |
| 9784083416 | Strong Acids | HF, HBr, HCl, HClO4, HI, HNO3, H2SO4 | 15 | |
| 9784083417 | Strong Bases | All Group 1 elements with OH- & Ca(OH)2, Sr(OH)2, Ba(OH)2, | 16 | |
| 9784083418 | Dilution Formula AND Equivalence point | M1V1 = M2V2 | 17 | |
| 9784083419 | Types of Chemical Reactions | Precipitation reactions, Acid-Base reactions, and Redox reactions | 18 | |
| 9784083420 | Precipitation reaction | An insoluble substance is formed as a result of the reaction | 19 | |
| 9784083421 | Spectator ions | Ions that do not participate in the reaction | 20 | |
| 9784083422 | Bronsted-Lowry acid | Proton/H+ donor | 21 | |
| 9784083423 | Bronsted-Lowry base | Proton/H+ acceptor | 22 | |
| 9784083424 | Arrhenius acid | Produces H+ (H3O+) in water | 23 | |
| 9784083425 | Arrhenius base | Produces OH- in water | 24 | |
| 9784083428 | Equivalence point | Enough titrant added to analyte where moles of acid= moles of base | 25 | |
| 9784083429 | Endpoint | Indicator changes color. Choose an indicator with an endpoint/color change near the equivalence point (pKa or pKb) | 26 | |
| 9784083430 | Redox reaction | Electrons are transferred | 27 | |
| 9784083431 | Oxidation | Loss of electrons (LEO) | 28 | |
| 9784083432 | Reduction | Gain of electrons (GER) | 29 | |
| 9784083433 | Oxidizing agent | Causes oxidation (is often reduced) | 30 | |
| 9784083434 | Reducing agent | Causes reduction (is often oxidized) | 31 | |
| 9784083435 | 1 standard atmosphere | 1 atm, 760 mm Hg, 760 torr, 101.3 kPa (Ref Table) | 32 | |
| 9784083437 | Boyle's Law | P1V1 = P2V2 | 33 | |
| 9784083438 | Charles's Law | V1 / T1 = V2 / T2 | 34 | |
| 9784083439 | Ideal Gas Law | PV = nRT | 35 | |
| 9784083440 | Molar mass of a gas | mm = dRT / P | 36 | |
| 9784083441 | Dalton's law of partial pressures | Ptot = P1 + P2 + P3... | 37 | |
| 9784083442 | Mole fraction | moles of substance/ moles total | 38 | |
| 9784083443 | KMT (kinetic molecular theory) | Volume of individual particles is negligible Particles are in constant motion Particles exert no forces on each other Collisions of particles with container walls are cause of pressure from gas | 39 | |
| 9784083445 | Diffusion | Mixing of gases | 40 | |
| 9784083446 | Effusion | Gas into a vacuum | 41 | |
| 9784083645 | Graham's law of effusion | AKA: gases with lower masses will diffuse faster |  | 42 |
| 9784083447 | Law of conservation of energy | Energy can be converted but never destroyed | 43 | |
| 9784083448 | Potential energy | Energy from position or composition/stored in bonds | 44 | |
| 9784083449 | Kinetic energy | Energy from motion | 45 | |
| 9784083450 | Heat | Transfer of energy with temperature | 46 | |
| 9784083451 | Work | Force acting over a distance | 47 | |
| 9784083452 | Exothermic | Energy out of the system | 48 | |
| 9784083453 | Endothermic | Energy into the system | 49 | |
| 9784083454 | First law of thermodynamics | The energy of the universe is constant | 50 | |
| 9784083457 | Heat capacity | heat absorbed / increase in temperature | 51 | |
| 9784083458 | Calorimetry equation | q = mCAT |  | 52 |
| 9784083459 | Hess's Law Rules | If a reaction is reversed, the sign of delta H is reversed delta H is proportional to the quantities of reactions and products - if you multiple reaction, multiply H | 53 | |
| 9784083460 | Standard enthalpy of formation | change in enthalpy with formation of one mole of compound from its elements | 54 | |
| 9784083461 | Change in enthalpy for reaction | sum of heat of formations of products - sum of heat of formations of reactions |  | 55 |
| 9784083462 | Wavelength | distance between two peaks or troughs in a wave | 56 | |
| 9784083463 | Frequency | number of cycles per second | 57 | |
| 9784083464 | Basic wave equation | speed of light = wavelength x frequency |  | 58 |
| 9784083465 | Energy of a photon equation | Planck's constant x speed of light / frequency |  | 59 |
| 9784083466 | Photoelectric effect | Effect occurring when electrons are emitted from the surface of a metal when light strikes it | 60 | |
| 9784083467 | Dual nature of light | Light acts as a wave and as particulate matter | 61 | |
| 9784083468 | de Broglie's equation | Wavelength of a particle |  | 62 |
| 9784083469 | Diffraction | Light is scattered from points or lines | 63 | |
| 9784083470 | Types of electromagnetic radiation (smallest to largest) | gamma, X-rays, UV, visible, IR, micro, radio | 64 | |
| 9784083471 | Types of electromagnetic radiation (largest to smallest) | radio, micro, IR, visible, UV, X-rays, gamma | 65 | |
| 9784083472 | Heisenberg Uncertainty Principle | We cannot know both the position and momentum of an electron (the more we know one, the less we know the other) | 66 | |
| 9784083473 | Pauli exclusion principle | Electrons with the same spin cannot occupy the same space | 67 | |
| 9784083474 | Aufbau principle | Progressively add electrons to each sub level | 68 | |
| 9784083475 | Hund's rule | Different electrons to different orbitals, same spin | 69 | |
| 9784083476 | Ionization energy | Energy required to remove a valence electron from an atom | 70 | |
| 9784083477 | Electron affinity | Energy change associated with the addition of an electron to a gaseous atom | 71 | |
| 9784083478 | Atomic radius trend | Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding) | 72 | |
| 9784083479 | Ionization energy trend | Increases across a period (electron shielding not complete), decreases down a group (more electron shielding) | 73 | |
| 9784083480 | Coulomb's law | Energy of interaction between a pair of ions |  | 74 |
| 9784083481 | Bond energy | Energy needed to break bond | 75 | |
| 9784083482 | Covalent bonding | Electrons are shared by nuclei | 76 | |
| 9784083483 | Electronegativity | Ability of an atom in a molecule to attract shared electrons to itself | 77 | |
| 9784083484 | Dipolar or dipole moment | Where the electrons move when passing another atom so that they temporarily create a postive side & negative side and then continue o their way. | 78 | |
| 9784083485 | Lattice energy | Change in energy when separated gas ions form an ionic solid Equation: LE = k(Q1Q2 / r) k is proportionality constant, Q is charge of ions, r is shortest distance between centers of ions | 79 | |
| 9784083486 | Localized electron model | Molecule is composed of atoms bound together by sharing pairs of electrons | 80 | |
| 9784083487 | Lone pairs | Pairs of electrons localized | 81 | |
| 9784083488 | Localized electron model parts | Lewis diagram, VSEPR model (geometry), type of atomic orbitals | 82 | |
| 9784083489 | Resonance | More than one valid Lewis structure | 83 | |
| 9784083490 | Bond angle of a linear shape? | 180 | 84 | |
| 9784083491 | Hybridization of a linear shape? | sp | 85 | |
| 9784083492 | Number of bonds in a linear shape? | 2 | 86 | |
| 9784083494 | Bond angle of a trigonal planar shape? | 120 | 87 | |
| 9784083495 | Hybridization of a trigonal planar shape? | sp2 | 88 | |
| 9784083496 | Number of bonds in a trigonal planar shape? | 3 | 89 | |
| 9784083498 | Bond angle of a bent shape? | ~109.5 | 90 | |
| 9784083499 | Hybridization of a bent shape? | sp2 | 91 | |
| 9784083500 | Number of bonds in a bent shape? | 2 | 92 | |
| 9784083502 | Bond angle of a tetrahedral shape? | 109.5 | 93 | |
| 9784083503 | Hybridization of a tetrahedral shape? | sp3 | 94 | |
| 9784083504 | Number of bonds in a tetrahedral shape? | 4 | 95 | |
| 9784083506 | Bond angle of a trigonal pyramidal shape? | ~109.5 | 96 | |
| 9784083507 | Hybridization of a trigonal pyramidal shape? | sp3 | 97 | |
| 9784083508 | Number of bonds in a trigonal pyramidal shape? | 3 | 98 | |
| 9784083509 | Number of nonbonding pairs in a trigonal pyramidal shape? | 1 | 99 | |
| 9784083516 | Bond angles of a trigonal bipyramidal shape? | 120, 90 | 100 | |
| 9784083517 | Hybridization of a trigonal bipyramidal shape? | sp3d | 101 | |
| 9784083518 | Number of bonds in a trigonal bipyramidal shape? | 5 | 102 | |
| 9784083520 | Bond angle of a see-saw shape? | <120 along middle, from middle to bottom or top <90 | 103 | |
| 9784083521 | Hybridization of a see-saw shape? | sp3d | 104 | |
| 9784083522 | Number of bonds in a see-saw shape? | 4 | 105 | |
| 9784083523 | Number of nonbonding pairs in a see-saw shape? | 1 | 106 | |
| 9784083524 | Bond angle of a T-shape? | <90 | 107 | |
| 9784083525 | Hybridization of a T-shape? | sp3d | 108 | |
| 9784083526 | Number of bonds in a T-shape? | 3 | 109 | |
| 9784083527 | Number of nonbonding pairs in a T-shape? | 2 | 110 | |
| 9784083528 | Bond angle of a linear (2) shape? | 180 | 111 | |
| 9784083529 | Hybridization of a linear (2) shape? | sp3d | 112 | |
| 9784083530 | Number of bonds in a linear (2) shape? | 2 | 113 | |
| 9784083531 | Number of nonbonding pairs in a linear (2) shape? | 3 | 114 | |
| 9784083532 | Bond angle of an octahedron? | 90 | 115 | |
| 9784083533 | Hybridization of an octahedron? | sp3d2 | 116 | |
| 9784083534 | Number of bonds in an octahedron? | 6 | 117 | |
| 9784083536 | Bond angle of a square pyramidal shape? | <90 | 118 | |
| 9784083537 | Hybridization of a square pyramidal shape? | sp3d2 | 119 | |
| 9784083538 | Number of bonds in a square pyramidal shape? | 5 | 120 | |
| 9784083539 | Number of nonbonding pairs in a square pyramidal shape? | 1 | 121 | |
| 9784083541 | Bond angle of a square planar shape? | 90 | 122 | |
| 9784083542 | Hybridization of a square planar shape? | sp3d2 | 123 | |
| 9784083543 | Number of bonds in a square planar shape? | 4 | 124 | |
| 9784083544 | Number of nonbonding pair in a square planar shape? | 2 | 125 | |
| 9784083546 | Metallic bond | Delocalized electron | 126 | |
| 9784083547 | Nonpolar covalent bond | Equal sharing of electrons | 127 | |
| 9784083548 | Polar covalent bond | Unequal sharing of electrons | 128 | |
| 9784083549 | Ionic bond | Transfer of electrons | 129 | |
| 9784083550 | Electronegativity differences | Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67) | 130 | |
| 9784083551 | Sigma bond | Bond between the s orbitals | 131 | |
| 9784083552 | Pi bond | Bond between the p orbitals | 132 | |
| 9784083553 | Hydrogen bond | Special type of dipole, hydrogen with N, F, or O atom. Must have an H bonded to other FON AND attracted to another H bonded to a FON | 133 | |
| 9784083554 | London dispersion forces | Between non polar molecules. Temporary dipole moment. | 134 | |
| 9784083555 | Alloy | Contains a mixture of elements and has metallic properties | 135 | |
| 9784083556 | Substitutional alloy | Metal atoms replaced by metal atoms of same size | 136 | |
| 9784083557 | Interstitial alloy | Small atoms in holes | 137 | |
| 9784083558 | Vapor pressure | Pressure of vapor at equilibrium | 138 | |
| 9784083560 | Temperature and vapor pressure? | Vapor pressure increases significantly with temperature | 139 | |
| 9784083561 | IMFs and vapor pressure? | High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure | 140 | |
| 9784083562 | Crystalline solids | Components organized in a lattice | 141 | |
| 9784083563 | Amorphous solids | Components frozen in place with no arrangement | 142 | |
| 9784083564 | Heat of fusion | Enthalpy change which occurs at the melting point when a solid melts | 143 | |
| 9784083565 | Sublimation | Solid directly to gas | 144 | |
| 9784083572 | Positive delta H | Energy absorbed | 145 | |
| 9784083573 | Negative delta H | Energy released | 146 | |
| 9784083574 | Pressure and solubility | Increases solubility of a gas | 147 | |
| 9784083575 | Henry's Law | Amount of gas dissolved proportional to pressure of gas above solution | 148 | |
| 9784083576 | Temperature and solubility | Increases solubility of solid, decreases solubility of gases | 149 | |
| 9784083584 | Reaction rate | Change of concentration over time (Rate = delta [A] / delta t) | 150 | |
| 9784083585 | Rate law | Rate depends on concentration, rate = k [a][b] | 151 | |
| 9784083586 | Integrated rate law | Concentrations depends on time (make graphs time vs CNR) | 152 | |
| 9784083587 | Initial rate | Instantaneous rate after reaction begins | 153 | |
| 9784083588 | Catalyst | Increases rate of reaction but not consumed | 154 | |
| 9784083589 | Surface area and rate | More surface area increases rate | 155 | |
| 9784083590 | Temperature and rate | Higher temperature increases rate | 156 | |
| 9784083591 | Zeroth order rate law | Rate = k | 157 | |
| 9784083593 | Zeroth order plot | [A] vs. t | 158 | |
| 9784083594 | Zeroth order slope | Slope = -k | 159 | |
| 9784083596 | First order rate law | Rate = k[A] | 160 | |
| 9784083597 | First order integrated rate law | ln[A] = - kt + ln[A]0 | 161 | |
| 9784083598 | First order plot | ln[A] vs. t | 162 | |
| 9784083599 | First order slope | Slope = -k | 163 | |
| 9784083600 | First order half life | t1/2 = 0.693 / k | 164 | |
| 9784083601 | Second order rate law | Rate = k[A]2 | 165 | |
| 9784083602 | Second order integrated rate law | 1/[A] = kt + 1/[A]0 | 166 | |
| 9784083603 | Second order plot | 1/[A] vs. t | 167 | |
| 9784083604 | Second order slope | Slope = k | 168 | |
| 9784083606 | Reaction mechanism | Series of steps | 169 | |
| 9784083607 | A --> products | Rate = k[A] | 170 | |
| 9784083608 | A + A --> products | Rate = k[A]2 | 171 | |
| 9784083609 | A + B --> products | Rate = k[A][B] | 172 | |
| 9784083610 | A + A + B --> products | Rate = k[A]2[B] | 173 | |
| 9784083611 | A + B + C --> products | Rate = k[A][B][C] | 174 | |
| 9784083612 | Rate determining step | Slowest step | 175 | |
| 9784083613 | Reaction mechanism requirements | Sum must give balanced equation, mechanism must agree with rate law | 176 | |
| 9784083614 | Equilibrium expression | Products raised to coeffs over reactants raised to coeffs see RT | 177 | |
| 9784235245 | Keq/Ka/Kb/Kp or just K | Used when THE REACTION IS AT EQUILIBRIUM | 178 | |
| 9784229438 | Q versus K | Q must be used when the reaction is NOT AT EQUILIBRIUM. They will ask you if, at that point, the reaction will need to proceed to the right (create more reactants) or to the left (create more products) in order to MATCH K | 179 | |
| 9784083615 | K = Q | Equilibrium, no change | 180 | |
| 9784083616 | K < Q | PROCEED to reactants (following the symbol <---) | 181 | |
| 9784083617 | K > Q | PROCEED to products (---->) | 182 | |
| 9784259060 | Proceed vs Shift | -Shifts occur only when the reaction HAS ALREADY BEEN at equilibrium and then something is added/removed/changed. -Proceed is used when they want to know what will happen in order to establish equilibrium in the first place! | 183 | |
| 9784083618 | Le Chatlier's Principle | Change imposed, equilibrium shifts to lessen change | 184 | |
| 9784083619 | More product added | Shift to reactants | 185 | |
| 9784083620 | More reactant added | Shift to product | 186 | |
| 9784083621 | How to change the pressure of a reaction system? | Add or remove gas, add an inert gas, change volume | 187 | |
| 9784083622 | Ka | Acid dissociation constant |  | 188 |
| 9784083623 | Strong acid | Equilibrium is far to the right, has weak conjugate base | 189 | |
| 9784083624 | Weak acid | Equilibrium is far to the left | 190 | |
| 9784083625 | Monoprotic acids | One acidic proton | 191 | |
| 9784083626 | Amphoteric | Can behave as an acid or a base (water) | 192 | |
| 9784083627 | Kw | Water dissociation constant |  | 193 |
| 9784083628 | pH | -log[H+] | 194 | |
| 9784083629 | pOH | -log[OH-] | 195 | |
| 9784083630 | pKa | -logKa | 196 | |
| 9784083631 | pH of strong acids | Depends on concentration of H+ ions | 197 | |
| 9784083632 | pH of weak acids | Find Ka and use an ice chart | 198 | |
| 9784083633 | Percent dissociation | Amount dissociated M / initial concentration M x 100% | 199 | |
| 9784083634 | Polyprotic acids | Dissociates in a stepwise manner, find Ka of each step | 200 | |
| 9784083635 | Bond strength and acid strength | Less bond strength, more acid strength | 201 | |
| 9784083636 | Common ion effect | Shift in equilibrium because of addition of common ion | 202 | |
| 9784083637 | Buffer | Resists a change in pH | 203 | |
| 9784083638 | Henderson Hasselbach Equation | Used to find the pH of a buffer Change it to: pH = pKa + log (moles base)/(moles acid) |  | 204 |
| 9784296981 | Using the H-H equation | If base is added = add those new moles to the base part (top) and subtract from the acid (bottom) If acid is added = add those new moles to the acid part (bottom) and subtract from the base (top) Turn K they give you to Ka or Kb (use Kw) | 205 | |
| 9784083639 | Strong acid-strong base titration curve | Equivalence point is 7 |  | 206 |
| 9784083640 | Weak acid-strong base titration curve | Equivalence point is greater than 7, has a halfway equivalence point |  | 207 |
| 9784083641 | Acid-base indicator | Changes color at the end point (not same as equivalence point) | 208 | |
| 9784083642 | pH of indicator | Ka/[H+] = [In-]/[HIn] = 1/10, ratio reversed for bases | 209 | |
| 9784284974 | Half-Equivalence Point AKA MIDPOINT | 1) pH = pKa | 210 | |
| 9784083643 | Ksp | Solubility product | 211 | |
| 9784272472 | Solubility product vs molar solubility | Solubility product = Ksp, must plug into expression Molar solubility = concentration in mol/L or M, either given or work backwards | 212 | |
| 9784193119 | Melting/Boiling Points: Ionic Compounds | Use Coulomb's law. Explanation: ions with smaller radii and/or larger charge will have greater electrostatic attraction and therefore have greater lattice energy, requiring more energy to melt/boil/dissolve. | 213 | |
| 9784205015 | Melting/Boiling Points: Molecules (covalent) | MUST MENTION IMFS see above. Example: H2O has a higher boiling point than CH4 because water has all three types of forces: LDF, dipole, and most importantly, hydrogen-bonding. CH4 only has LDF and thus the molecules are held together more weakly which requires less energy to boil/melt. etc. | 214 |
