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mcat chem
| Term | Definition |
|---|---|
| boiling point | when vapor pressure of liquid = atmospheric pressure; inversely related to vp; increases w/ more H bonds |
| boyle's law | pressure and volume inversely related; P1V1=P2V2 |
| charle's law | if pressure constant, volume and temp directly proportional; V1/T1=V2/T2 |
| gay-lussac's law | if volume constant, pressure and temp directly proportional; P1/T1=P2/T2 |
| heisenberg principle | impossible to know position and momentum of object simultaneously |
| lewis acid | accepts e- |
| lewis base | donates e- |
| bronsted acid | donate h+ |
| bronsted base | accepts h+ |
| arrhenius acid | releases h+ in water |
| arrhenius base | releases oh- in water |
| covalent bond | between 2 nonmetals; e- shared between molecules; each atom contributes an e- to share (disulfide bond) |
| coordinate covalent bond | e- shared from electron rich ligand to electron poor metal cation via orbital overlap |
| hess's law | if rxn takes place in several steps, total rxn enthalpy = sum of intermediate enthalpies |
| ideal gas law | negligible volume, elastic collisions, no intermolecular forces |
| electrolytic cell | nonspontaneous; ΔG° > 0; E°cell < 0; anode (+), cathode (-) |
| galvanic cell | spontaneous; ΔG° < 0; E°cell > 0; anode (-), cathode (+) |
| formal charge | valence # - # of bonds - # of lone e- |
| disproportionation | oxidation and reduction happens to the same element |
| volume of sphere | 4/3π*r³ |
| density of cubic unit cell | m/(2r)³ |
| slope from van't hoff plot | lnK = (-ΔH°/R * 1/T) + ΔS°/R; neg. slope means pos. enthalpy |
| endothermic rxn | pos. ΔH° b/c heat added to system; ΔS decreases |
| exothermic rxn | neg. ΔH° b/c lost from system; ΔS increases |
| dilution factor | (V1final/V1initial) * (V2final/V2initial) |
| closed system | can exchange heat/energy w/ surroundings |
| open system | can exchange heat/energy and matter w/ surroundings |
| isolated system | nothing can be exchanged w/ surroundings |
| strong acid | Ka > 1; completely dissociates into stable conjugate base that doesn't react |
| weak acid | Ka < 1; doesn't completely dissociate; forms unstable conjugate base that more readily reacts |
| unimolecular rxn | first order; units = M/s |
| zero order | units = 1/s; rate doesn't depend on substrate conc. |
| bimolecular rxn | second order; units = 1/M*s |
| melting point | increases with more hydrogen bonds and longer carbon chain |
| cation | smaller ionic radius b/c less e- = greater Zeff charge that pulls remaining e- closer to nucleus |
| anion | larger ionic radius b/c more e- = les Zeff charge; the repulsion pushes remaining e- away from nucleus |
| oxidation agent | causes other atom to be oxidized; stronger if E potential is more positive (gains e-) |
| reducing agent | causes other atom to be reduced; stronger if E potential is more negative (loses e-) |
| heat of fusion | energy to change solid to liquid |
| parts per million | %*10,000 |
| 1 cm³ | 1 g |
| green precipitates | from partially filled d orbitals (nickel, copper, chromium) |
| holoenzyme | apoenzyme + cofactor |
| apoenzyme | inactive protein component |
| zymogen | enzymes that must be cleaved to be activated |
| first order | rate depends on substrate conc. |
| metals | left side all the way to aluminum group on periodic table; highly conductive |
| nonmetals | carbon to neon and diagonally down; includes hydrogen; nonconductive |
| higher molecular weight | = fewer moles |
| Bohr model | e- move to lower energy orbits = emit radiation e- excited to higher energy orbits = absorb energy |
| flurophores | conjugated molecules; often times aromatic rings |
| CO2 | soluble in water |
| O2 | low solubility in water |
| group 1 elements | alkali metals; very reactive and form hydroxides (XOH) |
| group 2 elements | alkaline earth metals; their oxides not as reactive as group 1 |
| isoelectronic atoms | have same number of e-; the element with most neg. charge has largest atomic radius |
| doub | between aromatic rings and nucleotides |
| covalent regulation | attaching or removing a chemical group (phosphorylation) to alter activity |
| absorbance | decrease = thing being reduced increase = thing being oxidized |
| linear thermal expansion | ΔL = αLΔT |
| Keq > 1 | products favored, G<0, exergonic |
| Keq < 1 | reactants favored, G>0, endergonic |
| net reduction potential | reverse the half-rxn with lower standard potential; now that one is ox. and the other is red. then add them up |
| effective nuclear charge | Zeff = # protons - # of inner electrons ; to find # of e-, use e- configuration |
| CH3COOH | acetic acid = weak acid |
| sigma bond | end to end overlap of hybridized orbitals |
| pi bond | side to side overlap of nonhybridized p orbitals |
| equivalence point | vertical line on titration curve; where all H+ are neutralized (KH2PO4 has 2 equivalence pts b/c of its 2 H+) |
| combustion rxn | CH4 + 2 O2 -> CO2 + 2 H2O |
| temperature effect on density | density increases as temp decreases b/c molecules move around slower and get packed closer together |
| elements in same column | similar chemical properties; diff. physical properties |
| elements in same row | diff. chemical properties |
| log(A)= B | 10^B = A |
| buffers | made of weak acids/bases (Ka/b is small); need conjugate pair; should have pka within 1 unit of desired pH |
| breaking bonds | absorbs energy |
| forming bonds | releases energy |
| percent yield | actual yield/theoretical yield |
| noncovalent bonds | between nonmetal + metal; rely on electrostatic interaction s; weaker than covalent bonds (h bonds, van der waals, dipole-dipole, π-stacking/hydrophobic interactions) |
| conformational isomer | same atom connectivity, but diff. spatial arrangement; have same physical properties |
| constitutional/structural isomer | same molecular formula; diff. atom connectivity = diff. physical properties |
| oxygen oxidation state in H2O2 | -1 |
| rate law | k(conc. of reactants) |
| temp effect on gas | increasing temp = decrease in solubility decreasing temp = increase in solubility |
| pressure effect on gas | increasing pressure = increases solubility decreasing pressure = decreases solubility |
| state functions | depends only on initial and final states (enthalpy, temp, entropy, free energy, pressure, volume) |
| path functions | depends on path taken to achieve final state (work, heat) |
| electron affinity trend | stronger (more neg.) across period, weaker (less neg.) down a group |
| 1st ionization energy trend | increases across period, decreases down a group |
| ionic radius trend | decreases across period (b/c # protons increase and causes e- to be more attracted to nucleus), increase down a group |
| dalton's law | partial pressure = mole fraction * total pressure |
| intramolecular H bonding | occurs when both groups are axial (straight up/down) bc it's more stabilizing |
| henry's law of solubility | solubility = k*Partial pressure of gas |
| formation of complex ions | spontaneous b/c complex ion is very stable |
| nonpolar covalent bond | equal sharing of e- between atoms of same/similar electronegativity (H2, O2, Cl2) |
| lower molar mass | higher mole number (in 10L container, you can fit more ping pong balls than basketballs) |
| higher molar mass | lower mole number |
| conjugated system | 2n+4; sp3 carbon in ring breaks aromaticity; if double bond next to atom in ring = that atom's e- is not part of system; continuous chain of alternating pi bonds |
| faraday unit | F = 1 mol e- |
| empirical formula | smallest whole # ratio. of atoms; find moles and make ratio |
| molecular formula | exact # of atoms present |
| weak acid solubility | most soluble in base bc it gets neutralized to a salt; ionic salt is soluble |
| NAGSAG | always soluble; nitrate, acetate, group 1, sulfate, ammonium, group 17 (except fluourine) |
| volume thermal expansion | ΔV = 3αVΔT |
| area thermal expansion | ΔA = 2αAΔT |
| sublimation | solid -> gas |
| deposition | gas -> solid |
| paramagnetic | unpaired e-; spin alignment is parallel to magnetic field; attracted to magnetic field |
| diamagnetic | paired e-; spin alignment is anti-parallel to magnetic field; repelled from magnetic field |
| law of mass action | rate of reaction is proportional to the conc. of the reactants |
| to maintain pH of experiment | use buffer with a pKa within one pH unit more or less |
| half equivalence pt of weak/strong acid/base | pH = pka |
| specific heat | c = Q/mΔT |
| atoms with small atomic radii | form short, strong bonds (ie. C-H) |
| atoms with large atomic radii | form long, weak bonds (ie. C-C) |
| rydberg formula | ΔE = (-2.18*10^-18) x (1/nf^2 - 1/ni^2) |
| gamma particle | high energy photon; essentially has no mass and no charge |
| positron | positive particle that is same mass as electron |
| ladder of oxidation states | hypo-ous < -ous < -ic < -per-ic |
| eigen cation | central H3O+ surrounded by stable shell of 3 water molecules |
| ammonia | NH3 |
| ammonium | NH4+ |
| common ion effect | extra quantity of an ion is added and decreases solubility of soln; NaC --> Na + Cl, then more Cl is added |
| solubility rules | NAG SAG is always soluble except with 𝐂𝐚𝐒tro 𝐁e𝐚r |
| strong base | completely dissociates into stable conjugate acid that doesn't react |
| weak base | doesn't completely dissociate; forms unstable conjugate acid that more readily reacts |
| EDG | decrease acidity + increase basicity |
| EWG | increase acidity + decrease basicity |
| 1 atm | 760 torr and 101.3 kPa |
| 1 torr | 1 mmHg |
| kinetic energy of gas eqn (boltzman constant) | E = 3/2(kT) |
| normality | molarity of acidic hydrogens in soln. (.015M of H3PO4 = .045 normality) |
| Ksp eqn | only includes aqueous and gas molecules |
| Keq eqn | only includes aqueous and gas molecules |
| density of water | 1000 kg/m^3 |
| 1 m^3 = | 1000 L |
| voltage of electrochemical cell at equilibrium | 0 |
| spectator ions | unchanged by the reaction, appears as both reactant + product |
Created by:
reynangu