Terms : Hide Images
| 9753502863 | dalton's law of partial pressures | the partial pressure of a particular ideal gas while in a mix is the same as the pressure it would have in the same container on its own | 0 | |
| 9753502864 | kinetic molecular theory | can derive gas laws from basic assumptions and physics assumptions: gas molecules occupy no space, minimal interactions, perfect elastic collisions | 1 | |
| 9753502865 | when is pvnrt more true | low pressure (less interaction between molecules) small molecules (molecules are closer to 0 volume) | 2 | |
| 9753502866 | Vrms | root mean square velocity yeah that image where Mm is molar mass = √(∑v²/n) where n how many particles and v is velocity of a particle velocity of particle with average energy |  | 3 |
| 9753502867 | KE per particle | (3/2)RT = KEavg for particle | 4 | |
| 9753502868 | pvnrt for molecules | PV = NkT where N is number of molecules and k is boltzmann | 5 | |
| 9753502869 | boltzmann's constant | R/Na = ideal gas const/avogadro's number | 6 | |
| 9753502870 | diffusion | dispersion by random motion from higher to lower concentration | 7 | |
| 9753502871 | effusion | molecules moving out of tiny hole into vacuum, easier problem lighter molecule, higher T, higher P, less obstructions leads to higher effusion |  | 8 |
| 9753502872 | graham's law of effusion | rates of effusion same hole T, P rate₁/rate₂ = √(molar mass₂/molar mass₁) = velocity₁/velocity₂ | 9 | |
| 9753502873 | boltzmann distribution | curve of frequency of speeds of gas atoms in a sample higher T increases spread |  | 10 |
| 9753502874 | van der waals equation of state | revision to pv = nrt that more real (P + a(n/V)²)(V - nb) = nRT don't memorize but a is interactions and b is volume of molecule | 11 | |
| 9753502875 | system and surroundings | system: intersting, reactant-products surroundings: everything else | 12 | |
| 9753502876 | Work | W = F.x = -P∆V for const P | 13 | |
| 9753502877 | heat | non-work energy transfer vibrations, radiation | 14 | |
| 9753502878 | 0th law of thermo | heat goes from higher to lower | 15 | |
| 9753502879 | specific heat capacity | S = energy/(mass*∆T) | 16 | |
| 9753502880 | molar heat capacity | energy/(n*∆T) | 17 | |
| 9753502881 | calorimeter | thermos of water ideal: no heat loss and no heat capacity Tobject = Th20; Qobject = -Qh20 | 18 | |
| 9753502882 | doing calorimeter problems | Tobject = Th20; Qobject = -Qh20 specific heat object*mass*∆T = -(specific heat water*mass*∆T) | 19 | |
| 9753502883 | law of dulong and petit | metals have same specific heat per molar mass; higher molar mass linear increase in specific heat | 20 | |
| 9753502884 | thermal conductivity | how easily spread heat internally | 21 | |
| 9753502885 | molecular heat capacity | bigger molecule is higher heat capacity | 22 | |
| 9753502886 | enthalpy | H; ∆H = q | 23 | |
| 9753502887 | endo/exothermic | exothermic: heat released into surrounding world, negative enthalpy bc lose it endothermic: rarer, heat absorbed, positive enthalpy; energy gains | 24 | |
| 9753502889 | redox | reduction oxidation reaction reduction: gain e⁻, charge reduced oxidation: looses e⁻, charge increased | 25 | |
| 9753502890 | oxidation number | 1) monatomic ions: oxidation number = charge 2) sum of oxydation numbers = total charge 3) F = -1 4) O = -2 5) H = +1 all rules true unless violate higher rule | 26 | |
| 9753502891 | doing redox reactions | split into half that oxidized and half that reduced balance non-OH elements balance O on one side with H₂O on the other balance H with H⁺ ions on other side add up net charge on both sides and balance w/ e⁻ multiply halves separately to balance e⁻ then add them so e⁻ cancels | 27 | |
| 9753502892 | redox reactions in basic | solve for acidic solution then add OH⁻ to cancel H⁺ and cancel out extra H₂O formed on both sides | 28 | |
| 9753502893 | gauge pressure | absolute pressure - atmospheric pressure | 29 | |
| 9753502894 | absolute pressure | the actual pressure at a given point | 30 | |
| 9753502895 | pascal | N/m² = really small | 31 | |
| 9753502896 | bar | 100,000 pascals (100kPa) | 32 | |
| 9753502897 | atmosphere | atm = 101,325Pa ≅ 1bar | 33 | |
| 9753502898 | torr | 1mm of Hg (pressure needed to raise up 1mm of mercury) | 34 | |
| 9753502899 | PSI | pounds/inch² | 35 | |
| 9753502900 | barrometer | measures atmospheric pressure | 36 | |
| 9753502901 | manometer | height difference in U-tube is the pressure of the gas in container that you're measuring |  | 37 |
| 9753502902 | atmospheric pressure | atmospheric pressure = 1atm = 101,325Pa = 14.7PSI = 760torr ≅1bar = 1/1.01325bar | 38 | |
| 9753502903 | boyle's law | P₀V₀ = P₁V₁ with const temp and amount of gas | 39 | |
| 9753502904 | charles' law | for const pressure and amount of gas |  | 40 |
| 9753502905 | avogadro's law | for const pressure and temperature |  | 41 |
| 9753502906 | ideal gas law | PV = nRT pressure*volume = mols*gas constant*temperature (in kelvin) generally work down to 2 variables initial = constant = 2 variables final | 42 | |
| 9753502907 | STP | standard temperature and pressure 0C (273.15K) at 1atm at STP, 1mol = 22.4L for just about any gas | 43 | |
| 9753502908 | acid | anything releasing H⁺ into water | 44 | |
| 9753502909 | base | anything releasing OH⁻ into water | 45 | |
| 9753502910 | acid naming | if the anion ends in -ate or -ide; change that to an -ic (ie: nitrate-nitric acid) if the anion ends in -ite; change to -ous (ie: nitrite-nitrous acid) these just refer to anion and H when has no oxygen in it, add hydro- (ie: HCl hydrochloric acid, HNO3 nitric acid) | 46 | |
| 9753502911 | adding and subtracting O | per- is add oxygen (ClO₄⁻ from chlorate) -ite is subtract oxygen (ClO₂⁻ from chlorate) hypo____ite is subtract 2 oxygen (ClO⁻) |  | 47 |
| 9753502912 | VSEPR | valence shell electron pair repulsion: pairs of electrons will be angled as far from each other as possible each angle roughly equal but bigger angle with more electronegative or electron lone pair | 48 | |
| 9753502913 | linear bond | can also be trigonal bipyramidal with 3 lone pairs or octahedral with 4 lone pairs |  | 49 |
| 9753502914 | trigonal planar bond | 120 |  | 50 |
| 9753503047 | tetrahedral |  | 51 | |
| 9753502915 | trigonal bipyramidal | think linear and then trigonal planar across it |  | 52 |
| 9753503048 | octahedral |  | 53 | |
| 9753503049 | trigonal pyramidal |  | 54 | |
| 9753502916 | bent | water; can also be trigonal planar with 1 lone pair? |  | 55 |
| 9753503050 | see-saw |  | 56 | |
| 9753503051 | T-structure |  | 57 | |
| 9753502917 | electric dipole moment | qr; point from neg partial charge to positive partial charge |  | 58 |
| 9753502918 | polar molecules | bond is polar if 2 molecules have diff electronegativity molecules is polar of dipole moments don't cancel out from symmetry | 59 | |
| 9753502919 | network solid | network covalent solid in forever expanding network; formula just empirical diamond, graphite, silicon carbide, silicon dioxide hard to break and boil | 60 | |
| 9753502920 | ionic compounds | like network solid just with repeating pattern of ions |  | 61 |
| 9753502921 | solvent solute | solute dissolved in solvent | 62 | |
| 9753502922 | dissolved | broken into individual molecules or ions surrounded by solvent molecules; process of it called solvation or hydration in water | 63 | |
| 9753502923 | electrolyte | raises electrical conductivity when dissolved in water synonymous with salt (ionic compound) weak electrolytes only raise conductivity a bit since no disassociate much while strong electrolytes a lot | 64 | |
| 9753502924 | molarity | mols of solute/L of solution (M) | 65 | |
| 9753502925 | molality | mols of solute/kg of solvent (m) | 66 | |
| 9753502926 | mass percent | mass of solute/mass of solution | 67 | |
| 9753502927 | mole fraction | mols of solute/mols of solution | 68 | |
| 9753502928 | normality | molarity*active constituents per mol for H+; normality = 3M for H3N | 69 | |
| 9753502929 | precipitate | to change phase while dissolved in water (usually talk about solid) | 70 | |
| 9753502930 | equation types | chemical eq: KI(aq)+NaCl(aq) -> KCl(s)+NaI(aq) ionic eq: K⁺(aq)+I⁻(aq)+Na⁺(aq)+Cl⁻(aq) -> I⁻(aq)+Na⁺(aq)+KCl(s) net ionic eq: K⁺(aq)+Cl⁻(aq) -> KCl(s) | 71 | |
| 9753502931 | solubility | experimentally determined number for how much can be dissolved in; varies | 72 | |
| 9753502932 | highly soluble stuff | ionic compounds with: nitrate, ammonia, or alkali metals most ionic compounds with: halogens or sulfates | 73 | |
| 9753502933 | acid base reactions | stuff⁻(H⁺) + blah⁺(OH⁻) → H₂O + stuffblah | 74 | |
| 9753502934 | aq and stuff | (aq) - dissolved in water (s) - solid (l) - liquid (g) - gas | 75 | |
| 9753502935 | valence shell | outermost electrons that do the bonding or: the shell with the highest n value | 76 | |
| 9753502936 | gradient from ionic to covalent | ionic: just completely take electron to fill own shell covalent: share atom so in both shells inbetween: when electronegativity diff is >2 is ionic; inbetween is polar bond where share but more towards 1 atom | 77 | |
| 9753502937 | electronegativity | how much pulls electrons; Fl = 4 = most more up and right; difference of 2 is cutoff above which is called ionic; more difference is more polar Fl=4, decrease by 0.5 each on that row | 78 | |
| 9753502938 | lewis dot structure | shows valence electrons as dots |  | 79 |
| 9753502939 | octet rule | atoms need 8 valence electrons but there are exceptions and formal charge takes precedence Row 2 always obeys octet rule 8 = electrons in pairs + *all* electrons in bonds |  | 80 |
| 9753502940 | isomer | Molecules with the same formula but different structure | 81 | |
| 9753502941 | resonance | mult structures possible; sort of shifts between possibilities draw all with <=> between ie: carbonate could be double bond at any of those 3 bonds |  | 82 |
| 9753502942 | formal charge | approx charge on individual atom valence electrons - electrons in pairs - ½ of electrons in bonds when violate: want more neg charge on electronegative atom |  | 83 |
| 9753502943 | covalent compound naming | 2 elements: numerical prefix+element 1 numerical prefix+element 2+ide dihydrogen monoxide carbon tetrahydride | 84 | |
| 9753502944 | orbit model of atom | like san jose t shirt atoms fly in orbit like little planets around nucleus problems: + charge should like mega attract, accelerating when orbiting and accel electrons gives off EM radiation losing energy | 85 | |
| 9753502945 | bohr model | atoms orbit nucleus at set distances where they're stable emission spectra are jumps from one stable orbit to the next and releases certain wavelengths of light E = -13.6z²/n² where z is atom # and n is energy level of orbit; energy gap between is line spectra still wrong because orbiting and losing energy as radiation |  | 86 |
| 9753502946 | wavefunction | 3D model of electron location since behave as wave and particle psi (n, L, Ml, Ms) |  | 87 |
| 9753502947 | first quantum number | n = principle quantum number determine energy level, like n in bohr model; higher n is higher NRG; from >1 | 88 | |
| 9753502948 | second quantum number | fancy L = angular momentum quantum
0≤L| 89 | | |
| 9753502949 | third quantum number | M sub l = magnetic quantum -L≤M sub l≤L determines shape of that letter of orbit so S has 1 shape, P has 3 shapes (diff axes), d has 5 (weird) | 90 | |
| 9753502950 | fourth quantum number | M sub s = spin quantum M sub s = ±½; doesn't affect/isn't affected by other quantums | 91 | |
| 9753502951 | aufbau principle | electrons will fill lowest energy levels first if all are filled at lowest energy levels => ground state | 92 | |
| 9753502952 | pauli exclusion principle | only 1 electron for each combo of quantum numbers ie: n=1 -> L must be 0, Ml must b 0, spin is ±½ so 2 possible for S1 | 93 | |
| 9753502953 | why does wavefunction work | assumes all hydrogen atoms bc if just look at outermost, the rest of the positive charge and electrons combined look like a hydrogen atom, ignores interactions between electrons, so not all with the same n are same energy bc S and stuff are closer to nucleus so experience more pull | 94 | |
| 9753502954 | penetration | how close to nucleus a shell is, more penetration = closer = lower potential s most penetration then p and stuff, why pyramid and weird order | 95 | |
| 9753503052 | order of orbital filling |  | 96 | |
| 9753502955 | full electron configuration | saying how much in all orbitals C: 1s² 2s² 2p² | 97 | |
| 9753502956 | noble gas notation | [last noble gas] then shells outside that actually used in bonding Ba: [Xe] 6s² | 98 | |
| 9753502957 | electron config O²⁻ | [Ne] = 1s² 2s² 2p⁶ | 99 | |
| 9753502958 | weird electron config | Cr - only 1 electron in last S orbital, same for Cu | 100 | |
| 9753502959 | Hund's rule | in partially filled subshell, filled to maximize total spin |  | 101 |
| 9753502960 | 1st ionization energy | how much to pull off electron; more up (bc closer to nucleus) and to the right (larger nucleus); drops when start on new shell and from N to O bc big change spin very little variation in transition metals and lanth/act | 102 | |
| 9753502961 | 2nd+ ionization energies | goes up logarithmically with big jumps up in energy required each time you start on a new shell its like pulling electron off the next element back, so first off lithium ez, 2nd insane hard | 103 | |
| 9753502962 | 2 eq's for light | E = hf = planck's const*frequency c = fλ = velocity of light = frequency*wavelength | 104 | |
| 9753502963 | Isotope | combination of atomic number and atomic mass number; varying stability; chemical properties very similar except for small like hydrogen where large % mass change | 105 | |
| 9753502964 | Why mass on the periodic table isn't integer | it's an average of all isotopes also, mass defect | 106 | |
| 9753502965 | AMU | atomic mass unit roughly mass of proton and neutron and 2000 times the mass of an electron exactly: AMU = C₁₂/12 | 107 | |
| 9753502966 | mol | 6.02*10²³; scalar 1mol of AMU's = 1gram 1mol of C₁₂ = 12g | 108 | |
| 9753502967 | stoichiometry | study of how much reactants and products in rxn; shift numbering around to get balance of elements across both sides | 109 | |
| 9753502968 | theoretical yield | how much product should hypothetically be made by a certain combo of reactants | 110 | |
| 9753502969 | actual yield | how much product is really made as a percent of theoretical yield (how much should be made in a perfect world) difference is that not all react, some make diff reactions | 111 | |
| 9753502970 | percent composition | when you have the mass of different elements in a sample, divide by molar mass to get mols of each element then find ratio between them to get empirical formula real formula can be any multiple of empirical, find if you have molar mass of substance | 112 | |
| 9753502971 | combustion | basically react a compound with excess oxygen to produce a bunch of oxides H→H₂O; N→NO₂; C→CO₂; O→O₂ | 113 | |
| 9753502972 | combustion analysis | based on weight of oxides left over, find the mols of each oxide, then the mols of that element, then ratio between the mols for empirical, then if have molar mass can find oxygen or if have total starting mass, find oxygen by computing molar mass of what you have and then calculating oxygen to fill in extra | 114 | |
| 9753502973 | limiting reactants | reactant that runs out first in a reaction even the one with more mols or more mass can be limiting because it can be like 1A+5B→3C so even in you have more B, it can still limit just calc mols of limiting and then that's how much corresponding of others there is | 115 | |
| 9753502974 | valence | the number of electrons in the outer valence shell that are open for bonding | 116 | |
| 9753502975 | 2 ways that electrons bond atoms | it happens because atoms more stable with full shells ionic: one atom with way more electronegativity rips an electron to fill its own shell and empties the other shell; the charge pulls them together covalent: share an electron so it counts for both to fill shells | 117 | |
| 9753502976 | precision | all similar inaccuracies; point of sig figs |  | 118 |
| 9753502977 | accuracy | close to the truth | | 119 |
| 9753502978 | what count as sig figs | 1,000 - only the 1 is significant 1,000. - 4 sig figs line over a number - last sig fig 2.4390 - 5 sig figs 4.560*10³ - 4 sig figs 1,000,004 - 7 sig figs 0.0000034 - 2 sig figs | 120 | |
| 9753502979 | add/subtract sig figs | round to highest sig fig place value 14.9283+9.34+1234.5 = round to the .5 | 121 | |
| 9753502980 | multiplying/dividing sig figs | find result and only count the number of sig figs of the number with the least sig figs 4.35*1002*3 = 13076.1 = 10000 (1 sig fig) because 3 has only 1 sig fig | 122 | |
| 9753502981 | order of operations sig figs | regular PEMDAS; do NOT round after each step, just keep track of where the last sig fig is and keep going, round at the end | 123 | |
| 9753502982 | (4.53+5.8123)*(9.3+300) | 3000 | 124 | |
| 9753502983 | liter | 1L = 1000cm³ = 10x10x10cm | 125 | |
| 9753502984 | celsius and fahrenheit | F = 9/5C + 32; C = 5/9*(F-32) celsius is 0 is freezing and 100 is boiling | 126 | |
| 9753502985 | kelvin | 0k is impossible absolute 0; K = 273.15+C useful because when you mult by 2, actually 2x hotter | 127 | |
| 9753502986 | mixture | can be separated into different constituents without chemical reactions | 128 | |
| 9753502987 | compound | connected by chem bonds | 129 | |
| 9753502988 | heterogeneous mixture | looks like diff substances | 130 | |
| 9753502989 | homogeneous mixture | mixture but can't see different components | 131 | |
| 9753502990 | solvent | majority in solution, solute is minority solution is same as homogeneous mixture | 132 | |
| 9753502991 | element | can't split into something else | 133 | |
| 9753502992 | physical means of separation | distillation (boil off), fractional freezing (based on which freeze first), filtration, centrifugation, chromatography | 134 | |
| 9753502993 | law of multiple proportions | seen in systems where 2 elements make multiple compounds; the ratio between them has a smallest unit in the ratio -> atoms exist |  | 135 |
| 9753502994 | cathode ray tubes | beam of particles; put stuff in there and find that they are really small and neg charged | 136 | |
| 9753502995 | millikan oil drop exp | the drops were suspended by the E-field so can calc charge and find that all clear multiples of minimum charge = charge of an electron |  | 137 |
| 9753502996 | plum pudding model | based on millikan oil drop |  | 138 |
| 9753502997 | rutherford gold foil | alpha particles should be slightly deflected by plums in the pudding but some large deflection, calc that nucleus tiny, has all +, and most mass |  | 139 |
| 9753502998 | atomic # | protons in an element which determines the element ie: Z = protons in an element = 2 for He | 140 | |
| 9753502999 | atomic mass number | neutrons + protons = 4 for He = A | 141 | |
| 9753503000 | isotope | different number of neutrons for a given element; little change in oscillation and mass insignificant except small elements | 142 | |
| 9753503001 | mass defect | difference between mass of sum of parts and weighed mass is negative mass that is the amount of negative potential holding nucleus together m = e/c² | 143 | |
| 9753503002 | iupac table naming system | columns labeled 1-18 | 144 | |
| 9753503003 | weird table naming system | goes 1a 2a then weird b stuff for middle then 3-8a for the rightmost 6 rows ending in 8a with Noble gases | 145 | |
| 9753503004 | group 1 | alkali metals except hydrogen all ions 1+nonreactive, reg it's very reactive | 146 | |
| 9753503005 | group 2 | alkaline Earth metals 2+ ions nonreactive but reg are reactive | 147 | |
| 9753503006 | group 18 | Noble gases don't make ions or chem bonds | 148 | |
| 9753503007 | group 17 | halogens only 1- ions nonreactive, reg are reactive | 149 | |
| 9753503008 | group 16 | neutral or -2 ions only except oxygen which can be weird | 150 | |
| 9753503009 | group 15 | usually neutral but when it is upon it's -3 ions | 151 | |
| 9753503010 | group 14 | carbons and stuff ions are rare | 152 | |
| 9753503011 | iron ions | Fe, Fe2+, Fe3+ | 153 | |
| 9753503012 | iron symbol | Fe | 154 | |
| 9753503013 | sodium symbol | Na | 155 | |
| 9753503014 | potassium symbol | K | 156 | |
| 9753503015 | phosphorus symbol | P | 157 | |
| 9753503016 | silver symbol | Ag | 158 | |
| 9753503017 | gold symbol | Au | 159 | |
| 9753503018 | copper symbol | Cu | 160 | |
| 9753503019 | Cobalt symbol | Co | 161 | |
| 9753503020 | lead symbol | Pb | 162 | |
| 9753503021 | Mercury symbol | Hg | 163 | |
| 9753503022 | tungsten symbol | W | 164 | |
| 9753503023 | tin symbol | Sn | 165 | |
| 9753503024 | antimony symbol | Sb | 166 | |
| 9753503025 | magnesium symbol | Mg | 167 | |
| 9753503026 | manganese symbol | Mn | 168 | |
| 9753503027 | spell F | fluorine | 169 | |
| 9753503028 | chromium ions | Cr, Cr2+, Cr3+ | 170 | |
| 9753503029 | Cobalt ions | co, co2+, co3+ | 171 | |
| 9753503030 | nickel ions | ni, ni2+ | 172 | |
| 9753503031 | copper ions | cu, cu+, cu2+ | 173 | |
| 9753503032 | aluminum ions | Al, al3+ | 174 | |
| 9753503033 | silver ions | ag, ag+ | 175 | |
| 9753503034 | zinc ions | zn, zn2+ | 176 | |
| 9753503035 | tin ions | sn, sn2+, sn4+ | 177 | |
| 9753503036 | lead ions | pb, pb2+, pb4+ | 178 | |
| 9753503037 | Mercury ions | hg, hg sub 2 up 2+, hg2+ | 179 | |
| 9753503038 | cation | + ion | 180 | |
| 9753503039 | anion | - ion | 181 | |
| 9753503040 | cation naming | fe2+ = fe (ii) co 3+ = co iii hg sub 2 up 2+ = hg i | 182 | |
| 9753503041 | anion naming | element root + ide oxide carbide nitride sulfide etc | 183 | |
| 9753503042 | ionic compound naming | cation then anion like iron (ii) oxide number can be inferred because charges must balance | 184 | |
| 9753503053 | chlorate |  | 185 | |
| 9753503054 | hydroxide |  | 186 | |
| 9753503055 | nitrate |  | 187 | |
| 9753503056 | skip this |  | 188 | |
| 9753503057 | sulfate |  | 189 | |
| 9753503058 | permanganate |  | 190 | |
| 9753503059 | peroxide |  | 191 | |
| 9753503060 | phosphate |  | 192 | |
| 9753503061 | ammonium |  | 193 | |
| 9753503043 | acetate | or CH₃OO⁻ |  | 194 |
| 9753503044 | per_____________ | means add 1 oxygen to whatever ion follows the per ie: peroxide is 1 O more than reg oxide exception is permanganate | 195 | |
| 9753503045 | hydrogen sulfate | or bisulfate |  | 196 |
| 9753503062 | hydrogen phosphate |  | 197 | |
| 9753503046 | hydrogen carbonate | or bicarbonate | | 198 |
| 9753503063 | cyanide |  | 199 | |
| 9753503064 | dihydrogen phosphate |  | 200 | |
| 9753514343 | periodic trends: electronegative | electronegativity/electron affinity: more to up and right | 201 | |
| 9760563323 | periodic trends: atomic radii | as go right: decrease bc larger charge at center pull in as go down: increase bc more electron shells | 202 | |
| 9760764797 | hydrogen bonding | hydrogen bond to small electronegative atom w/ lone pairs gives hydrogen partial positive charge so can create a dipole-dipole interaction with another electronegative atom higher boiling point, surface tension |  | 203 |
| 9762027244 | dipole-dipole interaction | attraction between oppositely charged portions of polar molecules |  | 204 |
| 9762042553 | london dispersion forces | electrons are randomly jumping around so creates temporary dipole in various places which can cause attraction only intermolecular force in non-polar, more common in larger molecules | 205 | |
| 9762393632 | dipole moment | Dipole = Qr = charge*separation; how strong dipole is points towards electronegative | 206 | |
| 9763397414 | hybridization | when form mult bonds w/ valence electrons, may combine multiple shells so for a carbon, sp3 -> spin of +2 not 0 |  | 207 |
| 9763546586 | sigma and pi bonds | sigma is first, pi is any other bonds | 208 | |
| 9765097665 | heating curves | energy added vs temp line up and then lateral lines as energy for phase change |  | 209 |
| 9765212552 | dynamic equilibrium (phase) | balance between forward and back sublimation condensation or whatever | 210 | |
| 9765222121 | vapor pressure | pressure of a gas from fluid evaporation thing more from higher T and higher volatility | 211 | |
| 9765350022 | types of solids | molecular: held by intermolecular forces; ice ionic: ionic bonds, crystal; salt covalent network: repeating pattern; quartz metallic: metallic bonding; metals | 212 | |
| 9765500001 | temp and solubility | higher temp raise soluble solid higher temp lower soluble gas | 213 | |
| 9765506995 | colligative properties | properties of solutions change boiling point, freezing point, osmotic pressure, vapor pressure | 214 | |
| 9765622028 | rauolts law | vapor pressure = pressure of pure*mole fraction solvent | 215 | |
| 9778962426 | boiling point elevation | ∆T = iKm = vant hoff factor (how many things it splits into, nacl is 2)*constant*molality | 216 | |
| 9779025430 | osmotic pressure elevation | ∆osmotic = MRTi = molarity*R*T*vant hoff | 217 | |
| 9779110702 | types of chem rxns | synthesis - combine decomposition - split combustion - oxygen react w/ something displacement - atoms from one thing replace atoms in another double replacement - switch positive atoms with one another | 218 | |
| 9782819020 | equilibrium meaning | forward and backwards reactions balance | 219 | |
| 9782821215 | equilibrium constant | Kc |  | 220 |
| 9782823756 | equilibrium constant pressures | where all the stuff is in partial pressures; Kp multiply Kc by (RT)^n = Kp = RT^(number of product mols - number of reactant mols) |  | 221 |
| 9786919709 | reaction quotient | Q = Kc calculated when not in equilibrium if Q bigger than Kc, top more, products more, so move in reverse | 222 | |
| 9786944173 | catalyst equilibrium | no effect on equilibrium, only speed of rxns | 223 | |
| 9786991319 | what makes a strong acid | large A in HA, polar HA bond | 224 | |
| 9787034457 | Kw | equilibrium constant of water |  | 225 |
| 9787083547 | pH | -log[H+] | 226 | |
| 9787107573 | Ka | acid equilibrium constant |  | 227 |
| 9787149679 | polyprotic acid | Ka down a lot each time | 228 | |
| 9787156226 | Kb | equilibrium constant for base |  | 229 |
| 9787165192 | conjugate acid/base | when release H or OH, what left behind conjugate of strong does nothing conjugate of weak is weak of other thing | 230 | |
| 9787240063 | common ion effect | if you have hydrochloric acid or something, if you add more chloride ions, it will shift equilibrium left and increase pH | 231 | |
| 9794286049 | buffers | add conjugate base/acid in system with its acid/base when add more H or OH, consumes some of buffer but the other thing is weak and doesn't change do ICE table where add amount of strong acid to neutral and subtract from cation | 232 | |
| 9794334418 | henderson-hasselbalch | for buffer solution where Ka is for buffer |  | 233 |
| 9794509978 | titration curves | strong acid-strong base is like but mirrored version of right side where steep up and equivalence point at 7pH weak acid-strong base is like image, conjugate buffers, buffer actually raises pH so >7 at equivalence point |  | 234 |
