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AP Chem Memorization Final Flashcards

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13761501072AcetateC₂H₃O₂⁻0
13761501073BromateBrO₃⁻1
13761501077ChlorateClO₃⁻2
13761501081CyanideCN⁻3
13761501082HydroxideOH⁻4
13761501083IodateIO₃⁻5
13761501087NitrateNO₃⁻6
13761501091PermanganateMnO₄⁻7
13761501092ThiocyanateSCN⁻8
13761501093CarbonateCO₃²⁻9
13761501097ChromateCrO₄²⁻10
13761501098DichromateCr₂O₇²⁻11
13761501099OxalateC₂O₄²⁻12
13761501100PeroxideO₂²⁻13
13761501101SelenateSeO₄²⁻14
13761501102SilicateSiO₃²⁻15
13761501103SulfateSO₄²⁻16
13761501107ThiosulfateS₂O₃²⁻17
13761501108ArsenateAsO₄³⁻18
13761501109BorateBO₃³⁻19
13761501110CitrateC₆H₅O₇³⁻20
13761501111PhosphatePO₄³⁻21
13761501115AmmoniumNH₄⁺22
13761501116Mercury (I)Hg₂²⁺23
13761501117Mercury (II)Hg²⁺24
13761501118BicarbonateHCO₃⁻25
13761501119HydrideH⁻26
13761501120combustionC₂H₄ + O₂ → CO₂ + H₂O27
13761501121synthesisAg + Cl₂ → AlCl₃28
13761501122decompositionFeO → Fe + O₂29
13761501123Single replacementMg + AgCl -->Ag + MgCl₂30
13761501124Double replacementNaCl + PbO → PbCl₂ + Na₂O31
13761501125Acid base reactionHCl + NaOH → NaCl + H₂O32
13761501126first-order reactionsum of n & m is 1...if concentration of reactants doubles, so does products33
13761501127integrated first-order rate lawconcentration of the reactant as a function of time when n + m = 1, plot of ln[A] vs. time is a straight line34
13761501129second-order rate lawdoubling the concentration of A quadruples the reaction rate, rate = k[A]², plot of 1/[A] vs. t will be linear35
13761501130integrated second order rate law1/[A] = kt + 1/[A]36
13761501131zero-order reactionrate = k[A]^0 = k, rate is constant, does not change with concentration as does 1st & 2nd order37
13761501132integrated zero-order rate law[A] = -kt + [A]38
13761501133Rate∆[A] / ∆ t39
137615011340 Order Rate Lawrate = k40
137615011351st Order Rate Lawrate = k[A]41
137615011362nd Order Rate Lawrate = k[A]²42
137615011370 Order Integrated Rate Law[A] = -kt + [A]₀43
137615011381st Order Integrated Rate Lawln[A] = -kt + ln[A]₀44
137615011392nd Order Integrated Rate Law1/[A] = +kt + 1/[A]₀45
137615011400 Order Graph46
137615011411st Order Graph47
137615011422nd Order Graph48
13761501146Zero Order Half Lifet½ = [A]₀ / 2k49
137615011471st Order Half Lifet½ = 0.693 / k50
137615011482nd Order Half Lifet½ = 1 / k [A]₀51
13761501149k<1Left (k)52
13761501150k>1Right (k)53
13761501151k = 1At equilibrium (k)54
13761501152Q > kLeft (Q)55
13761501153Q < kRight (Q)56
13761501154Q = kAt Equilibrium (Q)57
13761501155Remove reactantLeft (reactant)58
13761501156Add reactantRight (product)59
13761501157Add inert gasNo change (gas)60
13761501158Add productLeft (reactant)61
13761501159Remove productRight (product)62
13761501213Volume of container increases, More moles on left/less moles on rightLeft (volume)63
13761501161Volume of container increases, More moles on right/less moles on leftRight (volume)64
13761501162Volume of container increases, Same number of moles on both sidesAt equilibrium (volume)65
13761501163Increase temperatureRight (temperature)66
13761501164Decrease TemperatureLeft (temperature)67
13761501165ExothermicLeft (exo/endo)68
13761501166EndothermicRight (exo/endo)69
13761501167∆ - HLeft (∆H)70
13761501168∆ + HRight (∆H)71
13761501169Volume of container decreases, More moles on left/less moles on rightright (volume)72
13761501170Volume of container decreases, More moles on right/less moles on leftleft (volume)73
13761501171Alkali metals, ammonium, nitratesalways soluble74
13761501176hydroxides, carbonates, phosphates, and sulfitesinsoluble except alkali & ammonium75
13761501178chlorides, bromides, and iodidessoluble except Ag, Pb, Hg, and Cu76
13761501184sulfidessoluble with alkali, ammonium, and alkaline only77
13761501185sulfatessoluble except Ca, Sr, Ba, Ra, Ag or Pb78
13761501191+ qendothermic (q)79
13761501192-qexothermic (q)80
13761501193+wsurroundings do work on the system (w)81
13761501194-wsystem does work on the surroundings (w)82
13761501195breaking bonds+ (bonds)83
13761501196forming bonds- (bonds)84
13761501197+ ∆ Habsorbing heat, endothermic (∆H)85
13761501198-∆Hreleasing heat, exothermic (∆H)86
13761501199+∆ S°spontaneous (∆S)87
13761501200-∆ S°not spontaneous (∆S)88
13761501201+∆ S° surrentropy of universe increases (∆S Surroundings)89
13761501218-∆ S° surrentropy of universe decreases (∆S Surroundings)90
13761501202+ ∆ G°NOT spontaneous (∆G)91
13761501203- ∆ G°Spontaneous (∆G)92
13761501204∆ G° = 0System is in Equilibrium (∆G)93
13761501205when +∆ S° and -∆Hspontaneous at ALL temps (∆S & ∆H)94
13761501206when +∆ S° and +∆Hspontaneous at only high temps (∆S & ∆H)95
13761501207when -∆ S° and -∆Hspontaneous only at low temps (∆S & ∆H)96
13761501208when -∆ S° and +∆HNOT spontaneous at any temps (∆S & ∆H)97
13761501209more gas moles on left (reactants)-∆ S°98
13761501210more gas moles on right (products)+∆ S°99
13761501211when +∆ G°∆ S° is,-100
13761501212when -∆ G°∆ S° is,+101
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