AP Chem Memorization Final Flashcards

13761501072	Acetate	C₂H₃O₂⁻	0
13761501073	Bromate	BrO₃⁻	1
13761501077	Chlorate	ClO₃⁻	2
13761501081	Cyanide	CN⁻	3
13761501082	Hydroxide	OH⁻	4
13761501083	Iodate	IO₃⁻	5
13761501087	Nitrate	NO₃⁻	6
13761501091	Permanganate	MnO₄⁻	7
13761501092	Thiocyanate	SCN⁻	8
13761501093	Carbonate	CO₃²⁻	9
13761501097	Chromate	CrO₄²⁻	10
13761501098	Dichromate	Cr₂O₇²⁻	11
13761501099	Oxalate	C₂O₄²⁻	12
13761501100	Peroxide	O₂²⁻	13
13761501101	Selenate	SeO₄²⁻	14
13761501102	Silicate	SiO₃²⁻	15
13761501103	Sulfate	SO₄²⁻	16
13761501107	Thiosulfate	S₂O₃²⁻	17
13761501108	Arsenate	AsO₄³⁻	18
13761501109	Borate	BO₃³⁻	19
13761501110	Citrate	C₆H₅O₇³⁻	20
13761501111	Phosphate	PO₄³⁻	21
13761501115	Ammonium	NH₄⁺	22
13761501116	Mercury (I)	Hg₂²⁺	23
13761501117	Mercury (II)	Hg²⁺	24
13761501118	Bicarbonate	HCO₃⁻	25
13761501119	Hydride	H⁻	26
13761501120	combustion	C₂H₄ + O₂ → CO₂ + H₂O	27
13761501121	synthesis	Ag + Cl₂ → AlCl₃	28
13761501122	decomposition	FeO → Fe + O₂	29
13761501123	Single replacement	Mg + AgCl -->Ag + MgCl₂	30
13761501124	Double replacement	NaCl + PbO → PbCl₂ + Na₂O	31
13761501125	Acid base reaction	HCl + NaOH → NaCl + H₂O	32
13761501126	first-order reaction	sum of n & m is 1...if concentration of reactants doubles, so does products	33
13761501127	integrated first-order rate law	concentration of the reactant as a function of time when n + m = 1, plot of ln[A] vs. time is a straight line	34
13761501129	second-order rate law	doubling the concentration of A quadruples the reaction rate, rate = k[A]², plot of 1/[A] vs. t will be linear	35
13761501130	integrated second order rate law	1/[A] = kt + 1/[A]	36
13761501131	zero-order reaction	rate = k[A]^0 = k, rate is constant, does not change with concentration as does 1st & 2nd order	37
13761501132	integrated zero-order rate law	[A] = -kt + [A]	38
13761501133	Rate	∆[A] / ∆ t	39
13761501134	0 Order Rate Law	rate = k	40
13761501135	1st Order Rate Law	rate = k[A]	41
13761501136	2nd Order Rate Law	rate = k[A]²	42
13761501137	0 Order Integrated Rate Law	[A] = -kt + [A]₀	43
13761501138	1st Order Integrated Rate Law	ln[A] = -kt + ln[A]₀	44
13761501139	2nd Order Integrated Rate Law	1/[A] = +kt + 1/[A]₀	45
13761501140	0 Order Graph		46
13761501141	1st Order Graph		47
13761501142	2nd Order Graph		48
13761501146	Zero Order Half Life	t½ = [A]₀ / 2k	49
13761501147	1st Order Half Life	t½ = 0.693 / k	50
13761501148	2nd Order Half Life	t½ = 1 / k [A]₀	51
13761501149	k<1	Left (k)	52
13761501150	k>1	Right (k)	53
13761501151	k = 1	At equilibrium (k)	54
13761501152	Q > k	Left (Q)	55
13761501153	Q < k	Right (Q)	56
13761501154	Q = k	At Equilibrium (Q)	57
13761501155	Remove reactant	Left (reactant)	58
13761501156	Add reactant	Right (product)	59
13761501157	Add inert gas	No change (gas)	60
13761501158	Add product	Left (reactant)	61
13761501159	Remove product	Right (product)	62
13761501213	Volume of container increases, More moles on left/less moles on right	Left (volume)	63
13761501161	Volume of container increases, More moles on right/less moles on left	Right (volume)	64
13761501162	Volume of container increases, Same number of moles on both sides	At equilibrium (volume)	65
13761501163	Increase temperature	Right (temperature)	66
13761501164	Decrease Temperature	Left (temperature)	67
13761501165	Exothermic	Left (exo/endo)	68
13761501166	Endothermic	Right (exo/endo)	69
13761501167	∆ - H	Left (∆H)	70
13761501168	∆ + H	Right (∆H)	71
13761501169	Volume of container decreases, More moles on left/less moles on right	right (volume)	72
13761501170	Volume of container decreases, More moles on right/less moles on left	left (volume)	73
13761501171	Alkali metals, ammonium, nitrates	always soluble	74
13761501176	hydroxides, carbonates, phosphates, and sulfites	insoluble except alkali & ammonium	75
13761501178	chlorides, bromides, and iodides	soluble except Ag, Pb, Hg, and Cu	76
13761501184	sulfides	soluble with alkali, ammonium, and alkaline only	77
13761501185	sulfates	soluble except Ca, Sr, Ba, Ra, Ag or Pb	78
13761501191	+ q	endothermic (q)	79
13761501192	-q	exothermic (q)	80
13761501193	+w	surroundings do work on the system (w)	81
13761501194	-w	system does work on the surroundings (w)	82
13761501195	breaking bonds	+ (bonds)	83
13761501196	forming bonds	- (bonds)	84
13761501197	+ ∆ H	absorbing heat, endothermic (∆H)	85
13761501198	-∆H	releasing heat, exothermic (∆H)	86
13761501199	+∆ S°	spontaneous (∆S)	87
13761501200	-∆ S°	not spontaneous (∆S)	88
13761501201	+∆ S° surr	entropy of universe increases (∆S Surroundings)	89
13761501218	-∆ S° surr	entropy of universe decreases (∆S Surroundings)	90
13761501202	+ ∆ G°	NOT spontaneous (∆G)	91
13761501203	- ∆ G°	Spontaneous (∆G)	92
13761501204	∆ G° = 0	System is in Equilibrium (∆G)	93
13761501205	when +∆ S° and -∆H	spontaneous at ALL temps (∆S & ∆H)	94
13761501206	when +∆ S° and +∆H	spontaneous at only high temps (∆S & ∆H)	95
13761501207	when -∆ S° and -∆H	spontaneous only at low temps (∆S & ∆H)	96
13761501208	when -∆ S° and +∆H	NOT spontaneous at any temps (∆S & ∆H)	97
13761501209	more gas moles on left (reactants)	-∆ S°	98
13761501210	more gas moles on right (products)	+∆ S°	99
13761501211	when +∆ G°	∆ S° is,-	100
13761501212	when -∆ G°	∆ S° is,+	101