AP Chemistry Flashcards

13906489454	Oxidation	loss of electrons	0
13906489455	Reduction	gain of electrons	1
13906498904	Oxide	a binary compound of oxygen with another element or group.	2
13906504333	Oxidizing agent	electron acceptor	3
13906507347	Reducing agent	electron donor	4
13906516611	Strong Acids	HCl, HBr, HI, HNO3, H2SO4, HClO4	5
13906520013	Strong bases	1A and heavy 2A hydroxides	6
13906546900	gas forming reactions	H2CO3 -> H2O + CO2 S + H2 -> H2S(g)	7
13906557366	Electrolyte	dissociates	8
13906562144	strong electrolyte	dissociates completely	9
13906566466	weak electrolyte	partially dissociate	10
13906577040	Periodicity	the repeating pattern of chemical and physical properties of the elements	11
13906577042	Coulombs Law	F=K q₁*q₂/r²	12
13906585298	Zeff (effective nuclear charge)	Z (Atomic #) - S (Screening constant = #inner electrons)	13
13906602440	Size of Atom trend	Increases down and left (Zeff increases)	14
13906614909	Size of ions	- Cations are smaller than original atom - Anions are larger - Ion size increases down a group - From left to right they get smaller (because nuclear charge increases), then suddenly larger (once it changes from cations to anions)	15
13906620512	Ionization energy	The amount of energy required to remove an electron from an atom	16
13906625198	Ionization energy trend	increases up and to the right	17
13906635480	Smaller atoms have ___ ionization energies	higher	18
13906642143	electron affinity	the energy change that occurs when an electron is acquired by a neutral atom	19
13906646192	electron affinity trend	increases to the right and up	20
13906655655	lattice energy	the energy released when one mole of an ionic crystalline compound is formed from gaseous ions	21
13906657346	Lattice energy trend	increases up and to the right	22
13906660713	Electronegativity	A measure of the ability of an atom in a chemical compound to attract electrons	23
13906660715	electronegativity trend	increases up and to the right	24
13906667326	Lewis dot structure steps		25
13906698255	free radicals	chemical particles with an odd number of electrons	26
13906700408	Hypervalent	molecules and ions with more than an octet of electrons around the central atom	27
13906702753	electron domain	in the VSEPR model, a region about a central atom in which an electron pair is concentrated	28
13906706501	Kinetic Molecular Theory of Gases	1. gases made up of negligible volume 2. no intermolecular attractions/repulsions 3. elastical collisions 4. constant random motion 5. kinetic energy of gas is related to T 6. same moles of gas=same kinetic energy	29
13906738308	Celcius to Kelvin	K=C+273	30
13906742475	van der Waals equation	[P+(an^2)/(V^2)][V-nb]=nRT a = strength of attraction b = Size of molecule	31
13906756410	Real Gas Law	Real gasses only conform to PV=nRT at Low pressures High temps	32
13906774475	Effusion	A process by which gas particles pass through a tiny opening	33
13906776273	Diffusion	Movement of molecules from an area of higher concentration to an area of lower concentration.	34
13906780719	Kinetic energy of gas	KE=1/2mv^2 Same Temp - KE = KE	35
13906789700	Grams law of effusion		36
13906803854	van der Waals forces	a slight attraction that develops between the oppositely charged regions of nearby molecules	37
13906808402	London dispersion forces	- Attractions between momentary dipole - All molecules - Polarizability	38
13906823114	London Dispersion forces are effected by...	Usually Weak Shape - Long skinny have stronger Weight - Increases with molecular weight. Larger clouds are easier to polarize	39
13906832748	dipole-dipole forces	attractions between oppositely charged regions of polar molecules	40
13906837310	dipole-dipole forces are effected by...	Polarity - Increases with increase in polarity	41
13906856563	Hydrogen Bonding	Very Strong Dipole-Dipole interaction with H + N, O, or F	42
13906867447	Viscosity	resistance to flow	43
13906868963	surface tension	A measure of how difficult it is to stretch or break the surface of a liquid	44
13906868964	Vapor Pressure	- As temp rises, the fraction of molecules having enough energy to escape increases - Pressure increase	45
13906905665	Boiling poing	When its Vapor pressure = Atmospheric Pressure	46
13906908591	Normal Boiling Point	The T that VP is 760 torr or 1 ATM	47
13906914380	Heat of fusion	Amount of energy required to change a substance from the solid phase to the liquid phase.	48
13906914381	heat of vaporization	The amount of energy required for the liquid at its boiling point to become a gas	49
13906916823	Triple Point	3 phases coexist	50
13906923821	rate of reaction depends on	Catalyst Higher Temp Concentration Homogeneous mixture	51
13906933541	Reaction rate equation (change in concentration	-Δ[A]/Δt = Δ[B]/Δt	52
13906942699	steric factor	Size + Orientation	53
13906950394	Rate Equation	rate = K[A]^a[B]^b	54
13923106378	Activated complex	a transitional structure that results from an effective collision and that persists while old bonds are breaking and new bonds are forming	55
13923112000	Maxwell-Boltzmann distribution	The distribution of energies (and therefore speeds) of the molecules in a gas or liquid.	56
13923138907	Arrhenius equation	K=Ae^(-Ea/RT) k is the rate constant A is pre-exponential factor: how often particles collide in correct orientation.	57
13923212924	reaction mechanism	the step-by-step sequence of reactions by which the overall chemical change occurs	58
13923222789	elementary reaction	a reaction in which reactants are converted to products in a single step	59
13923240000	molecularity	the number of molecules that participate as reactants in an elementary reaction	60
13923245948	rate law and order for elementary reactions is determined by	Coefficients	61
13923295642	Kp to Kc	Kp = Kc(RT)^delta n	62
13923303754	Kp = Kc when	there are the same number of moles of gas on each side of the equation	63
13923308986	Keq > 1	products are favored	64
13923311526	Keq < 1	reactants favored	65
13923330309	k = q when	System is in equilibrium	66
13923339118	Equilibrium Quotient	Q = [Products]/[Reactants]	67
13923905469	Q > K	shift left	68
13923908069	Q < K	shift right	69
13923917227	Amphiprotic	A species that can either accept or donate a proton.	70
13923917228	Amphoteric	a substance that can act as both an acid and a base	71
13923930504	Kw	1.0 x 10^-14	72
13923930505	pH	= -log[H+]	73
13923944849	% Ionization	[H3O+eq]/[HAinitial] x 100	74
13923964716	Ka	acid dissociation constant	75
13923964717	Kb	base dissociation constant	76
13923972850	Higher Kb	stronger base	77
13923972851	Lower Ka	weaker acid	78
13923975356	Higher Ka	stronger acid	79
13923975357	Lower Kb	weaker base	80
13923981939	polyprotic acid	an acid that can donate more than one proton per molecule	81
13923987418	Ka * Kb	Kw	82
13923991850	pH + pOH =	14	83
13923991852	pKa + pKb =	pKw = 14	84
13924011211	Factors affecting acid strenght	- Polarization of Hx bond - Stronger bond = weaker acid - Less stability = weaker acid	85
13924023595	If x is in same group bond strenght is _ important	more	86
13924048284	If x is in the same period, bond polarity is _ important	more	87
13924059537	Carboxilic Acid	COOH	88
13924078269	Carboxilic Acids draw ___ from ___ Increase ___ of bond Increases ____	- Electron density, OH bond - Polarity - Acidity	89
13924094001	Bottom Line of acid strenght	Anything that pulls electrons away from the ionizable hydrogen (making a weaker bond) makes the acid more acidic	90
13924113626	common ion effect	a decrease in the solubility of an ionic compound caused by the addition of a common ion	91
13924116202	Buffer	compound that prevents sharp, sudden changes in pH	92
13924119509	Henderson-Hasselbalch equation	pH = pKa + log [A-]/[HA]	93
13924124516	Strong acid-strong base titration curve	equivalence point: pH=7	94
13924134039	Weak acid-strong base titration curve	Equivalence point is greater than 7, has a halfway equivalence point	95
13924144006	strong acid weak base titration	Slow decline in pH followed by a rapid decrease at equivalence point. End point of indicator should be < 7.	96
13924196420	Ksp =	[prodA][prodB] (the bigger, the more soluble)	97
13924207529	Heat up and cool down	q = mc{delta}t	98
13924216368	Phase Change	q = n{delta}h fus/vap	99
13924230060	Hess's law	the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process	100
13924238421	calorimetry equation	mcdeltaT=mcdeltaT	101
13924286760	deltaSsurr=	-deltaH/T	102
13924300068	Oxidation occurs at the	anode	103
13924302664	Reduction occurs at the	cathode	104
13924307321	electromotive force (emf)	The power supplied by the supply per unit current.	105
13924328654	A stronger oxidizing agent exhibits more _______	Positive reduction potential	106