AP Chemistry Final Review Flashcards

9830990979	STP Conditions	0 degrees Celsius, 22.4 L	0
9830990980	Density	mass / volume	1
9830990981	Molarity	moles / L	2
9830990982	Distillation	Depends on differences in volatility	3
9830990983	Filtration	Separating a solid from a liquid	4
9830990984	Chromatography	Separating substances through differences in rates	5
9830990985	Law of conservation of mass	Mass is neither created nor destroyed	6
9830990986	Dalton's Atomic Theory	Each element is made up of tiny particles called atoms. The atoms of a given element are identical. Chemical compounds are forms when atoms of different elements combine with each other. Chemical reactions involve reorganization of the atoms (changes in the way they are bound together.)	7
9830990987	JJ Thomson	Cathode Ray, discovered the electron	8
9830990988	Millikan	Oil Drop Experiment, determined mass and magnitude of the electron	9
9830990989	Rutherford	Gold Foil Experiment, discovered nuclei, atoms have a lot of space	10
9830990990	Solubility Rules	Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA	11
9830990991	Solubility Rules Exceptions	Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)	12
9830990992	Strong Electrolytes	Good conductors, easily ionized	13
9830990993	Weak Electrolytes	Conduct currents very weakly	14
9830990994	Strong Acids	HF, HBr, HCl, HClO4, HI, HClO3, HNO3	15
9830990995	Strong Bases	All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,	16
9830990996	Dilution Formula	M1V1 = M2V2	17
9830990997	Types of Chemical Reactions	Precipitation reactions, Acid-Base reactions, and Redox reactions	18
9830990998	Precipitation reaction	An insoluble substance is formed as a result of the reaction	19
9830990999	Spectator ions	Ions that do not participate in the reaction	20
9830991000	Bronsted-Lowry acid	Proton donor	21
9830991001	Bronsted-Lowry base	Proton acceptor	22
9830991002	Arrhenius acid	Produces H+ (H3O+) in water	23
9830991003	Arrhenius base	Produces OH- in water	24
9830991004	Lewis acid	Electron pair donor	25
9830991005	Lewis base	Electron pair acceptor	26
9830991006	Equivalence point	Enough titrant added to analyte	27
9830991007	Endpoint	Indicator changes color	28
9830991008	Redox reaction	Electrons are transferred	29
9830991009	Oxidation	Loss of electrons (LEO)	30
9830991010	Reduction	Gain of electrons (GER)	31
9830991011	Oxidizing agent	Causes oxidation (is often reduced)	32
9830991012	Reducing agent	Causes reduction (is often oxidized)	33
9830991013	1 standard atmosphere	1 atm, 760 mm Hg, 760 torr, 101,325 Pa	34
9830991014	Pressure	force / area	35
9830991015	Boyle's Law	P1V1 = P2V2	36
9830991016	Charles's Law	V1 / T1 = V2 / T2	37
9830991017	Ideal Gas Law	PV = nRT	38
9830991018	Molar mass of a gas	dRT / P	39
9830991019	Dalton's law of partial pressures	Ptot = P1 + P2 + P3...	40
9830991020	Mole fraction	n1 / ntot	41
9830991021	KMT	Volume of individual particles is negligible Particles are in constant motion Particles exert no forces on each other Collisions of particles with container walls are cause of pressure from gas	42
9830991022	Root mean square velocity	Average velocity of gas particles	43
9830991023	Diffusion	Mixing of gases	44
9830991024	Effusion	Gas into a vacuum	45
9830991223	Graham's law of effusion		46
9830991025	Law of conservation of energy	Energy can be converted but never destroyed	47
9830991026	Potential energy	Energy from position or composition	48
9830991027	Kinetic energy	Energy from motion	49
9830991028	Heat	Transfer of energy with temperature	50
9830991029	Work	Force acting over a distance	51
9830991030	Exothermic	Energy out of the system	52
9830991031	Endothermic	Energy into the system	53
9830991032	First law of thermodynamics	The energy of the universe is constant	54
9830991033	Internal energy (delta E)	delta E = q + w	55
9830991034	Enthalpy (delta H)	delta H = delta E + P(delta V)	56
9830991035	Heat capacity	heat absorbed / increase in temperature	57
9830991036	Calorimetry equation	q = mCAT	58
9830991037	Hess's Law Rules	If a reaction is reversed, the sign of delta H is reversed delta H is proportional to the quantities of reactions and products	59
9830991038	Standard enthalpy of formation	change in enthalpy with formation of one mole of compound from its elements	60
9830991039	Change in enthalpy for reaction	sum of heat of formations of products - sum of heat of formations of reactions	61
9830991040	Wavelength	distance between two peaks or troughs in a wave	62
9830991041	Frequency	number of cycles per second	63
9830991042	Basic wave equation	speed of light = wavelength x frequency	64
9830991043	Energy of a photon equation	Planck's constant x speed of light / frequency	65
9830991044	Photoelectric effect	Effect occurring when electrons are emitted from the surface of a metal when light strikes it	66
9830991045	Dual nature of light	Light acts as a wave and as particulate matter	67
9830991046	de Broglie's equation	Wavelength of a particle	68
9830991047	Diffraction	Light is scattered from points or lines	69
9830991048	Types of electromagnetic radiation (smallest to largest)	gamma, X-rays, UV, visible, IR, micro, radio	70
9830991049	Types of electromagnetic radiation (largest to smallest)	radio, micro, IR, visible, UV, X-rays, gamma	71
9830991050	Heisenberg Uncertainty Principle	We cannot know both the position and momentum of an electron (the more we know one, the less we know the other)	72
9830991051	Pauli exclusion principle	Electrons with the same spin cannot occupy the same space	73
9830991052	Aufbau principle	Progressively add electrons to each sub level	74
9830991053	Hund's rule	Different electrons to different orbitals, same spin	75
9830991054	Ionization energy	Energy required to remove a valence electron from an atom	76
9830991055	Electron affinity	Energy change associated with the addition of an electron to a gaseous atom	77
9830991056	Atomic radius trend	Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)	78
9830991057	Ionization energy trend	Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)	79
9830991058	Coulomb's law	Energy of interaction between a pair of ions	80
9830991059	Bond energy	Energy needed to break bond	81
9830991060	Covalent bonding	Electrons are shared by nuclei	82
9830991061	Electronegativity	Ability of an atom in a molecule to attract shared electrons to itself	83
9830991062	Dipolar or dipole moment	Has center of positive and center of negative charge	84
9830991063	Lattice energy	Change in energy when separated gas ions form an ionic solid Equation: LE = k(Q1Q2 / r) k is proportionality constant, Q is charge of ions, r is shortest distance between centers of ions	85
9830991064	Localized electron model	Molecule is composed of atoms bound together by sharing pairs of electrons	86
9830991065	Lone pairs	Pairs of electrons localized	87
9830991066	Localized electron model parts	Lewis diagram, VSEPR model (geometry), type of atomic orbitals	88
9830991067	Resonance	More than one valid Lewis structure	89
9830991068	Bond angle of a linear shape?	180	90
9830991069	Hybridization of a linear shape?	sp	91
9830991070	Number of bonds in a linear shape?	2	92
9830991071	Name of a linear shape?	MX2	93
9830991072	Bond angle of a trigonal planar shape?	120	94
9830991073	Hybridization of a trigonal planar shape?	sp2	95
9830991074	Number of bonds in a trigonal planar shape?	3	96
9830991075	Name of a trigonal planar shape?	MX3	97
9830991076	Bond angle of a bent shape?	<120	98
9830991077	Hybridization of a bent shape?	sp2	99
9830991078	Number of bonds in a bent shape?	2	100
9830991079	Number of nonbonding pairs in a bent shape?	1	101
9830991080	Bond angle of a tetrahedral shape?	109.5	102
9830991081	Hybridization of a tetrahedral shape?	sp3	103
9830991082	Number of bonds in a tetrahedral shape?	4	104
9830991083	Name of a tetrahedral shape?	MX4	105
9830991084	Bond angle of a trigonal pyramidal shape?	<109.5	106
9830991085	Hybridization of a trigonal pyramidal shape?	sp3	107
9830991086	Number of bonds in a trigonal pyramidal shape?	3	108
9830991087	Number of nonbonding pairs in a trigonal pyramidal shape?	1	109
9830991088	Name of a trigonal pyramidal shape?asily ionized	MX3	110
9830991089	Bond angle of a V shape?	<109.5	111
9830991090	Hybridization of a V shape?	sp3	112
9830991091	Number of a bonds in a V shape?	2	113
9830991092	Number of nonbonding pairs in a V shape?	2	114
9830991093	Name of a V shape?	M2X	115
9830991094	Bond angles of a trigonal bipyramidal shape?	120, 90	116
9830991095	Hybridization of a trigonal bipyramidal shape?	sp3d	117
9830991096	Number of bonds in a trigonal bipyramidal shape?	5	118
9830991097	Name of a trigonal bipyramidal shape?	MX5	119
9830991098	Bond angle of a see-saw shape?	<120, <90	120
9830991099	Hybridization of a see-saw shape?	sp3d	121
9830991100	Number of bonds in a see-saw shape?	4	122
9830991101	Number of nonbonding pairs in a see-saw shape?	1	123
9830991102	Bond angle of a T-shape?	<90	124
9830991103	Hybridization of a T-shape?	sp3d	125
9830991104	Number of bonds in a T-shape?	3	126
9830991105	Number of nonbonding pairs in a T-shape?	2	127
9830991106	Bond angle of a linear (2) shape?	180	128
9830991107	Hybridization of a linear (2) shape?	sp3d	129
9830991108	Number of bonds in a linear (2) shape?	2	130
9830991109	Number of nonbonding pairs in a linear (2) shape?	3	131
9830991110	Bond angle of an octahedron?	90	132
9830991111	Hybridization of an octahedron?	sp3d2	133
9830991112	Number of bonds in an octahedron?	6	134
9830991113	Name of an octahedron?	MX6	135
9830991114	Bond angle of a square pyramidal shape?	<90	136
9830991115	Hybridization of a square pyramidal shape?	sp3d2	137
9830991116	Number of bonds in a square pyramidal shape?	5	138
9830991117	Number of nonbonding pairs in a square pyramidal shape?	1	139
9830991118	Name of a square pyramidal shape?	MX5	140
9830991119	Bond angle of a square planar shape?	90	141
9830991120	Hybridization of a square planar shape?	sp3d2	142
9830991121	Number of bonds in a square planar shape?	4	143
9830991122	Number of nonbonding pair in a square planar shape?	2	144
9830991123	Name of a square planar shape?	MX4	145
9830991124	Metallic bond	Delocalized electron	146
9830991125	Nonpolar covalent bond	Equal sharing of electrons	147
9830991126	Polar covalent bond	Unequal sharing of electrons	148
9830991127	Ionic bond	Transfer of electrons	149
9830991128	Electronegativity differences	Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)	150
9830991129	Sigma bond	Bond between the s orbitals	151
9830991130	Pi bond	Bond between the p orbitals	152
9830991131	Hydrogen bond	Special type of dipole, hydrogen with N, F, or O atom	153
9830991132	London dispersion forces	Between non polar molecules	154
9830991133	Alloy	Contains a mixture of elements and has metallic properties	155
9830991134	Substitutional alloy	Metal atoms replaced by metal atoms of same size	156
9830991135	Interstitial alloy	Small atoms in holes	157
9830991136	Vapor pressure	Pressure of vapor at equilibrium	158
9830991137	Vapor pressure formula (Hg column)	Patmosphere = Pvapor +Pmercury column	159
9830991138	Temperature and vapor pressure?	Vapor pressure increases significantly with temperature	160
9830991139	IMFs and vapor pressure?	High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure	161
9830991140	Crystalline solids	Components organized in a lattice	162
9830991141	Amorphous solids	Components frozen in place with no arrangement	163
9830991142	Heat of fusion	Enthalpy change which occurs at the melting point when a solid melts	164
9830991143	Sublimation	Solid directly to gas	165
9830991144	Triple point	Where all three states exist	166
9830991145	Critical temperature	Temperature above which vapor cannot be liquefied no matter the pressure	167
9830991146	Critical pressure	Pressure required to produce liquefaction at the critical temperature	168
9830991147	Critical point	Critical temperature and critical point	169
9830991148	Phase diagram	Representation of phases of a substance	170
9830991149	Heat of solution	Enthalpy change formation of a solution, sum of enthalpy values from each step	171
9830991150	Positive delta H	Energy absorbed	172
9830991151	Negative delta H	Energy released	173
9830991152	Pressure and solubility	Increases solubility of a gas	174
9830991153	Henry's Law	Amount of gas dissolved proportional to pressure of gas above solution	175
9830991154	Temperature and solubility	Increases solubility of solid, decreases solubility of gases	176
9830991155	Raoult's Law	Nonvolatile solute simply dilutes the solvent	177
9830991156	Negative deviation from Raoult's law	More IMFs, lower vapor pressure	178
9830991157	Positive deviation from Raoult's law	Less IMFs, more molecules escape, higher vapor pressure	179
9830991158	Colligative properties	Freezing point depression, boiling point elevation, osmotic pressure	180
9830991159	Tyndall effect	Scattering of light by particles	181
9830991160	Colloid	Suspension of particles	182
9830991161	Coagulation	Destruction of colloid by heating or adding electrolyte	183
9830991162	Reaction rate	Change of concentration over time (Rate = delta [A] / delta t)	184
9830991163	Rate law	Rate depends on concentration	185
9830991164	Integrated rate law	Concentrations depends on time	186
9830991165	Initial rate	Instantaneous rate after reaction begins	187
9830991166	Catalyst	Increases rate of reaction but not consumed	188
9830991167	Surface area and rate	More surface area increases rate	189
9830991168	Temperature and rate	Higher temperature increases rate	190
9830991169	Zeroth order rate law	Rate = k	191
9830991170	Zeroth order integrated rate law	[A] = -kt + [A]0	192
9830991171	Zeroth order plot	[A] vs. t	193
9830991172	Zeroth order slope	Slope = -k	194
9830991173	Zeroth order half life	t1/2 = [A]0 / 2k	195
9830991174	First order rate law	Rate = k[A]	196
9830991175	First order integrated rate law	ln[A] = - kt + ln[A]0	197
9830991176	First order plot	ln[A] vs. t	198
9830991177	First order slope	Slope = -k	199
9830991178	First order half life	t1/2 = 0.693 / k	200
9830991179	Second order rate law	Rate = k[A]2	201
9830991180	Second order integrated rate law	1/[A] = kt + 1/[A]0	202
9830991181	Second order plot	1/[A] vs. t	203
9830991182	Second order slope	Slope = k	204
9830991183	Second order half life	t1/2 = 1 / k[A]0	205
9830991184	Reaction mechanism	Series of steps	206
9830991185	A --> products	Rate = k[A]	207
9830991186	A + A --> products	Rate = k[A]2	208
9830991187	A + B --> products	Rate = k[A][B]	209
9830991188	A + A + B --> products	Rate = k[A]2[B]	210
9830991189	A + B + C --> products	Rate = k[A][B][C]	211
9830991190	Rate determining step	Slowest step	212
9830991191	Reaction mechanism requirements	Sum must give balanced equation, mechanism must agree with rate law	213
9830991192	Equilibrium expression	Products raised to coeffs over reactants raised to coeffs	214
9830991193	Q = k	Equilibrium, no shift	215
9830991194	Q > k	Shift to reactants	216
9830991195	Q < k	Shift to products	217
9830991196	Le Chatlier's Principle	Change imposed, equilibrium shifts to lessen change	218
9830991197	More product added	Shift to reactants	219
9830991198	More reactant added	Shift to product	220
9830991199	How to change the pressure of a reaction system?	Add or remove gas, add an inert gas, change volume	221
9830991200	Ka	Acid dissociation constant	222
9830991201	Strong acid	Equilibrium is far to the right, has weak conjugate base	223
9830991202	Weak acid	Equilibrium is far to the left	224
9830991203	Monoprotic acids	One acidic proton	225
9830991204	Amphoteric	Can behave as an acid or a base (water)	226
9830991205	Kw	Water dissociation constant	227
9830991206	pH	-log[H+]	228
9830991207	pOH	-log[OH-]	229
9830991208	pK	-logK	230
9830991209	pH of strong acids	Depends on concentration of H+ ions	231
9830991210	pH of weak acids	Find Ka and use an ice chart	232
9830991211	Percent dissociation	Amount dissociated M / initial concentration M x 100%	233
9830991212	Polyprotic acids	Dissociates in a stepwise manner, find Ka of each step	234
9830991213	Bond strength and acid strength	Less bond strength, more acid strength	235
9830991214	Common ion effect	Shift in equilibrium because of addition of common ion	236
9830991215	Buffer	Resists a change in pH	237
9830991216	Henderson Hasselbach Equation	Used to find the pH of a buffer	238
9830991217	Strong acid-strong base titration curve	Equivalence point is 7	239
9830991218	Weak acid-strong base titration curve	Equivalence point is greater than 7, has a halfway equivalence point	240
9830991219	Acid-base indicator	Changes color at the end point (not same as equivalence point)	241
9830991220	pH of indicator	Ka/[H+] = [In-]/[HIn] = 1/10, ratio reversed for bases	242
9830991221	Ksp	Solubility product	243

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AP Chemistry Final Review Flashcards

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