AP Chemistry Final Review Flashcards

8847084220	STP Conditions	0 degrees Celsius, 22.4 L	0
8847084221	Density	mass / volume	1
8847084222	Molarity	moles / L	2
8847084223	Distillation	Depends on differences in volatility	3
8847084224	Filtration	Separating a solid from a liquid	4
8847084225	Chromatography	Separating substances through differences in rates	5
8847084226	Law of conservation of mass	Mass is neither created nor destroyed	6
8847084227	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
8847084228	JJ Thomson	Cathode Ray, discovered the electron	8
8847084229	Millikan	Oil Drop Experiment, determined mass and magnitude of the electron	9
8847084230	Rutherford	Gold Foil Experiment, discovered nuclei, atoms have a lot of space	10
8847084231	Solubility Rules	Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA	11
8847084232	Solubility Rules Exceptions	Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)	12
8847084233	Strong Electrolytes	Good conductors, easily ionized	13
8847084234	Weak Electrolytes	Conduct currents very weakly	14
8847084235	Strong Acids	HF, HBr, HCl, HClO4, HI, HClO3, HNO3	15
8847084236	Strong Bases	All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,	16
8847084237	Dilution Formula	M1V1 = M2V2	17
8847084238	Types of Chemical Reactions	Precipitation reactions, Acid-Base reactions, and Redox reactions	18
8847084239	Precipitation reaction	An insoluble substance is formed as a result of the reaction	19
8847084240	Spectator ions	Ions that do not participate in the reaction	20
8847084241	Bronsted-Lowry acid	Proton donor	21
8847084242	Bronsted-Lowry base	Proton acceptor	22
8847084243	Arrhenius acid	Produces H+ (H3O+) in water	23
8847084244	Arrhenius base	Produces OH- in water	24
8847084245	Lewis acid	Electron pair donor	25
8847084246	Lewis base	Electron pair acceptor	26
8847084247	Equivalence point	Enough titrant added to analyte	27
8847084248	Endpoint	Indicator changes color	28
8847084249	Redox reaction	Electrons are transferred	29
8847084250	Oxidation	Loss of electrons (LEO)	30
8847084251	Reduction	Gain of electrons (GER)	31
8847084252	Oxidizing agent	Causes oxidation (is often reduced)	32
8847084253	Reducing agent	Causes reduction (is often oxidized)	33
8847084254	1 standard atmosphere	1 atm, 760 mm Hg, 760 torr, 101,325 Pa	34
8847084255	Pressure	force / area	35
8847084256	Boyle's Law	P1V1 = P2V2	36
8847084257	Charles's Law	V1 / T1 = V2 / T2	37
8847084258	Ideal Gas Law	PV = nRT	38
8847084259	Molar mass of a gas	dRT / P	39
8847084260	Dalton's law of partial pressures	Ptot = P1 + P2 + P3...	40
8847084261	Mole fraction	n1 / ntot	41
8847084262	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
8847084263	Root mean square velocity	Average velocity of gas particles	43
8847084264	Diffusion	Mixing of gases	44
8847084265	Effusion	Gas into a vacuum	45
8847084266	Graham's law of effusion		46
8847084267	Law of conservation of energy	Energy can be converted but never destroyed	47
8847084268	Potential energy	Energy from position or composition	48
8847084269	Kinetic energy	Energy from motion	49
8847084270	Heat	Transfer of energy with temperature	50
8847084271	Work	Force acting over a distance	51
8847084272	Exothermic	Energy out of the system	52
8847084273	Endothermic	Energy into the system	53
8847084274	First law of thermodynamics	The energy of the universe is constant	54
8847084275	Internal energy (delta E)	delta E = q + w	55
8847084276	Enthalpy (delta H)	delta H = delta E + P(delta V)	56
8847084277	Heat capacity	heat absorbed / increase in temperature	57
8847084278	Calorimetry equation	q = mCAT	58
8847084279	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
8847084280	Standard enthalpy of formation	change in enthalpy with formation of one mole of compound from its elements	60
8847084281	Change in enthalpy for reaction	sum of heat of formations of products - sum of heat of formations of reactions	61
8847084282	Wavelength	distance between two peaks or troughs in a wave	62
8847084283	Frequency	number of cycles per second	63
8847084284	Basic wave equation	speed of light = wavelength x frequency	64
8847084285	Energy of a photon equation	Planck's constant x speed of light / frequency	65
8847084286	Photoelectric effect	Effect occurring when electrons are emitted from the surface of a metal when light strikes it	66
8847084287	Dual nature of light	Light acts as a wave and as particulate matter	67
8847084288	de Broglie's equation	Wavelength of a particle	68
8847084289	Diffraction	Light is scattered from points or lines	69
8847084290	Types of electromagnetic radiation (smallest to largest)	gamma, X-rays, UV, visible, IR, micro, radio	70
8847084291	Types of electromagnetic radiation (largest to smallest)	radio, micro, IR, visible, UV, X-rays, gamma	71
8847084292	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
8847084293	Pauli exclusion principle	Electrons with the same spin cannot occupy the same space	73
8847084294	Aufbau principle	Progressively add electrons to each sub level	74
8847084295	Hund's rule	Different electrons to different orbitals, same spin	75
8847084296	Ionization energy	Energy required to remove a valence electron from an atom	76
8847084297	Electron affinity	Energy change associated with the addition of an electron to a gaseous atom	77
8847084298	Atomic radius trend	Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)	78
8847084299	Ionization energy trend	Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)	79
8847084300	Coulomb's law	Energy of interaction between a pair of ions	80
8847084301	Bond energy	Energy needed to break bond	81
8847084302	Covalent bonding	Electrons are shared by nuclei	82
8847084303	Electronegativity	Ability of an atom in a molecule to attract shared electrons to itself	83
8847084304	Dipolar or dipole moment	Has center of positive and center of negative charge	84
8847084305	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
8847084306	Localized electron model	Molecule is composed of atoms bound together by sharing pairs of electrons	86
8847084307	Lone pairs	Pairs of electrons localized	87
8847084308	Localized electron model parts	Lewis diagram, VSEPR model (geometry), type of atomic orbitals	88
8847084309	Resonance	More than one valid Lewis structure	89
8847084310	Bond angle of a linear shape?	180	90
8847084311	Hybridization of a linear shape?	sp	91
8847084312	Number of bonds in a linear shape?	2	92
8847084313	Name of a linear shape?	MX2	93
8847084314	Bond angle of a trigonal planar shape?	120	94
8847084315	Hybridization of a trigonal planar shape?	sp2	95
8847084316	Number of bonds in a trigonal planar shape?	3	96
8847084317	Name of a trigonal planar shape?	MX3	97
8847084318	Bond angle of a bent shape?	<120	98
8847084319	Hybridization of a bent shape?	sp2	99
8847084320	Number of bonds in a bent shape?	2	100
8847084321	Number of nonbonding pairs in a bent shape?	1	101
8847084322	Bond angle of a tetrahedral shape?	109.5	102
8847084323	Hybridization of a tetrahedral shape?	sp3	103
8847084324	Number of bonds in a tetrahedral shape?	4	104
8847084325	Name of a tetrahedral shape?	MX4	105
8847084326	Bond angle of a trigonal pyramidal shape?	<109.5	106
8847084327	Hybridization of a trigonal pyramidal shape?	sp3	107
8847084328	Number of bonds in a trigonal pyramidal shape?	3	108
8847084329	Number of nonbonding pairs in a trigonal pyramidal shape?	1	109
8847084330	Name of a trigonal pyramidal shape?asily ionized	MX3	110
8847084331	Bond angle of a V shape?	<109.5	111
8847084332	Hybridization of a V shape?	sp3	112
8847084333	Number of a bonds in a V shape?	2	113
8847084334	Number of nonbonding pairs in a V shape?	2	114
8847084335	Name of a V shape?	M2X	115
8847084336	Bond angles of a trigonal bipyramidal shape?	120, 90	116
8847084337	Hybridization of a trigonal bipyramidal shape?	sp3d	117
8847084338	Number of bonds in a trigonal bipyramidal shape?	5	118
8847084339	Name of a trigonal bipyramidal shape?	MX5	119
8847084340	Bond angle of a see-saw shape?	<120, <90	120
8847084341	Hybridization of a see-saw shape?	sp3d	121
8847084342	Number of bonds in a see-saw shape?	4	122
8847084343	Number of nonbonding pairs in a see-saw shape?	1	123
8847084344	Bond angle of a T-shape?	<90	124
8847084345	Hybridization of a T-shape?	sp3d	125
8847084346	Number of bonds in a T-shape?	3	126
8847084347	Number of nonbonding pairs in a T-shape?	2	127
8847084348	Bond angle of a linear (2) shape?	180	128
8847084349	Hybridization of a linear (2) shape?	sp3d	129
8847084350	Number of bonds in a linear (2) shape?	2	130
8847084351	Number of nonbonding pairs in a linear (2) shape?	3	131
8847084352	Bond angle of an octahedron?	90	132
8847084353	Hybridization of an octahedron?	sp3d2	133
8847084354	Number of bonds in an octahedron?	6	134
8847084355	Name of an octahedron?	MX6	135
8847084356	Bond angle of a square pyramidal shape?	<90	136
8847084357	Hybridization of a square pyramidal shape?	sp3d2	137
8847084358	Number of bonds in a square pyramidal shape?	5	138
8847084359	Number of nonbonding pairs in a square pyramidal shape?	1	139
8847084360	Name of a square pyramidal shape?	MX5	140
8847084361	Bond angle of a square planar shape?	90	141
8847084362	Hybridization of a square planar shape?	sp3d2	142
8847084363	Number of bonds in a square planar shape?	4	143
8847084364	Number of nonbonding pair in a square planar shape?	2	144
8847084365	Name of a square planar shape?	MX4	145
8847084366	Metallic bond	Delocalized electron	146
8847084367	Nonpolar covalent bond	Equal sharing of electrons	147
8847084368	Polar covalent bond	Unequal sharing of electrons	148
8847084369	Ionic bond	Transfer of electrons	149
8847084370	Electronegativity differences	Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)	150
8847084371	Sigma bond	Bond between the s orbitals	151
8847084372	Pi bond	Bond between the p orbitals	152
8847084373	Hydrogen bond	Special type of dipole, hydrogen with N, F, or O atom	153
8847084374	London dispersion forces	Between non polar molecules	154
8847084375	Alloy	Contains a mixture of elements and has metallic properties	155
8847084376	Substitutional alloy	Metal atoms replaced by metal atoms of same size	156
8847084377	Interstitial alloy	Small atoms in holes	157
8847084378	Vapor pressure	Pressure of vapor at equilibrium	158
8847084379	Vapor pressure formula (Hg column)	Patmosphere = Pvapor +Pmercury column	159
8847084380	Temperature and vapor pressure?	Vapor pressure increases significantly with temperature	160
8847084381	IMFs and vapor pressure?	High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure	161
8847084382	Crystalline solids	Components organized in a lattice	162
8847084383	Amorphous solids	Components frozen in place with no arrangement	163
8847084384	Heat of fusion	Enthalpy change which occurs at the melting point when a solid melts	164
8847084385	Sublimation	Solid directly to gas	165
8847084386	Triple point	Where all three states exist	166
8847084387	Critical temperature	Temperature above which vapor cannot be liquefied no matter the pressure	167
8847084388	Critical pressure	Pressure required to produce liquefaction at the critical temperature	168
8847084389	Critical point	Critical temperature and critical point	169
8847084390	Phase diagram	Representation of phases of a substance	170
8847084391	Heat of solution	Enthalpy change formation of a solution, sum of enthalpy values from each step	171
8847084392	Positive delta H	Energy absorbed	172
8847084393	Negative delta H	Energy released	173
8847084394	Pressure and solubility	Increases solubility of a gas	174
8847084395	Henry's Law	Amount of gas dissolved proportional to pressure of gas above solution	175
8847084396	Temperature and solubility	Increases solubility of solid, decreases solubility of gases	176
8847084397	Raoult's Law	Nonvolatile solute simply dilutes the solvent	177
8847084398	Negative deviation from Raoult's law	More IMFs, lower vapor pressure	178
8847084399	Positive deviation from Raoult's law	Less IMFs, more molecules escape, higher vapor pressure	179
8847084400	Colligative properties	Freezing point depression, boiling point elevation, osmotic pressure	180
8847084401	Tyndall effect	Scattering of light by particles	181
8847084402	Colloid	Suspension of particles	182
8847084403	Coagulation	Destruction of colloid by heating or adding electrolyte	183
8847084404	Reaction rate	Change of concentration over time (Rate = delta [A] / delta t)	184
8847084405	Rate law	Rate depends on concentration	185
8847084406	Integrated rate law	Concentrations depends on time	186
8847084407	Initial rate	Instantaneous rate after reaction begins	187
8847084408	Catalyst	Increases rate of reaction but not consumed	188
8847084409	Surface area and rate	More surface area increases rate	189
8847084410	Temperature and rate	Higher temperature increases rate	190
8847084411	Zeroth order rate law	Rate = k	191
8847084412	Zeroth order integrated rate law	[A] = -kt + [A]0	192
8847084413	Zeroth order plot	[A] vs. t	193
8847084414	Zeroth order slope	Slope = -k	194
8847084415	Zeroth order half life	t1/2 = [A]0 / 2k	195
8847084416	First order rate law	Rate = k[A]	196
8847084417	First order integrated rate law	ln[A] = - kt + ln[A]0	197
8847084418	First order plot	ln[A] vs. t	198
8847084419	First order slope	Slope = -k	199
8847084420	First order half life	t1/2 = 0.693 / k	200
8847084421	Second order rate law	Rate = k[A]2	201
8847084422	Second order integrated rate law	1/[A] = kt + 1/[A]0	202
8847084423	Second order plot	1/[A] vs. t	203
8847084424	Second order slope	Slope = k	204
8847084425	Second order half life	t1/2 = 1 / k[A]0	205
8847084426	Reaction mechanism	Series of steps	206
8847084427	A --> products	Rate = k[A]	207
8847084428	A + A --> products	Rate = k[A]2	208
8847084429	A + B --> products	Rate = k[A][B]	209
8847084430	A + A + B --> products	Rate = k[A]2[B]	210
8847084431	A + B + C --> products	Rate = k[A][B][C]	211
8847084432	Rate determining step	Slowest step	212
8847084433	Reaction mechanism requirements	Sum must give balanced equation, mechanism must agree with rate law	213
8847084434	Equilibrium expression	Products raised to coeffs over reactants raised to coeffs	214
8847084435	Q = k	Equilibrium, no shift	215
8847084436	Q > k	Shift to reactants	216
8847084437	Q < k	Shift to products	217
8847084438	Le Chatlier's Principle	Change imposed, equilibrium shifts to lessen change	218
8847084439	More product added	Shift to reactants	219
8847084440	More reactant added	Shift to product	220
8847084441	How to change the pressure of a reaction system?	Add or remove gas, add an inert gas, change volume	221
8847084442	Ka	Acid dissociation constant	222
8847084443	Strong acid	Equilibrium is far to the right, has weak conjugate base	223
8847084444	Weak acid	Equilibrium is far to the left	224
8847084445	Monoprotic acids	One acidic proton	225
8847084446	Amphoteric	Can behave as an acid or a base (water)	226
8847084447	Kw	Water dissociation constant	227
8847084448	pH	-log[H+]	228
8847084449	pOH	-log[OH-]	229
8847084450	pK	-logK	230
8847084451	pH of strong acids	Depends on concentration of H+ ions	231
8847084452	pH of weak acids	Find Ka and use an ice chart	232
8847084453	Percent dissociation	Amount dissociated M / initial concentration M x 100%	233
8847084454	Polyprotic acids	Dissociates in a stepwise manner, find Ka of each step	234
8847084455	Bond strength and acid strength	Less bond strength, more acid strength	235
8847084456	Common ion effect	Shift in equilibrium because of addition of common ion	236
8847084457	Buffer	Resists a change in pH	237
8847084458	Henderson Hasselbach Equation	Used to find the pH of a buffer	238
8847084459	Strong acid-strong base titration curve	Equivalence point is 7	239
8847084460	Weak acid-strong base titration curve	Equivalence point is greater than 7, has a halfway equivalence point	240
8847084461	Acid-base indicator	Changes color at the end point (not same as equivalence point)	241
8847084462	pH of indicator	Ka/[H+] = [In-]/[HIn] = 1/10, ratio reversed for bases	242
8847084463	Ksp	Solubility product	243

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AP Chemistry Final Review Flashcards

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