AP Chemistry Vocabulary Flashcards

9556175096	STP Conditions	0 degrees Celsius, 22.4 L	0
9556175097	Density	mass / volume	1
9556175098	Molarity	moles / L	2
9556175099	Distillation	Depends on differences in volatility	3
9556175100	Filtration	Separating a solid from a liquid	4
9556175101	Chromatography	Separating substances through differences in rates	5
9556175102	Law of conservation of mass	Mass is neither created nor destroyed	6
9556175103	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
9556175104	JJ Thomson	Cathode Ray, discovered the electron	8
9556175105	Millikan	Oil Drop Experiment, determined mass and magnitude of the electron	9
9556175106	Rutherford	Gold Foil Experiment, discovered nuclei, atoms have a lot of space	10
9556175107	Solubility Rules	Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA	11
9556175108	Solubility Rules Exceptions	Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)	12
9556175109	Strong Electrolytes	Good conductors, easily ionized	13
9556175110	Weak Electrolytes	Conduct currents very weakly	14
9556175111	Strong Acids	HF, HBr, HCl, HClO4, HI, HClO3, HNO3	15
9556175112	Strong Bases	All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,	16
9556175113	Dilution Formula	M1V1 = M2V2	17
9556175114	Types of Chemical Reactions	Precipitation reactions, Acid-Base reactions, and Redox reactions	18
9556175115	Precipitation reaction	An insoluble substance is formed as a result of the reaction	19
9556175116	Spectator ions	Ions that do not participate in the reaction	20
9556175117	Bronsted-Lowry acid	Proton donor	21
9556175118	Bronsted-Lowry base	Proton acceptor	22
9556175119	Arrhenius acid	Produces H+ (H3O+) in water	23
9556175120	Arrhenius base	Produces OH- in water	24
9556175121	Lewis acid	Electron pair donor	25
9556175122	Lewis base	Electron pair acceptor	26
9556175123	Equivalence point	Enough titrant added to analyte	27
9556175124	Endpoint	Indicator changes color	28
9556175125	Redox reaction	Electrons are transferred	29
9556175126	Oxidation	Loss of electrons (LEO)	30
9556175127	Reduction	Gain of electrons (GER)	31
9556175128	Oxidizing agent	Causes oxidation (is often reduced)	32
9556175129	Reducing agent	Causes reduction (is often oxidized)	33
9556175130	1 standard atmosphere	1 atm, 760 mm Hg, 760 torr, 101,325 Pa	34
9556175131	Pressure	force / area	35
9556175132	Boyle's Law	P1V1 = P2V2	36
9556175133	Charles's Law	V1 / T1 = V2 / T2	37
9556175134	Ideal Gas Law	PV = nRT	38
9556175135	Molar mass of a gas	dRT / P	39
9556175136	Dalton's law of partial pressures	Ptot = P1 + P2 + P3...	40
9556175137	Mole fraction	n1 / ntot	41
9556175138	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
9556175139	Root mean square velocity	Average velocity of gas particles	43
9556175140	Diffusion	Mixing of gases	44
9556175141	Effusion	Gas into a vacuum	45
9556175341	Graham's law of effusion		46
9556175142	Law of conservation of energy	Energy can be converted but never destroyed	47
9556175143	Potential energy	Energy from position or composition	48
9556175144	Kinetic energy	Energy from motion	49
9556175145	Heat	Transfer of energy with temperature	50
9556175146	Work	Force acting over a distance	51
9556175147	Exothermic	Energy out of the system	52
9556175148	Endothermic	Energy into the system	53
9556175149	First law of thermodynamics	The energy of the universe is constant	54
9556175150	Internal energy (delta E)	delta E = q + w	55
9556175151	Enthalpy (delta H)	delta H = delta E + P(delta V)	56
9556175152	Heat capacity	heat absorbed / increase in temperature	57
9556175153	Calorimetry equation	q = mCAT	58
9556175154	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
9556175155	Standard enthalpy of formation	change in enthalpy with formation of one mole of compound from its elements	60
9556175156	Change in enthalpy for reaction	sum of heat of formations of products - sum of heat of formations of reactions	61
9556175157	Wavelength	distance between two peaks or troughs in a wave	62
9556175158	Frequency	number of cycles per second	63
9556175159	Basic wave equation	speed of light = wavelength x frequency	64
9556175160	Energy of a photon equation	Planck's constant x speed of light / frequency	65
9556175161	Photoelectric effect	Effect occurring when electrons are emitted from the surface of a metal when light strikes it	66
9556175162	Dual nature of light	Light acts as a wave and as particulate matter	67
9556175163	de Broglie's equation	Wavelength of a particle	68
9556175164	Diffraction	Light is scattered from points or lines	69
9556175165	Types of electromagnetic radiation (smallest to largest)	gamma, X-rays, UV, visible, IR, micro, radio	70
9556175166	Types of electromagnetic radiation (largest to smallest)	radio, micro, IR, visible, UV, X-rays, gamma	71
9556175167	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
9556175168	Pauli exclusion principle	Electrons with the same spin cannot occupy the same space	73
9556175169	Aufbau principle	fill in order of increasing energy	74
9556175170	Hund's rule	each orbital must have 1 e- before it can have another	75
9556175171	Ionization energy	Energy required to remove a valence electron from an atom	76
9556175172	Electron affinity	Energy change associated with the addition of an electron to a gaseous atom	77
9556175173	Atomic radius trend	Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)	78
9556175174	Ionization energy trend	Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)	79
9556175175	Coulomb's law	Energy of interaction between a pair of ions	80
9556175176	Bond energy	Energy needed to break bond	81
9556175177	Covalent bonding	Electrons are shared by nuclei	82
9556175178	Electronegativity	Ability of an atom in a molecule to attract shared electrons to itself	83
9556175179	Dipolar or dipole moment	Has center of positive and center of negative charge	84
9556175180	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
9556175181	Localized electron model	Molecule is composed of atoms bound together by sharing pairs of electrons	86
9556175182	Lone pairs	Pairs of electrons localized	87
9556175183	Localized electron model parts	Lewis diagram, VSEPR model (geometry), type of atomic orbitals	88
9556175184	Resonance	More than one valid Lewis structure	89
9556175185	Bond angle of a linear shape?	180	90
9556175186	Hybridization of a linear shape?	sp	91
9556175187	Number of bonds in a linear shape?	2	92
9556175188	Name of a linear shape?	MX2	93
9556175189	Bond angle of a trigonal planar shape?	120	94
9556175190	Hybridization of a trigonal planar shape?	sp2	95
9556175191	Number of bonds in a trigonal planar shape?	3	96
9556175192	Name of a trigonal planar shape?	MX3	97
9556175193	Bond angle of a bent shape?	<120	98
9556175194	Hybridization of a bent shape?	sp2	99
9556175195	Number of bonds in a bent shape?	2	100
9556175196	Number of nonbonding pairs in a bent shape?	1	101
9556175197	Bond angle of a tetrahedral shape?	109.5	102
9556175198	Hybridization of a tetrahedral shape?	sp3	103
9556175199	Number of bonds in a tetrahedral shape?	4	104
9556175200	Name of a tetrahedral shape?	MX4	105
9556175201	Bond angle of a trigonal pyramidal shape?	<109.5	106
9556175202	Hybridization of a trigonal pyramidal shape?	sp3	107
9556175203	Number of bonds in a trigonal pyramidal shape?	3	108
9556175204	Number of nonbonding pairs in a trigonal pyramidal shape?	1	109
9556175205	Name of a trigonal pyramidal shape?asily ionized	MX3	110
9556175206	Bond angle of a V shape?	<109.5	111
9556175207	Hybridization of a V shape?	sp3	112
9556175208	Number of a bonds in a V shape?	2	113
9556175209	Number of nonbonding pairs in a V shape?	2	114
9556175210	Name of a V shape?	M2X	115
9556175211	Bond angles of a trigonal bipyramidal shape?	120, 90	116
9556175212	Hybridization of a trigonal bipyramidal shape?	sp3d	117
9556175213	Number of bonds in a trigonal bipyramidal shape?	5	118
9556175214	Name of a trigonal bipyramidal shape?	MX5	119
9556175215	Bond angle of a see-saw shape?	<120, <90	120
9556175216	Hybridization of a see-saw shape?	sp3d	121
9556175217	Number of bonds in a see-saw shape?	4	122
9556175218	Number of nonbonding pairs in a see-saw shape?	1	123
9556175219	Bond angle of a T-shape?	<90	124
9556175220	Hybridization of a T-shape?	sp3d	125
9556175221	Number of bonds in a T-shape?	3	126
9556175222	Number of nonbonding pairs in a T-shape?	2	127
9556175223	Bond angle of a linear (2) shape?	180	128
9556175224	Hybridization of a linear (2) shape?	sp3d	129
9556175225	Number of bonds in a linear (2) shape?	2	130
9556175226	Number of nonbonding pairs in a linear (2) shape?	3	131
9556175227	Bond angle of an octahedron?	90	132
9556175228	Hybridization of an octahedron?	sp3d2	133
9556175229	Number of bonds in an octahedron?	6	134
9556175230	Name of an octahedron?	MX6	135
9556175231	Bond angle of a square pyramidal shape?	<90	136
9556175232	Hybridization of a square pyramidal shape?	sp3d2	137
9556175233	Number of bonds in a square pyramidal shape?	5	138
9556175234	Number of nonbonding pairs in a square pyramidal shape?	1	139
9556175235	Name of a square pyramidal shape?	MX5	140
9556175236	Bond angle of a square planar shape?	90	141
9556175237	Hybridization of a square planar shape?	sp3d2	142
9556175238	Number of bonds in a square planar shape?	4	143
9556175239	Number of nonbonding pair in a square planar shape?	2	144
9556175240	Name of a square planar shape?	MX4	145
9556175241	Metallic bond	Delocalized electron	146
9556175242	Nonpolar covalent bond	Equal sharing of electrons	147
9556175243	Polar covalent bond	Unequal sharing of electrons	148
9556175244	Ionic bond	Transfer of electrons	149
9556175245	Electronegativity differences	Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)	150
9556175246	Sigma bond	Bond between the s orbitals	151
9556175247	Pi bond	Bond between the p orbitals	152
9556175248	Hydrogen bond	Special type of dipole, hydrogen with N, F, or O atom	153
9556175249	London dispersion forces	Between non polar molecules	154
9556175250	Alloy	Contains a mixture of elements and has metallic properties	155
9556175251	Substitutional alloy	Metal atoms replaced by metal atoms of same size	156
9556175252	Interstitial alloy	Small atoms in holes	157
9556175253	Vapor pressure	Pressure of vapor at equilibrium	158
9556175254	Vapor pressure formula (Hg column)	Patmosphere = Pvapor +Pmercury column	159
9556175255	Temperature and vapor pressure?	Vapor pressure increases significantly with temperature	160
9556175256	IMFs and vapor pressure?	High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure	161
9556175257	Crystalline solids	Components organized in a lattice	162
9556175258	Amorphous solids	Components frozen in place with no arrangement	163
9556175259	Heat of fusion	Enthalpy change which occurs at the melting point when a solid melts	164
9556175260	Sublimation	Solid directly to gas	165
9556175261	Triple point	Where all three states exist	166
9556175262	Critical temperature	Temperature above which vapor cannot be liquefied no matter the pressure	167
9556175263	Critical pressure	Pressure required to produce liquefaction at the critical temperature	168
9556175264	Critical point	Critical temperature and critical point	169
9556175265	Phase diagram	Representation of phases of a substance	170
9556175266	Heat of solution	Enthalpy change formation of a solution, sum of enthalpy values from each step	171
9556175267	Positive delta H	Energy absorbed	172
9556175268	Negative delta H	Energy released	173
9556175269	Pressure and solubility	Increases solubility of a gas	174
9556175270	Henry's Law	Amount of gas dissolved proportional to pressure of gas above solution	175
9556175271	Temperature and solubility	Increases solubility of solid, decreases solubility of gases	176
9556175272	Raoult's Law	Nonvolatile solute simply dilutes the solvent	177
9556175273	Negative deviation from Raoult's law	More IMFs, lower vapor pressure	178
9556175274	Positive deviation from Raoult's law	Less IMFs, more molecules escape, higher vapor pressure	179
9556175275	Colligative properties	Freezing point depression, boiling point elevation, osmotic pressure	180
9556175276	Tyndall effect	Scattering of light by particles	181
9556175277	Colloid	Suspension of particles	182
9556175278	Coagulation	Destruction of colloid by heating or adding electrolyte	183
9556175279	Reaction rate	Change of concentration over time (Rate = delta [A] / delta t)	184
9556175280	Rate law	Rate depends on concentration	185
9556175281	Integrated rate law	Concentrations depends on time	186
9556175282	Initial rate	Instantaneous rate after reaction begins	187
9556175283	Catalyst	Increases rate of reaction but not consumed	188
9556175284	Surface area and rate	More surface area increases rate	189
9556175285	Temperature and rate	Higher temperature increases rate	190
9556175286	Zeroth order rate law	Rate = k	191
9556175287	Zeroth order integrated rate law	[A] = -kt + [A]0	192
9556175288	Zeroth order plot	[A] vs. t	193
9556175289	Zeroth order slope	Slope = -k	194
9556175290	Zeroth order half life	t1/2 = [A]0 / 2k	195
9556175291	First order rate law	Rate = k[A]	196
9556175292	First order integrated rate law	ln[A] = - kt + ln[A]0	197
9556175293	First order plot	ln[A] vs. t	198
9556175294	First order slope	Slope = -k	199
9556175295	First order half life	t1/2 = 0.693 / k	200
9556175296	Second order rate law	Rate = k[A]2	201
9556175297	Second order integrated rate law	1/[A] = kt + 1/[A]0	202
9556175298	Second order plot	1/[A] vs. t	203
9556175299	Second order slope	Slope = k	204
9556175300	Second order half life	t1/2 = 1 / k[A]0	205
9556175301	Reaction mechanism	Series of steps	206
9556175302	A --> products	Rate = k[A]	207
9556175303	A + A --> products	Rate = k[A]2	208
9556175304	A + B --> products	Rate = k[A][B]	209
9556175305	A + A + B --> products	Rate = k[A]2[B]	210
9556175306	A + B + C --> products	Rate = k[A][B][C]	211
9556175307	Rate determining step	Slowest step	212
9556175308	Reaction mechanism requirements	Sum must give balanced equation, mechanism must agree with rate law	213
9556175309	Equilibrium expression	Products raised to coeffs over reactants raised to coeffs	214
9556175310	Q = k	Equilibrium, no shift	215
9556175311	Q > k	Shift to reactants	216
9556175312	Q < k	Shift to products	217
9556175313	Le Chatlier's Principle	Change imposed, equilibrium shifts to lessen change	218
9556175314	More product added	Shift to reactants	219
9556175315	More reactant added	Shift to product	220
9556175316	How to change the pressure of a reaction system?	Add or remove gas, add an inert gas, change volume	221
9556175317	Ka	Acid dissociation constant	222
9556175318	Strong acid	Equilibrium is far to the right, has weak conjugate base	223
9556175319	Weak acid	Equilibrium is far to the left	224
9556175320	Monoprotic acids	One acidic proton	225
9556175321	Amphoteric	Can behave as an acid or a base (water)	226
9556175322	Kw	Water dissociation constant	227
9556175323	pH	-log[H+]	228
9556175324	pOH	-log[OH-]	229
9556175325	pK	-logK	230
9556175326	pH of strong acids	Depends on concentration of H+ ions	231
9556175327	pH of weak acids	Find Ka and use an ice chart	232
9556175328	Percent dissociation	Amount dissociated M / initial concentration M x 100%	233
9556175329	Polyprotic acids	Dissociates in a stepwise manner, find Ka of each step	234
9556175330	Bond strength and acid strength	Less bond strength, more acid strength	235
9556175331	Common ion effect	Shift in equilibrium because of addition of common ion	236
9556175332	Buffer	Resists a change in pH	237
9556175333	Henderson Hasselbach Equation	Used to find the pH of a buffer	238
9556175334	Strong acid-strong base titration curve	Equivalence point is 7	239
9556175335	Weak acid-strong base titration curve	Equivalence point is greater than 7, has a halfway equivalence point	240
9556175336	Acid-base indicator	Changes color at the end point (not same as equivalence point)	241
9556175337	pH of indicator	Ka/[H+] = [In-]/[HIn] = 1/10, ratio reversed for bases	242
9556175338	Ksp	Solubility product	243
9556185984	Avogadro's Number	6.022 x 10^23, number of particles in a mole of a pure substance	244
9556222985	Ion	same number of protons + neutrons, different e- number	245
9556227504	anion	negatively charged ion (more electrons than protons)	246
9556229613	cation	positively charged ion (more protons than electrons)	247
9556240988	Mendelev and Meyer	creators of the periodic table	248
9556247932	Dalton's discoveries	-atoms go to "elements -elements go to molecules -compounds have constant ratio	249
9556253770	substance	either a molecule or compound, both can be called this	250
9556275358	compound	name of ionic bonded substances	251
9556279437	molecule	covalent bonded substances	252
9556281740	ionic bond	- transfer of electrons - typically nonmetal + metal - held together by electrostatic forces - high melting and boiling points	253
9556297821	stable	lower energy =	254
9556302616	interstitial alloy	metal atoms with two vastly different radii combine	255
9556305501	substitutional alloy	forms with atoms of similar radii	256
9556310091	sigma bond	first covalent bond formed between two atoms	257
9556314501	pi bond	additional bonds beyond the sigma	258

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AP Chemistry Vocabulary Flashcards

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