AP Chemistry Final Review Flashcards

6688451750	STP Conditions	0 degrees Celsius, 22.4 L	0
6688451751	Density	mass / volume	1
6688451752	Molarity	moles / L	2
6688451753	Distillation	Depends on differences in volatility	3
6688451754	Filtration	Separating a solid from a liquid	4
6688451755	Chromatography	Separating substances through differences in rates	5
6688451756	Law of conservation of mass	Mass is neither created nor destroyed	6
6688451757	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
6688451758	JJ Thomson	Cathode Ray, discovered the electron	8
6688451759	Millikan	Oil Drop Experiment, determined mass and magnitude of the electron	9
6688451760	Rutherford	Gold Foil Experiment, discovered nuclei, atoms have a lot of space	10
6688451761	Solubility Rules	Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA	11
6688451762	Solubility Rules Exceptions	Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)	12
6688451763	Strong Electrolytes	Good conductors, easily ionized	13
6688451764	Weak Electrolytes	Conduct currents very weakly	14
6688451765	Strong Acids	HF, HBr, HCl, HClO4, HI, HClO3, HNO3	15
6688451766	Strong Bases	All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,	16
6688451767	Dilution Formula	M1V1 = M2V2	17
6688451768	Types of Chemical Reactions	Precipitation reactions, Acid-Base reactions, and Redox reactions	18
6688451769	Precipitation reaction	An insoluble substance is formed as a result of the reaction	19
6688451770	Spectator ions	Ions that do not participate in the reaction	20
6688451771	Bronsted-Lowry acid	Proton donor	21
6688451772	Bronsted-Lowry base	Proton acceptor	22
6688451773	Arrhenius acid	Produces H+ (H3O+) in water	23
6688451774	Arrhenius base	Produces OH- in water	24
6688451775	Lewis acid	Electron pair donor	25
6688451776	Lewis base	Electron pair acceptor	26
6688451777	Equivalence point	Enough titrant added to analyte	27
6688451778	Endpoint	Indicator changes color	28
6688451779	Redox reaction	Electrons are transferred	29
6688451780	Oxidation	Loss of electrons (LEO)	30
6688451781	Reduction	Gain of electrons (GER)	31
6688451782	Oxidizing agent	Causes oxidation (is often reduced)	32
6688451783	Reducing agent	Causes reduction (is often oxidized)	33
6688451784	1 standard atmosphere	1 atm, 760 mm Hg, 760 torr, 101,325 Pa	34
6688451785	Pressure	force / area	35
6688451786	Boyle's Law	P1V1 = P2V2	36
6688451787	Charles's Law	V1 / T1 = V2 / T2	37
6688451788	Ideal Gas Law	PV = nRT	38
6688451789	Molar mass of a gas	dRT / P	39
6688451790	Dalton's law of partial pressures	Ptot = P1 + P2 + P3...	40
6688451791	Mole fraction	n1 / ntot	41
6688451792	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
6688451793	Root mean square velocity	Average velocity of gas particles	43
6688451794	Diffusion	Mixing of gases	44
6688451795	Effusion	Gas into a vacuum	45
6688451796	Graham's law of effusion		46
6688451797	Law of conservation of energy	Energy can be converted but never destroyed	47
6688451798	Potential energy	Energy from position or composition	48
6688451799	Kinetic energy	Energy from motion	49
6688451800	Heat	Transfer of energy with temperature	50
6688451801	Work	Force acting over a distance	51
6688451802	Exothermic	Energy out of the system	52
6688451803	Endothermic	Energy into the system	53
6688451804	First law of thermodynamics	The energy of the universe is constant	54
6688451805	Internal energy (delta E)	delta E = q + w	55
6688451806	Enthalpy (delta H)	delta H = delta E + P(delta V)	56
6688451807	Heat capacity	heat absorbed / increase in temperature	57
6688451808	Calorimetry equation	q = mCdeltaT	58
6688451809	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
6688451810	Standard enthalpy of formation	change in enthalpy with formation of one mole of compound from its elements	60
6688451811	Change in enthalpy for reaction	sum of heat of formations of products - sum of heat of formations of reactions	61
6688451812	Wavelength	distance between two peaks or troughs in a wave	62
6688451813	Frequency	number of cycles per second	63
6688451814	Basic wave equation	speed of light = wavelength x frequency	64
6688451815	Energy of a photon equation	Planck's constant x speed of light / frequency	65
6688451816	Photoelectric effect	Effect occurring when electrons are emitted from the surface of a metal when light strikes it	66
6688451817	Dual nature of light	Light acts as a wave and as particulate matter	67
6688451818	de Broglie's equation	Wavelength of a particle	68
6688451819	Diffraction	Light is scattered from points or lines	69
6688451820	Types of electromagnetic radiation (smallest to largest)	gamma, X-rays, UV, visible, IR, micro, radio	70
6688451821	Types of electromagnetic radiation (largest to smallest)	radio, micro, IR, visible, UV, X-rays, gamma	71
6688451822	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
6688451823	Pauli exclusion principle	Electrons with the same spin cannot occupy the same space	73
6688451824	Aufbau principle	Progressively add electrons to each sub level	74
6688451825	Hund's rule	Different electrons to different orbitals, same spin	75
6688451826	Ionization energy	Energy required to remove a valence electron from an atom	76
6688451827	Electron affinity	Energy change associated with the addition of an electron to a gaseous atom	77
6688451828	Atomic radius trend	Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)	78
6688451829	Ionization energy trend	Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)	79
6688451830	Coulomb's law	Energy of interaction between a pair of ions	80
6688451831	Bond energy	Energy needed to break bond	81
6688451832	Covalent bonding	Electrons are shared by nuclei	82
6688451833	Electronegativity	Ability of an atom in a molecule to attract shared electrons to itself	83
6688451834	Dipolar or dipole moment	Has center of positive and center of negative charge	84
6688451835	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
6688451836	Localized electron model	Molecule is composed of atoms bound together by sharing pairs of electrons	86
6688451837	Lone pairs	Pairs of electrons localized	87
6688451838	Localized electron model parts	Lewis diagram, VSEPR model (geometry), type of atomic orbitals	88
6688451839	Resonance	More than one valid Lewis structure	89
6688451840	Bond angle of a linear shape?	180	90
6688451841	Hybridization of a linear shape?	sp	91
6688451842	Number of bonds in a linear shape?	2	92
6688451843	Name of a linear shape?	MX2	93
6688451844	Bond angle of a trigonal planar shape?	120	94
6688451845	Hybridization of a trigonal planar shape?	sp2	95
6688451846	Number of bonds in a trigonal planar shape?	3	96
6688451847	Name of a trigonal planar shape?	MX3	97
6688451848	Bond angle of a bent shape?	<120	98
6688451849	Hybridization of a bent shape?	sp2	99
6688451850	Number of bonds in a bent shape?	2	100
6688451851	Number of nonbonding pairs in a bent shape?	1	101
6688451852	Bond angle of a tetrahedral shape?	109.5	102
6688451853	Hybridization of a tetrahedral shape?	sp3	103
6688451854	Number of bonds in a tetrahedral shape?	4	104
6688451855	Name of a tetrahedral shape?	MX4	105
6688451856	Bond angle of a trigonal pyramidal shape?	<109.5	106
6688451857	Hybridization of a trigonal pyramidal shape?	sp3	107
6688451858	Number of bonds in a trigonal pyramidal shape?	3	108
6688451859	Number of nonbonding pairs in a trigonal pyramidal shape?	1	109
6688451860	Name of a trigonal pyramidal shape?asily ionized	MX3	110
6688451861	Bond angle of a V shape?	<109.5	111
6688451862	Hybridization of a V shape?	sp3	112
6688451863	Number of a bonds in a V shape?	2	113
6688451864	Number of nonbonding pairs in a V shape?	2	114
6688451865	Name of a V shape?	M2X	115
6688451866	Bond angles of a trigonal bipyramidal shape?	120, 90	116
6688451867	Hybridization of a trigonal bipyramidal shape?	sp3d	117
6688451868	Number of bonds in a trigonal bipyramidal shape?	5	118
6688451869	Name of a trigonal bipyramidal shape?	MX5	119
6688451870	Bond angle of a see-saw shape?	<120, <90	120
6688451871	Hybridization of a see-saw shape?	sp3d	121
6688451872	Number of bonds in a see-saw shape?	4	122
6688451873	Number of nonbonding pairs in a see-saw shape?	1	123
6688451874	Bond angle of a T-shape?	<90	124
6688451875	Hybridization of a T-shape?	sp3d	125
6688451876	Number of bonds in a T-shape?	3	126
6688451877	Number of nonbonding pairs in a T-shape?	2	127
6688451878	Bond angle of a linear (2) shape?	180	128
6688451879	Hybridization of a linear (2) shape?	sp3d	129
6688451880	Number of bonds in a linear (2) shape?	2	130
6688451881	Number of nonbonding pairs in a linear (2) shape?	3	131
6688451882	Bond angle of an octahedron?	90	132
6688451883	Hybridization of an octahedron?	sp3d2	133
6688451884	Number of bonds in an octahedron?	6	134
6688451885	Name of an octahedron?	MX6	135
6688451886	Bond angle of a square pyramidal shape?	<90	136
6688451887	Hybridization of a square pyramidal shape?	sp3d2	137
6688451888	Number of bonds in a square pyramidal shape?	5	138
6688451889	Number of nonbonding pairs in a square pyramidal shape?	1	139
6688451890	Name of a square pyramidal shape?	MX5	140
6688451891	Bond angle of a square planar shape?	90	141
6688451892	Hybridization of a square planar shape?	sp3d2	142
6688451893	Number of bonds in a square planar shape?	4	143
6688451894	Number of nonbonding pair in a square planar shape?	2	144
6688451895	Name of a square planar shape?	MX4	145
6688451896	Metallic bond	Delocalized electron	146
6688451897	Nonpolar covalent bond	Equal sharing of electrons	147
6688451898	Polar covalent bond	Unequal sharing of electrons	148
6688451899	Ionic bond	Transfer of electrons	149
6688451900	Electronegativity differences	Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)	150
6688451901	Sigma bond	Bond between the s orbitals	151
6688451902	Pi bond	Bond between the p orbitals	152
6688451903	Hydrogen bond	Special type of dipole, hydrogen with N, F, or O atom	153
6688451904	London dispersion forces	Between non polar molecules	154
6688451905	Alloy	Contains a mixture of elements and has metallic properties	155
6688451906	Substitutional alloy	Metal atoms replaced by metal atoms of same size	156
6688451907	Interstitial alloy	Small atoms in holes	157
6688451908	Vapor pressure	Pressure of vapor at equilibrium	158
6688451909	Vapor pressure formula (Hg column)	Patmosphere = Pvapor +Pmercury column	159
6688451910	Temperature and vapor pressure?	Vapor pressure increases significantly with temperature	160
6688451911	IMFs and vapor pressure?	High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure	161
6688451912	Crystalline solids	Components organized in a lattice	162
6688451913	Amorphous solids	Components frozen in place with no arrangement	163
6688451914	Heat of fusion	Enthalpy change which occurs at the melting point when a solid melts	164
6688451915	Sublimation	Solid directly to gas	165
6688451916	Triple point	Where all three states exist	166
6688451917	Critical temperature	Temperature above which vapor cannot be liquefied no matter the pressure	167
6688451918	Critical pressure	Pressure required to produce liquefaction at the critical temperature	168
6688451919	Critical point	Critical temperature and critical point	169
6688451920	Phase diagram	Representation of phases of a substance	170
6688451921	Heat of solution	Enthalpy change formation of a solution, sum of enthalpy values from each step	171
6688451922	Positive delta H	Energy absorbed	172
6688451923	Negative delta H	Energy released	173
6688451924	Pressure and solubility	Increases solubility of a gas	174
6688451925	Henry's Law	Amount of gas dissolved proportional to pressure of gas above solution	175
6688451926	Temperature and solubility	Increases solubility of solid, decreases solubility of gases	176
6688451927	Raoult's Law	Nonvolatile solute simply dilutes the solvent	177
6688451928	Negative deviation from Raoult's law	More IMFs, lower vapor pressure	178
6688451929	Positive deviation from Raoult's law	Less IMFs, more molecules escape, higher vapor pressure	179
6688451930	Colligative properties	Freezing point depression, boiling point elevation, osmotic pressure	180
6688451931	Tyndall effect	Scattering of light by particles	181
6688451932	Colloid	Suspension of particles	182
6688451933	Coagulation	Destruction of colloid by heating or adding electrolyte	183
6688451934	Reaction rate	Change of concentration over time (Rate = delta [A] / delta t)	184
6688451935	Rate law	Rate depends on concentration	185
6688451936	Integrated rate law	Concentrations depends on time	186
6688451937	Initial rate	Instantaneous rate after reaction begins	187
6688451938	Catalyst	Increases rate of reaction but not consumed	188
6688451939	Surface area and rate	More surface area increases rate	189
6688451940	Temperature and rate	Higher temperature increases rate	190
6688451941	Zeroth order rate law	Rate = k	191
6688451942	Zeroth order integrated rate law	[A] = -kt + [A]0	192
6688451943	Zeroth order plot	[A] vs. t	193
6688451944	Zeroth order slope	Slope = -k	194
6688451945	Zeroth order half life	t1/2 = [A]0 / 2k	195
6688451946	First order rate law	Rate = k[A]	196
6688451947	First order integrated rate law	ln[A] = - kt + ln[A]0	197
6688451948	First order plot	ln[A] vs. t	198
6688451949	First order slope	Slope = -k	199
6688451950	First order half life	t1/2 = 0.693 / k	200
6688451951	Second order rate law	Rate = k[A]2	201
6688451952	Second order integrated rate law	1/[A] = kt + 1/[A]0	202
6688451953	Second order plot	1/[A] vs. t	203
6688451954	Second order slope	Slope = k	204
6688451955	Second order half life	t1/2 = 1 / k[A]0	205
6688451956	Reaction mechanism	Series of steps	206
6688451957	A --> products	Rate = k[A]	207
6688451958	A + A --> products	Rate = k[A]2	208
6688451959	A + B --> products	Rate = k[A][B]	209
6688451960	A + A + B --> products	Rate = k[A]2[B]	210
6688451961	A + B + C --> products	Rate = k[A][B][C]	211
6688451962	Rate determining step	Slowest step	212
6688451963	Reaction mechanism requirements	Sum must give balanced equation, mechanism must agree with rate law	213
6688451964	Equilibrium expression	Products raised to coeffs over reactants raised to coeffs	214
6688451965	Q = k	Equilibrium, no shift	215
6688451966	Q > k	Shift to reactants	216
6688451967	Q < k	Shift to products	217
6688451968	Le Chatlier's Principle	Change imposed, equilibrium shifts to lessen change	218
6688451969	More product added	Shift to reactants	219
6688451970	More reactant added	Shift to product	220
6688451971	How to change the pressure of a reaction system?	Add or remove gas, add an inert gas, change volume	221
6688451972	Ka	Acid dissociation constant	222
6688451973	Strong acid	Equilibrium is far to the right, has weak conjugate base	223
6688451974	Weak acid	Equilibrium is far to the left	224
6688451975	Monoprotic acids	One acidic proton	225
6688451976	Amphoteric	Can behave as an acid or a base (water)	226
6688451977	Kw	Water dissociation constant	227
6688451978	pH	-log[H+]	228
6688451979	pOH	-log[OH-]	229
6688451980	pK	-logK	230
6688451981	pH of strong acids	Depends on concentration of H+ ions	231
6688451982	pH of weak acids	Find Ka and use an ice chart	232
6688451983	Percent dissociation	Amount dissociated M / initial concentration M x 100%	233
6688451984	Polyprotic acids	Dissociates in a stepwise manner, find Ka of each step	234
6688451985	Bond strength and acid strength	Less bond strength, more acid strength	235
6688451986	Common ion effect	Shift in equilibrium because of addition of common ion	236
6688451987	Buffer	Resists a change in pH	237
6688451988	Henderson Hasselbach Equation	Used to find the pH of a buffer	238
6688451989	Strong acid-strong base titration curve	Equivalence point is 7	239
6688451990	Weak acid-strong base titration curve	Equivalence point is greater than 7, has a halfway equivalence point	240
6688451991	Acid-base indicator	Changes color at the end point (not same as equivalence point)	241
6688451992	pH of indicator	Ka/[H+] = [In-]/[HIn] = 1/10, ratio reversed for bases	242
6688451993	Ksp	Solubility product	243

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AP Chemistry Final Review Flashcards

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