AP Chemistry Final Review Flashcards

12501615468	STP Conditions	0 degrees Celsius, 22.4 L	0
12501615469	Density	mass / volume	1
12501615470	Molarity	moles / L	2
12501615471	Distillation	Depends on differences in volatility	3
12501615472	Filtration	Separating a solid from a liquid	4
12501615473	Chromatography	Separating substances through differences in rates	5
12501615474	Law of conservation of mass	Mass is neither created nor destroyed	6
12501615475	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
12501615476	JJ Thomson	Cathode Ray, discovered the electron	8
12501615477	Millikan	Oil Drop Experiment, determined mass and magnitude of the electron	9
12501615478	Rutherford	Gold Foil Experiment, discovered nuclei, atoms have a lot of space	10
12501615479	Solubility Rules	Chlorates, Acetates, Sulfates, Halogens, Nitrates, Group IA	11
12501615480	Solubility Rules Exceptions	Calcium, Barium, Strontium, Mercury, Silver, Lead (Sulfates) Mercury, Silver, Lead (Halogens)	12
12501615481	Strong Electrolytes	Good conductors, easily ionized	13
12501615482	Weak Electrolytes	Conduct currents very weakly	14
12501615483	Strong Acids	HF, HBr, HCl, HClO4, HI, HClO3, HNO3	15
12501615484	Strong Bases	All Group IA elements with OH- Ca(OH)2, Sr(OH)2, Ba(OH)2,	16
12501615485	Dilution Formula	M1V1 = M2V2	17
12501615486	Types of Chemical Reactions	Precipitation reactions, Acid-Base reactions, and Redox reactions	18
12501615487	Precipitation reaction	An insoluble substance is formed as a result of the reaction	19
12501615488	Spectator ions	Ions that do not participate in the reaction	20
12501615489	Bronsted-Lowry acid	Proton donor	21
12501615490	Bronsted-Lowry base	Proton acceptor	22
12501615491	Arrhenius acid	Produces H+ (H3O+) in water	23
12501615492	Arrhenius base	Produces OH- in water	24
12501615493	Lewis acid	Electron pair donor	25
12501615494	Lewis base	Electron pair acceptor	26
12501615495	Equivalence point	Enough titrant added to analyte	27
12501615496	Endpoint	Indicator changes color	28
12501615497	Redox reaction	Electrons are transferred	29
12501615498	Oxidation	Loss of electrons (LEO)	30
12501615499	Reduction	Gain of electrons (GER)	31
12501615500	Oxidizing agent	Causes oxidation (is often reduced)	32
12501615501	Reducing agent	Causes reduction (is often oxidized)	33
12501615502	1 standard atmosphere	1 atm, 760 mm Hg, 760 torr, 101,325 Pa	34
12501615503	Pressure	force / area	35
12501615504	Boyle's Law	P1V1 = P2V2	36
12501615505	Charles's Law	V1 / T1 = V2 / T2	37
12501615506	Ideal Gas Law	PV = nRT	38
12501615507	Molar mass of a gas	dRT / P	39
12501615508	Dalton's law of partial pressures	Ptot = P1 + P2 + P3...	40
12501615509	Mole fraction	n1 / ntot	41
12501615510	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
12501615511	Root mean square velocity	Average velocity of gas particles	43
12501615512	Diffusion	Mixing of gases	44
12501615513	Effusion	Gas into a vacuum	45
12501615715	Graham's law of effusion		46
12501615514	Law of conservation of energy	Energy can be converted but never destroyed	47
12501615515	Potential energy	Energy from position or composition	48
12501615516	Kinetic energy	Energy from motion	49
12501615517	Heat	Transfer of energy with temperature	50
12501615518	Work	Force acting over a distance	51
12501615519	Exothermic	Energy out of the system	52
12501615520	Endothermic	Energy into the system	53
12501615521	First law of thermodynamics	The energy of the universe is constant	54
12501615522	Internal energy (delta E)	delta E = q + w	55
12501615523	Enthalpy (delta H)	delta H = delta E + P(delta V)	56
12501615524	Heat capacity	heat absorbed / increase in temperature	57
12501615525	Calorimetry equation	q = mCAT	58
12501615526	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
12501615527	Standard enthalpy of formation	change in enthalpy with formation of one mole of compound from its elements	60
12501615528	Change in enthalpy for reaction	sum of heat of formations of products - sum of heat of formations of reactions	61
12501615529	Wavelength	distance between two peaks or troughs in a wave	62
12501615530	Frequency	number of cycles per second	63
12501615531	Basic wave equation	speed of light = wavelength x frequency	64
12501615532	Energy of a photon equation	Planck's constant x speed of light / frequency	65
12501615533	Photoelectric effect	Effect occurring when electrons are emitted from the surface of a metal when light strikes it	66
12501615534	Dual nature of light	Light acts as a wave and as particulate matter	67
12501615535	de Broglie's equation	Wavelength of a particle	68
12501615536	Diffraction	Light is scattered from points or lines	69
12501615537	Types of electromagnetic radiation (smallest to largest)	gamma, X-rays, UV, visible, IR, micro, radio	70
12501615538	Types of electromagnetic radiation (largest to smallest)	radio, micro, IR, visible, UV, X-rays, gamma	71
12501615539	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
12501615540	Pauli exclusion principle	Electrons with the same spin cannot occupy the same space	73
12501615541	Aufbau principle	Progressively add electrons to each sub level	74
12501615542	Hund's rule	Different electrons to different orbitals, same spin	75
12501615543	Ionization energy	Energy required to remove a valence electron from an atom	76
12501615544	Electron affinity	Energy change associated with the addition of an electron to a gaseous atom	77
12501615545	Atomic radius trend	Decreases across a period (more effective nuclear charge), increases down a group (more electron shielding)	78
12501615546	Ionization energy trend	Increases across a period (electron shielding not complete), decreases down a group (more electron shielding)	79
12501615547	Coulomb's law	Energy of interaction between a pair of ions	80
12501615548	Bond energy	Energy needed to break bond	81
12501615549	Covalent bonding	Electrons are shared by nuclei	82
12501615550	Electronegativity	Ability of an atom in a molecule to attract shared electrons to itself	83
12501615551	Dipolar or dipole moment	Has center of positive and center of negative charge	84
12501615552	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
12501615553	Localized electron model	Molecule is composed of atoms bound together by sharing pairs of electrons	86
12501615554	Lone pairs	Pairs of electrons localized	87
12501615555	Localized electron model parts	Lewis diagram, VSEPR model (geometry), type of atomic orbitals	88
12501615556	Resonance	More than one valid Lewis structure	89
12501615557	Bond angle of a linear shape?	180	90
12501615558	Hybridization of a linear shape?	sp	91
12501615559	Number of bonds in a linear shape?	2	92
12501615560	Name of a linear shape?	MX2	93
12501615561	Bond angle of a trigonal planar shape?	120	94
12501615562	Hybridization of a trigonal planar shape?	sp2	95
12501615563	Number of bonds in a trigonal planar shape?	3	96
12501615564	Name of a trigonal planar shape?	MX3	97
12501615565	Bond angle of a bent shape?	<120	98
12501615566	Hybridization of a bent shape?	sp2	99
12501615567	Number of bonds in a bent shape?	2	100
12501615568	Number of nonbonding pairs in a bent shape?	1	101
12501615569	Bond angle of a tetrahedral shape?	109.5	102
12501615570	Hybridization of a tetrahedral shape?	sp3	103
12501615571	Number of bonds in a tetrahedral shape?	4	104
12501615572	Name of a tetrahedral shape?	MX4	105
12501615573	Bond angle of a trigonal pyramidal shape?	<109.5	106
12501615574	Hybridization of a trigonal pyramidal shape?	sp3	107
12501615575	Number of bonds in a trigonal pyramidal shape?	3	108
12501615576	Number of nonbonding pairs in a trigonal pyramidal shape?	1	109
12501615577	Name of a trigonal pyramidal shape?asily ionized	MX3	110
12501615578	Bond angle of a V shape?	<109.5	111
12501615579	Hybridization of a V shape?	sp3	112
12501615580	Number of a bonds in a V shape?	2	113
12501615581	Number of nonbonding pairs in a V shape?	2	114
12501615582	Name of a V shape?	M2X	115
12501615583	Bond angles of a trigonal bipyramidal shape?	120, 90	116
12501615584	Hybridization of a trigonal bipyramidal shape?	sp3d	117
12501615585	Number of bonds in a trigonal bipyramidal shape?	5	118
12501615586	Name of a trigonal bipyramidal shape?	MX5	119
12501615587	Bond angle of a see-saw shape?	<120, <90	120
12501615588	Hybridization of a see-saw shape?	sp3d	121
12501615589	Number of bonds in a see-saw shape?	4	122
12501615590	Number of nonbonding pairs in a see-saw shape?	1	123
12501615591	Bond angle of a T-shape?	<90	124
12501615592	Hybridization of a T-shape?	sp3d	125
12501615593	Number of bonds in a T-shape?	3	126
12501615594	Number of nonbonding pairs in a T-shape?	2	127
12501615595	Bond angle of a linear (2) shape?	180	128
12501615596	Hybridization of a linear (2) shape?	sp3d	129
12501615597	Number of bonds in a linear (2) shape?	2	130
12501615598	Number of nonbonding pairs in a linear (2) shape?	3	131
12501615599	Bond angle of an octahedron?	90	132
12501615600	Hybridization of an octahedron?	sp3d2	133
12501615601	Number of bonds in an octahedron?	6	134
12501615602	Name of an octahedron?	MX6	135
12501615603	Bond angle of a square pyramidal shape?	<90	136
12501615604	Hybridization of a square pyramidal shape?	sp3d2	137
12501615605	Number of bonds in a square pyramidal shape?	5	138
12501615606	Number of nonbonding pairs in a square pyramidal shape?	1	139
12501615607	Name of a square pyramidal shape?	MX5	140
12501615608	Bond angle of a square planar shape?	90	141
12501615609	Hybridization of a square planar shape?	sp3d2	142
12501615610	Number of bonds in a square planar shape?	4	143
12501615611	Number of nonbonding pair in a square planar shape?	2	144
12501615612	Name of a square planar shape?	MX4	145
12501615613	Metallic bond	Delocalized electron	146
12501615614	Nonpolar covalent bond	Equal sharing of electrons	147
12501615615	Polar covalent bond	Unequal sharing of electrons	148
12501615616	Ionic bond	Transfer of electrons	149
12501615617	Electronegativity differences	Nonpolar covalent (0-0.4), polar covalent (0.4-1.67), ionic (above 1.67)	150
12501615618	Sigma bond	Bond between the s orbitals	151
12501615619	Pi bond	Bond between the p orbitals	152
12501615620	Hydrogen bond	Special type of dipole, hydrogen with N, F, or O atom	153
12501615621	London dispersion forces	Between non polar molecules	154
12501615622	Alloy	Contains a mixture of elements and has metallic properties	155
12501615623	Substitutional alloy	Metal atoms replaced by metal atoms of same size	156
12501615624	Interstitial alloy	Small atoms in holes	157
12501615625	Vapor pressure	Pressure of vapor at equilibrium	158
12501615626	Vapor pressure formula (Hg column)	Patmosphere = Pvapor +Pmercury column	159
12501615627	Temperature and vapor pressure?	Vapor pressure increases significantly with temperature	160
12501615628	IMFs and vapor pressure?	High IMFs --> low vapor pressure, Low IMFs --> high vapor pressure	161
12501615629	Crystalline solids	Components organized in a lattice	162
12501615630	Amorphous solids	Components frozen in place with no arrangement	163
12501615631	Heat of fusion	Enthalpy change which occurs at the melting point when a solid melts	164
12501615632	Sublimation	Solid directly to gas	165
12501615633	Triple point	Where all three states exist	166
12501615634	Critical temperature	Temperature above which vapor cannot be liquefied no matter the pressure	167
12501615635	Critical pressure	Pressure required to produce liquefaction at the critical temperature	168
12501615636	Critical point	Critical temperature and critical point	169
12501615637	Phase diagram	Representation of phases of a substance	170
12501615638	Heat of solution	Enthalpy change formation of a solution, sum of enthalpy values from each step	171
12501615639	Positive delta H	Energy absorbed	172
12501615640	Negative delta H	Energy released	173
12501615641	Pressure and solubility	Increases solubility of a gas	174
12501615642	Henry's Law	Amount of gas dissolved proportional to pressure of gas above solution	175
12501615643	Temperature and solubility	Increases solubility of solid, decreases solubility of gases	176
12501615644	Raoult's Law	Nonvolatile solute simply dilutes the solvent	177
12501615645	Negative deviation from Raoult's law	More IMFs, lower vapor pressure	178
12501615646	Positive deviation from Raoult's law	Less IMFs, more molecules escape, higher vapor pressure	179
12501615647	Colligative properties	Freezing point depression, boiling point elevation, osmotic pressure	180
12501615648	Tyndall effect	Scattering of light by particles	181
12501615649	Colloid	Suspension of particles	182
12501615650	Coagulation	Destruction of colloid by heating or adding electrolyte	183
12501615651	Reaction rate	Change of concentration over time (Rate = delta [A] / delta t)	184
12501615652	Rate law	Rate depends on concentration	185
12501615653	Integrated rate law	Concentrations depends on time	186
12501615654	Initial rate	Instantaneous rate after reaction begins	187
12501615655	Catalyst	Increases rate of reaction but not consumed	188
12501615656	Surface area and rate	More surface area increases rate	189
12501615657	Temperature and rate	Higher temperature increases rate	190
12501615658	Zeroth order rate law	Rate = k	191
12501615659	Zeroth order integrated rate law	[A] = -kt + [A]0	192
12501615660	Zeroth order plot	[A] vs. t	193
12501615661	Zeroth order slope	Slope = -k	194
12501615662	Zeroth order half life	t1/2 = [A]0 / 2k	195
12501615663	First order rate law	Rate = k[A]	196
12501615664	First order integrated rate law	ln[A] = - kt + ln[A]0	197
12501615665	First order plot	ln[A] vs. t	198
12501615666	First order slope	Slope = -k	199
12501615667	First order half life	t1/2 = 0.693 / k	200
12501615668	Second order rate law	Rate = k[A]2	201
12501615669	Second order integrated rate law	1/[A] = kt + 1/[A]0	202
12501615670	Second order plot	1/[A] vs. t	203
12501615671	Second order slope	Slope = k	204
12501615672	Second order half life	t1/2 = 1 / k[A]0	205
12501615673	Reaction mechanism	Series of steps	206
12501615674	A --> products	Rate = k[A]	207
12501615675	A + A --> products	Rate = k[A]2	208
12501615676	A + B --> products	Rate = k[A][B]	209
12501615677	A + A + B --> products	Rate = k[A]2[B]	210
12501615678	A + B + C --> products	Rate = k[A][B][C]	211
12501615679	Rate determining step	Slowest step	212
12501615680	Reaction mechanism requirements	Sum must give balanced equation, mechanism must agree with rate law	213
12501615681	Equilibrium expression	Products raised to coeffs over reactants raised to coeffs	214
12501615682	Q = k	Equilibrium, no shift	215
12501615683	Q > k	Shift to reactants	216
12501615684	Q < k	Shift to products	217
12501615685	Le Chatlier's Principle	Change imposed, equilibrium shifts to lessen change	218
12501615686	More product added	Shift to reactants	219
12501615687	More reactant added	Shift to product	220
12501615688	How to change the pressure of a reaction system?	Add or remove gas, add an inert gas, change volume	221
12501615689	Ka	Acid dissociation constant	222
12501615690	Strong acid	Equilibrium is far to the right, has weak conjugate base	223
12501615691	Weak acid	Equilibrium is far to the left	224
12501615692	Monoprotic acids	One acidic proton	225
12501615693	Amphoteric	Can behave as an acid or a base (water)	226
12501615694	Kw	Water dissociation constant	227
12501615695	pH	-log[H+]	228
12501615696	pOH	-log[OH-]	229
12501615697	pK	-logK	230
12501615698	pH of strong acids	Depends on concentration of H+ ions	231
12501615699	pH of weak acids	Find Ka and use an ice chart	232
12501615700	Percent dissociation	Amount dissociated M / initial concentration M x 100%	233
12501615701	Polyprotic acids	Dissociates in a stepwise manner, find Ka of each step	234
12501615702	Bond strength and acid strength	Less bond strength, more acid strength	235
12501615703	Common ion effect	Shift in equilibrium because of addition of common ion	236
12501615704	Buffer	Resists a change in pH	237
12501615705	Henderson Hasselbach Equation	Used to find the pH of a buffer	238
12501615706	Strong acid-strong base titration curve	Equivalence point is 7	239
12501615707	Weak acid-strong base titration curve	Equivalence point is greater than 7, has a halfway equivalence point	240
12501615708	Acid-base indicator	Changes color at the end point (not same as equivalence point)	241
12501615709	pH of indicator	Ka/[H+] = [In-]/[HIn] = 1/10, ratio reversed for bases	242
12501615710	Ksp	Solubility product	243

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AP Chemistry Final Review Flashcards

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