AP Chemistry Flashcards

9734384835	atomic radius	distance between nuclei of adjacent atoms in an element	0
9734403486	atomic radius increases going ___ and ____ when on the periodic table	down and left	1
9734405475	ionization energy	the energy required to remove an electron from a gaseous atom	2
9734418188	ionization energy increases going ___ and ___ when on the periodic table	up and right	3
9734427357	electronegativity	the relative ability of an atom in a bond to attract electrons (excludes noble gases)	4
9734441713	electronegativity increases going ___ and ___ when on the periodic table	up and right	5
9734475585	isotope	same element with different amount of neutrons	6
9734479643	ion	charged particle/atom	7
9734490112	-ate ->	-ic	8
9734490113	-ite ->	-ous	9
9734492387	-ide ->	hydro___ic acid	10
9734501637	pauli exclusion principle	electrons of the same spin can not occupy the same orbital	11
9734505210	aufbau principle	electrons fill orbitals in a sequence of most stability	12
9734513447	hund's rule	electrons must occupy each sub-orbital by one pairing up	13
9734521047	octet rule	all atoms like to have 8 valance electrons	14
9734540574	principle quantum number (n)	orbital in which the electron is located. higher n is higher energy of the electron because it is less tightly bonded to the nucleus	15
9734553601	angular momentum quantum number (l)	shows the shape of the atomic orbital - l=0 (s orbital) - l=1 (p orbital) - l=2 (d orbital) - l=3 (f orbital)	16
9734577098	magnetic quantum number (m)	shows the orientation of the orbital - can be -l to l	17
9734581312	electron spin number (s)	shows the spin state of the electron in an orbital - can be -1/2 or 1/2	18
9734592299	polar covalent bond	covalent bond where electrons spend more time around a more electronegative atom	19
9734603594	lattice energy	the energy released when an ionic compound is formed	20
9734630969	Enthalpy of formation (ΔH°f)	the overall enthalpy of the formation of ONE mole of a compound. it is the summation of all the steps involved in the formation of the compound	21
9734672958	bond polarity	measure of how equally the electrons in a bond are shared between the two atoms of the bond	22
9734693075	sigma bond (σ)	-electron density is along the bond axis -end to end overlap of orbitals	23
9734707284	pi bonds	-electron density is above and below the bond axis	24
9734713878	single bonds are....	sigma bonds (σ)	25
9734720056	double bonds are...	1 sigma bond and 1 pi bond	26
9734723560	triple bonds are...	1 sigma bond and 2 pi bonds	27
9734731343	strong electrolyte	when a compound 100% dissociates in a solvent	28
9734738366	strong acid	100% dissociates in water -H+ donor -OH acceptor	29
9734741257	strong base	100% dissociates in water -OH donor -H+ acceptor	30
9734755468	oxidation	when an electron loses electrons (oxidation numbers increase)	31
9734760987	reduction	when an element gains electrons (oxidation number decreases)	32
9734771560	dipole-dipole attraction	attraction between polar particles	33
9734774671	ion-dipole attraction	attraction between cation or anion with a dipole	34
9734783549	dipole induced dipole attraction	when a polar molecule causes an instantaneous dipole in a nonpolar molecule	35
9734791838	hydrogen bonding	strongest intermolecular force, when Hydrogen bonds with Oxygen or Nitrogen or Fluorine	36
9734797281	london dispersion forces	weakest intermolecular force, temporary dipoles that occur due to unsymmetrical distribution of electrons	37
9734835303	heat of fusion	energy from solid to liquid	38
9734848111	heat of vaporization	energy from liquid to gas	39
9734854080	heat of sublimation	energy from solid to gas (skipping liquid)	40
9734863350	triple point	conditions where solid,liquid,gas phases coexist	41
9734865725	critical point	critical temperature and pressure, beyond this point gas cannot be condensed into liquid	42
9734875303	boiling point	the point at which vapor pressure is equal to atmospheric pressure	43
9734885198	molality	mols of solute per kg of solvent	44
9734888228	mol fraction	mols of solute / mols of all parts of solution	45
9734904691	monatomic gases	noble gases	46
9734918134	dalton's law of partial pressures	the total pressure of a mixture of gases equals the sum of the pressures that each gas would exert if it were present alone	47
9734945790	bond enthalpy	H= E breaking - E forming -breaking = reactants -forming = products	48
9734968093	reaction rate	the change in concentration of reactants or products per unit time (mol/L*s)	49
9734995575	rate law	links reaction rate with concentrations of reactants at constant temperatures and order perameters rate=k(A)^x * (B)^y for A+B->C	50
9735017601	reaction order	(x , y) 0=zero order 1=1st order 2=second order	51
9735027014	zero order	when the rate of a reaction is independent of reactant concentration -rate=k	52
9735036448	first order	when the rate of reactant depends on the concentration of one reactant -linearly graphed	53
9735043112	second order	when a rate depends of either 1 second order reactant or 2 first order reactants	54
9735060892	activation energy	the minimum amount of energy required for reactants to undergo a reaction	55
9735066855	chemical equilibrium	when the forward and reverse reaction proceeds at equal rates	56
9735072078	law of mass action	rate of any reaction is proportional to the product(s) of the reacting substances raised to the power of its coefficients	57
9735081392	k>1	product favored	58
9735083734	k<1	reactant favored	59
9735083735	k=1	equilibrium position	60
9735092741	k=	concentration of products / concentration of reactants	61
9735110213	reactant quotient (Q)	when the law of mass action is applied to initial concentrations and compared to the Keq to determine the equilibrium shift -the ratio of products to reactants	62
9735123979	Q=k	equilibrium position	63
9735127020	Q>k	equilibrium shifts left to reactants	64
9735128856	Q	equilibrium shifts right to products	65
9735148452	when you increase the concentration of reactants...	equilibrium goes to the products	66
9735159201	when you decrease the concentration of the reactants...	equilibrium goes to the reactants	67
9735164176	when you increase the concentration of the products...	equilibrium goes to the reactants	68
9735168962	when you decrease the concentrations of products...	equilibrium goes to the products	69
9735173206	when you increase pressure...	equilibrium goes to the least amount of mols of gas	70
9735176333	when you decrease pressure...	equilibrium goes to the most amount of mols of gas	71
9735189544	endothermic rxn : temp increase =	equilibrium goes to the products -delta H needed	72
9735196196	endothermic rxn : temp decrease =	equilibrium goes to the reactants -delta H needed	73
9735202928	exothermic rxn : temp increase =	equilibrium goes to the reactants -delta H needed	74
9735207288	exothermic rxn : temp decrease =	equilibrium goes to the products -delta H needed	75
9735211929	negative delta H	exothermic rxn	76
9735214491	positive delta H	endothermic rxn	77
9735227238	solubility product	ksp . concentration of product ions times the concentration of the reactant ions that are present in a saturated solution of an ionic compound	78
9735238899	Q>ksp	super-saturated solution, precipitation is favored	79
9735243900	Q	unsaturated solution, dissolved state is favored	80
9735248626	common ion effect	when the concentration of an ion is increased, more solid will precipitate (solubility lowers)	81
9735263909	conjugate acid	compound that results after an H+ is accepted	82
9735271053	conjugate base	compound that results after an H+ is donated	83
9735304816	a buffer system includes...	a weak acid or base with a salt containing its conjugate base	84
9735311597	buffer solution	a solution that resists changes in pH	85
9735317004	strong acid with a strong base pH curve		86
9735323196	weak acid with a strong base pH curve		87
9735328279	weak base with a strong acid pH curve		88
9735332481	diprotic acid pH curve		89
9735343102	entropy	calculation of disorder / randomness within the universe (S)	90
9735353259	free energy	the amount of useful work that can be obtained from a process at constant temp (298 k) and pressure (1 atm) (G)	91
9735361702	positive delta G	non-spontaneous	92
9735366186	negative delta G	spontaneous	93
9735370273	cathode	reduction occurs, accepting electrons	94
9735372755	anode	oxidation occurs, donating electrons -the half rxn with the lowest E value is reversed	95
9735386921	line notations	anode components on the left, cathode on the right. divide by a double line	96
9735393892	dead battery	a redox rxn at equilibrium	97
9777614485	viscosity	resistance of a liquid to flow	98
9777624009	crystalline solid	contain highly ordered structures, with a regular pattern	99
9777629491	amorphous solids	structures are not completely regular	100
9777669441	cohesive forces	inter-molecular forces that bind similar molecules to one another	101
9777682946	adhesive forces	inter-molecular attractions that bind a substance to a surface	102
9777695661	vapor pressure	the pressure exerted by the vapor when at equilibrium	103
9777699486	volatile liquid	a liquid that evaporates readily	104
9777723370	boyle's law	P1V1=P2V2 -graph of V vs. P inverse relationship curve	105
9777732820	charle's law	V1/T1=V2/T2 -graph of V vs. T is linear	106
9777745143	Gay Lussac's Law	P1/T1=P2/T2	107
9777750603	ideal gas law	PV=nRT	108
9777756271	avogadro's law	the volume of gas maintained at constant temperature and pressure is directly proportional to the number of moles of the gas	109
9777770331	partial pressure	the pressure exerted by a particular component of a mixture	110
9777803502	graham's law of diffusion	rate1/rate2= square root of (molar mass2/molar mass1)	111
9777856353	arrhenius equation	relates activation energy, number of collisions, and fraction of effective collisions k=Ae^-Ea/RT	112
9777905096	catalysts	increases the rate at which equilibrium is achieved	113
9777974696	reducing agent	the species that is oxidized	114
9777977324	oxidizing agent	the species that is reduced	115
9777985201	salt bridge	allows ions to move to maintain charge neutrality in both half-cells	116