AP Chemistry Flashcards

4737723216	protons	determines element	0
4737723509	nuetrons	determines isotope	1
4737723950	neutrons+protons (protons+neutrons)	equation to find mass number	2
4737726287	6.022x10^23	mole quantity	3
4737729059	moles=grams/molar mass	equation to convert between grams and moles	4
4737729398	gram per mole	technically the same as an AMU	5
4737730936	Moles=PV/RT	equation to calculate the number of moles in a gas, with pressure in atm and volume in liters and temperature in kelvins, (R is the gas constant)	6
4737797883	0.0821 L atm/mol k	gas constant (R)	7
4737799172	22.4 liters	at STP one mole always occupies this many liters	8
4737801213	moles=liters/(22.4L.mol)	equation to convert volume of gas to number of moles at STP	9
4737802385	moles/liters of solution	molarity equation	10
4739890483	# of atomsxrelative atomic mass/total mass	equation to calculate percent composition	11
4739893387	empirical formula	the simplest ratio of elements in a compound	12
4739893388	molecular formula	the actual formula for a substance	13
4739906308	divide each mole value by lowest value	how do you correctly retrieve the empirical formula from moles for a substance	14
4739911807	0.1	you may round within this value when dividing moles by moles to give a ratio to an empirical formula	15
4739914827	divide compounds molar mass by empirical formulas molar mass	how do you retrieve the molecular formula of a given compound with a molar mass (using the empirical formula)	16
4739915820	multiply each atoms relative atomic mass by # of atoms then add them together	how do you retrieve the molar mass of a compound from it's formula	17
4739916929	quantized	electrons possess this property, which allows them to be in different energy states, however not between those states	18
4739917556	potential energy	this quantity increases as an electron increases in distance from the nucleus	19
4739917834	Aufbau principle	when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy	20
4739919111	Pauli Exclusion principle	two electrons which share an orbital cannot have the same spin, with one clockwise, and the other counterclockwise	21
4739919585	Hund's Rule	when an electron is added to a sub shell, it will always occupy an empty orbital if one is available, and pair up if no empty orbitals are avilable	22
4739928668	coulombs law	states that the amount of energy that an electron has depends on it's distance form the nucleus of an atom	23
4739929609	E=k(+q)(-q)/r	coulombs law equation with k as coulombs constant, +q as the magnitude of the positive charge, -q that of the negative, and r as the distance between charges	24
4739936061	more	the greater the charge of the nucleus (are therefore, electrons) the ____ energy an electron will have	25
4741528629	removal energy	binding energy, will always be positive, energy it takes to remove an electron from an atom	26
4741529746	quantized	Max Planck figured out that all electromagnetic energy is this, that's, for a given frequency of radiation (or light), all possible energies are multiples of a certain unit of energy, called a quantum	27
4741533106	small specific steps	according to Max Planck's quantum theory, energy changers do not occur smoothly but rather in ______	28
4741536520	electromagnetic energy	when atoms absorb energy in this form, electrons jump to higher energy levels, and when electrons drop down to lower energy levels, they release this	29
4741537643	Neils Bohr	used quantum theory to predict that electrons orbit the neucleas at specific, fixed radii which each orbital represented on the periodic table as periods	30
4743728880	ΔE=hv=hc/λ	relationship between change in energy level (ΔE) and the electromagnetic radiation absorbed or emitted with v as frequency, h as planck's constant, c as the speed of light, and λ as wavelength	31
4743728881	Same	the energy levels of electrons in a particular atom are always the ___ for that atom, meaning atoms can be identified by their radiation spectra	32
4743728882	c=λv	equation which assists electromagnetic radiation and energy equation, relates speed of light to wavelength and frequency, so that λ and v are inverse	33
4743728883	Higher, shorter	____ frequencies and ____ wavelengths lead to more energy	34
4743728884	Ionization energy	the amount of electromagnetic radiation that would prove too much for the various binding energies of an electron of the atom and allow it to be ejected	35
4743728885	Binding energy + kinetic energy	Incoming Radiation energy equals this, so that all excess energy which does not go into breaking the electron free is converted into K.E for the ejected electron	36
4743728886	Further	electrons which were originally ___ from the nucleus require less energy to eject, and thus will be moving faster	37
4743728887	Photoelectron spectra (PES)	graphs the amount of ionization energy for all ejected electrons, with relative # of ejected electrons as the y axis and the binding energy as the x, which decreases going from left to right	38
4743728888	Decreases	In a Photoelectron spectra, the x axis (binding energies) ____ going from left to right	39
4743728889	Noble gas	a shorthand notation for electron configurations of elements is to place the symbol of the previous periods ___ and then filling in the rest with the remaining upper energy levels	40
4743728890	John Dalton	presented basic ideas about atoms, such as as there are many kinds, which are classified as elements, and these combine to form compounds which contain elemental ratios, and that atoms are never created or destroyed in chemical reactions	41
4743728891	Robert Millikan	was able to calculate the charge on a an electron by examining the behavior of charged oil drops in an electric field	42
4743728892	Closer, more	the ____ an electron to the nucleus, the more strongly it is attracted, and the ___ protons in that nucleus, the stronger those electrons are attracted	43
4743728893	Shielding	term which describes how electrons are repelled by the electrons surrounding another atom, making the valence electrons of the atom less attracted to that atom's nucleus	44
4743728894	Smaller	cations are generally ____ than atoms	45
4743728895	Larger	anions are generally _____ than atoms	46
4743728896	Greater	the second ionization energy is ____ than the first ionization energy	47
4751384881	Stable, lower energy state	Atoms engage in chemical reactions in order to reach a more _______	48
4751384882	Electrostatic attractions	what holds together ionic solids, occurs between ions next to each other in a lattice structure	49
4751384883	Solid, high	any substance held together by ionic bonds will usually be a ____ at room temps. And will have very ___ melting and boiling points	50
4751384884	Greater charge	this in ionic bonds leads to higher melting points	51
4751384885	Smaller ions	if charges are the same for 2 ionic bonds, then this must be considered, so that the one with this property has the higher melting point	52
4751384886	Coulombic attraction	smaller ions have greater ______, so their melting points are much higher	53
4751384887	Stronger	through both charges and size, which ever ionic compound has ____ bonds will have higher melting points	54
4751384888	Localized, liquid	in an ionic solid, electrons are ____ around an atom, making them poor conductors, however in the _____ phase, they can conduct electricity because their ions are free to move, even when retaining the original property	55
4751384889	Interstitial alloy	an alloy which the metals have 2 vastly different radii	56
4751384890	Substitutional alloy	alloy formed of 2 similar radii metals,	57
4751384891	Brass, substituted	___ is a good example of substitutional alloy, since the atoms of zinc are _____ for some copper atoms to create the alloy	58
4751384892	Steel, interstices	___ is a good example of an interstitial alloy, for the carbons occupy the _____ between the iron atoms	59
4751384893	Longest, least	single bonds have one sigma bond and a bond order of one, with the ____ bond length and ___ bond energy	60
4751384894	Sigma, pi	bonds first start with one ___ bond, like a single bond, then each additional bond adds a ___ bond	61
4751384895	Network solids	atoms held together by a lattice of covalent bonds, visualized as one big molecule, and are very HARD and have very HIGH melting and boiling points	62
4751384896	Poor	since electrons are localized in a network solid, they are very _____ conductors of electricity	63
4751384897	Carbon, silicon	most network solids are compounds of ___ and ___ because they both have 4 valence electrons, allowing them to form many covalent bonds	64
4751384898	Doping	a process when an impurity is added to an existing lattice	65
4751384899	Three valence electrons, attract	when doping silicon, some silicon atoms are replaced by atoms with ______, creating missing bonds which _____ other electrons, increasing conductivity	66
4751384900	P-doping	ex. When doping silicon, so that silicon atoms are replaced by 3 valence (in general, less electrons) electron atoms, creating missing bonds which positively charge the lattice and allow electrons to fill in the holes, which when they move, leave the holes again, causing a chain reaction, named for "positively charged holes"	67
4751384901	N-doping	ex. When doping silicon, so that silicon atoms are replaced by 5 valence (in general, more electrons) electron atoms, creating extra valence electrons which negatively charge the lattice, and create excess electrons which can move around the lattice, "negatively charge electrons"	68
4751384902	Semiconductor	silicon serves as this when doped with other elements	69
4751384903	dipole	a pair of equal and oppositely charged or magnetized poles separated by a distance.	70
4751384904	Negative dipole, positive dipole	in terms of polarity, the more electronegative element receives a _____, while the less electronegative atom gets a ____	71
4751384905	Negative dipole	the element which attracts electrons more in an covalent bond gets this dipole	72
4751384906	Dipole movement	the polarity of a molecule is measured by this, so the more of this, the more polar a molecule	73
4751384907	Greater, greater	the ___ hte charge at the ends of the dipole and the ___ the distance between the charges, the greater the value of the dipole moment	74
4751384908	Intermolecular forces	must be broken for covalent substances to phase change, though molecular bonds are not actually broken, just those between molecules	75
4751384909	Ionic substances	in contrast to covalent substances, these substances do break bonds when phase changing	76
4751384910	Dipole-dipole forces	occur between polar molecules, so that the positive end of one polar molecule is attracted to the negative end of another polar molecule	77
4751384911	Polarity, dipole movement	molecules with greater ____ will have greater dipole-dipole attraction, so molecules with ___ tend to have higher melting and boiling points	78
4751384912	Weak, low	dipole-dipole attractions are relatively ___, and these substances boil at very __ temperatures	79
4751384913	Gases or liquids	most dipole-dipole substances are these phases at room temperature due to low melting points	80
4751384914	Hydrogen Bonds	much stronger than normal dipole-dipole forces because it when this occurs, the element gives up its lone electron, creating virtually no shielding to the naked nucleus	81
4751384915	Higher	hydrogen bonds have ___ melting and boiling points than most intermolecular forces substances	82
4751384916	London dispersion forces	occur between all molecules, very weak interactions that occur due to random electron movement, so that for a few seconds, a nonpolar molecule may have all electrons on one side, creating a fleeting polarity, and weak dipole	83
4751384917	More electrons	molecules with _____ will experience greater london dispersion forces	84
4751384918	Higher, weaker	though substances that experience greater london dispersion forces with more electrons will have ____ boiling and melting points, overall they are even ____ than dipole-dipole forces, and will melt and boil at even lower temperatures	85
4751384919	Gas	the state of matter london-dispersion force substances usually exist within at room temperature	86
4751384920	Hydrogen Bonds, Non-hydrogen bond permanent dipoles, London dispersion forces (larger the better)	how is bond strength ordered according to the IMF ranking	87
4751384921	Covalent, ionic	the melting and boiling points of ____ substances are almost always lower than that of _____ substances	88
4751384922	Metallic bonding, network covalent bonding	_____,which is usually monoatomic tend to be extremely strong and possess high melting points, though ____ are the STRONGEST form of bonding that exist, with extremely high melting points	89
4751384923	Weak, london dispersion forces	solid particles packed closely, gases spread out, or in other words, substances with ___ intermolecular forces, such as _________ are usually gases at room temp	90
4751384924	Liquids, water	substances with strong intermolecular forces, such as hydrogen bonds, tend to be ______ at room type, like ______	91
4751384925	ionic, solid	_____ do not experience intermolecular forces, their phase instead determined by their bonds, which are significantly stronger than intermolecular forces of covalent molecules, allowing them to be usually ____ at room temp	92
4751384926	Direct, higher	there is a ___ relationship between temperature and vapor pressure, the ___ the temperature of the liquid, the more able the molecules are to breaking free into vapor	93
4751384927	Intermolecular forces, stronger	if two liquids are at the same temperature, vapor pressure is then dependent primarily on ______, with the ___ those forces are, the less likely the molecules are to escape that liquid, making the vapor pressure lower	94
4751384928	Resonance forms	the same molecular compound, but with a different location for the double bond	95
4751384929	# of individual bonds /# of bonds	how to calculate bond order, with # of total bonds as all bonds, so that double bonds are 2 and single 1	96
4751384930	Boron	another exception to the octet rule with a stability at 6 ELECTRONS	97
4751384931	12	the maximum amount of electrons an element can hold when exceeding the octet rule	98
4751384932	n=3	any element from this period AND GREATER can have expanded octets, though none from the lower level (C, N, O etc.)	99
4751384933	D	the subshell available to some molecules so that an element can expand from the 8 electron count, why some noble gases can form bonds	100
4751384934	Formal charge	used to decide which form of the lewis structure is more likely	101
4751384935	Valence electrons-assigned (lewis) electrons	how to calculate formal charge	102
4751384936	Fewer, formal charge	if the charge of both molecules are the same, the ___ # of ATOMS there are with actual ____ is the more likely structure	103
4751384937	Overall charge	the formal charge for polyatomic atoms should equal the_____	104
4751384938	VSEPR model (Valence shell electron-pair repulsion model)	what is used to predict the geometries of molecules so that electron pairs are as far apart as possible	105
4751384939	Bonds count as one (one) (1)	for each atom holding the bond when calculating formal charge, how much does a bond count as?	106
4751384940	Sp, linear	if the central atom has 2 electron pairs, then it has _____ hybridization and it's basic shape is _____	107
4751384941	Sp^2, trigonal planar	if the central atom has 3 electron pairs, then it has _____ hybridization and it's basic shape is _____	108
4751384942	Double, triple, lone electron pairs	___ and ___ bonds are treated the same in single bonds for geometry, though these have slightly more repulsive strength and will occupy more space, though ____ have more repulsive strength than bonding pairs, causing even more reduced bond angles	109
4751384943	sp^3, tetrahedral	if the central atom has 4 electron pairs, then it has _____ hybridization and it's basic shape is _____	110
4751384944	109.5 degrees	Tetrahedral bond angles with no lone pairs	111
4751384945	120 degrees	trigonal planar bond angles with no lone pairs	112
4751384946	dsp^3, trigonal bipyramidal	if the central atom has 5 electron pairs, then it has _____ hybridization and it's basic shape is ____	113
4751384947	Horizontal, vertical	in trigonal bipyramidal shapes, place lone pairs in axial or ___ position, and in octahedral, place the lone pairs in equatorial or ___ position	114
4751384948	d^2sp^3, octahedral	if the central atom has 6 electron pairs, then it has _____ hybridization and it's basic shape is _____	115
4751384949	Absolute temperature	the Kinetic Energy of an ideal gas is directly proportional to its ____, with the greater this is, the greater the average KE of the gas molecules	116
4751384950	Joules	KE is measured in what?	117
4751384951	Same, identity	If several different gases are present in a sample at a given temp, all gases will have the ____ kinetic energy, that is, the KE of gas depends on the absolute temperature, and not the ___ of the gas	118
4751384952	Forces of attraction	there are none of these between gas molecules in an ideal gas	119
4751384953	Losing any energy	gas molecules are in constant motion, colliding with each other and the walls of their container without ___________	120
4751384954	Maxwell-Boltzmann diagram	shows the range of velocities for molecules of a gas, velocity (m/s) as x axis, and # of molecules as y	121
4751384955	Ranges	gases at greater temperatures have greater ____ for velocity	122
4751384956	Smaller	Gases with ______ mass need to have greater velocities in order to have kinetic energy identical with the other gases of equal temperature on a Maxwell Boltzmann diagram, so these mass type gases will have greater velocity ranges than those of the opposite mass	123
4751384957	PV=nRT	Ideal gas equation, with P as pressure, V is volume, n as # of moles, and T as ab. Temp.	124
4751384958	R	variable which stands for the gas constant	125
4751384959	Increases, increases	If V is constant, as P ______, T increases, as T _____, P increases (IGE)	126
4751384960	Inversely, decreases	With T constant, P and V are ___ related, so that as P increases, V ____ and vice versa (IGE)	127
4751384961	Increases, increases	If Pressure is constant, as temp increases, V ____ and as V increases, T ____ (IGE)	128
4751384962	Dalton's Law	the total pressure of a mixture of gases is just the sum of all partial pressures of individual gases	129
4751384963	Proportional, 25%	the partial pressure of a gas is ___ to the # of moles, so if 25 % of the mixture is helium, the the partial pressure due to helium will be ____	130
4751384964	Pa=P(total)(Xa), Xa=moles of gas A/total moles of gas	partial pressure equation and Xa equation	131
4751384965	Larger	the actual volume of a gas under nonideal equations will be ___ than the predicted volume of the IGE	132
4751384966	Stick, smaller (stick, lesser)	when gas molecules ___ together due to intermolecular forces becoming significant, there are fewer particles bouncing around, so that the real pressure is ___ than the predicted IGE pressure	133
4751384967	MM=D(RT)/P	IGE shifted equation which allows you to find molar mass given density	134
4751384968	molarity	expresses concentration of a solution in terms of volume, most widely used unit of concentration	135
4751384969	Brackets	if the chemical symbol is in ___ on the test, that means they are talking about MOLARITY	136
4751384970	Mole fraction	gives the fraction of moles of a given substance S out of the total moles present in a sample	137
4751384971	Xs	mole fraction symbol	138
4751384972	Moles of substance s/ total # of moles in solution	mole fraction Xs equals this expression	139
4751384973	Like dissolves like	rule relating polarity to solute to solvent dissolving matchmaking	140
4751384974	More	The ___ ions present in an ionic compound, the greater the conductivity of that compound will be when the ions are dissociated	141
4751384975	Chromatography	the separation of a mixture by passing it in solution through a medium in which the components of the solution move that different rates	142
4751384976	Polar	The more ___ the substance is, the more it will move up the paper strip in ink chromatography as water is _____, and this property attracts ____ substances	143
4751384977	Red, blue	usually, ____ is the pigment which travels the furthest up the sheet, meaning that this pigment was the most polar, while the ____ stayed put or travelled very little, since it was the least polar	144
4751384978	Rf (retention factor)	measures the distance the ink traveled along the paper	145
4751384979	Rf=distance traveled by solute/distance traveled by solvent front	equation for retention factor	146
4751384980	Stronger	the ____ the attraction between the solute and solvent front, the larger the Rf value would be	147
4751384981	Red	in the black, red, yellow, blue example, which color had the highest Rf value	148
4751384982	Reversed	in the case of a nonpolar solvent, the results of a polar solvent would be ____, with blue travelling the farthest and red the least	149
4751384983	Column chromatography	a column is packed with a stationary substance, then the solution to be separated is injected into the bottom, where it adheres to the stationary phase, then another solution is injected which passes through the stationary phase, attracted the separated substance with varying degrees, with the more attracting substances leaving faster	150
4751384984	Eluent	the solution which attracts the analyte to pass through the stationary phase, is the substance that 1) apsses through the stationary phase and 2) comes after the analyte	151
4751384985	Analyte	the substance which is to be separated, is attracted by eluent to pass through, the more attracted components of this will flow faster through, 1) first to be injected and 2) AT THE BEGINNING adheres to the stationary phase	152
4751384986	Condenser	a piece of glassware with a smaller tube running through a larger tube with hose connections on it, allowing water to run through, inner tube cooled, but not outer tube	153
4837526852	lone electron pairs	these can take the place of bonded atoms in hybridization strucutres	154