Terms : Hide Images
| 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 |
