Honors Chemistry freshman and sophtmore final flashcards
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| 1973901629 | Significant Figures | Number of digits in a figure that express the precision of a measurement instead of its magnitude. Record one decimal place farther than what is marked. | 0 | |
| 1973901630 | determining significant figures | every nonzero number is significant zeroes appearing between nonzero numbers are significant zeroes to left of significant digit are nonsignificant zeroes to right and after decimal place are always significant zeroes to the right but not before a decimal place are nonsignificant | 1 | |
| 1973901631 | adding and subtracting significant figures | the answer should due rounded off so as to contain the same number of decimal places as the number with the least number of decimal places. In other words, an answer can be only as precise as the number with the least precision. | 2 | |
| 1973901632 | multiplying and dividing significant figures | the answer should be rounded off to contain the same number of digits as found in the LEAST precise of the values. | 3 | |
| 1973901633 | Accuracy | how close a measurement is to the actual value %error= |experimental -actual value| ------------------------ x100 actual value | 4 | |
| 1973901634 | Precision | How close measurements are to each other (how fr away from each other) %difference=|experimental value-average value| ------------------------------ x100 average value | 5 | |
| 1973901635 | Atomos Model | Created by John Dalton (1802), JJ thompson, Ruthford, bohr evidence: law of conservation of mass, law of definite pre portions, law of multiple proportions Conclusions: -All matter is composed of atoms -Atoms of an element are identical -Atoms of different elements are different from each other -Compounds form by combining atoms in small whole # ratios -Chemical reactions occur by combining the same atoms in a different way | 6 | |
| 1973901636 | Plum pudding model | Created by JJ Thompson (1904) and Robert milikan (1911) Evidence: Cathode ray tube, oil drop experiment Conclusion: all atoms contain the same small, negative charged particle (mass/charge). the particle's charge is 1.6x10⁻¹⁹. | 7 | |
| 1973901637 | Cathode ray tube | Results: -beam travels from cathode to anode -spinning pinwheel shows that the beam has mass -bending of beam shows that it is negatively charged -radius of curvature exposes the ratio of particles Thompson changes the cathode materials and gas inside tube. Same mass/charge ratio regardless of construction Conclusion: All atoms contain the same small, negatively charged particles JJ thompson couldn't find the ratio of mass to charge (continues with oil drop experiment) | 8 | |
| 1973901638 | Oil drop experiment | Created by robert millikan (1911) Procedure: -measures radius of oil drops -determines charge on oil drops -all oil droplets had different charges Results: Oil drops all have a charge that is a multiple of a small # Conclusion: Atoms contain a small negative particle whose charge is 1.6x10⁻¹⁹ C. | 9 | |
| 1973901639 | Law of conservation of mass | mass cannot be created nor destroyed | 10 | |
| 1973901640 | Law of definite porportions | the %, by mass, of elements in a compound is constant | 11 | |
| 1973901641 | law of multiple proportions | if two elements form more than one compound, then the ratio of mass of element A that combines with one gram of element B is in small whole number ratios. | 12 | |
| 1973901642 | Theory | well tested explanation of results | 13 | |
| 1973901643 | Nuclear model | Created by: Ernst Ruthford (1911) evidence: gold foil experiment conclusion: atoms are mostly empty space, there are small dense, positively charged areas in an atom (nucleus) | 14 | |
| 1973901644 | Gold Foil Experiment | created by : ernst rutherford Results: Most alpha particles passed straight through some deflected at small angles a few particles deflected backwards conclusion: atoms are mostly empty space small dense positively charged areas in an atom | 15 | |
| 1973901645 | alpha particle | nucleus of helium atom No electrons | 16 | |
| 1973901646 | Isotope | atoms that have the same number of protons but different numbers of neutrons | 17 | |
| 1973901647 | Planetary Model | Created: Neils Bohr evidence: electrons in atoms orbit in nucleus electrons orbit stabily in shells | 18 | |
| 1973901648 | ions | charged particles different # of electrons can be monatomic (one atom) or polyatomic (more than one atom) | 19 | |
| 1973901649 | cations | fewer e⁻ than p+ | 20 | |
| 1973901650 | anion | more e⁻ than p+ | 21 | |
| 1973901651 | atomic weight | average mass of isotopes in an element | 22 | |
| 1973901652 | density | mass/volume | 23 | |
| 1973901653 | alkali metal | any metal i group 1a of periodic table as you go down it gets more explosive as you go down the ionization energy gets lower as you go down electronegativity gets lower as you go down the atomic radius increases | 24 | |
| 1973901654 | alkaline earth metal | any metal in group 2a of periodic table as you go down the ionization energy gets lower as you go down electronegativity gets lower as you go down the atomic radius increases | 25 | |
| 1973901655 | Halogens | nonmetal in group 7a of periodic table | 26 | |
| 1973901656 | Noble gases | an element in group 8a, s and p sub levels are filled not reactive does not attract electrons (no electronegativity) | 27 | |
| 1973901657 | transition metals | metals not apart of any special group | 28 | |
| 1973901658 | inner transition metal | the metals separate of the actual periodic table | 29 | |
| 1973901659 | mendeleev | created of periodic table (1869) organizes elements by relative atomic weight groups by similar properties leaves gaps for undiscovered element predict properties of missing elements | 30 | |
| 1973901660 | chemical formulas | come from mass % in compounds (mass ratio) ratio of atoms in a compound Amount- chemical formulas give # of pieces, from the mass | 31 | |
| 1973901661 | Mole | heap or pile of things in an element 1mole =6.02x10²³ particles molar mass 22.4 L/mole (for every element) at STP | 32 | |
| 1973901662 | amadeo awagadio | created the idea that there is som huge # of atoms (a pile) who's mass in grams is equal to its relative atomic mass in amu's. | 33 | |
| 1973901663 | amu | atomic mass units | 34 | |
| 1973901664 | molar mass | mass of one mole (atomic weight) | 35 | |
| 1973901665 | mole→particles | # moles x 6.02x10²³ particles | 36 | |
| 1973901666 | mole→volume | # moles x 22.4L/mole | 37 | |
| 1973901667 | mole→mass | # moles x molar mass | 38 | |
| 1973901668 | mass→mole | mass / molar mass | 39 | |
| 1973901669 | volume→mole | volume /22.4L | 40 | |
| 1973901670 | particles→mole | # particles / 6.02x10²³ | 41 | |
| 1973901671 | particles | the number of atoms or molecules in an element | 42 | |
| 1973901672 | emperical formula | expermentally determined GIVES RATO OF ATOMS divide everything by the smallest # of atoms in one of the elements, it gives the ratio. -if given the mass, then find the number of moles then convert to atoms. TO FIND: a) find moles b) find simplest ratio (by /ing by smallest # of moles) -when you have %, assume 100g. | 43 | |
| 1974028813 | Diatomic elements | elements when found in natue are in groups of 2 (A₂) elements: H₂, N₂, O₂, F₂, Cl₂ Br₂, I₂ | 44 | |
| 1974028814 | aq (aqueous) | dissolved in water | 45 | |
| 1974028815 | s(soluable) | dissolves in water | 46 | |
| 1974028816 | i (insoluable) | doesn't dissolve in water | 47 | |
| 1974028817 | molecular formula | shows the ratio of atoms in experiment | 48 | |
| 1974088351 | Electromagnetic Radiation Spectrum | The spectrum of light lowest energy to left, highest energy to right lowest frequency at left, highest to right long wavelength to left, short to right Light included: radio, microwave, infrared, visible light, ultraviolet, xray, gamma ray. all travel at 3.00x10⁸m/s | 49 | |
| 1974088352 | RADAR | radio detection and raging | 50 | |
| 1974088353 | wavelength | distance between corresponding parts of successive waves. measured in meters. (meters/wave) | 51 | |
| 1974088354 | frequency | # of waves that pass a point in a given amount of time (waves/second)=hertz (Hz) | 52 | |
| 1974088355 | amplitude | waves height from bottom of wave to crest | 53 | |
| 1974088356 | speed of light (light equation) | constant=wavelength x frequency where c= 3.00x10⁸m/s | 54 | |
| 1974088357 | relationship between wavelength and frequency | as wavelength increases, frequency decreases (inverse relationship) | 55 | |
| 1974088358 | indirect proportion | a graph where y is proportional to 1/x y=k(1/x)... k=slope inverse relationship- if one value goes up the other value goes down | 56 | |
| 1974088359 | direct proportion | a graph where y is proportional to x. | 57 | |
| 1974088360 | energy of light equation | E=h x frequency where h=6.63x10⁻³⁴j/hz any light wave | 58 | |
| 1974088361 | mili | 10⁻³ | 59 | |
| 1974088362 | micro | 10⁻⁶ | 60 | |
| 1974088363 | nano | 10⁻⁹ | 61 | |
| 1974088364 | kilo | 10³ | 62 | |
| 1974088365 | mega | 10⁶ | 63 | |
| 1974088366 | periodic | regularly occurring event | 64 | |
| 1974088367 | quantization | only certain allowed quantities | 65 | |
| 1974088368 | production of color | 1) excite e⁻ to higher E level (add energy) 2) e⁻ drops to ground state emitting energy | 66 | |
| 1974088369 | Periodic trends | atomic radius, ionization energy, electronegativity | 67 | |
| 1974088370 | Atomic radius | distance between the nucleus and outer e⁻ -increases top to bottom -decreases left→right biggest at lower left corner of periodic table. smallest at upper right corner of periodic table | 68 | |
| 1974088371 | Ionization energy | how much energy is needed to remove an electron from a gaseous atom -decreases top to bottom -increases left→right lowest at lower left corner of table. highest at upper right corner. | 69 | |
| 1974088372 | electronegativity | ability to attract electrons by forming bonds(noble gasses have none bc they don't attract e⁻ bc outer electron shell is full) -decreases top to bottom -increases left→right lowest at lower left corner of table. highest at upper right corner. (ignore noble gases) | 70 | |
| 1974088373 | atomic spectra | bright line spectra -e⁻ absorbs energy (only absorb certain wavelength) moves to higher energy level -electrons return to ground state emitting E | 71 | |
| 1974088374 | molecular spectra | not bright lines -e⁻ absorb E (only certain wavelength) -e⁻ don't return to ground state immediately | 72 | |
| 1974088375 | heisenberg uncertainty principle | you may not know both the position and momentum (velocity) of a particle | 73 | |
| 1974088376 | s orbitals | spheres. gets bigger as # gets bigger (4s>2s) 1 on each level | 74 | |
| 1974088377 | p orbitals | pea shapes bigger energy=bigger orbitals 3 on each level | 75 | |
| 1974088378 | d orbitals | lobe shape bigger energy=bigger orbitals 5 on each level | 76 | |
| 1974088379 | f orbitals | 7 on each level | 77 | |
| 1974146875 | electronic configuration rules | aufbau principle, pouli exclusion principle, hunds rule | 78 | |
| 1974146876 | aufbau principle | electrons occupy lowest available energy level (lazy elections) | 79 | |
| 1974146877 | Pouli exclusion principle | An orbital can hold at most two electors. electrons mush have opposite spins to be in the same oprital | 80 | |
| 1974146878 | Hunds rule | electrons will occupy separate orbitals unless energy considerations fore them to occupy the same orbital. | 81 | |
| 1974146879 | Energy increasing levels | 1s2s2p3s3p4s3d4p5s4d5p6s4f... | 82 | |
| 1974209923 | valence e⁻ | electrons in highest energy level f and d levels will never be valence e⁻ | 83 | |
| 1974209924 | Naming ions | name cation( first element) name anion (second element) change end to ide | 84 | |
| 1974209925 | ionic compounds | composed of cations and anions composed of metals and nonmetals | 85 | |
| 1974209926 | ionic bond | bond between metals or metals and nonmetals that bond because one loses an electron and the other needs and electron anything that is 50% or more ionic character, then it is an ionic bond. | 86 | |
| 1974209927 | covalent bond | bond between nonmetals in which both shares the same electron | 87 | |
| 1974209928 | molecular compounds | composed of only nonmetals composed of only covalent bonds | 88 | |
| 1974209929 | naming ionic compounds | metals with nonmetals 1) name the cation a. if only one, go and name cation b. if more than one, use roman numeral to give the cation charge. cation is the metal 2) name the anion | 89 | |
| 1974209930 | naming molecular compounds | 1)use greek prefixes to state how many atoms of each type 2) change last name to -ide | 90 | |
| 1974209931 | mono | one | 91 | |
| 1974209932 | di | 2 | 92 | |
| 1974209933 | tri | 3 | 93 | |
| 1974209934 | tetra | 4 | 94 | |
| 1974209935 | pent | 5 | 95 | |
| 1974209936 | hexa | 6 | 96 | |
| 1974209937 | hepta | 7 | 97 | |
| 1974209938 | octa | 8 | 98 | |
| 1974209939 | nona | 9 | 99 | |
| 1974209940 | deca | 10 | 100 | |
| 1974209941 | Acids | something with H⁺ makes it an acid ionic compounds with H⁺ as the cation | 101 | |
| 1974209942 | Naming acids | 1) name according to anion that is present 2) name anions | 102 | |
| 1974209943 | naming -ite anions in acid | _________ous acid | 103 | |
| 1974209944 | naming -ate anions in acid | ___________ic acid | 104 | |
| 1974209945 | naming -ide anion in acid | hydro______ic acid | 105 | |
| 1974209946 | Balanced reactions | -accurately reflect the conservation of mass -can change coefficients -cannot change formula | 106 | |
| 1974209947 | combustion reaction | substance + oxygen→oxides Hints: look for things that can produce oxides | 107 | |
| 1974209948 | Single replacement reaction | element+ionic→different element +related ionic Hints: metals replace cations nonmetals replace anions | 108 | |
| 1974209949 | Double replacement | ionic + ionic→related ionic+related ionic Hints: switch last names | 109 | |
| 1974209950 | Decomposition reaction | compound→substance +substance Hints: Look for CO₂, H₂O and O₂ check what remains is a ligitiment formula | 110 | |
| 1974209951 | Combination reaction | substance + substance →compound Hints: Look to produce common ionic cmpds. metal oxide+H₂O→ metal hydroxide nonmetal oxide + H₂O→acid | 111 | |
| 1974209952 | Limiting reagent | the reactant that runs out first | 112 | |
| 1974209953 | excess reagent | reactant that you have enough of | 113 | |
| 1974209954 | decant | pour off liquid and save solid | 114 | |
| 1974209955 | % yeild | actual yeild --------- x100% possible yeild (theoretical yeild)→calculated value | 115 | |
| 1974209956 | manipulated variable | changed variable | 116 | |
| 1974209957 | responding variable | variable observed | 117 | |
| 1974209958 | heterogeneous mixture | composition is not uniform (separate) | 118 | |
| 1974209959 | Homogenous mixture | composition is uniform | 119 | |
| 1974209960 | physical change | some properties of a material change, but the composition of the material does not hange | 120 | |
| 1974209961 | Chemical change | the composition of something completely changes | 121 | |
| 1974446244 | Ammonium | NH₄⁺ | 122 | |
| 1974446245 | Acetate | C₂H₃O₂⁻ | 123 | |
| 1974446246 | Chlorate | ClO₃⁻ | 124 | |
| 1974446247 | Chlorite | ClO₂⁻ | 125 | |
| 1974446248 | Cyanide | CN⁻ | 126 | |
| 1974446249 | Hydrogen Carbonate | HCO₃⁻ | 127 | |
| 1974446250 | Hydrogen sulfate | HSO₄⁻ | 128 | |
| 1974446251 | Hydrogen sulfite | HSO₃⁻ | 129 | |
| 1974446252 | Hydroxide | OH⁻ | 130 | |
| 1974446253 | Hypochlorite | ClO⁻ | 131 | |
| 1974446254 | Iodate | IO₃⁻ | 132 | |
| 1974446255 | Nitrate | NO₃⁻ | 133 | |
| 1974446256 | Nitrite | NO₂⁻ | 134 | |
| 1974446257 | Perchlorate | ClO₄⁻ | 135 | |
| 1974446258 | Permanganate | MnO₄⁻ | 136 | |
| 1974446259 | Carbonate | CO₃²⁻ | 137 | |
| 1974446260 | chromate | CrO₄²⁻ | 138 | |
| 1974446261 | Dichromate | Cr₂O₇²⁻ | 139 | |
| 1974446262 | Hydrogen Phoshate | HPO₄²⁻ | 140 | |
| 1974446263 | Oxalate | C₂O₄²⁻ | 141 | |
| 1974446264 | Selenate | SeO₄²⁻ | 142 | |
| 1974446265 | sulfate | SO₄²⁻ | 143 | |
| 1974446266 | Sulfite | SO₃²⁻ | 144 | |
| 1974446267 | Arsenate | AsO₄³⁻ | 145 | |
| 1974446268 | Phosphate | PO₄³⁻ | 146 | |
| 1974446269 | Phosphite | PO₃³⁻ | 147 | |
| 1974446270 | theoretical yield | the calculated yield | 148 | |
| 2081888269 | element | simplest form of matter that has a unique set of properties | 149 | |
| 2081889937 | compound | contains two or more elements chemically combines in a fixed proportion. can be broken down into simpler substance | 150 | |
| 2081894985 | chemical change | change that produces matter with a different composition than the original matter | 151 | |
| 2081901154 | substance | if the composition of a material is fixed, the material is a substance. | 152 | |
| 2081903077 | mixture | if the composition of a material may vary, the material is a mixture | 153 | |
| 2081909084 | mass number of an element | the total number of protons and neutrons in an atom | 154 | |
| 2081914892 | How do you determine the number of neutrons in an atom? | number of neutrons=mass number-atomic number | 155 | |
| 2081919942 | how do you write the shorthand notation using the atomic number and the mass number? | the chemical symbol Au, the atomic number is the subscript. the mass number is the superscript (¹⁹⁷₇₉Au) or can be written just using the mass number (gold - 197) | 156 | |
| 2081959528 | atomic mass | the weighted average mass of the atoms in a naturally occurring sample of the element. how to determine: take all the masses you have for that element (protons and neutrons) and average them.... mass of the protons and the neutrons | 157 | |
| 2083974139 | Relationship between pressure and volume | p₁xv₁=p₂xv₂ indirect proportion only if temperature is constant | 158 | |
| 2083979392 | relationship between pressure and temperature | p₁/t₁=p₂/t₂ direct proportion only if volume is constant | 159 | |
| 2083984138 | relationship between volume and temperature | v₁/t₁=v₂/t₂ direct proportion only if pressure is constant | 160 | |
| 2083989512 | combined gas law | (p₁xv₁)/t₁=(p₂xv₂)/t₂ | 161 | |
| 2083993974 | ideal gas law | pv=nRt preassure x volume= moles x constant x temperature | 162 | |
| 2083997934 | value of R in atmospheric units | .0821 atmxL/molexk | 163 | |
| 2084001536 | value of R in kPa | 8.31 kPaxL/molexk | 164 | |
| 2084004058 | value of R in mmHg and torr | 62.4mmHg(or torr)xL/molexk | 165 | |
| 2084007424 | values at STP | 0ºC, 273 K, 101.3 kPa, 1.0 atm, 760 mmHg or torr, | 166 | |
| 2084015526 | preassure formula | force/area | 167 | |
| 2084019504 | rate of speed of diffusion formula | Ua .......√ molar mass b ------- = -------------- Ub......... mollar mass a | 168 | |
| 2084047220 | binary compound | where 2 elements react to join in a compoud | 169 |
