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Chem 105 Midterm 1
| Term | Definition |
|---|---|
| deposition | gas to solid |
| sublimation | solid to gas |
| intensive physical properties | always the same color, odor, density |
| extensive physical properties | depends length, volume, width |
| law of definite proportions | in a chemical compound the proportions by mass of the elements that compose it are fixed ex: water is 89% oxygen, no matter where it came from |
| law of multiple proportions | when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element will always be in a ratio of small whole numbers |
| atomic theory | elements come from small units of matter |
| Joule | (kg * m^2)/s^2 |
| micro | 10^-6 |
| nano | 10^-9 |
| pico | 10^-12 |
| femto | 10^-15 |
| atto | 10^-18 |
| zepto | 10^-21 |
| mega (M) | 10^6 |
| Giga | 10^9 |
| tera | 10^12 |
| peta | 10^15 |
| exa | 10^18 |
| zetta | 10^21 |
| adding/subtracting sig figs | report answer to the same amount as decimal places as the number with the least amount of decimals ex: 1.2 has one decimal place, and 4.71 has two. The limiting measurement is 1.2, with the fewest decimal places. |
| calculating average atomic mass | (atomic mass of isotope) * (% abundance of isotope) |
| when using two isotopes and trying to find percent or mass of each you can replace y with ______ and then solve for x | y=(1-x) |
| frequency (v - nu) is measured in | Hz = 1 inverse seconds |
| wavelength and frequency (energy) are | inversely proportionate (as one increases, the other decreases and vice versa) |
| energy and frequency are | proportional (increase and decrease at the same time) |
| 1 eV | electron volts 1 eV = 1.602 x 10^-19 J |
| If your equation is general physics → If your equation is atomic-scale (photons, electrons, band gaps)** → If your equation involves photoelectric effect or surface electron emission** → use φ (work function), and specify units (eV or J). | use J use eV use φ (work function), and specify units (eV or J). |
| emission spectrum | emits a few frequiencies (therefore it is black with a few colors emitted) |
| absorption spectrum | absrobs some of the frequencies (therefore it is rainbow with a few missing absorbed colors) |
| going down in energy (from n=3 to n=2) | emission (energy released) |
| going up in energy (n=1 to n=2) | absoption (energy needed to get up higher) |
| normal wavelength equation vs de brogerlie wavelength equation | light waves, sound waves, etc particle behaving like a wave |
| delta x | uncertainty in position |
| delta (mv) (nu) | uncertainty in electron speed (frequency) m is the mass |
| SIE (trident) describes... | an allowed energy state of an electron has 3 quantum numbers |
| SIE^2 | gives probability density orbital - 90% of the volume of that density probability per unit volume of finding an electron at a certain time and a certain place |
| s orbitals | sphere l=0 |
| p orbitals | dumbell l=1 |
| d orbitals | clovers l=3 |
| f orbitals | weird shapes l=3 |
| number of orbitals in a shell | n^2 |
| number of orbitals in a subshell | 2l + 1 (or count the m sub l values) ex: l=3 which means m can be -3, -2, -1, 0, 1, 2, 3 --> 7 (2*3 +1) |
| n | principal quantum number shell number orbital size principal energy level positive interger |
| l | angular momentum quantum number sublevel shape/orbital type ranges from 0 to n-1 |
| m sub l | magnetic quantum number orientation (-l to l) |
| m sub s | electron spin (2 electrons in each orbital) "spin up" +1/2 or " spin down" -1/2 |
| Pauli exclusion principle | no two electrons in a multielectron atom can have the same set of values for the 4 quantum numbers unique address for each electron |
| total nodes | n-1 (planar+ radial nodes) |
| planar nodes | l |
| radial nodes | n-1-l |
| aufbau principle | "to build up" electrons fill lowest energy level first and then build up |
| Pauli Exclusion principle | only 2 electrons can be placed in each orbital |
| Hund's Rule | fill all orbitals with one electron first :socially awkward" - electrons don't want to go together |
| all unaired electrons have the same spin so it's usually ____ because that's usually lower energy | spin up |
| EXCEPTIONS Cr (cromium) | [Ar]4s^1 3d^5 (d orbital stole one of s's electrons) |
| EXCEPTIONS Mo (Molybdenum) | [Kr]5s^1 4d^5 |
| EXCEPTIONS Cu (copper) | [Ar]4s^1 3d^10 |
| EXCEPTIONS Ag (silver) | [Kr]5s^1 4d^10 |
| EXCEPTIONS Au (gold) | [Xe] 6s^1 5d^10 |
| ground state vs excited state | ground state - all electrons are in the lowest possible outcomes excited state - 1 or more electrons have been excited to higher orbitals ex: Carbon: 1s^2 2s^1 2p^3 (one of the 2s electrons jumped to the 2p orbitals) |
| general trend for transition medals | lose electrons to form cations lose s electrons first (which is why in the electron configuration they are down a level) |
| cations | positive lose electrons SMALLER |
| anions | negative gain electrons BIGGER |
| diamagnetic | all electrons are paired repelled by magnetic field |
| paramagnetic | at least one unpaired electron |
| ferromagnetic | unpaired electrons spontaneously align their spins without an external field ex: all electrons are spin up in separate orbitals create own magnetic field |
| degenerate | same subshell (same n and l) |
| metalloids | Sb, Te, Si, B, sometimes As and Ge |
| Z sub eff | Z effective effective nuclear charge |
| Z sub eff = | Z - S Z - number of protons (atomic number) S is shielding factor, number of core electrons. The core electrons shield the outer electrons from the inner, positive nucleus |
| example of Z sub eff equation | Z sub eff of N is = 7 (atomic number) - 5 (inner electrons, 1s^2 not 2s^2, 2s^3) = +5 |
| Z sub eff across a row/period | Z eff increases , valence electrons are helf more tightly oxygen (8) has more portons to hold the electrons more tightly than nitrogen, right behind it (7) |
| Z sub eff down a column | Z sub eff increases but attractive force decreases elecments are getting more protons, but also more electrons |
| atomic radius/size | gets bigger as you move to the left and to the bottom why? because there are less protons as you move to the left, so less force pulling in the electrons for a smaller radius as you go down there are more electrons, meaning the radius is larger |
| electron affinity definition and trend | energy change that occurs when a neutral atom gains an electron (negative) becomes more negative as you go to the right and up |
| electron affinity trends reasoning | because the more right you are, the stronger tendency to gain an electron (to become isoelectronic with noble gases on the far right) the more up, the smaller the shell, meaning it takes less energy to gain an electron (lower energy change) |
| ionization energy definition and trends | amount of energy required to remove an electron, each successive energy gets higher each time (positive) increases as you go up and right |
| ionization energy trends reasoning | as you got to the right, proton pull increases, making it harder to remove electrons (more energy required) as you go up, electrons are closer are more attracted to the nucleus so it is harder to break them off (more energy required) |
| noble gases _______ want to gain or lose electrons | do not their shells are already filled and stable |
| EXPERIMENTS Cathode Ray Tube - Thompson | particles in a tube were attracted to a positive magnet proved there is a negatively charged particle |
| EXPERIMENTS Oil Drop - Milikan | Oil drops in a two layer cylinder would hover in the magnetic field found charge and mass of an electron |
| EXPERIMENTS Gold Foil - Rutherford | put a barrier around a gold plate and shot particles at it, found most went thought and only a few bounced back proved an atom is mostly open space, and contains a small, dense, positive nucleus |
| EXPERIMENTS Radiation - Curie | Found different types of radiation: alpha (2+), can't go through paper beta (-1) can't go trhough led gamma (0) can't go through thick led |
| EXPERIMENTS De Broglie | found electrons behave like waves, oscillating made De Broglie wave equation |
| EXPERIMENTS Heisenberg | uncertainty equation |
| EXPERIMENTS Schrodinger | found solutions to wave equation, quantum numbers |
| EXPERIMENTS Mendelev | made periodic table by arranging elements according to weight and properties |
| gamma | 10^-12 |
| x-ray | 10^-10 |
| UV | 10^-8 |
| visible light (in nm) | 380-740 nm |
| IR | 10^-5 |
| microwave | 10^-2 |
| radio | 10^3 |
| violet | 380-440 nm |
| blue | 440-485 nm |
| cyan | 485-510 nm |
| green | 510-565 nm |
| yellow | 565-590 nm |
| orange | 590 - 625 nm |
| red | 625-740 nm |
| Dalton | hard sphere model of atom, billiard balls with hooks |
| Planck | blackbody radiation by quantizing energy |
| Bohr | quantized energy levels |
| element vs compound | pure substance vs 2 or more different elements |
| homogenous vs hetergenous | homogenous - pure substance evenly mixed heterogenous - substances distributed (oil on top of water) |
| 20.6 | 3 sig figs |
| 0.004 | 1 sig fig |
| 0.000090 | 2 sig figs |
| 400 | 1 sig fig |
| 400. | 3 sig figs |
| physical process do not change the identity but chemical processes ___ alter the identity | DO |
| law of definite proportions law of multiple proportions | definite: one compound, one fixed ration multiple: several compounds, ratios between them |
| exact numbers vs measured numbers | exact numbers: 3 ping pong balls, can count, definitions (a marathon is 26.2 miles) measured numbers: stick is 3 cm long (could be 3.001) |
| definitions have _____ sig figs | infinite |
| final digit contains error, this is the estimated digit so, do not report digits beyond __________ digit | last/estimated |
| accuracy vs precision | accuracy: how close the average value is to the true value (within 1 %) precision: how close several measurements are to each other (within 1%) |
| rows of periodic table | periods |
| columns of periodic table | groups or families |
| areas of periodic table | alkali metals (far left) alkali earth metals transition metals halogens noble gases lanthinide series alchilde series |
| objects absorb/emit energy, not continuously, but in small specific quantities called | quanta |
| Ephoton = hv | yay |
| "work function" | each metal requires a unique, minimum energy to remove an electron |
| when electrons relax and move down energy levels they are | emitting light change in energy is negative |
| when electrons are excited and move up energy levels they are | absorbing photons change in energy is positive |
| the energy gap from 1 to 2 is a lot _____ than the energy gap from 2 to 3 and so on | bigger |
Created by:
anyasalmon