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Chem Midterm
Chapters 1-9
| Question | Answer |
|---|---|
| Aufbau Priciple | electrons full orbitals from the bottom up |
| electron configuration | the location of electrons in an atom |
| Hund's rule | electrons will go into an empty orbital rather than one with another electron |
| diamagnetic | atoms with no unpaired electrons |
| paramagnetic | atoms with unpaired electrons |
| condensed configuration | use the noble gas to the "left" |
| electron configuration of Copper | 1s2 2s2 2p6 3s2 3p6 4s1 3d10 |
| Electron configuration of Chromiunm | 1s2 2s2 2p6 3s2 3p6 4s1 3d5 |
| ground state | electrons in the lowest possible energy levels |
| excited state | an electron is moved into a higher level |
| effective nuclear charge | the amount of "pull" the valence electrons feel increases left to right across period does not change up to down in a group |
| Zeff | Zeff= Z-S Z(# of protons) S(# of shielding electrons) |
| valence electrons | electrons in the outermost shell |
| shielding electrons | the electrons that are not valence, the inner electrons |
| Atomic Radius | distance from the nucleus to the valence electrons increases from top to bottom within a group decreases left to right across a period |
| Ionization energy | the amount of energy needed to remove a valence electron from an atom decreases from top to bottom within a group increases left to right within a period |
| electronegativity | the measure of how much an atom "hogs" electrons in a covalent bond decreases moving down within a group increases left to right within a period |
| reactivity | nonmetals increases left to right within a period, metals decrease |
| matter | has mass and occupies space |
| element | cannot be broken down |
| compound | bonded atoms of different elements |
| atoimc element | an element with only one mmolecule |
| molecular element | an element with more than one molecule |
| homogeneous mixture | a mixture where everything is evenly dispursed |
| heterogeneous mixture | a mixture with a clear division between the different particles |
| chemical change | one substance is destroyed and another is created, irreversible |
| physical change | the arrangement of molecules is changed, reversible |
| indicators of chemical change | colour change, giving off heat/light, absorbing heat, bubbling, precipitate forming |
| solid | rigid structure, definite shape, dense, not compressible |
| liquid | takes the shape of container, dense, not compressible |
| gas | fills the container it is in, low density, compressible |
| phase change | when matter goes from one state to another, physical change |
| heat | the energy of moving particles |
| physical property | can be determined without hanging the identity of the object, size. shape, density, boiling point, melting point |
| chemical property | can be determined by changing a substance |
| filtration | separates particles based on size |
| settling | seperates particles based on density |
| chromatography | separates based on traveling distance, mass |
| distillation | separates based on boiling point |
| meaursing | go to one place more than the tool gives you |
| sig figs, with a decimal point | Moving from left to right, count from the first nonzero digit to the final digit |
| sig figs without a decimal point | Moving from left to right, count from the first nonzero digit to the last nonzero digit |
| adding/subtracting with fig figs | answer has the same decimal place as problem |
| multiplying/diving with sig figs | answer has the same sig figs as problem |
| precision | consistency |
| accurate | how close it is to the true value |
| average deviation | a measurement of variation for a set of data |
| percent error | a measurement of the accuracy of the data |
| systematic error | an error that effects the whole lab, every data point |
| random error | happens for only one data set, not continuous |
| molecular compounds | made of two non-metals |
| ionic compound | made of a metal and a non-metal |
| covalent bond | holds together a molecular compounds, atoms share electrons |
| ionic bond | holds together an ionic compound, atoms stick toghether |
| poly-atomic ion | made of multiple atoms, behaves like a single particle |
| nitrate | NO3 (-1) |
| sulfate | SO4 (-2) |
| phosphate | PO4 (-3) |
| ammomium | NH4 (+1) |
| carbonate | CO3 (-2) |
| bicarbonate | HCO3 (-1) |
| hydroxide | OH (-1) |
| acetate | C2H3O2 (-1) |
| molecular compound prefix: 1 | mono |
| molecular compound prefix: 2 | di |
| molecular compound prefix: 3 | tri |
| molecular compound prefix: 4 | tetra |
| molecular compound prefix: 5 | penta |
| molecular compound prefix: 6 | hexa |
| molecular compound prefix: 7 | hepta |
| molecular compound prefix: 8 | octo |
| one mole | 6.022*10^23 particles(atoms) |
| molar mass | the mass of one mole of an element |
| solving for moles | grams/molar mass |
| solving for grams | molar mass*moles |
| solving for molar mass | grams/moles |
| molecular formula | the number of every atoms is shown in the subscripts |
| empirical formula | the ratio of elements is shown in the subscripts |
| how to find molecular formula | experimental molar mass/empirical molar mass=multiple |
| percent composition | the percentage by mass of each element in a compund |
| how to find the empirical formula from percent composition | percent -> Mass -> moles / smallest * till whole |
| chemical equation | the description of a chemical reaction |
| reactants | chemicals to the left of the arrow in a chemical equation |
| producats | chemicals to the rights of the arrow in a chemical equation, what the reaction creates |
| state symbols | the phase of matter a chemical is in, states in parentheses in a chemical equation |
| aqueous | a chemical dissolved in water |
| coefficients | indicate the number of molecules needed in a chemical equation |
| catalyst | a substance that speeds up a chemical reaction, written above the arrow in a chemical equation |
| Δ | indicates that reactants should be heated in a chemical reaction |
| law of conservation of mass | matter can not be created of destroyed |
| Stoichiometry | mathematics of the molar ratios in a chemical reaction |
| limiting reactant/reagent | the chemical that is used up first in a chemical equation |
| ICE chart | Initial, change, end. Written in moles |
| theoretical yield | the maximum amount of product that can be made given the limiting reagent |
| percent yield | the percent of product made compared to the amount of product that could have been made |
| calculating percent yield | (actual amount of product/theoretical yield) *100 |
| synthesis | A + B -> AB |
| decomposition | AB -> A + B |
| Single replacment | A + BC -> B + AC |
| double replacement | AB + CD -> CB + AD |
| Combustion | CxHyOz + O2 -> CO2 + H2O |
| combustion tricks | coefficient of CH is half of H2O Subscript of C in CH is same of coefficient of C |
| diatomic 7 | elements that can only live alone is groups of 2 |
| the elements of diatomic 7 | hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine |
| atomism | the idea that everything is made of atoms |
| Democritus | Greek philospher credited with the idea of atomism |
| Joseph Proust | French scientist credited with Law of definite proportions |
| Law of Definite Proportions | Any given compound always contains the same ratio of element |
| John Dalton | English scientist credited with law of multiple proportions |
| Law of Multiple proportions | If two elements can form two or more different compounds, a fixed amount of the first element will combine with whole number multiples of the second element. |
| J. J. Thomphson | discovered the electron |
| Plum pudding model | created by Thompson, shows the electron in the atom |
| Robert Millikan | Used oil can experiment to determine the charge of an electron |
| charge of an electron | 1.602 × 10^-19coulombs or 1 atomic unit |
| Ernest Rutherford | Uses the gold foil experiment to discover the nucleus |
| line spectra | the wavelengths of light emitted by an element |
| electromagnetic (EM) wave | the energy emitted from an atom when an electron "falls" back down |
| frequency | the rate or level of energy |
| wavelength | the distance between two waves of energy |
| speed of light | 3.00 × 10^8 m/s |
| electromagnetic spectrum | the range of electromagnetic waves and frequencies |
| spectroscope | used to see the different wavelengths of light emitted by an element |
| Niels Bohr | came up with the idea of electron orbits |
| quantized electrons | Only certain distances from the nucleus (energy levels) were allowed |
| orbits | set paths for electrons |
| Werner Heisenberg | developed the uncertainty principle |
| uncertainty principle | it is impossible to know the exact position of an electron |
| orbital | the region in which an electron could be present |
| proton | +1 charge, 1 atomic mass |
| nuetron | neutral charge, 1 atomic mass |
| electron | -1 charge, ≈0 atomic mass |
| atomic number | the number of protons in a nucleus |
| isotype | 2 atoms of the same element (same # of protons), but with different masses |
| atomic mass | the weighted average of the naturally occurring isotopes of an element |
| electrical charge | the overall charge of an atom based on the # of protons and electrons |
| strong force | the force that keeps the atom together |
| ratio of neutrons to protons for small nuclei | 1:1 |
| ratio of nuetrons to protons for large sucli | 1.5:1 |
| most stable nuclei | nickel and iron |
| binding energy | energy released by the particles when the strong force is applied |
| mass defect | the amount of mass lost when the binding energy is released |
| radiation | high speed subatomic particles, a type of electromagnetic radiation |
| alpha decay | the nucleus emits and alpha particle, a cluster of 2 protons and 2 nuetrons |
| beta decay | the nucleus emits a beta particle, which is an electron |
| gamma emission | electromagnetic wave than is emitted, no charge or mass |
| electron capture | the nucleus gains an electron, and emits x-rays |
| positron emission | the nucleus emits a positron, a positively charged electron |
| predicting nuclear decay | above 82 protons; beta decay less than 82 protons; alpha decay |
| decay chain | the continuous decay of an atom until it reaches stability |
| fission | when a nucleus splits into two smaller nuclei |
| critical mass | atom is just large enough to sustain the chain reaction |
| super-critical mass | when the atom is too charge to sustain the chain reaction |
| nuclear reactor | uses fission of uranium to create energy |
| half life | the time it takes for a sample of radioactive material to decay |
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