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Chapters 1-9

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