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evil chem crap
chemistry 1150
| Question | Answer |
|---|---|
| of the same or similar kind of nature | homogeneous |
| consisting of dissimilar or diverse ingredients or constitutes | heterogeneous |
| only a single type of matter is present(only one elemental substance) | pure substance |
| occurs when two or more pure substances are intermingled with each other | mixtures |
| mixtures in which the composition is identical throughout | homogeneous mixtures |
| a mixture in which the composition is not the same throughout | heterogeneous mixture |
| this indicates the number of atoms of each element that make up the smallest possible piece of a compound | chemical formula |
| chemical formula for two hydrogen atoms and one oxygen atom | H2O |
| transformation of a pure substance leaving it as the same substance but in a different state | physical transformation |
| these properties include color, odor, and taste | physical properties |
| when a pure substance goes from solid state directly to gas state without going through the liquid state | sublimation |
| transformation of a pure substance leaving it as a different substance or substances | chemical transformation |
| the starting substances during chemical transformation | reactants |
| the new substance formed from chemical transformation | products |
| at normal atmospheric pressure water boils at | 100 C |
| a ______ will greatly increase the rate of a chemical reaction without getting involved in the chemical reaction | catalysts |
| A+B > AB- reactants a & b combine to form a more complexed molecule | synthesis reactions |
| AB> A + B- the molecule AB is broken down into smaller molecules causing energy to be released | decomposition reactions |
| AB + CD> AD + CB-involve both synthesis and decomposition reactions, both reactants exchange parts to yield a new compound | double replacement reactions |
| A + BC > B + AC- two reactants exchange molecules to form a new product | single replacement reactions |
| CH + O> CO + H20- when reactants exchange molecules causing these to ignite, and the end products are a gas and H2O | combustion reactions |
| zeros within a number are always | significant figures |
| zeros that do nothing but set the decimal point are always | not significant figures |
| trailing zeros that aren't needed to hold the decimal point are always | significant figures |
| 4308 and 40.05 contain____ significant figures | 4 |
| 470,000 and 0.10000 contain ____ significant figures. | 2 |
| 4.00 and 400 contain______ significant figures | 3 |
| negatively charged subatomic particle | electron |
| positively charged subatomic particle | proton |
| subatomic particle found to carry no charge | neutron |
| the number of protons found in an element | atomic number |
| the number of protons and neutron found in an element | atomic mass |
| different versions of the same element that have the same atomic number but a different atomic mass | isotope |
| an atom in which the electron/proton balance is not maintained , cations + charge, anions - charge | ion |
| the distance from a peak in one wave to the peak in the next wave, always expressed in meters or nanometers | wavelength |
| the number of waves that pass each second and are expressed in hertz(Hz) | frequency |
| electrons orbit around a nucleus in fixed energy levels, electrons are found in specific energy levels and nowhere else, electron energy levels are qunatized | bohr model |
| electrons in the outer levels of bohr diagrams | valance electrons |
| n=1 2n2= 2 X 1(2) | 2 electrons |
| n=2 2n2= 2x 2(2) | 8 electrons |
| n=3 2n2= 2x 3(2) | 18 electrons |
| n=4 2n2= 2 x 4(2) | 32 electrons |
| each outer electron is represented by one dot around the atomic symbol in | lewis dot |
| electrons occupy energy subshells within each shell that are designated | s, p, d, and f |
| the number of subshells in each level is the same as the number on the | main level |
| the first energy level has one subshell designated | 1s |
| the second energy level has two subshells designated | 2s, 2p |
| the third energy level has three subshells designated | 3s, 3p, and 3d |
| n=1(2 electrons) has a subshell capacity of | 1s2 |
| n=2 (8 electrons) has a subshell capacity of | 1s2, 2p6 |
| n=3 (18 electrons)has a subshell capacity of | 1s2, 2p6, 3d10 |
| n=4 (32 electrons) has a subshell capacity of | 1s2, 2p6, 3d10, 4f14 |
| electrons react to form compounds in a way to put eight electrons in there outermost valence shell | octet rule |
| metals are always____ ions | positive |
| nonmetals are always____ ions | negative |
| the charge of an ion is equal to its________ | group number |
| metals lose all their valance electrons to form | cations |
| nonmetals gain electrons to fill their outer shell and form | anions |
| generally the # of ____ is equal to the # of____ | electrons; protons |
| equation to calculate wavelength energy | E=hc/λ |
| an atom defined as the arrangement of electrons at the lowest total energy | ground state |
| when one or more of an atoms electrons are located in higher levels of energy shells | excited state |
| collection of atoms bound together | molecule |
| any substance comprised of distinct molecules | molecular substance |
| comprised of two or more types of elements | molecular compound |
| comprised of only one type of element | elemental substance |
| the attractive forces that hold atoms together in molecules | chemical bonds |
| involves the transfer of electrons | ionic bonding |
| involves the sharing of electrons | covalent bonding |
| formation of chemical bonds always releases | energy |
| breaking of chemical bonds always requires | energy |
| the number of dots in a lewis dot structure corresponds to the number of | valence electrons |
| determine total number of valence electrons, connect atoms with a single bond, place remaining electrons as lone pairs, if each does not have an octet change lone pair to bonding pairs | steps to drawl a lewis dot diagram with bonds |
| these are valid dot diagrams that differ by electron placement | resonance forms |
| these are ions that are made up of multiple atoms | polyatomic ions |
| Na2S | sodium sulfide |
| MgCl2 | magnesium chloride |
| Al2O3 | aluminum oxide |
| Li3N | lithium nitride |
| FeCl2 | ferrous chloride/Iron(II) chloride |
| FeCl3 | ferric chloride/Iron(III) chloride |
| CuCl | Copper(I)chloride |
| CuCl2 | Copper(II) chloride |
| CoCl2 | cobalt(II) chloride |
| CoCl3 | cobalt(III) chloride |
| Hg2Cl2 | mercury(I) chloride |
| HgCl2 | mercury(II) chloride |
| SnCl2 | tin(II) chloride |
| SnCl4 | tin(IV) chloride |
| Pcl3 | phosphorous tricloride |
| P4O6 | tetraphosphorous hexoxide |
| P4O10 | tetraphorphorous decoxide |
| SF6 | sulfure hexafluoride |
| SO2 | sulfur dioxide |
| SO3 | sulfure trioxide |
| NO2 | nitrogen dioxide |
| N2O4 | dinitrogen tetroxide |
| N2O5 | dinitrogen pentoxide |
| NH4+ | ammonium |
| CH3CO2- | acetate |
| CH- | cyanide |
| NO2- | nitrite |
| NO3- | nitrate |
| Co3(2) | carbonate |
| HCO3 | bicarbonate |
| SO3(2)- | SULFITE |
| SO4(2)- | SULFATE |
| HSO4- | BISULFATE |
| MnO4- | PERMANGANATE |
| PO4(3)- | PHOSPHATE |
| HPO4(2)- | HYDROGEN PHOSPHATE |
| H2PO4- | DIHYDROGEN PHOSPHATE |
| ClO- | HYPOCHLORITE |
| ClO2- | CHLORITE |
| ClO3- | CHLORATE |
| ClO4- | PERCHLORATE |
| CrO4(2)- | CHROMATE |
| Cr2O7(2)- | DICHROMATE |
| O2(2)- | PEROXIDE |
| HF | HYDROFLUORIC ACID |
| HCl | HYDROCHLORIC ACID |
| HI | hydroiodic acid |
| HCN | HYDROCYANIC ACID |
| H2S | HYDROSULFURIC ACID |
| an acid is any substance that dissociates in water to yield | an H+ ion |
| a base is any substance that dissociates in water to yield | an OH- ion |
| group IA metals always form | +1 ions |
| group IIA ions always form | +2 ions |
| group IIIA ions will form | +3 ions |
| group IVA will form | +2 and +4 ions |
| group V will gain 3 electrons to form | -3 ions |
| group VI will gain two electrons to form | -2 ions |
| group VII gain one electron to form | -1 ions |
| when writing chemical formulas _____ goes first and _____ goes second | metal; non metal |
| the sum total charge of an ionic compound must equal | zero |
| heat, color change, emission of light, formation of gas or a solid precipitate are all | evidence of a chemical change |
| balance equations by placing_____ before reactants and the products | coefficients |
| the study of the quantitative aspects of chemical reactions | stoichiometry |
| one mol is_____ of anything | 6.022 x 10(23) |
| 1 mole of an atom has a molar mass equal to its | atomic weight |
| to calculate %yield | actual yield/theoretical yield x 100 |
| any reactant that is present in short supply relative to the other reatants according to the demands of a balanced equation | limiting reactant |
| in a solution the substance present in the greatest amount is called | solvent |
| all substances other than the solvent in a solution are called | solutes |
| solutions in which water are the solvent are called | aqueous solutions |
| formation of attractive forces between solvent particles and solute particles | ion-dipole forces |
| we must overcome the solute-solute attractive forces, ΔE is positive | solute-seperation step |
| we must over come the solvent-solvent attractive forces and pry solvent particles apart to make room for solute particles, ΔE is positive | solvent-seperation step |
| as solute-solvent attractive forces develop, energy is released, ΔE is negative | solvation step |
| ΔE solute separation + ΔE solvent separation + ΔE solvation= | ΔE total |
| if ΔE total < 0 | the substance will dissolve |
| if ΔE total >) | the substance will probably not dissolve |
| the maximum amount of a solute that can be dissolved in a given amount of solvent is called | solubility of the solute |
| when the maximum amount of solute is dissolved in a solution it is | saturated solution |
| these have many molecules with nonpolar tails and polar heads grouped together | micelle |
| moles of solute/1L of solution= | molarity |
| mass of diluted solution x volume of diluted solution/ mass of stock solution= | volume of stock solution |
| grams of solute/grams of solution x 100= | percent composition by mass |
| volume of solute/volume of solution x 100= | percent composition by volume |
| grams of solute/volume of solution x 100= | percent composition by mass/volume |
| consider _____ if its sour to the taste, turns litmus paper red, eats away active metals by reacting with them to produce hydrogen gas | acidic |
| considered _____ if its bitter to the taste, turns litmus paper dark blue, produced aqueous solutions that felt slippery to the touch | basic |
| a substance in an aqueous solution that conducts an electrical current | electrolyte |
| a substance in an aqueous solution that does not conduct an electrical current | nonelectrolyte |
| completely dissociates into ions upon dissolving in water | strong electrolyte |
| partially dissociates into ions upon dissolving in water | weak electrolyte |
| a water soluble compound that dissociates in water to give large numbers of H3O+ ions | strong acid |
| a water soluble compound that dissociates partially in water to produce only a few H3O+ ions | weak acid |
| an acid that can give off two H3O+ ions | diprotic acid |
| an acid that can give off one H3O+ ions | monoprotic acid |
| and acid that can give off three H3O+ ions | tetraprotic acid |
| the equilibrium constant for the reaction between a base and water= | Kb |
| the equilibrium constant for the reaction between a acid an water= | Ka |
| holds the value of 10(-14) at 25 degrees C | Kw |
| the splitting of ionic compounds into individual charge components | dissociation |
| a mole of any substance has a mass in grams equal to the | molecular/atomic mass |
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