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