Flashcards and Answers – Final Review
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| alkali metals |
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| group 1a elements in the periodic table |
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| alkaline earth metals |
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| group 2a elements on the periodic table |
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| halogens |
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| group 7a elements on the periodic table |
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| noble gases |
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| group 8a elements, the s and p sublevels of the highest occupied energy level are filled |
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| representative elements |
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| group 1a through 7a, display a wide range of physical and chemical properties, s and p sublevels of the highet occupied energy level are not filled, its group number equals the number of electron in its highet occupied energy level |
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| representative elements |
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| group 1a through 7a, display a wide range of physical and chemical properties, s and p sublevels of the highet occupied energy level are not filled, its group number equals the number of electron in its highet occupied energy level |
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| transition metal |
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| one of the groub B elements in which the highest occupieds sublevel and a nearby d sublevel generally contain electrons |
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| inner transition metal |
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| highest occupied s sublevel and a nearby f sublevel generally contain electrons |
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| valence electrons |
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| electronsin the highest occupied energ level |
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| valence electrons |
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| electronsin the highest occupied energ level |
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| octet rule |
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| by Gibert Lewis in foring compounds, atoms tend to achieve electron configurations of a noble gas |
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| halide ion |
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| ions produced when atoms of chlorine and other halogens gain electrons all halide ions have a charge of 1- |
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| ionic compounds |
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| compounds composed of anions and cations usually metal cations and nonmetal anions electrically neutral |
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| ionic compounds |
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| compounds composed of anions and cations usually metal cations and nonmetal anions electrically neutral |
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| ionic compounds |
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| compounds composed of anions and cations usually metal cations and nonmetal anions electrically neutral |
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| ionic bond |
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| the electrostatic forces that hold ions together in ionic compounds |
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| ionic bond |
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| the electrostatic forces that hold ions together in ionic compounds |
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| chemical formula |
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| shows the kinds and numbers of atoms in the smallest representative unit of that substance eg: NaCl |
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| formula unit |
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| lowest whole-number ratio of ions in an ionic compound eg: NaCl (1:1), MgCl2 (1:2) |
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| properties of ionic compounds |
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| chrystalline solids at room temperature high melting points can conduct an electrical current when melted or dissolve in water |
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| coordination number |
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| the number o ions of opposite charge that surroud the ion in a chrystal |
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| metallic bonds |
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| the attraction of the free-floating valence electrons forthe positively charged metal ions forces of attraction that hold metals together |
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| alloys |
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| mixtures composed of two or more elements, at least one of which is a metal eg: brass=copper+zinc |
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| covalent bond |
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| held together by sharing electrons |
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| molecule |
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| neutral group of atoms joined by covalent bonds |
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| diatomic molecule |
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| molecule consisting of two atoms |
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| molecular compound |
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| comound composed of molecules tend to have lower melting and boiling points than ionic compounds |
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| molecular formula |
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| chemical formula of a molecular compound shows how many atoms of each element a molecule contains |
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| single covalent bond |
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| two atoms hld together by sharing a pair of electrons |
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| structural formula |
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| represents the covalent bonds by dashes and shows the arrangement of covalently bonded atoms |
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| unshared pair |
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| lone pair, non-bonding pair pair of valence electrons that is not shared between atoms |
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| double covalent bond |
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| bond that involves two shared pair of electrons |
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| triple covalent bond |
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| bond formed by sharing three pairs of electrons |
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| coordinate covalent bond |
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| covalent bond in which one atom contributes both bonding electrons |
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| polyatomic ion |
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| a tightly bond grup of atoms that has a positive or negative charge and behaves as unit eg: NH4+ |
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| bond dissociation energy |
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| the enery required to break the bond between two covalently bonded atoms |
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| resonance structure |
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| a structure that occurs when it is possible to draw two or more valid electron dot structures |
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| the octet rule cannot be satisfied when |
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| a molecule's total number of valence electrons is an odd number |
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| monatomic ions |
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| consist of a single atom with a positive or negative charge resulting from the loss or gain of one ormore valence electrons |
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| polyatomic ions |
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| ions composed of more than one atom their names usually end in -ite or -ate |
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| binary compound |
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| composed of two elements and can either be ionic or molecular |
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| prefixes for binary compounds |
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| 1 - mono, 2 - di, 3 - tri,4 - tetra, 5 - penta, 6 - hexa, 7 - hepta, 8 - octa, 9 - nona, 10 - deca |
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| law of definite proportions |
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| in samples of any chemical compound, the masses of the masses of the elements are always in the same proportions |
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| law of multiple proportions |
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| whenever the same two elements form more than one compound, he different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers |
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| -ide ending indicates |
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| binary compound |
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| -ide ending indicates |
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| binary compound |
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| -ide ending indicates |
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| binary compound |
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| -ite or -ate endings |
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| polyatomic ion that includes oxygen -ate indicates more oxygen |
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| prefixes indicate |
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| the compound is molecular |
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| roman numeral after the name of a cation |
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| shows the ionic charge of the cation |
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| mole |
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| 6.02 x 1023 representative particles of that substance and is in the SI unit for measuring the amount of a substance |
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| Avogadro's number |
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6.02 x 102 the number of representative particles in a mole |
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| molar mass |
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| the mass of a mole of an element to calculte: find the number of grams of each element in one mole of the compound, then add the masses of the elements in the compound |
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| Avogadro's hypothesis |
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| equal volumes of gases at the same temperature and pressure contain equal numbers of particles |
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| standard tempeature and pressure (STP) |
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| 0 degrees celcius 273 K 1 atm 101.3 kPa |
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| chemical equation |
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| a representation of a chemical reaction the formulas of the reactants are connectd by an arrow with the formuls of the products |
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| skeleton equation |
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| chemical equation that does not indicate the relative amounts of the reactants and products |
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| catalyst |
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| a substance that speeds up a reaction but is not used up |
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| coefficients |
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| small whole numbers that are placed in front of the formulas in an equation in order to balance it |
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| balanced equation |
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| each side of the equation has the same number of each atoms of each element and mass is conserved |
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| combination reaction |
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| chemical change in which two or more substances react to form a single new substance |
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| decomposition reaction |
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| chemical change in which a single compound breaks down into two or more simpler products |
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| single replacement reaction |
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| chemical change in which one element replaces a second element in a compound |
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| activity series |
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| lists metal in order of decreasing activity a reactive metal will replace any metal listed below it in the activity series |
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| double replacement reaction |
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| chemical change involving an exchange of positive ions between two compounds |
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| combustion reaction |
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| chemical change in which an element or compound reacts with oxygen often proucing energy in the form of heat and light |
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| stoichiometry |
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| the calculation of quantities in chemical reactions |
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| mole ratio |
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| conversion factor derived from the coefficients of a balanced chemical equation interpreted in terms of moles |
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| kinetic energy |
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| the energy an object has because of its motion |
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| kinetic theory |
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| gas pressure |
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| results from the force exerted by a gas per unit surface area of an object |
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| vacuum |
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| an empty space with no particles and no pressure |
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| atmospheric pressure |
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| results from the collision of atoms and molecules in air with objets |
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| barometer |
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| device used to measure atmospheric pressure |
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| pascal (Pa) |
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| SI unit of pressure, very small amount |
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| standard atmosphere (atm) |
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| the pressure required to support 760 mm of mercury in a mercury barometer at 5 degrees C |
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| compressibility |
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| a measure of how much the volume of matter decreases under pressure |
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| Boyle's law |
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| for a given mass of gas at constant temperature, the volume of the gas varies inversely with the pressure P1 x V1=P2 x V2 |
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| Charles's law |
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| the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant V1/T1=V2/T2 |
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| Gay-Lussac's law |
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| the pressure of a gas is directly proportional tote Kelvin temperature if the volume remains constant P1/T1=P2/T2 |
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| combined gas law |
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| calculations when only amount is constant P1 x V1 /T1=P2 x V2 /T2 |
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| ideal gas constant |
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| (R) 8.31 (LxkPa)/(Kxmol) |
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| ideal gas law |
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| PV=nRT |
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