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| SI unit for amount of substance |
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| the number of entities to the mass of a sample of those entities |
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| the mass per mole of its entities and has units of grams per mole |
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| multiply by 6.022 x 10^23 atoms/mol |
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| ((moles of X in formula x molar mass of X (g/mol))/ (grams of 1 mol of compound)) x100 |
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| mass of compound x ((mass of element in 1 mol of compound) / (mass of 1 mol of compound)) |
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| the amount that contains Avogadro's number of chemical entities |
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| the lowest whole number of moles, and thus the relative number of atoms |
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| the actual number of atoms of each element in a molecule |
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| the relative placement and connections of atoms in the molecule |
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| combustion analysis is used to measure |
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| the amounts of carbon and hydrogen in a combustible organic compound |
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| two or more compounds with the same molecular formula but different properties |
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| the identities and qualities of substances of substances in a chemical or physical change |
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| amount of product calculated from the molar ratio in the balanced equation |
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| the amount of product actually obtained |
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| theoretical and actual yields are expressed in units of |
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| amount (moles) or mass (grams) |
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| (actual yield / theoretical yield) *100 |
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| solution dissolving the solute |
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| water's great solvent power arises from ______ and ______ which create _________ |
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| the uneven distribution of electron charge and a bent molecular shape which create a polar molecule |
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| what makes a polar molecule |
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| combination of polar bonds and a bent shape |
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| replacing attractions with others between several water molecules and each ion |
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| surrounded closely by solvent molecules |
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| soluble ionic compounds are electrolytes |
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Definition
| the ions are free to move, and thus, the solution conducts electricity |
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| three types of equations to represent aqueous ionic reactions |
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Definition
molecular equations
total ionic equations
net ionic equations |
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| molecular equations shows |
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| all the reactants and products as if they were intact undissociated compounds |
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| total ionic equations show |
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| all the soluble ionic substances dissociated into ions |
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| ions that are unchanged on both sides of the equation |
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| net ionic equations shows |
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| only the actual chemical change by eliminating the spectator ions |
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| in a precipitation reaction |
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Definition
| 2 soluble ionic compounds react to form an insoluble product |
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| insoluble product formed in a precipitation reaction |
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| key event in a precipitation reaction |
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| the formation of an insoluble product through the net removal of ions form solution |
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| double displacement reaction |
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| acid-base reaction occurs when |
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| an acid reacts with a base |
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| a substance that produces H+ ions when dissolved in water |
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| a substance that produces OH- ions when dissolved in water |
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| acidic solutions arise when |
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| certain covalent H-containing molecules dissociate into ions in water |
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| dissociate completely into ion |
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| dissociate very little into ions |
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| when no further change in the amounts of reactants and products occur |
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Definition
| the reaction has reached a state of equilibrium |
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| ionic compound that results from the reaction of an acid and a base |
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| the acid-base reaction is a |
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| the known concentration of one solution is used to determine the unknown concentration of another |
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| is a substance whose color is different in acid than in base |
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| equivalence point occurs when |
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| the amount (mol) of H+ ions in the original volume of acid has reacted with the same amount (mol) of OH- ions from the buret |
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| a tiny excess of OH- ions changes the indicator to its basic color (pink) |
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| oxidation reduction reaction |
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| the formation of a compound from its ELEMENTS (or the reverse process) |
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| net movement of electrons from one reactant to another |
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| the species doing the oxidizing (causing the electron loss) |
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| the species doing the reducing (causing the electron gain) |
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| the charge the atom would have if electrons were transferred completely, not shared |
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+1 with nonmetals
-1 with metals |
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-1 with peroxides
-2 with everything else |
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| O.N. for metals in elemental form |
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| transfer electrons are never free because |
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| the reducing agent loses electrons and the oxidizing agent gains them simultaneously |
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| three types of redox reactions |
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Definition
combination
decomposition
displacement |
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| combination redox reaction |
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Definition
combining two elements
combining compounds and elements |
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metal and nonmetal form ionic compound
two nonmetals form a covalent compound |
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| decomposition redox reaction |
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| a compound forms two or more products, at least one of which is an ELEMENT |
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| types of decomposition redox reactions |
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thermal decomposition
electrolytic decomposition |
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| when the energy absorbed is heat |
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| electrolytic decomposition |
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| in the process of electrolysis, a compound absorbs electrical energy and decomposes into its elements |
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| displacement redox reactions |
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| the number of substances on the two sides of the equation remains the same, but atoms (or ions) exchange places |
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| types of displacement redox reactions |
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double displacement
single displacement |
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| double displacement redox reaction |
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Definition
atoms of two compounds exchange places
examples- precipitation, acid-base reactions |
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| single displacement redox reaction |
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| one of the substances is an element |
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| the process of combining with oxygen, most commonly with the release of heat and the production of light, as in a flame |
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| Compounds in which molecules of water are associated with the ions of the compounds |
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| Law of Conservation of Matter |
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| Matter can not be created nor destroyed |
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| Indicates the number of moles involved in the reaction. |
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| Also known as the mole ratio. A ratio of the coefficients from two molecules in the balanced equation |
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| The reactant, that limits the amount of product produced. |
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| Measuring Concentrations of Compounds in Solution Equation |
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| Solutions in which water is the solvent |
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| types of Aqueous Solutions |
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Precipitation
Acid-Base
Oxidation-Reduction |
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Term
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Definition
All common salts of the Group 1A elements and ammonium are soluble.
All common acetates (CH3CO2-), nitrates (NO3-), perchlorates (ClO4-), and chlorates (ClO3-) are soluble.
All compounds of Group 7A elements (other than F) with metals are soluble except those of silver (Ag), mercury (Hg) and lead (Pb)
All compounds of F with metals are soluble except those of magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and lead (Pb)
All sulfates are soluble except those of barium (Ba), strontium (Sr), lead (Pb), calcium (Ca), silver (Ag), and mercury (Hg).
Except for those in rule 1, carbonates (CO32-), hydroxides (OH-), oxides phosphates (PO43-), chromates (CrO42-) and sulfides are all insoluble |
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| General properties of acids |
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Definition
Sour taste
Act corrosive
React with bases to form salt and water |
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| general properties of bases |
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Bitter taste
Feel slippery
React with acids to form salt and water |
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| The force exerted on an object divided by the area over which it is exerted. |
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| The Compressibility of Gases (when moles and temp are constant) |
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| if a given quantity of gas is held at a constant pressure, its volume is directly proportional to the Kelvin temperature |
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| According to Boyle's Law, the volume of an amount of gas is |
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| inversely proportional to the pressure |
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| According to Charles' Law, the volume of an amount of gas is |
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| directly proportional to the Kelvin temperature at a costant pressure. |
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| General or Combined Gas Law Equation |
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| the volume of a gas at a given temperature and pressure is directly proportional to the amount of gas in moles. |
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| The amount (n,mols) of any compound is given by its mass (m) divided by its molar mass (M). |
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| Density of a gas equation |
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| the pressure of each gas in the mixture |
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| Dalton’s Law of Partial Pressure |
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| the pressure of a mixture of ideal gases is the sum of the partial pressures of the different gases in the mixture. |
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| Dalton’s Law of Partial Pressure Equation |
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| Each gas in the mixture acts _______ and can therefore can be considered to behave as an ______. |
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| independently of all of the others and can therefore be considered to behave as an ideal gas. |
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| The molecules in a gas sample do not ________ |
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| all move at the same speed. |
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| All gases, regardless of their molecular mass, have the same ______ at the same ______. |
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| average kinetic energy at the same temperature. |
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| The average kinetic energy of gas particles is proportional to ____ |
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Definition
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| the mixing of two or more gases due to their random molecular motions |
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| the movement of a gas through a tiny opening in a container into another container where the pressure is very low. |
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| The rate of effusion of a gas is inversely proportional to the square root of the mass of its particles. |
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| _______ molecules with _______ average speeds strike the barrier more often and pass more often through it |
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| developed to take into account the cases in which the ideal gas equation breaks down. |
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| the mixing of two or more gases due to their random molecular motions |
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| gas volume changes significantly with |
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| increasing the force on the piston ____ the gas volume |
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| gases have ____ densities |
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| the force exerted per unit of surface area |
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| used to measure atmospheric pressure |
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| one that exhibits linear relationships among volume, pressure, temperature and amount of gas |
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| 0*C (273.15 K) and 1 atm (760 torr/ mmHg) |
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X1 x Ptotal
X1 = mole fraction (n1/ntotal) |
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| Postulates of Kinetic Molecular Theory |
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Definition
Postulate 1: Particle volume - assumed to be zero
Postulate 2: Particle motion - constant random straight line
Postulate 3: Particle collision - elastic |
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| temperature is a measure of |
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| the average kinetic energy of a particle |
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| the rate of effusion of a gas is inversely proportional to the square root of its molar mass |
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| the movement of one gas through another |
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