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88 Cards in this Set
- Front
- Back
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Stiochiometry
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is mass and quantity relationships among reactants and products in a chemical rxn
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limiting reactant
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is the reactant that limits the amount of product formed in a rxn
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Experated
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is the amount of product that should be produced based on calculations
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actual yeild
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is the amount of product that is really obtained from a chemical reaction
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heat of fusion
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is the heat necessary to convert a given amount of a solid to a liquid
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heat of vaporation
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is the heat necessary to vaporize a given amount of liquid
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heat of formation
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is the heat released during the synthesis of 1 moleof compound from its elements
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heat of solution
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is the heat created when a solute is dissolved in a solvent
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heat of combustion
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is the heat energy released when a substance reacts with oxygen to form CO2 and H2O
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Enthalpy
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is the total energy content of a system
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enthalpy change
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is the heat energy released or absorbed when a physical or chemical change occurs at constant pressure
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enthalpy change formula
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delta H=H(products)-H(reactants)
deltaH is - =exothermic deltaH is + = endothermic |
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Activation Energy
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is the minimum amount of energy that must be supplied to a system to start a chemical change
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Hess's Law
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the total enthalpy change for a chemical or physical change is the same whether it takes chemical change
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Entropy
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is the measure of the randomness or disorder of a system
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Entropy formula
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delta S=S(products)-S(reactants)
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free energy
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is the quantity of energy related to the capacity of a system to do work, which can beused to predict spontaineity
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Free energy formula
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deltaG=deltaH-TdeltaS
delatG is - =spontanious rxn deltaG is + =nonspontaneous rxn deltaG is 0=state of equilibrium |
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Diffusion
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is the movement of one subtance through another
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Gases
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have mass, exert pressure, properties are explained by a kinetic molecular theory that describes the behavior of the submicroscopic particles that make up gas
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ideal gas
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is a model that effectively describes the behavior of real gases at conditions close to STP
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atmosphoric pressure
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the force the air in the atmosphere on the earth
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Arogadro's Principle
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stated that gases with equivalent volumes under the same conditions have equal # of paticles, applies only to gases
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Charles Law
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states that at constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute temp.
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Charles Law formula
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v1/t1=v2-t2
absolute zero=-273.15'C |
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Boyles Law
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is the pressure and the volume of a sample of gas at constant temp are inversley proportional to each other
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Boyles law Formula
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P1V1=P2V2
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Combined Gas law
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connects both Boyles and charles laws
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Dalton's law of Partial Pressures
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staes that the sum of the partial pressures of all the components in a gas mixture is equal to the total pressure of the gas mixture
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Dalton's law of Partial Pressures formula
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PT=Pa+Pb+Pc+...
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Grahams Law
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states that under the same conditions(constant temp and pressure), gases diffuse at a rate inverely proportional to the square roots of their densities
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Grahams Law Formula
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V1/V2=Square root of (M2/M1)
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ideal gas laws
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describes the physical behavior of an ideal gas in terms of the pressure, volume, temperature, and the # of moles
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ideal gas laws formula
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Pv=nRT
R=0.0821 |
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Phase diagram
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is a graphic representation of the relationships between the physical state of a substance and its pressures and temp
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Triple point
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the temp and pressure at which all three states of matter exist at equilibrium
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Sublimation
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is a change in state from a solid to a gas
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Cupillary action
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is the measure of a liquids tendency to decrease its surface are to a minimum
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suspension
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is a mixture that appears to be uniform while being in stirred, but seperates into different pahases when agitation ceases
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solute
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is the substance being dissolved
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solvent
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is the substance doing the dissolving
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miscible
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liquids or gases that will dissolve in each other
-immiscible is opposite |
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soluble
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able to be dissolved in a particular solvent
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saturated solution
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is a solution that has dissolved all the solute it can hold at a given temp
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unsaturated solution
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is any solution that can disslove more solute at a given temperature
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supersaturated solution
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is a solution that contains more solute that a saturated one has at the temp
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concentrated solution
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a large amount of solute is dissolved in the solvent
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diluted solution
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a small amount of solute is dissolved in the solvent
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molarity
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the # of moles of solute dissolved in each liter of solution
m=moles of solute/liters of solution |
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molality
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the # of moles dissolved in each kilogram of solvent
M=moles solute/Kg of solvent |
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mole fraction
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the # of moles of one component divided by the toatal #of moles in solution
x=mole component/total mol solution |
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Henry's LAw
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the amount of gas dissolved in a solvent is proportional to the partial pressure of that gas over the solvent
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Dissociate
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a process using energy to seperate a compound into ions in water
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solvation
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the process by which water molecules surrond each ion as it moves into sol'n
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colligative properties
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a physical property that is depentent on the # of particles present rather than on the size, mass, or characteristic of those particles
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Lechateliers Principle
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whe a system at equilibrium is disturbed by applying stress, it attains a new equilibrium position to accommodate the change and relieve the stress
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common ion
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an ion that comes from two or more substances making up a chemical rxn
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common ion effect
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a process in which an ionic compound becomes less soluble upon the addition of one of its ions by adding another compound
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strong acid
weak acid |
any acid that dissiociates completely in aqueous sol'n
-any acid that partially dissiociates in aqueous sol'n |
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Strong base
weak base |
any base that dissiociates completely in aqueous sol'n
-any base thatm partially dissiociates in aqueous sol'n |
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Arrhenius acid
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any compound that produces H+ ions in aqueous sol'n
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Arrhenius Base
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Any compound the produces OH- ions in aqueous sol'n
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amphoteric
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having the properties as acting as an acid or a base
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conjugate base
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acid loses H+ ion
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Conjuate acid
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whan a base accepts H+ ion
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acid dissociation constant
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the equilibrium constant for the rxn of an aqueous weak base w/ water
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Base dissociation constant
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the equilibrium constant for the rxn of an aqueous weak base w/ water
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pH
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# that is derived from the concentration of the hydronium ion H3O+ in sol'n
pH=-log(H3O+) |
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Titration
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an analytical procedure used to determine the concentration of a sample by reacting it with a standard sol'n
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standard solution
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a sol'n of percisely known concentration
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Equivalence Point
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point at which the concentration of H3O ions is the same as the concentration of OH- ions
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eridpoint
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the point at which the indicator changes color
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Buffer
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a system consisting of conjugate acid-base pair that is capable of resisting changes in pH when small amounts of acid and base are added
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Becquerel
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discovered radioactivity in 1896
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transmutation
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is the process of changing one element to a another through nuclear decay
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half-life
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the amount of time it takes for half the nuclides in a sample of a given radioactive isotope to decay
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geiser counter
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produces an electric current in the presence of a radioactive substance
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fission
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splitting up of atomic nucleus
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Fussion
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combining atomic nucleus
reach 1 million 'C |
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Organic chemistry
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study of carbon compounds
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properties of organic molecules
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insoluble in water, low melt/boiling point, decomposes easliy when heated
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alkanes
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simplest hydrocarbons only single bonds
CnH2n+2 |
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alkenes
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at least i double bond
CnH2n |
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alkynes
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at least one triple bond
CnH2n-2 |
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molecular formula
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chemical formula that indicates the # of each atom in a molecular compound
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structural formula
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formula that indicates how atoms in a molecule are bonded to each other
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condensed structural formula
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condensed version of structural formula that does not include dashes as bonds
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functional group
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group of atoms that determines an organic molecules chemical properties
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