Karteikarten
Chem test 4
Karten in diesem Stapel (97)
- 1In terms of Kinetic energy, --- has the most, --- has a moderate amount, and --- has the least amount of Kinetic energygas, liquid, solid
- 2Gasassumes both the volume and shape of its container, compressible, flows easily, rapid diffusion
- 3liquidassumes the shape of its container, does not expand to fill container, is virtually incompressible, flows readily, slow diffusion
- 4solidretains its own shape and volume, virtually incompressible, does not flow, diffusion is EXTREMELY slow
- 5intermolecular forces attractions are ---, and covalent bonds are ---weak, strong
- 6dipole-dipole forcesthe negative side of one dipole attracts the positive side of another dipole, the greater the polarity of the bond the greater the attraction
- 7london dispersion forcesattractions between nonpolar molecules, a temporary dipole between molecules
- 8london dispersion forces are only important when molecules are ---- very close to each other and are affected byshape
- 9polarizabilitythe ease of which the electron distribution can be distorted
- 10hydrogen bonding are --- than the normal dipole- dipel interactionstronger
- 11hydrogen bonding effects --- (3 things)melting point, boiling point, and specific heat
- 12ion-dipole interactionfoforces between an ion and the partial charge of the end of a polar molecule
- 13ion-dipole interactions are --- than a dipole-dipole attractionstronger
- 14Order of molecular interactions (strongest to weakest)ion-ion
hydrogen bonding
ion-dipole
london dispersion forces = dipole-dipole - 15viscosityresistance of a liquid to flow
- 16surface tensioncohesive attraction that causes a liquid to minimize its surface area
- 17vaporizationliquid to gas
- 18condensationgas to liquid
- 19meltingsolid to liquid
- 20freezingliquid to solid
- 21sublimationsolid to gas
- 22depositiongas to solid
- 23heat of fusionenergy needed to change a solid into a liquid
- 24heating curvetemperature vs. the amount of heat added
- 25critical temperaturethe highest temperature at which a liquid can form
- 26critical pressurethe pressure required to form a liquid at the critical temperature
- 27vapor pressurethe pressure exerted by a vapor in equilibrium with its liquid or solid phase
- 28substances with a high vapor pressure evaporate --- readily than substances with a low vapor pressuremore
- 29volatile substancesliquids that evaporate readily
- 30normal boiling point of a liquid is its boiling point at --- pressure1 atm
- 31a liquid boils when?its vapor pressure equals its atmospheric pressure
- 32phase diagramtemperature vs. pressure for a substance
- 33the triple pointthe point on the phase diagram where 3 phases exist in equilibrium
- 34chemical kineticshow fast a reaction occurs
- 35factors that affect reaction ratesconcentration of reactants, temperature, catalysts
- 36the physical state of reactants also affect reaction rates becausegases and liquids react faster than 2 solids or a solid with a gas
- 37unit of reaction rate1/s
- 38average rate =change in [B]/ change in time
- 39instantaneous rate isthe rate at a particular point in a reaction
- 40reaction rates can change withtime
- 41the rate is directly proportional to the ----concentration
- 42concentration unitsM=mol/L
- 43Rate =k[reactant 1]^m[reactant 2]^n
- 44k is constant but it varies with-----temperature
- 45rate ratio =(concentration ratio)^n
- 46if a concentration doubles are the rate doubles that concentration is a --- orderfirst
- 47if a concentration doubles and the rate increases by 4 that concentration is a --- ordersecond
- 48Rate = k[reactant 1]^m[reaction 2]^n m+n =?the overall reaction order
- 49units of k for: 1st order 2nd order 3rd order1st order: 1/s
2nd order: 1/Ms
3rd order: 1/M^2s - 50half-life is the athe amount of time it takes for a reactant to reach half of its original concentration
- 51a second order reaction rare could look like --- or ----rate = k[A]^2
rate = k[A][B] - 52reaction rates increase when ---temperature increases
- 53the collision modelas temperature goes up, molecules move faster, so there are more collisions per second. as collision increases the reaction rate increases
- 54activation energythe energy it takes to start a reation
- 55elementary reactionsreactions that occur in a single event or step
- 56the number of --- in an elementary reaction determine its molecularityreactants
- 57For elementary reactions refer to table 14.3lkh;lk
- 58the rate of an elementary reaction is based on its ---molecularity
- 59catalysisa substance that increases the rate of a reaction without being consumed
- 60homogeneous catalysisthe catalyst and the reactants are in the same phase
- 61heterogeneous catalysisthe catalyst and the reactants are in different phases
- 62equilibriumoccurs when opposing reactions are proceeding at equal rates
- 63for equilibrium, the products and the reactants don't have to be the same. the --- of both the the forward and reverse reactions have to be the samerates
- 64the equilibrium constant (K) is a numerical value of the expression for a system (aA+bB <->cC+dD) at equilibrium K=[C]^c[D]^d/[A]^a[B]^b
- 65K equilibrium=[products]^m/[reactants]^n
- 66units for Kunitless
- 67K changes when --- changestemperature
- 68If K is very large (>>1) the equilibrium lies to the right of the equation and there is a large amount of ---products
- 69If K is very small (<<1) the equlibrium lies to the left, there is a large amount of ---reactants
- 70the equilibrium constant for the reverse reaction is --- the equilibrium constant for the forward reactionone over the equilibrium constant of the forward reaction
- 71What cannot be included in equilibrium K?solids and liquids
- 72Q is a number obtained by----- and then comparing it to the given Kdividing the coefficients products of the equation by the coefficients reactants
- 73if Q < K in an equilibrium reactionthe reaction shifts to the right and produces more products
- 74if Q > K in an equilibrium reactionthe reaction shifts to the left and produces more reactants
- 75if a system at equilibrium is disturbed by a change in ---, ---, or --- of one of the components, the system with shift its equilibrium to counteract the disturbancetemperature, pressure, or the concentration
- 76increasing the pressure or or decreasing the volume will cause the equilibrium to shift reducing themols of gas
- 77when temperature increased in the direction that absorbsheat (if the forward reaction is endothermic, more products will form)
- 78Bronsted-Lowry acids and basesacid - a substance that can donate a proton to another substance
Base - a substance that can accept a proton from another substance - 79acid(0-6) something that when dissolved in water increases the H ion concentration
- 80base( 8-14)something that when dissolved in water increases the OH concentration
- 81water is a --- substanceneutral (7)
- 82conjugate acid-base pairstwo substances in an acid base reaction that differ by the presence or absence of a proton
(HCl acid and Cl is its conjugate base) - 83the stronger the acid or base, the ---- its conjugateweaker
- 84H2O can act as an --- pr ---acid, base
- 85water can react with itself, this is called---=autoionization
- 86in neutral water [H30]?[OH]=
- 87in acidic water [H30]?[OH]>
- 88in basic water [H30]?[OH]<
- 89pH=-log[H]
- 90on the pH scale acids are from0-7
- 91on the pH scale bases are from7-14
- 92pOH=-log[OH]
- 93pH+pOH=14
- 94anions -- protons from water to form a weak acid, making the solution more basicaccept
- 95cations --- tend to decrease the pH of the solution ei making the solution more ---acidic
- 96factors that determine acid strengththe polarity of the bond, bond strength, the stability of the conjugate base
- 97lewis acids and basesacid - an electron pair acceptor
base - an electron pair donor
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- Karteikarten am Chem test 4, erstellt von H Evans am 07/12/2022.
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