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60 Cards in this Set
- Front
- Back
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Formal charge of molecules/ions
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# valence electrons - shared electrons/2 - nonbonding electrons
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energy of a quantum
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E=hf
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Planck's constant
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h = 6.62 * 10^-34 J*s
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max electrons in an energy level
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2n^2
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max electrons in a subshell
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4l+2
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electron configuration subshell ordering formula
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n + l
smaller sum is listed first, if same number, the lower energy level goes first |
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amu
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mass in grams of 6.022 * 10^23 molecues/atoms
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molar mass
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grams/mole
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percent composition
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(mass X / molecular mass)100%
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percent yield
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(actual yield/theoretical yield)100%
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density
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mass/volume
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ideal gas law
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PV=nRT
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gas constant
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R=0.0821 L*atm/mol*K
R=8.314 J/mol*K |
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Boyle's Law
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P1V1=P2V2
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Charles' Law
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V1/T1=V2/T2
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Gay-Lussac's Law
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P1/T1=P2/T2
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Avogadro's Law
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n1/V1=n2/V2
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Combined gas law
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P1V1/n1T1=P2V2/n2/T2
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Dalton's Law of Partial Pressures
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Pt=Pa+Pb+...
Pa=Pt*(na/nt) |
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average kinetic energy of gases
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1/2mv2=3/2(1.38)T
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Diffusion/Effusion
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r1/r2=sqrt(molar mass 2/molar mass 1)
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rate of a reaction
A+B->C |
rate = k[A]^x[B]^y
k, x, and y are found experimentally |
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half-life
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amount of substance remaining after n half-lives = (1/2)^n
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molarity
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M=moles/liter solvent
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molality
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m= moles/kg solvent
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percent composition by mass
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(mass X / total mass)100%
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equilibrium constant
aA+bB->cC+dD |
Kc or Keq = ([C]^c[D]^d)/([A]^a[B]^b)
products\reactants only aqueous or gaseous species included |
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pH
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pH=-log[H+]
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pOH
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pOH=-log[OH-]
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Kw
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Kw=[H+][OH-]=10^-14
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pH + pOH =
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14
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Ka
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Ka=([H+][conjugate base])/[acid]
bigger = stronger acid |
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Kb
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Kb=10^-14/Ka
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Normality
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N=M*(# of H+ or OH-)
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Titrations
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VaNa=VbNb
MaVa=MbVb |
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Henderson-Hasselbach equation for buffers
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pH=pKa + log ([A-]/[HA])
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Calorimetery
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dH=mc*dT
c=specific heat |
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standard enthalpy of formation for reactions
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dHrxn=sum(dHf products) - sum(dHf reactants)
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Gibb's Free Energy
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dG=dH-T*dS
Goose Hunters Take Shotguns |
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free energy and equilibrium
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dG=-RTlnKeq
standard 25 C, 1 atm, 1 M |
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free energy not at equilibrium
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dG=standard dG + RTlnQ
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boiling point elevation
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dTb=iKb*m
Kb=boiling constant |
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freezing point depression
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dTf=iKf*m
Kf=freezing constant |
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osmotic pressure
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pi=iMRT
pressure needed to prevent water from crossing a semipermeable membrane |
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Vapor Pressure Lowering
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P solution= (P pure solvent)(mole fraction solvent)
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mole fraction
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X=mol A/total moles
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Dilution
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C1V1=C2V2
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Solubility constant
AmBn (s) ->mA^n+ + nB^m- |
Ksp = [A^n+]^m[B^m-]^n
at equilibrium Qsp if not at equilibrium |
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Qsp>Ksp
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supersaturated
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Qsp<Ksp
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unsaturated
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Qsp=Ksp
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equilibrium
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Keq>1
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more products
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Keq<1
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more reactants
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Keq=1
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reactants = products
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alpha decay
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release of a He atom
atomic mass-4 atomic number-2 |
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beta decay
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release of an electron when a neutron becomes a proton
atomic mass stays the same atomic number +1 |
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positron decay
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release of a positron (positive electron) when a proton becomes a neutron
atomic mass stays the same atomic number -1 |
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Gamma decay
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release of energy
no change to atomic mass or number |
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Reduction Potential
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Ecell=Eox+Ered
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Nernst equations
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Ecell= standard E-(0.06/n * log Keq)
Ecell= standard E-(RT/nF * lnKeq) |
