chem crazy review

• • ide


  hyro___ic acid
• • ite


  __ous acid
• • ate


  ___ic acid
• Ideal gas


  • High temp
  • Low pressure
  • Small particles/molecules
  • Weak IMFs
• Real gas


  • Low temps
  • High pressure
  • Large particle/molecules
  • Strong IMFs
• Like dissolves like


  Based on polaribility, not based on ions
• Retention factor


  Distance traveled by component/distance traveled by solvent
• Microwave radiation


  Cause molecules to rotate
• Infrared radiation


  Molecules vibrate
• UV/visible light


  Make transition to different energy level
• Percent Error Equation


  % Error = (Experimental - Accepted)/Accepted x 100
• Percent Yield Equation

  %Yield = Actual Yield/Theoretical Yield x 100
• Cell Potential Equation

  Eocell = Eocathode - Eoanode
• Anode/Cathode Identification

  An Ox (anode is oxidation), Red Cat (reduction at cathode)
• ΔG meaning


  Negative is thermodynamically favorable, Positive is thermodynamically unfavorable
• Solubility Rules

  • Na+, K+, NH4+, and NO3- are always soluble
• Strong Acids

  • HCl
  • HBr
  • HI
  • H2SO4
  • HNO3
  • HClO4
• The more dissociates


  Stronger acid = weaker conjugate base
• If pH < pKa

  [acid]>[conjugate base]
• If pH > pKa

  [HA] < [A-]
• Strong acids/bases can't form buffers
• Ecell depends how close q to K

  If not close, Ecell=high, if close Ecell=low
• When -H


  Driven by enthalpy
• When +S


  Driven by entropy
• Thermodynamically favorable(k)


  K>1
• Thermodynamically unfavorable


  K<1
• Heat of fusion/vaporization


  q = mΔHfus, q = mΔHvap (or if in moles q = nΔHfus, q =n ΔHvap)
• Coulomb's Law helps explain ionization energy, atomic radius, electronegativity, electron affinity, lattice energy, and bond energies
• Mixtures


  Combining more than one pure substance
• Ionization energy


  Amount of energy required to remove a valence electron from an atom, the more attracted an electron is to nucleus, the higher the ionization energy
• Ionization energy down a column


  Energy levels added, increases r (Coulomb's Law), decreases attraction, lower IE
• Ionization energy across a row


  Protons added, while in same energy level, increases q (Coulomb's Law), increases attraction, higher IE
• Atomic radius


  Increases down a column
• Electronegativity


  Ability of atom in molecule to attract shared electrons, highest in upper right corner of periodic table
• Electron affinity


  How likely to gain electron, also highest in upper right corner of periodic table
• Lattice energy


  Energy released when forming 1 mol of an ionic substance from gas-state, individual ions (applies only to ionic crystals)
• Lattice energy

  Higher charges = more attraction = higher lattice energy (most important), Smaller atomic radii = more attraction = higher lattice energy (less important)
• Bond energies


  Energy absorbed to break 1 mol of the type of bond indicated (applies only to molecular bonds)
• Bond energies

  Single-Bonds = 1 shared set of electrons, each nucleus is weakly attracted, low bond energy, long bond length. Double-Bonds = 2 shared sets of electrons, each nucleus is more strongly attracted, higher bond energy, shorter bond length. Triple-Bonds = 3 shared sets of electrons, each nucleus is even more strongly attracted, even higher bond energy, even shorter bond length.
• Dilutions


  M1V1 = M2V2 - but be careful whether the question asks what the final volume should be, or how much water/solvent should be ADDED to the original sample to create that final volume.