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MCAT General Chemistry

  1. proton charge
    1.6 *10 ^-19 columbs
  2. "z" atomic number
    atomic number is equal to the number of proton found in an atom if the element.
  3. "A"mass number
    protons plus neutrons
  4. electrons are 1/2000 of a proton
    small
  5. atomic weight
    averaged weight of naturally occuring isotope of an element found on the periodic table
  6. half life
    • longer the half life the more stable gives info on the proportion of isotopes of the element
    • as A and Z increase half life increase
  7. plancks equation
    • energy of quanta
    • E=hF
    • h=6.6*10^-34J*seconds
  8. speed of light
    • v=f*λ
    • 3*10^8m/s
  9. angular momentum(L)
    L=mνr
  10. kinetic energy
    1/2 mv^2
  11. angular momentum of an electron orbiting a hydrogen nucleus
    L=nh/2pi
  12. energy of an electron
    E=rh/n^2
  13. rydberg unit of energy
    2.18*10*-18
  14. general energy rule
    All systems tend toward minimal energy
  15. Electrons get "AHED"
    • A- absorb light 
    • higher potential
    • Excited 
    • Distant from nucleus
  16. Lyman series
    • hydrogen emission lies corresponding from n> or =2 to n=1.
    • to 2 is the Balmer series 
    • Paschen
    • 4 to 3
  17. energy
    • inversely proportional to wavelength
    • negative energy of photon means that there is absorption and vice versa
  18. uniqueness of elements
    each element has a characteristic set of energy level thus a characteristic AES and AAS
  19. general color rule
    we see color that is reflected and not absorbed by a compund
  20. basic numerical equivalents for fractions
    • 1/16=0.0625
    • 1/8=0.125
    • 1/20=0.05
    • 1/7=0.14
    • 1/9=0.11
    • 1/36=0.0325
    • 1/6=0.16
    • 1/12=0.083
  21. heinsberg uncertainty principle
    cannot pinpoint the exact location of an electron in an orbital at a given time
  22. pauli exclusion
    no two electrons can have nthe same four quantum numbers in a given atom
  23. subshells
    shapes of the particle is dependent on the subshell that it is found in.
  24. aufbau principle
    electrons fill from lowest to highest energy subshell
  25. hunds rule
    • within a subshell that has more than one orbital.orbitals are filled do that the maximum amount of half-filled orbitals with parrallel spins is achieved.
    • in a diagram each electron would fill their own orbital.
    • half-filled and fully filled shells have lower energy thus more stability
  26. paramagnetic
    • parrel spin in unpaired electrons
    • They will orient their spins in alignment with a magnetic field
    • causes an attraction
    • para like to pair up. be attracive. fill in allign
  27. diamagnetic
    • like to diverge of depart
    • does not align w/ b field and repelled by the b field 
    • They already have their paired electrons
  28. sugars are classified
    aldose and ketose
  29. Heisenberg uncertainty principle
    the postion and momentum of an electron is impossible to detect at any given time
  30. aufba's principle
    the subshells must fill from highest to lowest
  31. hund's rule
Author
Ianagarrick
ID
327473
Card Set
MCAT General Chemistry
Description
Gen chem MCAT review
Updated

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