MCAT CHEM 1

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allenwhycheng
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59451
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MCAT CHEM 1
Updated:
2011-01-12 18:15:09
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chemistry mcat study flashcards
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  1. atomic emission spectrum?
    unique spectrum of light when an atom's electron falls to their ground states
  2. atomic absorption spectrum?
    spectrum of light absorbed when electrons are excited to higher energy level
  3. equation for maximum number electron in a shell?
    2n2
  4. what does azimuthal (2nd) quantum number (l) represent
    subshell
  5. what does magnetic (3rd) quantum number represent
    orbital, possible value from -l to l
  6. how many orbitals can each subshell accommodate
    • s: 0 -----1
    • p: -1,0,1 ------3
    • d: -2,-1,0,1,2 ------5
    • f : -3,-2,-1,0,1,2,3 ------7
  7. how many 4th quantum number (ms) are possible for an electron? what are they?
    2... they are -1/2, +1/2
  8. paramagnetic material?
    has unpaired electrons
  9. diamagnetic material
    has no unpaired electrons
  10. what is the valence config for an element in each of the following groups
    1.VA
    2.IIIA
    3.VIIIA
    4.VB
    5.VIB
    • 1.s2p3
    • 2.s2p1
    • 3.s2p6
    • 4.s2d3
    • 5.s1d5
  11. what is ionization energy (IE)
    energy required to completely remove an electron from an atom
  12. compare the values of the first and second ionization energy of an atom
    second always higher than the first
  13. what is electron affinity
    energy released when an atom accepts an electron
  14. what is electronegativity
    a measure of the attraction an atom has for electrons in a chemical bond
  15. characteristics of ionic compounds
    form crystal lattice, conduct electricity in solution, have high melting and boiling points
  16. what types of bond forms btwn atoms with small differences in electronegativity (.4 - 1.7)
    polar covalent
  17. coordinated covalent bond
    bond in which a pair of electron originates from just one of the atoms
  18. 3 steps for determining geometric configuration
    • 1.draw Lewis structure of the molecule
    • 2.count the bonding and non bonding electron pairs in the valence shell of the central atom
    • 3.arrange the electron pairs around the central atom so that they are as far apart as possible
  19. 3 types of intermolecular forces
    • dipole-dipole
    • hydrogen bonding
    • dispersion forces
  20. formula for gram equivalent weight
    gram equivalent weight=molar mass/ n
  21. formula for calculating equivalents?
    equivalents=weight of compound/ gram equivalent weight
  22. empirical formula?
    simplest whole number ration of the elements present in a compound
  23. formula for calculating percent composition
    mass of X in compound/ molecular weight of compound x100%
  24. Zn(s) + CuSO4(aq)-->Cu(s) +ZnSO4 (aq)
    1.total ionic equation
    2.net ionic equation
    3.spectator ions?
    • 1.Zn (s) + Cu2+ (aq) +SO42- (aq) ---> Cu (s) + Zn2+(aq) +SO42-(aq)
    • 2.Zn (s) + Cu2+(aq)--->Cu (s) +Zn2+(aq)
    • 3.SO42-
  25. elementary rxn?
    rxn that cant be decomposed into other rxn
  26. general formula for the rate law of
    aA+bB--->cC+dD
    rate=k[A]x[B]y
  27. what is enthalpy change of a rxn (delta H)
    the difference btwn potential energy of the products and the potential energy of the reactants.
  28. equilibrium constant for
    A+3B--->2C+2D
    Keq=[C]2[D]2/[A][B]3
  29. does Keq for a rxn consistent for all temp?
    no, it's specific for a given temp
  30. if there is much more product than reactant at equilibrium, what can be said of Keq?
    K>1

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