Chem101 c.11--Test2.txt

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dmk5154
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137036
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Chem101 c.11--Test2.txt
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2012-02-22 18:07:04
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chem101
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chem101 test 2 c.11 Oribtals etc.
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  1. Energy being transmitted from one place to another by light is _________
    electromagnetic radiation (waves on a seagull!)
  2. the distance between two consecutive wave peaks is the ______________
    wavelength (lambda)
  3. the __________ indicates how many wave peaks pass a certain point per given time period.
    frequency (nu, "v")
  4. a beam of light traveling through space is a stream of tiny packets of energy called _____________
    photons
  5. only certain values are allowed (i.e. all hydrogen atoms have the same set of discrete energy levels). They are _______
    quantized
  6. the ____________ model of the atom describes how the electron's position is represented (not a circular orbit)
    wave mechanical
  7. a representation of the space occupied by an electron in an atom (the probability distribution for the electron) is known as a(n) __________
    orbital
  8. Red wavelength photons are ________________ while blue wavelengths are ______.
    Long, short (short length = higher amplitude = more energy)
  9. a model succeeding the Bohr Model of hydrogen. This model explains electron orbits for atoms fall in a probability map:
    The wave mechanical model
  10. 1S orbital is the ______________ energy state, the "ground state"
    lowest
  11. ______________ levels, (represented by n=1, n=2 etc) hold each layer of orbitals (1s, 2s 2p, 3s 3p 3d� etc) within each (n) "electron apartments"
    principle energy levels
  12. principle energy levels are divided into __________, which increase with (n) (such as s, p, d, f)
    sublevels
  13. S sublevel holds ___ electrons max
    2 (1box*2electrons)
  14. P sublevel holds a max of ___ electrons
    6 (3box*2electrons)
  15. D sublevel holds a max of ___ electrons
    10 (5 boxes*2electrons)
  16. F sublevel holds a max of ____ electrons
    14 (7boxes*2electrons)
  17. an atomic orbital can hold a maximum of 2 electrons, and those electrons must have opposite spins. this is the _____ principle
    Pauli exclusion principle
  18. 1s^1 is an example of Hydrogen's ________________
    electron configuration
  19. an orbital diagram/ box diagram would be represented by a box with ____ inside
    arrows ( indicating electron spin)
  20. the electrons in the outermost principle energy level of an atom are _____ electrons-- Important because these are the ones that form bonds
    Valence
  21. inner electrons of a lower sublevel that do not form bonds are called ___________ electrons
    core
  22. Family 1 & 2 have __ outermost orbitals, while transition metals have __ and Families 3-8 have __ outermost orbital
    s; d; p
  23. __________ series fills the 7 4f orbitals
    Lanthanide
  24. _____________ series (14 elements) fills the 7 5f orbitals
    actinide
  25. When an orbital contains d sublevels, the next principle energy level (n+1) will have an 's' sublevel. Which will fill first?
    the n+1 S orbital
  26. Element families/groups ____ are main group elements, or representative elements.
    1-8
  27. ____ tend to lose electrons to form positive ions, while ___________ tend to gain an electron and become negative ions
    metals; non-metals
  28. the energy required to remove an electron from an individual atom in the gas phase is _____________
    ionization energy
  29. (From left to right across a given PT period): what trends occurs? name 3:
    (1) atomic size decreases --which means� (2) nuclear energy increases! & (3) electronegativity increases (up to 4.0)
  30. (From top to bottom across a given Family/Group): what trends occur?
    Atomic size increases (needing larger orbitals to hold greater amounts of electrons)
  31. a period has the same _______________ level, while a family/group has the same ___________
    principle energy level (period 4 = n=4); number of electrons in the outermost orbital (Group 5= 5 electrons)

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