chem110-test1.txt

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Author:
dmk5154
ID:
161881
Filename:
chem110-test1.txt
Updated:
2012-07-10 07:14:37
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psu chem 110 CHEM
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psu chem 110 Su '12 - Test 1
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  1. Measures the strength of an ionic bond. It is the change in energy when 1 mol of ionic compound is separated to isolated ions in the gas phase
    Lattice Energy
  2. inner orbital electrons screen outer electrons. This results in outer electrons experiencing less attraction/nuclear charge.
    Zeff (Effective nuclear charge)
  3. Electron configuration for Cr and Cu: _ orbital fills before _
    3d;4s
  4. Atomic radius ______ going down a group, and _______ going right to left (when n= larger, e- are further away)
    increases, increases
  5. Ionic size __________ down a group and ______ across (left to right) a period
    increases; decreases
  6. the energy required to remove an electron from an atom or gas phase
    ionization energy
  7. Ionization energy ________ as successive electrons are removed
    increases
  8. I1, First ionization energy __________ down a group, and ________ across a period right to left. (radius gets larger = easier to remove an electron)
  9. energy needed to add an electron ( more negative = more stable)
    electron affinity
  10. valence electrons traded to form a nobel gas configuration (Na+Cl-)
    ionic bond
  11. For Melting point and Lattice energy (strength of bond): they ______ as ion charge increases
    INCREASE
  12. as ion size increases, lattice energy ___________
    decreases
  13. atoms with the same number of electrons
    isoelectronic
  14. the change of heat energy + or -
    enthalpy
  15. __= 1kg m^2/s^2
    1J
  16. emitting energy is ___________thermic, absorbing energy is _____thermic
    exo, endo
  17. no two identical electrons (particles with half-integer spin) may occupy the same quantum state simultaneously.
    Pauli exclusion principle
  18. if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs.
    Hund's rule

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