Chem 1C chapter 14

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  1. Bonding
    overlap or orbitals on 2 atoms to form a molecular orbital
  2. Orbital
    Describes the region where electrons are likely to be (95%)
  3. Sigma bond
    First bond, symmetrical with respect to rotation along bond axis
  4. Pi bond
    Second and third bonds, not symmetrical with respect to rotation along bond axis
  5. MO Theory
    Form molecular orbitals by making linear combination of atomic orbitals
  6. How many molecular orbitals per atomic orbital
  7. Bonding orbital
    high electron density between nuclei
  8. Antibonding orbital
    Low electron density between nuclei-contains node
  9. How many electrons per molecular orbital
  10. Bonding/antibonding higher or lower in energy than AO
  11. Pauli Exclusion principle only applies to
    Molecular orbitals
  12. Bond order formula
  13. Li2-N2 order of molecular orbitals
    σ2s, σ2s*, π2p, σ2p, π2p*, σ2p*
  14. O2, F2, beyond molecular orbitals
    σ2s,  σ2s*,  σ2p,  π2p,  π2p*, σ2p
  15. Paramagnetic
    Unpaired electron spins, attracted to magnetic field
  16. Diamagnetic
    Paired spins, repelled by magnetic field
  17. Heteronuclear Diatomics
    • Molecule consisting of 2 different atoms
    • If molecule contains only 2nd period elements except O or F, use Li2-N2 filling order
  18. What orbitals contribute significantly to molecular orbitals
    valence orbitals
  19. Delocalization
    When you have a network of adjacent atoms with unhybridized p orbitals, the pi bond spreads over entire network
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Chem 1C chapter 14
2014-11-24 02:14:03
Chem 1C

Chem 1C chapter 14
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