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15 Cards in this Set
- Front
- Back
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valence bond theory |
mixing of atomic orbitals producing hybrid orbitals; overlap of pure or hybridized orbitals; electron density concentrated in region of overlap; stable molecule forms when potential energy has decreased to minimum |
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molecular orbital theory |
creation of set of orbitals belonging to whole molecule; orbitals are mathematical functions indicating probability of finding electrons in central regions of molecule; assigns electrons to molecule - producing molecular orbitals |
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hybridized orbitals |
blended atomic orbitals for covalent bond formation; produce an experimentally observed shape of the molecule - produce working model |
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steps to develop hybridization scheme |
1) write Lewis structure 2) use VSEPR theory to establish electron pair geometry 3) describe molecular geometry; find lone pairs and single electrons used in bonding 4) select hybridization scheme |
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sigma bonds |
end-to-end overlapping with concentrated electron density b/w nuclei of atoms; extremely strong |
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pi bonds |
sideways overlapping with electron density concentrated above and below plane of nuclei; not as strong as sigma |
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domains |
represent number of bonds b/w elements |
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Heisenburg uncertainty principle |
electron is not at a fixed point in space; electrons occupy an orbital with characteristic wave function - square is probability density; orbital is spread out/delocalized over more than 1 atom |
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bonding orbtial |
formed by constructive interference; lower energy and greater stability; electron density greatest b/w nuclei of bonding atoms |
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antibonding orbital |
formed by destructive interference; decreased probability of finding electron and decreased molecular stability; higher energy and lower stability; electron density = 0, b/w nuclei of bonding atoms |
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formation of bonding molecular orbitals |
constructive interference; increase in amplitude analogous to buildup of electron; bonding encouraged due to high electron charge density b/w 2 nuclei |
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formation of antibonding molecular orbitals |
destructive interferences - decrease in electron density; charge density b/w atomic nuclei is low; nuclei are not screened, strong repulsions occur and bond weakened |
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bond order (molecular orbitals) |
electrons in both the bonding and antibonding orbitals are considered |
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paramagnetic |
electron spins are parallel; net magnetic fields are reinforced; found experimentally (molecular orbital theory) |
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diamagnetic |
electron spins are antiparallel; magnetic effects cancel out; slightly repelled by magnet |
