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18 Cards in this Set
- Front
- Back
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Orbital approx |
-assumes multielectron wavefunction product of 1 electron wave functions -neglects electron electron repulsion because wave functions describes 1 e systems |
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Penetration. |
Electron distance from nucleus |
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Valence bond theory |
-pictures bonds as sharing of electron pair -gives us hybrid orbitals and resonance |
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Bonding orbitals |
Wavefunction lower energy than atomic orbitals Increased electron density between atoms |
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VBT and resonance |
-different arrangement of electrons True structure is superposition of wavefunction describing different positions for electrons |
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Variational principle |
Wavefunction calculated energy never less than true value of energy |
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Promotion |
Pictures atoms forming bonds based on an excited state electron configuration Don’t actually have to form excited atoms to form bond Mostly occurs when atom in slightly excited state |
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Hybridization |
Combination of AO on same atom |
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MO theory |
Linear combination of AO that describe electrons in molecules |
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MOT |
Allows for deloc of electrons VBT dosent allow |
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MOT bonding orbitals |
Lower energy and higher electron density |
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MO probability |
Best described as the square of the wavefunction |
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MO Antinonding |
Higher energy than AO Have a node perp to intermolecular axis |
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Energy of molecular orbital changes with distance between atoms |
Bond |
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Sheilding |
-across periodic table +1 e and +1 p. proton not fully shielded by electron -more nuclear charge felt up and to the right |
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Molecular orbital |
-one electron wavefunction Can be bonding antibonding and no bonding |
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VB THEORY |
-allows for hybrid and resonance -promotion and variation also included |
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MO THEORY |
-dosent explicitly define hybrid and resonance but can be described -electrons delocalized -electrons delocalized which isn’t allowed In VB THEORY |
