bonding in diatomic molecules - boston universityquantum.bu.edu/courses/ch102-spring-2015/quantum...
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Boston University Slideshow Title Goes HereFigures on slides 4‐6, 8, 9, 18, 19, 22 and 32−34 are used with permission from Clayden et al., Organic Chemistry (Oxford University Press, 2000), © 2007 Oxford University Press.
Figures on slides 7, 14‐16, 0, 23 and 24 are used with permission from Mahaffy et al., Chemistry: Human Activity, Chemical Reactivity (Nelson, 2011), © 2011 Nelson Education Ltd.
Figure on slides 26 are used with permission from Laird, University Chemistry (McGraw‐Hill, 2009), © 2009 The McGraw‐Hill Companies.
Bonding in diatomic molecules
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Atoms interact by merging waves
AO + AO 2 MOs
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Relative AO phase determines MO character Bonding in diatomic molecules
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σMO’s have cylindrical symmetryBonding in diatomic molecules
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1sσ and 1sσ*Bonding in diatomic molecules
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1sσ and 1sσ*
Mahaffy et al., Figure 10.20
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1sσ (lower) and 1sσ* (upper)Bonding in diatomic molecules
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σ is “bonding” and σ* is “antibonding”Bonding in diatomic molecules
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Bonding PE, KE and total E
Attractive (< 0) PE is opposed by repulsive (> 0) KE.Molecular size is at minimum of total E.
Bonding in diatomic molecules
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Antibonding PE, KE and total E
Repulsive (> 0) PE enhanced by repulsive (> 0) KE. No minimum of total E ‐‐‐ atoms fly apart!
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Bonding and antibonding total E
What matters are the total bonding and antibonding E at the bonding minimum versus the AO energies‐‐‐the energy at infinite separation.
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Correlation diagrams …
… summarize bonding and antibonding effects
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Filling of MO’s H2 MO configuration
Mahaffy et al., Figure 10.20
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Filling of MO’s He2 MO configuration
Mahaffy et al., Figure 10.21
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Filling of MO’s Li2 MO configuration
Mahaffy et al., Figure 10.22
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Bond order
(bonding e‐’s – antibonding e‐’s)/2Division by two is because a single bond shares a pair of
electrons
H2+ = H∙H+ bond order = 1/2
H2 = H:H bond order = 1He2 bond order = 0He2+ bond order = …?
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1s (and 2s) σ and σ*Bonding in diatomic molecules
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2pzσ and 2pzσ*Bonding in diatomic molecules
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2pzσ and 2pzσ*
Mahaffy et al., Figure 10.23
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2pzσ (lower) and 2pzσ* (upper)Bonding in diatomic molecules
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2pxπ and 2pxπ*Bonding in diatomic molecules
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2pxπ and 2pxπ*
Mahaffy et al., Figure 10.24
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Homonuclear diatomics, up to N2
Mahaffy et al., Figure 10.25
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Homonuclear diatomics, after N2
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Homonuclear diatomics
Laird, University Chemistry, Figure 3.4
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Homonuclear diatomicsChallenge: Of H2, Li2, and Be2, which is/are most stable?Challenge: In Li2, what contribution to bonding is due to MO’s
made from 1s AO’s?Challenge: N2, O2, F2, Ne2
TurningPoint lesson: Homonuclear diatomic molecules
http://goo.gl/404yQ
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Which AO’s combine?
SOE: Symmetry, Overlap, Energy Symmetry: Which AO’s can combine to form MO’s? Overlap: Which AO’s combine with the greatest
bonding/antibonding effect? Energy: How does relative AO energy affect composition of
MO’s?
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Symmetry: Net overlap or not?
For a pair of AO’s to give a (bonding/antibonding) pair of MO’s, there must be net overlap (in‐phase or net out‐of‐phase).
If in‐phase and out of phase overlap exactly balance, the AO’s remain uncombined, as nonbonding orbitals.
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Overlap: Greater the better
The more net overlap, the greater the bonding/antibonding effect.
Core AO’s have least overlap Valence AO’s have greatest overlap Bonding due to MO’s made from valence AO’s
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Energy: Closer the better
The closer AO’s are in energy, the greater the bonding/antibonding effect.
If AO’s have same energy (identical atoms, homonuclear bond), MO’s will be 50% of each AO.
If AO’s have different energy (different atoms, heteronuclear bond), … Bonding MO more lower energy AO Antibonding MO more higher energy AO
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Energy: Closer the betterBonding in diatomic molecules
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Energy: Closer the betterBonding in diatomic molecules
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Energy: Closer the betterBonding in diatomic molecules
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TurningPoint lesson: Symmetry – Overlap – Energy
http://goo.gl/tQiAj
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