Bonding in diatomic moleculesCH101 Fall 2012Boston UniversityBoston 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 molecules2Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereAtoms interact by merging wavesAO + AO 2 MOsBonding in diatomic molecules3Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereRelative AO phase determines MO character Bonding in diatomic molecules4Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Hereσ MO’s have cylindrical symmetryBonding in diatomic molecules5Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here1sσ and 1sσ*Bonding in diatomic molecules6Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here1sσ and 1sσ*Mahaffy et al., Figure 10.20Bonding in diatomic molecules7Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here1sσ (lower) and 1sσ* (upper)Bonding in diatomic molecules8Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Hereσ is “bonding” and σ*is “antibonding”Bonding in diatomic molecules9Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereBonding PE , KE and total EAttractive (< 0) PE is opposed by repulsive (> 0) KE.Molecular size is at minimum of total E.Bonding in diatomic molecules10Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereAntibonding PE , KE and total ERepulsive (> 0) PE enhanced by repulsive (> 0) KE. No minimum of total E ‐‐‐ atoms fly apart!Bonding in diatomic molecules11Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereBonding and antibonding total EWhat matters are the total bonding and antibonding E at the bonding minimum versus the AO energies‐‐‐the energy at infinite separation.Bonding in diatomic molecules12Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereCorrelation diagrams …… summarize bonding and antibonding effectsBonding in diatomic molecules13Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereFilling of MO’s H2MO configurationMahaffy et al., Figure 10.20Bonding in diatomic molecules14Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereFilling of MO’s He2MO configurationMahaffy et al., Figure 10.21Bonding in diatomic molecules15Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereFilling of MO’s Li2MO configurationMahaffy et al., Figure 10.22Bonding in diatomic molecules16Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereBond order(bonding e‐’s – antibonding e‐’s)/2Division by two is because a single bond shares a pair of electronsH2+= H∙H+ bond order = 1/2H2= H:H bond order = 1He2 bond order = 0He2+ bond order = …?Bonding in diatomic molecules17Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here1s (and 2s) σ and σ*Bonding in diatomic molecules18Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here2pzσ and 2pzσ*Bonding in diatomic molecules19Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here2pzσ and 2pzσ*Mahaffy et al., Figure 10.23Bonding in diatomic molecules20Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here2pzσ (lower) and 2pzσ* (upper)Bonding in diatomic molecules21Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here2pxπ and 2pxπ*Bonding in diatomic molecules22Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes Here2pxπ and 2pxπ*Mahaffy et al., Figure 10.24Bonding in diatomic molecules23Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereHomonuclear diatomics, up to N2Mahaffy et al., Figure 10.25Bonding in diatomic molecules24Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereHomonuclear diatomics, after N2Bonding in diatomic molecules25Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereHomonuclear diatomicsLaird, University Chemistry, Figure 3.4Bonding in diatomic molecules26Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereHomonuclear 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, Ne2TurningPoint lesson: Homonuclear diatomic moleculeshttp://goo.gl/404yQ Bonding in diatomic molecules27Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereWhich 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?Bonding in diatomic molecules28Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereSymmetry: 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.Bonding in diatomic molecules29Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereOverlap: 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’sBonding in diatomic molecules30Copyright © 2012 Dan Dill [email protected] University Slideshow Title Goes HereEnergy: 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
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