Zumdahl, Hfst. 9. Intermoleculaire Binding. Intermoleculaire Binding (overzicht modellen 2) Intermoleculaire Binding (overzicht modellen)
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1 Zumdahl, Hfst. 9 Hybridisatie (9.1) orbital theorie ( ) bindingsvolgorde binding diatomic molecules binding heteronucleaire moleculen Combinatie LE en M theorie (9.5) p. 351: A bond will form if the energy of the aggregate is lower than that of the separate atoms NB: voor het verklaren van het bestaan van moleculen, die dus een lage toestand vertegenwoordigen, zijn steeds uitgebreidere modellen nodig. (overzicht modellen) (overzicht modellen 2) Quantumchemie is overkoepelend model plossing vaak onmogelijk (complexe moleculen) Benadering nu mogelijk met computermodellen Echter, onderstaande modellen gebaseerde op quantumchemie stellen ons in staat >90 of zelfs 99% van alle moleculen te begrijpen. Gelokaliseerde electronmodellen (Hoofdstuk 8) - Van Ionbinding tot Covalente Binding - Valence Bond model: valentie-electronen spelen hoofdrol bij chemische binding Covalent: Lewis model voor Electronenverdeling in moleculen i Resonantie VSEPR Niet alleen electronen-verdeling, maar ook verklaring waarom chemische binding in organische moleculen stabiel zijn waarom ze een bepaalde ruimtelijke structuur hebben Hybridisatie (Hfk. 9.1) Verklaring van het bestaan van een aantal bijzonder moleculen en eigenschappen die niet te verklaren zijn met de voorgaande modellen Gedelokaliseerde electronmodellen (hfk ) - M theorie Localized Electron Model (8-9.1) of atomic Underlying assumption: A molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic of the bound atoms. Hfst. 8: ionbinding covalent; Lewis Hfst 9: gehybridiseerde atomic Definition Model Most important types; examples sp 3 methaan sp 2 etheen sp ethyn Additional types that explain exceptions to ctet-rule sp 2 d / sp 3 d 2 / sp 3 d 2 1
2 - Definition -Model The mixing of atomic to form special for bonding Quantumchemie: het is mogelijk oplossingen te vinden van de Schrodinger vergelijking die aangeven dat in plaats van s en p atomic er gemixte bestaan rond een atoom die onderling gelijkwaardig zijn Voorbeelden: sp 3, sp 2, sp 1. Per atoom kunnen atomic s, p (en evt. d) samen verschillende gehybridiseerde orbitalen vormen 2. Deze kunnen vervolgens een binding aangaan met een ander atoom 1. Met een s of p orbitaal 2. Met eveneens een gehybridiseerd orbitaal 3. Dit leidt tot eenσ- of π-binding 3. Elk individueel atoom reageert zo, dat de laagste toestand voor het kan worden bereikt Hybridized - uitwerking sp 3 hybridisatie whenever a set of 4 equivalent tetrahedral atomic is required by an atom in a molecule, this model assumes that the atom adopts a set of sp 3 sp 2 analogous: whenever 3 equivalent, triagonale bindingshoeken 120 o sp analogous: whenever 2 equivalent,.. Straight, bindingshoeken 180 o NTABENE: als de Lewisstructuur een vrij electronenpaar aangeeft bij een atoom, dan telt dat als een binding. Hybridized uitwerking 2 sp 2 : in dit geval onstaan er 3 gelijkwaardige orbitalen voor bindingen of vrije electronenparen in die richtingen 1 vrij p-orbital, (oorspronkelijk atomic orbital) in vlak loodrecht op de driehoek sp: - 2 gelijkwaardige orbitalen 2 vrije p-orbitalen loodrecht op de as van de sp orbitalen en loodrecht op elkaar (p y en p z Hybridisation vorming van binding Hybridized - Voorbeelden Twee typen bindings-orbitaal: er worden σ-bond orbital en/of π-bond orbitalen gevormd Altijd één sigma (σ) binding welke langs de internucleaire as ligt. Combinatie van (, sp, sp2, sp3) met (, sp, sp2, sp3); Combinatie van ( met ) 0, 1 of 2 pi (π ) bond orbital Deze ligt in de ruimte boven en onder de internucleaire as Bestaat altijd uit een combinatie van twee niet-gehybridiseerde atomic p orbitalen (p y en p z ) Bonding around C-atom: all four sp 3 maybe used for σ-bonding (CH 4 ) or combination of sp 2 and π-bonding of (double bond) (C 2 H 4 ) or combination of sp and 2 π-bonds of (triple bond) (C 2 H 2,C 2 ) 2
3 Hybridized - voorbeelden The Localized Electron Model Bonding around -atom: sp 3 : two for σ-bonding, 2 free electron pairs example: CH 3 H one for σ-bonding, 3 free electron pairs, example: H 3 C - ; sp 2 : one double bond (σ- ) and π-bonding of orbital; 2 free electron pairs; example: C 2 (double bond), formaldehyde H 2 C sp: one for σ-bonding and 2 π-bonds of (triple bond); example: C Procedure to draw the Loc. Electron Model 1. Draw the Lewis structure(s) ( ) 2. Determine the arrangement of electron pairs (VSEPR model;) VSEPR: valence shell electron-pair repulsion model, Specify the necessary hybrid (9.1) Name Example rbitals for σ-bonding Free p- π-bonding sp 3 methaan 4 0 sp 2 etheen 3 1 sp ethyn 2 2 sp 2 d / sp 3 d / sp 3 d 2?? hybr. type hybr. type C for C: for : BF - 4 for B: for F: XeF 2 for Xe: for F: S 2 for S: for : 1. Draw Lewis-structure 2. Determine electron pair arrangement (VSEPR) 3. Determine hybridisation required per atom - procedure 1. Draw Lewis-structure: (p. 377 Zumdahl) sum all valence electrons; divide them so that all atoms to achieve NGEC (Noble Gas Electronic Configuration; I.e. 8 electron pairs (ctet rule) all atoms net zero formal charge or charge as low as possible; net sum of electrons (lone pairs + half bonding pairs) = valence of atom 2. Determine electron pair arrangement (VSEPR) spatial arrangement to minimize electron pair repulsions (8.13; p. 390 Zumdahl) - procedure (2) 3. Determine hybridisation required per atom From step 1: locations of double/triple bonds From step 2: spatial arrangement (NB step can be skipped first, and checked later on) Per atom: derive from step 1 the number N of free p- to accommodate all double/triple bonds; sp x ; and x = 3-N; N>2: d orbital involved! Per atom: check whether spatial arrangement of hybrid fits with result step 2. 3
4 - result C for C: sp for : sp BF - 4 for B: sp 3 for F: sp 3 XeF 2 for Xe: dsp 3 for F: sp 3 S 2 for S: sp 2 for : sp 2 Prediction of shape of molecule Consider the allene molecule H 2 C=C=CH 2 A) Are all four hydrogen atoms in the same plane? B) If not, what is their spatial relationship; Explain orbital theorie Gelokaliseerde electronmodellen Ionbinding Lewisstructuren VSEPR Valence Bond model Hybridisatie Gedelokaliseerde electronmodellen M theorie orbital theorie ( ) bindingsvolgorde binding diatomic molecules binding heteronucleaire moleculen Combinatie LE en M theorie (9.5) M theory: rbitals M theory Yet another model? Basic assumptions M energy diagram - H 2 - He 2 - Li 2 - B 2 - verview Combination M-VB Model: Electrons shared between two atoms can be thought to be in a rbital that is predicted by the Schrodinger Equation. Assumption: Analogous to atomic, molecules will strive to reach minimum energy configuration Consequence: existing M s will be filled from lowest energy onwards. 4
5 M theory - assumptions (cont d) In order to participate in M s, atomic must overlap in space. Therefore, only valence of atoms contribute significantly to Ms. M - Another model M offers quantum-chemically correct explanation of structure of molecules that were previously described as exhibiting resonance structures M is new theory that explains and supports the model simplification of the resonance structure theory In addition, offers explanation why complex reaction mechanisms occur Example: atmospheric ZNE chemistry! M - Again, natural systems evolve to state of minimum energy M - (1) H 2 M theory predicts that atomic (A) recombine to yield: M s with lower energy than A s: Bonding rbitals M s with higher energy than A s: Anti-Bonding rbitals σ * σ H H 2 H M - (2) He 2 Bond rder (B) He σ * σ He 2 He M helps to predict which molecules are stable, and which are not; indicator: B Difference between the number of electrons in bonding M s and number of electrons in anti-bonding M s divided by two. B is indication of relative stability of a molecular bond, and hence of a molecule 5
6 M - (3) Li 2 Be 2 M energy levels: B 2 σ * σ * s-p orbital mixing verzicht: p.436 σ x * π y * π z * σ x π y π z σ σ Li Li 2 Li What is B of both these molecules Which one is likely to be stable? Be Be 2 Be B σ * σ B 2 B M - energy levels Shift for B 2 C 2 N 2 N 2 σ x * π y * π z * σ x π y π z M - energy levels No shift for 2 F 2 2 σ x * π y * π z * π y π z σ x σ * σ * N σ N 2 N σ 2 M - energy levels N σ x * Magnetism Use for diatomic molecules adjacent in Per. Syst. N CN etc. π y * π z * σ x π y π z σ * Paramagnetism unpaired electrons attracted to induced magnetic field Diamagnetism paired electrons repelled from induced magnetic field σ 2 6
7 utcomes of M Model M theorie 1 As bond order increases, bond energy increases and bond length decreases. 2 N 2 has a triple bond, and a correspondingly high bond energy. 3 2 is paramagnetic. This is predicted by the M model, not by the Lewis model, which predicts diamagnetism. M diagram H 2 - He 2 Li 2 B 2 verzicht Combinatie M-VB Combining LE and M Models σ bonds can be described as being localized. π bonding must be treated as being delocalized. 7
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