Coordination Chemistry IV Reactions and Mechanisms PDF

Chapter 12 Coordination Chemistry IV Reactions and Mechanisms  Coordination Compound Reactions Goal is to understand reaction mechanisms Primarily substitution reactions, most are rapid Cu(H2O)62+ + 4 NH3  [Cu(NH3)4(H2O)2]2+ + 4 H2O but some are slow [Co(NH3)6]3+ + 6 H...

Chapter 12 Coordination Chemistry IV Reactions and Mechanisms  Coordination Compound Reactions Goal is to understand reaction mechanisms Primarily substitution reactions, most are rapid Cu(H2O)62+ + 4 NH3  [Cu(NH3)4(H2O)2]2+ + 4 H2O but some are slow [Co(NH3)6]3+ + 6 H3O+  [Co(H2O)6]3+ + 6 NH4+  Coordination Compound Reactions Labile compounds - rapid ligand exchange (reaction half-life of 1 min or less) Inert compounds - slower reactions Labile/inert labels do not imply stability/instability (inert compounds can be thermodynamically unstable) - these are kinetic effects In general: – Inert: octahedral d3, low spin d4 - d6, strong field d8 square planar – Intermediate: weak field d8 – Labile: d1, d2, high spin d4 - d6, d7, d9, d10  Substitution Mechanisms Two extremes: Dissociative (D, low coordination number intermediate) Associative (A, high coordination number intermediate) SN1 or SN2 at the extreme limit Interchange - incoming ligand participates in the reaction, but no detectable intermediate – Can have associative (Ia) or dissociative (Id) characteristics Reactions typically run under conditions of excess incoming ligand We’ll look briefly at rate laws (details in text), consider primarily octahedral complexes Substitution Mechanisms  Substitution Mechanisms Pictures: Substitution Mechanisms  Determining mechanisms What things would you do to determine the mechanism?  Dissociation (D) ML X  ML + X Mechanism 5 5 k1, k-1 ML5 + Y  ML5Y k2 1st step is ligand dissociation. Steady-state hypothesis assumes small [ML5], intermediate is consumed as fast as it is formed d[ML5 Y] k2 k1[ML5 X][Y] = dt kĞ1[X] + k2 [Y] Rate law suggests intermediate must be observable - no examples known where it can be detected and measured Thus, dissociation mechanisms are rare - reactions are more likely to follow an interchange-dissociative mechanism  Interchange Mechanism ML5X + Y  ML5X.Y k1, k–1 ML5X.Y  ML5Y + X k2 RDS 1st reaction is a rapid equilibrium between ligand and complex to form ion pair or loosely bonded complex (not a high coordination number). The second step is slow. d[ML5 Y] k2 K1[M]0 [Y]0 k2 K1[M]0 [Y]0 =  dt 1 + K1[Y]0 + (k2 /kĞ1 ) 1 + K1[Y]0 Reactions typically run under conditions where [Y] >> [ML5X]  Interchange Mechanism Reactions typically run under conditions where [Y] >> [ML5X] [M]0 = [ML5X] + [ML5X.Y] [Y]0  [Y] Both D and I have similar rate laws: If [Y] is small, both mechanisms are 2nd order (rate of D is inversely related to [X]) If [Y] is large, both are 1st order in [M]0, 0-order in d[ML5 Y] k2 K1[M]0 [Y]0 k2 K1[M]0 [Y]0 [Y] =  dt 1 + K1[Y]0 + (k2 /kĞ1 ) 1 + K1[Y]0 d[ML5 Y] k k [ML5 X][Y] = 2 1 dt kĞ1[X] + k2 [Y]  Interchange Mechanism D and I mechanisms have similar rate laws: Dissociation Interchange ML5X  ML5 + X k1, k-1 ML5X + Y  ML5X.Y k1, k–1 ML5 + Y  ML5Y k2 ML5X.Y  ML5Y + X k2 RDS If [Y] is small, both mechanisms are 2nd order (and rate of D mechanism is inversely related to [X]) If [Y] is large, both are 1st order in [M]0, 0-order in [Y]  Association (A) Mechanism ML5X + Y  ML5XY k1, k-1 ML5XY  ML5Y + X k2 1st reaction results in an increased coordination number. 2nd reaction is faster d[ML5 Y] k1k2 [ML5 X][Y] =  k[ML5 X][Y] dt kĞ1 + k2 Rate law is always 2nd order, regardless of [Y] Very few examples known with detectable intermediate  Factors affecting rate Most octahedral reactions have dissociative character, square pyramid intermediate Oxidation state of the metal: High oxidation state results in slow ligand exchange [Na(H2O)6]+ > [Mg(H2O)6]2+ > [Al(H2O)6]3+ Metal Ionic radius: Small ionic radius results in slow ligand exchange (for hard metal ions) [Sr(H2O)6]2+ > [Ca(H2O)6]2+ > [Mg(H2O)6]2+ For transition metals, Rates decrease down a group Fe2+ > Ru2+ > Os2+ due to stronger M-L bonding Dissociation Mechanism Evidence: Stabilization Energy and rate of H2O exchange Entering Group Effects Small incoming ligand effect = D or Id mechanism Entering Group Effects Not close = Ia mechanism Close = Id mechanism Activation Parameters RuII vs. RuIII substitution  Conjugate Base Mechanism onjugate base mechanism: complexes with NH3-like or H2O ligands ose H+, ligand trans to deprotonated ligand is more likely to be ost. [Co(NH3)5X]2+ + OH- ↔ [Co(NH3)4(NH2)X]+ + H2O (equil) [Co(NH3)4(NH2)X]+  [Co(NH3)4(NH2)]2+ + X- (slow) [Co(NH3)4(NH2)]2+ + H2O  [Co(NH3)5H2O]2+ (fast) Conjugate Base Mechanism Conjugate base mechanism: complexes with NR3 or H2O ligands, lose H+, ligand trans to deprotonated ligand is more likely to be lost. Reaction Modeling using Excel Programming  Square planar reactions Associative or Ia mechanisms, square pyramid intermediate Pt2+ is a soft acid. For the substitution reaction trans-PtL2Cl2 + Y → trans-PtL2ClY + Cl– in CH3OH ligand will affect reaction rate: PR3>CN–>SCN–>I–>Br–>N3–>NO2–>py>NH3~Cl–>CH3OH Leaving group (X) also has effect on rate: hard ligands are lost easily (NO3–, Cl–) soft ligands with  electron density are not (CN–, NO2–)  Trans effect In square planar Pt(II) compounds, ligands trans to Cl are more easily replaced than others such as ammonia Cl has a stronger trans effect than ammonia (but Cl– is a more labile ligand than NH3) CN– ~ CO > PH3 > NO2– > I– > Br– > Cl– > NH3 > OH– > H2O Pt(NH3)42+ + 2 Cl–  PtCl42– + 2 NH3 Sigma bonding - if Pt-T is strong, Pt-X is weaker (ligands share metal d-orbitals in sigma bonds) Pi bonding - strong pi-acceptor ligands weaken P-X bond Predictions not exact Trans Effect: Trans Effect: First steps random loss of py or NH3 Trans Effect:  Electron Transfer Reactions Inner vs. Outer Sphere Electron Transfer Outer Sphere Electron Transfer Reactions Rates Vary Greatly Despite Same Mechanism Nature of Outer Sphere Activation Barrier  Inner Sphere Electron Transfer Co(NH3)5Cl2+ + Cr(H2O)62+  (NH3)5Co-Cl-Cr(H2O)54+ + H2O Co(III) Cr(II) Co(III) Cr(II) (NH3)5Co-Cl-Cr(H2O)54+ (NH3)5Co-Cl-Cr(H2O)54+ Co(III) Cr(II) Co(II) Cr(III) H2O + (NH3)5Co-Cl-Cr(H2O)54+ (NH3)5Co(H2O)2+ + (Cl)Cr(H2O)52+  Inner Sphere Electron Transfer Co(NH3)5Cl2+ + Cr(H2O)62+  (NH3)5Co-Cl-Cr(H2O)54+ + H2O Co(III) Cr(II) Co(III) Cr(II) (NH3)5Co-Cl-Cr(H2O)54+ (NH3)5Co-Cl-Cr(H2O)54+ Co(III) Cr(II) Co(II) Cr(III) H2O + (NH3)5Co-Cl-Cr(H2O)5  (NH3)5Co(H2O)2+ + (Cl)Cr(H2O)52+ 4+ Nature of Activation Energy: Key Evidence for Inner Sphere Mechanism:  Example [CoII(CN)5]3- + CoIII(NH3)5X2+  Products Those with bridging ligands give product [Co(CN)5X]2+.