Carbon monoxide substitution in the metal radical V(CO)6 proceeds at or below room temperature to form monosubstitution products V(CO)5L (L=phosphine or phosphite). The substitution occurs solely by a second-order process according to a rate law that is first order in both V(CO)6 and phosphorus nucleophile. The rate of reaction is strongly dependent on the basicity and size of the ligand. Activation parameters further support the associative nature of the reaction: P(n-Bu)3, △H*=7.6 4±0.4 kcal/mol, △S*=-25.2±1.7cal/mol.deg; P(OMe)3, △H*=10.9±0.2kcal/mol, △S*=-22.6±0.8cal/mol.deg; PPh3, △H*=10.0±0.4kcal/mol, △S*=-27.8±1.6cal/mol.deg. The rate of substitution of V(CO)6 by PPh3 is unchanged under 1 atm of carbon monoxide or in the presence of [V(CO)6]-. The carbon monoxide substitution reactions of V(CO)sL with additional L also proceed by an associative mechanism with the rate of substitution approximately three orders of magnitude slower than for V(CO)6. The disubstituted product adopts the cis stereochemistry with small phosphorus donor ligands or with chelating phosphines. For L=P(OMe)3, activation parameters were determined: △H*=13.2±0.4kcal/mol, △S*=-27.6±1.8 cal/mol.deg. Phosphine exchange reactions of V(CO)sL were also observed indicating that, in addition to carbon monoxide, phosphine ligands on vanadium are substitution labile. Nucleophilic attack of P(n-Bu)3 at V(CO)5[P(n-Bu)3] is l05 times slower than that at V(CO)6, presumably because the increased electron density on the metal hinders nucleophilic attack. Quantitative comparisons between the 17-electron complex V(CO)6 and its 18-electron analogue Cr(CO)6 indicate that associative carbon monoxide substitution takes place 1010 times faster in the vanadium system.

Detailed kinetic data are reported for the reactions of M(CO)6 (where M=Cr, Mo, and W) with Me3NO, in the absence and in the presence of triphenylphosphine (PPha). The rates of reaction are first-order in concentrations of M(CO)6 and of Me3NO but zero-order in PPh8 concentration. The rates of reaction decrease in the order W>Mo>Cr. A mechanism is proposed which involves attack on a carbonyl carbon with the formation of coordinatively unsaturated intermediates of the type M(CO)5, which then rapidly react with an entering ligand. Compared with other nucleophiles reported to react by carbonyl attach in M(CO)6 substrates, Me3NO is a strong nucleophile. Qualitatively, the nucleophilic strengths decrease in the order MeLi>Me3NO>PhCH2MgBr>>N3->NCO->NCS->C1->Br->I-.

Reported are the rates of reaction and activation parameters for CO substitution reactions of M3(CO)12 (M=Fe, Ru, Os) with L (L = PPh3, P(OPh)3, AsPh3) in the presence of (CH3)3NO. In aprotic solvents the reactions are too fast to follow by conventional spectroscopy, but the rates decrease with added protonic solvents. Reactions are readily monitored at room temperature in the mixed solvent CHC13-C2H5OH (v/v, 2:1), and the rates of reaction are inversely proportional to the concentration of C2H5OH. It is suggested that this is due to hydrogen bonding to give (CH3)3NO…HOC2H5, which is unreactive compared with the very reactive free (CH3)3NO at these reaction conditions. The rates of formation of M3(CO)llL are first-order in concentrations of metal cluster and of (CH3)3NO but zero-order in concentration of L. This suggests a mechanism that involves a nucleophilic attack of the O atom of (CH3)3NO on the C atom of a CO, accompanied by oxidation of CO to CO2. Since CO2 is a good leaving group, its departure from the metal clusters affords the active intermediates M3(CO)II. These then rapidly react with entering ligands to form the monosubstituted products M3(CO)11. The rates of reaction decrease in the order F3(CO)12>Ru3(CO)12>Os3(CO)12, and an attempt is made to account for the observed relative rates.

Reported are rates of reaction and activation parameters for CO substitution by PPh3 of M(CO)5 (M=Fe, Ru, Os) in the presence of (CH3)3NO. The reactions follow a second-order rate law, being first-order in concentrations of M(CO)5 and of (CH3)3NO but zero-order in PPh3 concentration. The reaction rates show an approximate overall fourfold increase in the order Fe<Ru<Os. This contrasts the roughly 40-fold decrease in rate in the order Fe>Ru> Os for M3(CO)12. An attempt is made to account for the relative reaction rates of the M(CO)5 compounds and for why the order differs from that of the corresponding metal carbonyl clusters.

The complex V(CO)5(NO) undergoes substitution of CO at or below 0℃ by L=PMe3, PPh3, P(O-i-Pr)3, P(OMe)3, and NEt3 to yield V(CO)4L(NO). Substitution proceeds according to a two-term rate law: -d[V(CO)5(NO)]/dt=kl[V(CO)5(NO)]+k2[V(CO)5(NO)] [L]. For the extremely weak NEt3 nucleophile, the substitution reaction occurs only via the k1 path. Substitution of a second CO ligand to afford V(CO)3(PMe3)2(NO) proceeds solely by a dissociative pathway and is 106 times slower than loss of CO from V(CO)5(NO) at 25℃. The thermal instability of V(CO)5(NO) results from facile CO dissociation at room temperature, which occurs faster than in any other first-row-metal carbonyl or carbonyl nitrosyl. This remarkable reactivity of V(CO)5(NO) may be attributed to a trans effect from the NO ligand. Ground-state SCF-Xa-DV calculations have been performed for V(CO)5(NO) and compared with those for V(CO)6. In V(CO)5(NO), the fully occupied r-bonding t2s orbitals split into b2(dxy) and e(dxz,yz) orbitals. The e level, which can π-bond to NO, is preferentially stabilized, and the NO π-orbital contribution is 4-5 times that of the axial CO ligand. This superior 7r-acceptor character of NO also leads to the purple color of V(CO)5(NO). One-electron transitions from the b2(dxy) and e(dxz,yz) levels into a low-lying empty NO π* orbital are calculated at 2.29 and 2.52 eV and observed experimentally at 2.23 and 3.14 eV, respectively.