Metal-ligand bond dissociation energies in CpMn(CO)2L complexes

A Comparative Study of Tricarbonylmanganese Photoactivatable CO Releasing Molecules (PhotoCORMs) by Using the Myoglobin Assay and Time‐Resolved IR Spectroscopy

“…This might explain why we just see one new band since the second one should then be obscured by the E band of the tricarbonyl complex. As such, dicarbonyl complexes are also photolabile, they are only transient species, which might explain the low intensity of the band at 1840–1860 cm –1 21. In the cases of [Mn(CO) 3 (tpm)]OTf ( 1 ) and [Mn(CO) 3 (tpp)]OTf ( 5 ), the highest intensities of the newly formed band can be observed.…”

“…Relevant sections of the IR spectra taken after 0, 3 and 6 min of irradiation are shown in Figure 3. [21] In the cases of [Mn(CO) 3 (tpm)]OTf (1) For compounds [Mn(CO) 3 (2-tip NMe )]OTf (3) and [Mn(CO) 3 (tpp)]OTf (6), we also followed the change of the band intensities in the carbonyl region with variation of the excitation wavelength. In any case, after prolonged irradiation (ca.…”

Organometallic photochemistry at the end of its first century

“…For example, the energy necessary to break a typical metal-carbonyl bond is ca. 190-210 kJ/mol [97], while 400 nm light corresponds to ca. 300 kJ/mole.…”

Ultrafast Infrared Studies of Bond Activation in Organometallic Complexes

“…Typically, the energy required to break a transition-metal-CO bond is about 45-50 kcal/mol. 40 The energy carried by a 295 or 325 nm laser beam is equivalent to 97 or 88 kcal/mol, respectively. With these numbers in mind, the nascent metal dicarbonyl resulting from the loss of a CO ligand would have to deposit to its environment at least ∼40 kcal/ mol of energy before forming an observable intermediate.…”