Among the metal carbonyls [Mn(CO)6]
+, [Ti(CO)6], [Cr(CO)6] and [V(CO)6]
−, the C-O bond
order would be lowest in
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Ti(CO)6...as. .The Ti− complex, involving the only d5 metal in a host of d6 metals, is actually the one with thesmallest bond order because it has the leastnumber of electrons in the t2g orbitals, which are always nonbonding if σ donation is present but πacceptance is not, and may be at least a bit bonding when π acceptance is additionallypresent.
The less electrons present in the t2g bondingorbitals, the less bonding character, and thus theweaker the metal-ligand interactions are.
Additionally, because it is the transition metal out of these four that has the largest ionic radius (yet uses the same set of d orbitals), its metal-ligand distance is largest, and that weakens the metal-ligand interactions a bit more.
The less electrons present in the t2g bondingorbitals, the less bonding character, and thus theweaker the metal-ligand interactions are.
Additionally, because it is the transition metal out of these four that has the largest ionic radius (yet uses the same set of d orbitals), its metal-ligand distance is largest, and that weakens the metal-ligand interactions a bit more.
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