2d. State, with justification, whether you expect nitric oxide (NO) to be a stronger or weaker pi-acceptor ligand than CO? The ability of ligands to accept л-electron density from the metal into their low-lying empty orbitals increase with increase in the electronegativity of their atoms because it decreases the energy of vacant * molecular orbitals and make them more suitable to accept í electron density from metal d orbital. NO is strictly an organometallic ligand and is a radical with 1 valence electrons. When bound, NO is referred to as the nitrosyl ligand and can bond in one of two modes to d-metal atoms, in either a bent or a linear, In the linear, the ligand is considered to be the NO+ cation which is isoelectronic with CO and the bonding can be considered in a similar. In bent, NO is considered to behave as NO- that donate 2 electrons. In the case of NO and CO, NO is a weaker pi-acceptor ligand than CO. Even nitrogen is mor electronegative than carbon, the electronic structure of the ligand's π* orbital is a more significant factor in determining its strength. [5] The T* orbital of NO is partially filled with an unpaired electron, which makes it less efficient in accepting electron density from the metal's d orbitals. On the other hand, the fully empty pi*orbital of CO can strongly overlap with the metal's d orbitals, resulting in a stronger π-back bonding interaction and a stronger metal-ligand bond.

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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2d. State, with justification, whether you expect nitric oxide (NO) to be a stronger or
weaker pi-acceptor ligand than CO?
The ability of ligands to accept л-electron density from the metal into their low-lying empty
orbitals increase with increase in the electronegativity of their atoms because it decreases the
energy of vacant * molecular orbitals and make them more suitable to accept í electron density
from metal d orbital.
NO is strictly an organometallic ligand and is a radical with 1 valence electrons. When bound, NO is
referred to as the nitrosyl ligand and can bond in one of two modes to d-metal atoms, in either a bent
or a linear, In the linear, the ligand is considered to be the NO+ cation which is isoelectronic with CO
and the bonding can be considered in a similar. In bent, NO is considered to behave as NO- that
donate 2 electrons.
In the case of NO and CO, NO is a weaker pi-acceptor ligand than CO. Even nitrogen is mor
electronegative than carbon, the electronic structure of the ligand's π* orbital is a more significant
factor in determining its strength. [5]
The T* orbital of NO is partially filled with an unpaired electron, which makes it less efficient in
accepting electron density from the metal's d orbitals. On the other hand, the fully empty pi*orbital
of CO can strongly overlap with the metal's d orbitals, resulting in a stronger π-back bonding
interaction and a stronger metal-ligand bond.

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what about this answer ? Is this also correct? Isn't it contradict? "

However, the back-donation from the metal center to CO's empty 2π* orbital is less extensive than with NO. This is because CO's 2π* orbital is higher in energy compared to NO's 2π* orbital.

In summary, both NO and CO are pi-acceptor ligands due to their empty 2π* orbitals. However, NO is expected to be a stronger pi-acceptor ligand than CO because of the presence of the unpaired electron in its 2π* orbital and the lower energy of this orbital. The stronger pi-acceptor ability of NO can lead to a more stable metal-ligand bond, as well as greater electron density redistribution between the metal center and the ligand."

I'm so confused NO is weaker or stronger pi-acceptor ligands

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