The complex ion Ru(phen) ^2+ has been used as a probe for...

The complex ion Ru(phen) ${ }^{2+}$ has been used as a probe for the structure of DNA. (Phen is a bidentate ligand.) a. What type of isomerism is found in $\mathrm{Ru}(\mathrm{phen})_{3}^{2+} ?$ b. Ru(phen) $_{3}^{2+}$ is diamagnetic (as are all complex ions of $\mathrm{Ru}^{2+}$ ). Draw the crystal field diagram for the $d$ orbitals in this complex ion.

The complex ion Ru(phen) ${ }^{2+}$ has been used as a probe for the structure of DNA. (Phen is a bidentate ligand.)
a. What type of isomerism is found in $\mathrm{Ru}(\mathrm{phen})_{3}^{2+} ?$
b. Ru(phen) $_{3}^{2+}$ is diamagnetic (as are all complex ions of $\mathrm{Ru}^{2+}$ ). Draw the crystal field diagram for the $d$ orbitals in this complex ion.

Key Concepts

Strong Field Ligands and Diamagnetism in d6 Complexes

When a d6 metal ion, such as Ru2+, is coordinated by strong field ligands, the crystal field splitting is significant enough to force the pairing of electrons in the lower energy t2g orbitals. This electron pairing leads to a diamagnetic complex, meaning all electrons are paired, and there is no net magnetic moment. This concept is essential for understanding the electronic configuration and magnetic behavior of many octahedral complexes in transition metal chemistry.

Optical Isomerism in Coordination Complexes

In coordination chemistry, optical isomerism occurs when a complex can exist as non-superimposable mirror images, known as enantiomers. For octahedral complexes with three bidentate ligands, such as tris?chelates, the spatial arrangement of the ligands results in distinct ? (delta) and ? (lambda) forms, which are key examples of optical isomers. This type of isomerism is important for understanding how molecular chirality can arise in metal complexes and its effects on interactions with chiral environments, including biological systems like DNA.

Crystal Field Theory in Octahedral Complexes

Crystal field theory describes the splitting of the metal ion d orbitals in the presence of ligands arranged in a specific geometry. In an octahedral complex, the five d orbitals split into two sets: the lower energy t2g (dxy, dxz, dyz) orbitals and the higher energy eg (dx2?y2, dz2) orbitals. This splitting is fundamental to predicting the electronic structure, magnetic properties, and color of the complex, and is crucial for analyzing complexes that employ strong field bidentate ligands.

Transcript

00:03 So here the question is the complex ion, i .u.

00:08 Phe .n.

00:09 Tries 2 plus has been used as a prop for the structure of dna.

00:17 That is phan is actually a bidentid ligand.

00:23 So this we have to remember my answer that it is bidental ligand.

00:29 And what type of isomarism is found in this first part is and the second is this complex is diamagnetic as all complex ions of rutanium 2 plus draw the crystal field diagram for the d orbitals in the complex ion so for giving the first answer that is a what type of isomorism is present in the complex.

01:09 Now if it is biidently ligand, we are supposed to know the structure first and then only we can write the isomelism present in it.

01:22 So, ruthenium should be at the center with plus two configuration and it should be octahedral geometry.

01:37 So in the octahedral geometry we have to remember that four bonds are in one plane and one is above the plane and other should be below the plane.

01:57 So here one biotented ligand is present that is 110 phenythroline and this compounds this one we can write in short form that this nitrogen is the element which is forming the coordinate bond with the central atom, metal atom and this is biotented ligand.

02:29 So in short we can write this is p -h -e -n.

02:37 This is one structure.

02:39 Second one is this nitrogen and this nitrogen and another molecule that is p -h -e -n.

02:49 So this is another part and here again this is attestin nitrogen.

02:56 And both are joined together by p -hem.

03:03 So these are the three bidentate ligands which are forming the octahedral complex.

03:14 Now this complex, if it is octahedral complex, these four bonds should be in the same plane and one is above the plane and other should be below the brain and this we have to imagine...

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