<h3 id="successcoordination-compoundssuccess"><Success>Coordination Compounds</Success></h3> <h3 id="successlecture-4success"><Success>Lecture-4</Success></h3> <div style='float: left; width:99%;text-align:left;font-size:30px'> </div> <div style='float: right; width:50%;'> <!----> </div>

<h3 id="successequilibriasuccess"><Success>Equilibria</Success></h3> <div style='float: left; width:100%; font-size:30px; text-align:left'> <ul> <li>Need to know the $K_f$ whether it is energetically favored to the right</li> <li>A large $K_f$ would mean that coordination by en is favored over $NH_3$</li> <li>${[Ni(NH_3)_6]^{2+}+3en \rarr [Ni(en)_3]^{2+}+6NH_3}$</li> <li>$K_f=\frac{[Ni(en)_3][NH_3]^6}{[Ni(NH_3)_6][en]^3}$</li> <li>One ligand is replaced by another</li> </ul> </div> <div style='float: right; width:0%;'> <!----> <!----> <!--<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/cd3d2bdf-d735-43b8-0bad-f68e42c07600/public" style='width:70%'>--> </div>

### <Success>Equilibria</Success> <div style='float: left; width:50%; font-size:30px; text-align:left'> </div> <div style='float: center; width:100%;'> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/cd3d2bdf-d735-43b8-0bad-f68e42c07600/public" style='width:70%'> </div>

<h3 id="successvalence-bond-theorysuccess"><Success>Valence bond theory</Success></h3> <div style='float: left; width:100%;text-align:left;font-size:30px;'> <ul> <li>Valence bond theory considers that the overlapping atomic orbitals of the participating atoms form a chemical bond</li> <li>In terms of valence bond theory, the filled orbital of the ligand overlaps with an empty orbital of the metal ion</li> <li>The VB model proposes that the geometry of the complex ion depends on the hybridization of the metal ion</li> </ul> </div> <div style='float: right; width:0%;'> <!--<img src = 'https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/24aab050-772e-49a3-36fb-ba5e92d46e00/public' width='80%'>--> <!----> </div>

<h3 id="successvalence-bond-theorysuccess-1"><Success>Valence bond theory</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> <ul> <li>The atomic orbitals for bonding may be hybrids. Often, the bonding atomic orbitals have a character of several possible types of orbitals. The methods to get an atomic orbital with the proper character for the bonding is called hybridization</li> </ul> </div> <div style='float: right; width:50%;'> <img src = 'https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/24aab050-772e-49a3-36fb-ba5e92d46e00/public' width='80%'> <!----> </div>

<h3 id="successisomerism-in-coordination-compoundssuccess"><Success>Isomerism in coordination compounds</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> <p><strong>Tetrahedral Geometry:</strong> $[CoCl_4]^{2-}$ three unpaired electrons, which makes it paramagnetic and attracted by magnets</p> <ul> <li>$Co^{2+}$ is $sp^3$ hybridized in tetrahedral $CoCl^{2-}_4$ complex ion</li> <li>$Ni^{2+}$ is $dsp^2$ hybridized in the square planar $Na(CN)^{2+}_4$ complex ion</li> <li>$Ag^+$ is sp hybridized in the linear $Ag(NH_3)^+_2$ ion</li> </ul> </div> <div style='float: right; width:50%;'> <!----> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/82f01a06-1e8c-4dea-9bfc-5addc462d300/public" style='width:100%'> </div>

<h3 id="successtetrahedral-geometrysuccess"><Success>Tetrahedral geometry</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> </div> <div style='float: center; width:100%;'> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/aff2ec11-a2ec-43cc-97f7-13af24f03c00/public" style='width:100%'> </div> <div style='float: right; width:50%;'> <!--<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/82f01a06-1e8c-4dea-9bfc-5addc462d300/public" style='width:100%'>--> </div>

<h3 id="successbonding-in-coordination-compoundssuccess"><Success>Bonding in coordination compounds</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> <ul> <li>Hybrid orbitals and bonding in the tetrahedral $[Zn(OH)_4]^{2+}$ ion</li> </ul> </div> <div style='float: right; width:50%;'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/78594866-51b1-4fb7-c9c8-40522c4d0800/public" style='width:100%'> </div>

<h3 id="successbonding-in-coordination-compoundssuccess-1"><Success>Bonding in coordination compounds</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> <ul> <li>Hybrid orbitals and bonding in the square planar $[Ni(CN)_4]^{2+}]$ ion</li> </ul> </div> <div style='float: right; width:50%;'> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/0da5eda9-ed53-4022-938e-00563e01ce00/public" style='width:70%'> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/61360293-44dc-44f8-8648-ff2d9ffa4300/public" style='width:70%'> </div>

<h3 id="successbonding-in-coordination-compoundssuccess-2"><Success>Bonding in coordination compounds</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px'> <ul> <li>The hybrid orbitals in the octahedral $[Cr(NH_3)_6]^{3+}$ ion.</li> </ul> </div> <div style='float: right; width:50%;'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/48af9038-298f-4a92-5a3f-f41ac5a63e00/public" style='width:100%'> </div>

<h3 id="successmagnetic-propertiessuccess"><Success>Magnetic properties</Success></h3> <div style='float: left; width:99%;text-align:left;font-size:30px;'> <ul> <li>Magnetic moment of coordination compounds can be measured by the magnetic susceptibility experiments</li> <li>$[Fe(CN)_6]^{3-}$ has magnetic moment of a single unpaired electron while $[FeF_6]^{3-}$ has a paramagnetic moment of five unpaired electrons</li> </ul> </div> <div style='float: right; width:0%;'> <p><img alt="image" src="https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-12-unit-09-chapter-04-coordination-compounds-l-4_5-strjq9hp15o-11.jpg"></p> </div>

<h3 id="successhybridizationsuccess"><Success>Hybridization</Success></h3> <div style='float: left; width:0%;text-align:left;font-size:30px'> </div> <div style='float: center; width:100%;'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/f04a7027-763e-422f-d898-17899d7d6c00/public" style='width:70%'> </div>

<h3 id="successdeficiencies-of-vb-approach12success"><Success>Deficiencies of VB approach(1/2)</Success></h3> <div style='float: left; width:99%;text-align:left;font-size:30px;'> <ul> <li>Assumes that all d orbitals in a complex are equal in energy</li> <li>The arbitrary use of 3d and 4d orbitals for bonding, energy differential is often ignored</li> <li>The theory is unable to adequately explain electronic and magnetic properties of complexes</li> <li>VBT is widely used in organic and main group element chemistry</li> <li>In transition metal chemistry VBT is superseded by the Crystal Field Theory (CFT)</li> <li>In combination with MOT it is often referred to as the Ligand Field Theory (LFT)</li> </ul> </div> <div style='float: right; width:0%;'> <p><img alt="image" src="https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-12-unit-09-chapter-04-coordination-compounds-l-4_5-strjq9hp15o-13.jpg"></p> </div>

<h3 id="successdeficiencies-of-vb-approach22success"><Success>Deficiencies of VB approach(2/2)</Success></h3> <div style='float: left; width:99%;text-align:left;font-size:30px;'> <ol> <li>Do not provide quantitative interpretation of magnetic data</li> <li>Can not explain the color of the compounds</li> <li>Unable to give a quantitative interpretation of the thermodynamic or kinetic stabilities</li> <li>Exact predictions are not possible for tetrahedral and square planar complexes</li> <li>Can not distinguish between weak and strong ligands</li> </ol> </div> <div style='float: right; width:0%;'> <p><img alt="image" src="https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-12-unit-09-chapter-04-coordination-compounds-l-4_5-strjq9hp15o-14.jpg"></p> </div>

<h3 id="successoctachedral-fieldsuccess"><Success>Octachedral field</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> <h4 id="d-orbitalslook-attentively-along-the-axis">d-orbitals:look attentively along the axis</h4> <ul> <li>Linear combination of $d_z^2-d_x^2$ and $d_z^2-d_y^2$</li> <li>$d_{2z^{2-}x^{2-}y^2}$</li> </ul> <h4 id="in-octachedral-field">In Octachedral Field</h4> </div> <div style='float: right; width:50%;'> <!----> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/b6c8e8b1-7b19-4e70-9707-a8cb316ac300/public" style='width:70%'> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/23598eaa-a752-48e3-0c5b-9a91f33ac200/public" style='width:70%'> </div>

<h3 id="successcrystal-field-theorysuccess"><Success>Crystal field theory</Success></h3> <div style='float: left; width:0%;text-align:left;font-size:30px;'> </div> <div style='float: center; width:100%;'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/7b676c24-037c-4848-37bc-900e6c000400/public" style='width:100%'> </div>

<h3 id="successcrystal-field-splittingsuccess"><Success>Crystal field splitting</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> <ul> <li>$d_{z^2}$ and $d_{x^2-y^2}$ orbitals point at the ligands and have higher energies than other d-electrons</li> <li>This energy gap $(\Delta)$ is called crystal field splitting</li> </ul> </div> <div style='float: right; width:50%;'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/0ca7335b-dbfc-461d-4bc9-e49da353b000/public" style='width:100%'> </div>

<h3 id="successabsorptionsuccess"><Success>Absorption</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px;'> <ul> <li>Absorption spectra of different complexes indicate the crystal field splitting energy depends on the ligand’s nature</li> <li>For $Ni^{2+}$ complexes $\Delta$ increases as the ligand changes from $H_2O$ to $NH_3$ to ethylenediamine (en)</li> </ul> </div> <div style='float: right; width:50%;'> <!----> <img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/3c74c9ab-471a-4f97-21ab-87068341fa00/public" style='width:100%'> </div>

<h2 id="successthank-yousuccess"><Success>Thank you</Success></h2> <div style='float: left; width:99%;text-align:left;font-size:30px'> </div> <div style='float: right; width:0%;'> <p><img alt="image" src="https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-12-unit-09-chapter-04-coordination-compounds-l-4_5-strjq9hp15o-258-3585.6.jpg"></p> </div>