### <Success>d and f-block elements</Success> ### <Success>Lecture 5</Success> <div style='float: left; width:50%;text-align:left;font-size:30px'> </div> <div style='float: right; width:50%;'> <!---->

<h3 id="successthe-inner-transition-elements-f-blocksuccess"><Success>The Inner Transition Elements (f-block)</Success></h3> <div style='float: left; width:0%;font-size:30px;text-align:left;'> <!--#### F- block--> <!--* Geochemistry > Nature--> <!--* Rare earths--> <!--* 3d--> <!--* 4d $\quad \quad 4f$--> <!--* 5d $\quad \quad 5f$--> </div> <div style='float: right; width:100%;'> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/a69dfcfd-aa33-40c8-c631-37c40b05ca00/public"></p> <!----> <!--.jpg)--> </div>

<h3 id="successthe-inner-transition-elements-f-blocksuccess-1"><Success>The Inner Transition Elements (f-block)</Success></h3> <div style='float: left; width:100%;font-size:30px;text-align:left;'> <ul> <li>It contains of the two series, lanthanoids (the fourteen elements following lanthanum) and actinoids (the fourteen elements following actinium)</li> </ul> <h4 id="electronic-configurations"><strong>Electronic Configurations</strong></h4> <ul> <li>The electronic configurations of all the tripositive ions (the most stable oxidation state of all the lanthanoids) are of the form $4f^n$</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-08-chapter-05-d-and-f-block-elements-l-5_5-2ofsmt6eujy-12(2).jpg"></p> </div>

<h3 id="successthe-inner-transition-elements-f-blocksuccess-2"><Success>The Inner Transition Elements (f-block)</Success></h3> <div style='float: left; width:100%;font-size:30px;text-align:left;'> <h4 id="general-features"><strong>General features</strong></h4> <ul> <li>All the lanthanoids are silvery white soft metals and tarnish rapidly in air. The hardness increases with increasing atomic number, samarium being steel hard. Their melting points range between 1000 to 1200 K but samarium melts at 1623 K.</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-08-chapter-05-d-and-f-block-elements-l-5_5-2ofsmt6eujy-057-0516.0.jpg"></p> </div>

### <Success>The Inner Transition Elements (f-block)</Success> <div style='float: left; width:50%;font-size:30px;text-align:left;'> <ul> <li><strong>Electronic Configuration and radii of Lanthanum and Lanthanoids</strong></li> </ul> </div> <div style='float: right; width:50%;'> <!----> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/5ccfab8a-549e-468b-c1a3-76e506f09000/public"></p> </div>

<h3 id="successthe-inner-transition-elements-f-blocksuccess-3"><Success>The Inner Transition Elements (f-block)</Success></h3> <div style='float: left; width:0%;font-size:30px;text-align:left;'> <!--* 4f & 5f--> <!--* Geochemistry $>$ Nature--> <!--* Rare of earths--> <!--* Atomic <ins>sizes</ins> - 4f$\rightarrow$ Alloying--> <!--#### Ionic Sizes:- --> <!--i) solid structure--> <!--$Fe(OH_2)_6^{3+} \xrightarrow {aq.} complex$--> <!--ii) $Ln(H_2O)_x^{m+}$--> <!--increase in the stability--> </div> <div style='float: right; width:100%;'> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/d7fce08c-87e6-459d-d685-9291be287d00/public"></p> <!----> </div>

<h3 id="successd-blocksuccess"><Success>d-block</Success></h3> <div style='float: left; width:0%;font-size:30px;text-align:left;'> <!--iii) OM ---> <!--* More ionic than d-block elements Ln-C & Tr-C catalysis--> <!--$La^{3+}\quad Lu^{3+}$--> <!--* Charge Size--> </div> <div style='float: right; width:100%;'> <!----> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/70a75d37-c791-4bbc-3651-dcd5cb4ca600/public"></p> </div>

<h3 id="successatomic-and-ionic-sizessuccess"><Success>Atomic and Ionic Sizes</Success></h3> <div style='float: left; width:50%;font-size:30px;text-align:left;'> <ul> <li>The lanthanide contraction. i.e. the reduction in size of the $Ln^{3+}$ ion from $La^{3+}$ (103 pm) to $Lu^{3+}$ (86.1 pm)</li> <li>It is often explained by the poor shielding of the 5s and 5p electrons by the 4f electrons</li> </ul> </div> <div style='float: right; width:50%;'> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/1f6f5cf3-0720-40c1-6f1e-ac7f70f20b00/public"></p> <!--.jpg)--> </div>

<h3 id="successatomic-and-ionic-sizessuccess-1"><Success>Atomic and Ionic Sizes</Success></h3> <div style='float: left; width:50%;font-size:30px;text-align:left;'> <p><strong>Electronic configurations and Radii of Lanthanum and Lanthanoids</strong></p> </div> <div style='float: right; width:50%;'> <!----> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/f75eb181-97e0-49e9-fd6e-319403e9d100/public"></p> </div>

<h3 id="successoxidation-statessuccess"><Success>Oxidation states</Success></h3> <div style='float: left; width:99%;font-size:30px;text-align:left;'> <ul> <li>The chemistry of the lanthanides is dominated by the +3 oxidation state</li> <li>In Ln compounds the 6s electrons and (usually) one 4f electron are lost and the ions have the configuration [Xe]4f</li> <li>All the lanthanide elements exhibit the oxidation state +3</li> <li>In addition, Ce can lose its single f-electron to form Ce with the stable electronic configuration of xenon</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-08-chapter-05-d-and-f-block-elements-l-5_5-2ofsmt6eujy-164.jpg"></p> </div>

<h3 id="successoxidation-statessuccess-1"><Success>Oxidation states</Success></h3> <div style='float: left; width:0%;font-size:25px;text-align:left;'> <!--* 5d $\tiny\checkmark$ $\quad \quad$ $Ce^{3+}$ $\quad 4f^{1}\rightarrow Ce^{+4}$--> <!-- $\quad \quad \quad \quad Pr^{4+}$--> <!-- $\quad \quad \quad \quad Tb^{4+}$--> <!--* Monazite $Ln^{3+}PO_4 \rightarrow$ Sand--> <!--* Bastneansite $Ln^{3+}CO_3F$--> <!--* $LnX_3$--> <!--* $Ln_2O_3$--> </div> <div style='float: right; width:100%;'> <!----> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/86328233-3e1d-401a-bb90-940e52c6d100/public"></p> </div>

<h3 id="successimportant-point-of-oxidation-statessuccess"><Success>Important point of oxidation states</Success></h3> <div style='float: left; width:100%;font-size:25px;text-align:left;'> <ul> <li>$Eu^{3+}$ can gain an electron to form $Eu^{2+}$ with the $f^7$ configuration</li> <li>It has the extra stability of a half-filled shell, Other than $Ce^{IV}$ and $Eu^{2+}$</li> <li>None of the lanthanoides are stable in oxidation states other than +3 in aqueous solution</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-08-chapter-05-d-and-f-block-elements-l-5_5-2ofsmt6eujy-165(1).jpg"></p> </div>

<h3 id="successimportant-pointsuccess"><Success>Important point</Success></h3> <div style='float: left; width:100%;font-size:25px;text-align:left;'> <ul> <li>The value$E^o$ for $Ce^{4+}Ce^{3+}$ is + 1.74 V</li> <li>It can oxidize water</li> <li>Formation of $Ce^{IV}$ is favored by its noble gas configuration</li> <li>$ Ln^{3+}(aq) + 3e\rightarrow Ln(s)$</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-08-chapter-05-d-and-f-block-elements-l-5_5-2ofsmt6eujy-231.jpg"></p> </div>

<h3 id="successspectra-emissionsuccess"><Success>Spectra emission</Success></h3> <div style='float: left; width:0%;text-align:left;font-size:30px'> <!--* 5d $\tiny\checkmark$ $\quad \quad$ $Ce^{3+}$ $\quad 4f^{1}\rightarrow Ce^{+4}$--> <!--$\quad \quad \quad \quad Pr^{4+}$--> <!--$\quad \quad \quad \quad Tb^{4+}$--> <!--* Monazite $Ln^{3+}PO_4$--> <!--$\quad \downarrow$--> <!--Sand--> <!--* Bastneansite $Ln^{3+}CO_3F$--> <!--* $LnX_3$--> <!--* $Ln_2O_3$--> </div> <div style='float: right; width:100%;'> <!----> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/405f16e3-c104-4efc-c29a-39c050449400/public"></p> </div>

<h3 id="successlanthanoidessuccess"><Success>Lanthanoides</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px'> <ul> <li>Client reactions of the lanthanoid</li> </ul> </div> <div style='float: right; width:50%;'> <!----> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/8b9855e5-eb22-4886-6aa7-7c8ca025c400/public"></p> </div>

<h3 id="successactinoidssuccess"><Success>Actinoids</Success></h3> <div style='float: left; width:0%;text-align:left;font-size:30px'> <!--**Actinium & noids**--> <!--* Series radioactive rays--> <!--* Nuclear + Analytical Chemistry--> <!--<span style="color:blue">OCR not complete</span>--> </div> <div style='float: right; width:100%;'> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/6a24ee8a-19b4-463f-5f40-8c145f905a00/public"></p> <!----> </div>

<h3 id="successactinoidssuccess-1"><Success>Actinoids</Success></h3> <div style='float: left; width:50%;text-align:left;font-size:30px'> <!--<span style="color:blue">add Table</span>--> <p><strong>The Actinoids</strong></p> <ul> <li>Earlier members have relatively long half-lives</li> <li>Table 8.10: Soms Properties of Arttalum and Actinalde</li> </ul> </div> <div style='float: right; width:50%;'> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/d233ffa7-1981-44fe-f636-27fc583fcf00/public"></p> </div>

<h3 id="successelectronic-configurationssuccess"><Success>Electronic configurations</Success></h3> <div style='float: left; width:100%;text-align:left;font-size:30px'> <ul> <li>$7s^2$ and variable occupancy of the 5f and 6d subshells</li> <li>The 5f orbitals look like the 4f orbitals in their angular part of the wave-function, they are not as hidden as 4f orbitals and hence 5f electrons can take part in bonding to a far greater extent</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-08-chapter-05-d-and-f-block-elements-l-5_5-2ofsmt6eujy-249(3).jpg"></p> </div>

<h3 id="successstructuresuccess"><Success>Structure</Success></h3> <div style='float: left; width:0%;text-align:left;font-size:30px'> <!--<span style="color:blue">OCR not complete</span>--> </div> <div style='float: right; width:100%;'> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/3d48c06b-379d-4c0e-5079-4991c4505000/public"></p> <!----> </div>

<h3 id="successoxidation-statesuccess"><Success>Oxidation state</Success></h3> <div style='float: left; width:100%;text-align:left;font-size:30px'> <ul> <li>There is a greater range of oxidation states,</li> <li>which is in part attributed to the fact that the 5f, 6d and 7s levels.</li> <li>comparable energies.</li> </ul> </div> <div style='float: right; width:0%;'> <!--.jpg)--> <p><img alt="alt text" src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/f63cd7f0-0451-4e48-fd08-f2ec13aa4c00/public"></p> </div>

<h2 id="successthank-yousuccess"><Success>Thank you</Success></h2> <div style='float: left; width:50%;text-align:left;font-size:30px'> </div> <div style='float: right; width:50%;'> <!----> </div>