{"id":12664,"date":"2026-06-04T11:49:10","date_gmt":"2026-06-04T11:49:10","guid":{"rendered":"https:\/\/www.vedprep.com\/exams\/?p=12664"},"modified":"2026-06-04T12:11:57","modified_gmt":"2026-06-04T12:11:57","slug":"ferrocene-for-iit-jam","status":"publish","type":"post","link":"https:\/\/www.vedprep.com\/exams\/iit-jam\/ferrocene-for-iit-jam\/","title":{"rendered":"Ferrocene: Master Guide For IIT JAM 2027"},"content":{"rendered":"<p><strong>Ferrocene<\/strong> For IIT JAM is a crucial topic in inorganic chemistry that requires a deep understanding of its structure, properties, and applications. It is essential for CSIR NET, IIT JAM, CUET PG, and GATE aspirants to master this subject to excel in their exams.<\/p>\n<h2><strong>Syllabus: Inorganic Chemistry for IIT JAM\u00a0<\/strong><\/h2>\n<p data-path-to-node=\"1\">If you are gearing up for <a href=\"https:\/\/jam2026.iitb.ac.in\/files\/syllabus_CY.pdf\" rel=\"nofollow noopener\" target=\"_blank\"><strong>IIT JAM<\/strong><\/a>, you already know that organometallic chemistry is a heavyweight topic. Specifically, <b data-path-to-node=\"1\" data-index-in-node=\"132\">Ferrocene<\/b> and its sandwich-complex cousins form a major chunk of the syllabus. For CSIR NET grads, you will find this under Section 3 (Transition Metal Chemistry), while for our IIT JAM crew, it is tucked neatly into Chapter 2 (Transition Metal Complexes and Organometallic Compounds).<\/p>\n<p data-path-to-node=\"2\">When you are hitting the books, classic texts like O.P. Tandon\u2019s <i data-path-to-node=\"2\" data-index-in-node=\"65\">Inorganic Chemistry<\/i> or the heavy-hitting <i data-path-to-node=\"2\" data-index-in-node=\"106\">Advanced Inorganic Chemistry<\/i> by Atkins and Jones are excellent go-tos. They break down the structural quirks and reaction pathways of these compounds quite well. Here at <b data-path-to-node=\"2\" data-index-in-node=\"276\">VedPrep<\/b>, we always tell our students to skip the mindless memorization and instead focus on <i data-path-to-node=\"2\" data-index-in-node=\"368\">why<\/i> these complexes behave the way they do. Master the fundamentals of metal-ligand bonding here, and you will breeze through a ton of exam questions.<\/p>\n<h2><strong>Understanding Ferrocene For IIT JAM: Structure and Properties<\/strong><\/h2>\n<p data-path-to-node=\"5\">Let\u2019s talk about what <strong>Ferrocene<\/strong> actually looks like. Imagine a classic street-cart ice cream sandwich\u2014you have two crunchy chocolate wafers holding a scoop of vanilla ice cream right in the middle. In <strong>Ferrocene<\/strong>, those two wafers are flat, five-membered aromatic rings called cyclopentadienyl (<span class=\"math-inline\" data-math=\"C_5H_5^-\" data-index-in-node=\"293\">C<sub>5<\/sub>H<sub>5<\/sub><sup>&#8211;<\/sup><\/span>) ligands, and the ice cream is a single iron (<span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"348\">Fe<sup>2+<\/sup><\/span>) atom sandwiched perfectly between them.<\/p>\n<p data-path-to-node=\"6\">Now, let&#8217;s clear up a massive piece of misinformation in the original text: <b data-path-to-node=\"6\" data-index-in-node=\"76\">Ferrocene is absolutely NOT paramagnetic.<\/b> In fact, this is a classic trap that catches students off guard in exams! Let\u2019s break down the actual math and chemistry so you never lose marks on this:<\/p>\n<ul data-path-to-node=\"7\">\n<li>\n<p data-path-to-node=\"7,0,0\"><b data-path-to-node=\"7,0,0\" data-index-in-node=\"0\">Oxidation State:<\/b> The overall complex is neutral. Since each cyclopentadienyl ring carries a <span class=\"math-inline\" data-math=\"-1\" data-index-in-node=\"92\">-1<\/span>\u00a0charge, the iron center sits in a <span class=\"math-inline\" data-math=\"+2\" data-index-in-node=\"129\">+2<\/span>\u00a0oxidation state (<span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"149\">Fe<sup>2+<\/sup><\/span>).<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"7,1,0\"><b data-path-to-node=\"7,1,0\" data-index-in-node=\"0\">Electron Counting:<\/b> An isolated iron atom has 8 valence electrons. Lose two to become <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"85\">Fe<sup>2+<\/sup><\/span>, and you are left with a <span class=\"math-inline\" data-math=\"d^6\" data-index-in-node=\"118\">d<sup>6<\/sup><\/span>\u00a0configuration.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"7,2,0\"><b data-path-to-node=\"7,2,0\" data-index-in-node=\"0\">Crystal Field Splitting:<\/b> Because the cyclopentadienyl rings are incredibly strong-field ligands, they split the <span class=\"math-inline\" data-math=\"d\" data-index-in-node=\"112\">d<\/span>-orbitals in a way that forces all 6 of those <span class=\"math-inline\" data-math=\"d\" data-index-in-node=\"159\">d<\/span>-electrons to pair up completely in the lower-energy bonding orbitals (<span class=\"math-inline\" data-math=\"e_{2g}\" data-index-in-node=\"231\">e<\/span><sub><span class=\"math-inline\" data-math=\"e_{2g}\" data-index-in-node=\"231\">2g<\/span><\/sub> and <span class=\"math-inline\" data-math=\"a_{1g}\" data-index-in-node=\"242\">a<sub>1g<\/sub><\/span>).<\/p>\n<\/li>\n<\/ul>\n<p data-path-to-node=\"8\">Because there are exactly <b data-path-to-node=\"8\" data-index-in-node=\"26\">zero<\/b> unpaired electrons, <b data-path-to-node=\"8\" data-index-in-node=\"51\">Ferrocene is completely diamagnetic.<\/b> If you run the spin-only formula:<\/p>\n<p data-path-to-node=\"8\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-medium wp-image-20802 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/unpaired-electrons-300x88.png\" alt=\"unpaired electrons\" width=\"300\" height=\"88\" srcset=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/unpaired-electrons-300x88.png 300w, https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/unpaired-electrons.png 311w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<p data-path-to-node=\"10\">Since <span class=\"math-inline\" data-math=\"n = 0\" data-index-in-node=\"6\">n = 0<\/span>\u00a0(where <span class=\"math-inline\" data-math=\"n\" data-index-in-node=\"19\">n<\/span>\u00a0is the number of unpaired electrons), the magnetic moment <span class=\"math-inline\" data-math=\"\\mu\" data-index-in-node=\"79\">\u03bc<\/span>\u00a0is exactly <span class=\"math-inline\" data-math=\"0\\text{ B.M.}\" data-index-in-node=\"94\">0 B.M.<\/span><\/p>\n<p data-path-to-node=\"11\">Keep this locked in your memory bank because examiners love testing this specific property to see who actually understands ligand field theory versus who is just guessing.<\/p>\n<h2><strong>Ferrocene For IIT JAM: Preparation and Synthesis Methods<\/strong><\/h2>\n<p data-path-to-node=\"14\">how do we actually cook up this compound in a lab? There are two main recipes you need to know for the exam.<\/p>\n<p data-path-to-node=\"15\">First, you can heat up cyclopentadiene with iron pentacarbonyl (<span class=\"math-inline\" data-math=\"Fe(CO)_5\" data-index-in-node=\"64\">Fe(CO)<sub>5<\/sub><\/span>). Think of it like a rowdy group of friends moving into an apartment\u2014the incoming cyclopentadienyl rings are way more aggressive, so they boot out the carbonyl groups, leaving you with a highly stable <strong>Ferrocene<\/strong> molecule.<\/p>\n<p data-path-to-node=\"16\">The second method\u2014and one we emphasize heavily in our prep sessions at <b data-path-to-node=\"16\" data-index-in-node=\"71\">VedPrep<\/b>\u2014is reacting sodium cyclopentadienide (<span class=\"math-inline\" data-math=\"C_5H_5Na\" data-index-in-node=\"117\">C<sub>5<\/sub>H<sub>5<\/sub>Na<\/span>) with iron(II) chloride (<span class=\"math-inline\" data-math=\"FeCl_2\" data-index-in-node=\"151\">FeCl<sub>2<\/sub><\/span>). Note that the original text mentioned iron(III) chloride (<span class=\"math-inline\" data-math=\"FeCl_3\" data-index-in-node=\"218\">FeCl<sub>3<\/sub><\/span>), which is a common mix-up! While you <i data-path-to-node=\"16\" data-index-in-node=\"263\">can<\/i> use FeCl\u2083, it requires an extra step because the cyclopentadienyl anion has to act as a reducing agent to bring <span class=\"math-inline\" data-math=\"Fe^{3+}\" data-index-in-node=\"380\">Fe<sup>3+<\/sup><\/span>\u00a0down to <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"396\">Fe<sup>2+<\/sup><\/span>\u00a0first. Using <span class=\"math-inline\" data-math=\"FeCl_2\" data-index-in-node=\"417\">FeCl\u2082<\/span> directly is much cleaner because the <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"396\">Fe<sup>2+<\/sup><\/span>\u00a0ions instantly pair up with the <span class=\"math-inline\" data-math=\"C_5H_5^-\" data-index-in-node=\"501\">C<sub>5<\/sub>H<sub>5<\/sub><sup>&#8211;<\/sup><\/span>\u00a0anions to yield pure, orange crystals of <strong>Ferrocene<\/strong>.<\/p>\n<p data-path-to-node=\"17\">This incredible stability comes down to the perfect covalent sharing of electrons between the iron atom and the <span class=\"math-inline\" data-math=\"\\pi\" data-index-in-node=\"112\">\u03c0<\/span>-clouds of the two organic rings, giving the complex a full 18-electron valence shell.<\/p>\n<h2><strong>Ferrocene For IIT JAM: Applications and Importance<\/strong><\/h2>\n<p data-path-to-node=\"20\"><strong>Ferrocene<\/strong> isn\u2019t just an abstract molecule meant to torture you during exam season; it is actually a massive workhorse in the real world. In industrial chemistry, it acts as a phenomenal catalyst, helping speed up reactions like turning unsaturated oils into stable plastics without needing crazy high temperatures or crushing pressures.<\/p>\n<p data-path-to-node=\"21\">The medical field is also tinkering with it. Scientists are building <strong>Ferrocene<\/strong> derivatives to act as smart missiles against cancer cells and nasty microbes, using the molecule&#8217;s unique shape to disrupt bad cellular machinery. Over in materials science, it is used to spin out conducting polymers and specialized magnetic resonance imaging (MRI) contrast agents.<\/p>\n<h3 data-path-to-node=\"22\">Why It Matters:<\/h3>\n<ul data-path-to-node=\"23\">\n<li>\n<p data-path-to-node=\"23,0,0\"><b data-path-to-node=\"23,0,0\" data-index-in-node=\"0\">Electronics:<\/b> It helps build flexible organic light-emitting diodes (OLEDs).<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"23,1,0\"><b data-path-to-node=\"23,1,0\" data-index-in-node=\"0\">Versatility:<\/b> It serves as a starting block for creating other incredibly complex, redox-active molecules.<\/p>\n<\/li>\n<\/ul>\n<h2><strong>Common Mistakes to Avoid: Ferrocene For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"26\">Let\u2019s chat about where students usually trip up so you can dodge those landmines on test day.<\/p>\n<p data-path-to-node=\"27\">First off, do not mistake the bonding in <strong>Ferrocene<\/strong> as purely ionic. Even though we talk about <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"94\">Fe<sup>2+<\/sup><\/span> and <span class=\"math-inline\" data-math=\"C_5H_5^-\" data-index-in-node=\"106\">C<sub>5<\/sub>H<sub>5<\/sub><sup>&#8211;<\/sup><\/span> ions when we break down oxidation states, the actual bonding in the sandwich complex is heavily covalent. The cloud of electrons from the aromatic rings shares space directly with the iron atom&#8217;s <span class=\"math-inline\" data-math=\"d\" data-index-in-node=\"311\">d<\/span>-orbitals.<\/p>\n<p data-path-to-node=\"28\">Second, because it looks a bit exotic, students often assume <strong>Ferrocene<\/strong> must be hyper-reactive and ready to fall apart at any moment. The reality is quite the opposite. Because it satisfies the 18-electron rule and possesses aromatic stability, it is incredibly robust. It resists attacks by acids and bases and handles high heat like a absolute champ.<\/p>\n<h2><strong>Exam Strategy: Tips and Tricks for Ferrocene For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"31\">When you are staring down an organometallics question, remember that <strong>Ferrocene<\/strong> (Fe(C\u2085H\u2085)\u2082)\u00a0is essentially an aromatic beast. Because those cyclopentadienyl rings behave a lot like benzene, <strong>Ferrocene<\/strong> loves undergoing <b data-path-to-node=\"31\" data-index-in-node=\"219\">Electrophilic Aromatic Substitution (EAS)<\/b>. It will readily take part in Friedel-Crafts acylation, but it absolutely hates direct nitration or halogenation because strong oxidizing acids will just ruin the iron center.<\/p>\n<p data-path-to-node=\"32\">Another quick tip: do not confuse its synthesis with the classic Williamson ether synthesis\u2014that is for ethers, not sandwich complexes! Focus your energy on how the cyclopentadienyl anion is generated and how it coordinates with the metal. At <a href=\"https:\/\/www.vedprep.com\/online-courses\"><b data-path-to-node=\"32\" data-index-in-node=\"243\">VedPrep<\/b><\/a>, we always recommend sketching out these mechanism pathways by hand at least a few times. Seeing how the electrons move makes it a lot easier to recall under exam pressure.<\/p>\n<h2><strong>Solved Example<\/strong><\/h2>\n<p data-path-to-node=\"35\">Let\u2019s look at a typical problem you might encounter to make sure everything we just covered clicks.<\/p>\n<p data-path-to-node=\"36\"><b data-path-to-node=\"36\" data-index-in-node=\"0\">Question:<\/b> A student reacts sodium cyclopentadienide with anhydrous <span class=\"math-inline\" data-math=\"FeCl_2\" data-index-in-node=\"67\">FeCl<sub>2<\/sub><\/span>\u00a0to form an orange, crystalline organometallic compound. Identify the compound, state the oxidation state of the central metal, and determine its magnetic behavior.<\/p>\n<p data-path-to-node=\"37\"><strong>Solution:<\/strong><\/p>\n<ul data-path-to-node=\"38\">\n<li>\n<p data-path-to-node=\"38,0,0\"><b data-path-to-node=\"38,0,0\" data-index-in-node=\"0\">Identification:<\/b> The compound is <strong>Ferrocene<\/strong>, <span class=\"math-inline\" data-math=\"Fe(\\eta^5-C_5H_5)_2\" data-index-in-node=\"43\">Fe(\u03b7<sup>5<\/sup>-C<sub>5<\/sub>H<sub>5<\/sub>)<sub>2<\/sub><\/span>.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"38,1,0\"><b data-path-to-node=\"38,1,0\" data-index-in-node=\"0\">Oxidation State:<\/b> Each cyclopentadienyl ligand has a <span class=\"math-inline\" data-math=\"-1\" data-index-in-node=\"52\">-1<\/span>\u00a0charge. To keep the complex neutral, the iron atom must be in the <span class=\"math-inline\" data-math=\"+2\" data-index-in-node=\"121\">+2<\/span>\u00a0oxidation state (<span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"141\">Fe<sup>2+<\/sup><\/span>).<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"38,2,0\"><b data-path-to-node=\"38,2,0\" data-index-in-node=\"0\">Magnetic Behavior:<\/b> As an <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"25\">Fe<sup>2+<\/sup><\/span> system (<span class=\"math-inline\" data-math=\"d^6\" data-index-in-node=\"41\">d<sup>6<\/sup><\/span>) surrounded by strong-field cyclopentadienyl ligands, all 6 electrons completely pair up in the lower <span class=\"math-inline\" data-math=\"e_{2g}\" data-index-in-node=\"147\">e<sub>2g<\/sub><\/span> and <span class=\"math-inline\" data-math=\"a_{1g}\" data-index-in-node=\"158\">a<sub>1g<\/sub><\/span>\u00a0orbitals. With 0 unpaired electrons, the compound is strictly <b data-path-to-node=\"38,2,0\" data-index-in-node=\"227\">diamagnetic<\/b>.<\/p>\n<\/li>\n<\/ul>\n<table style=\"width: 100%; height: 99px;\" data-path-to-node=\"39\">\n<thead>\n<tr style=\"height: 48px;\">\n<td style=\"height: 48px;\"><strong>Compound<\/strong><\/td>\n<td style=\"height: 48px;\"><strong>Core Structure<\/strong><\/td>\n<td style=\"height: 48px;\"><strong>Magnetic Nature<\/strong><\/td>\n<td style=\"height: 48px;\"><strong>Valence Electron Count<\/strong><\/td>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"height: 51px;\">\n<td style=\"height: 51px;\"><span data-path-to-node=\"39,1,0,0\"><b data-path-to-node=\"39,1,0,0\" data-index-in-node=\"0\">Ferrocene<\/b> <span class=\"math-inline\" data-math=\"Fe(C_5H_5)_2\" data-index-in-node=\"10\">Fe(C<sub>5<\/sub>H<sub>5<\/sub>)<sub>2<\/sub><\/span><\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"39,1,1,0\">Sandwich complex (<span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"18\">Fe<sup>2+<\/sup><\/span> between two parallel <span class=\"math-inline\" data-math=\"C_5H_5^-\" data-index-in-node=\"47\">C5H5-<\/span>\u00a0rings)<\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"39,1,2,0\"><b data-path-to-node=\"39,1,2,0\" data-index-in-node=\"0\">Diamagnetic<\/b> (Zero unpaired electrons)<\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"39,1,3,0\">18 Electrons (Stable)<\/span><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2><strong>Real-World Applications: Ferrocene in Materials Science<\/strong><\/h2>\n<p data-path-to-node=\"42\">To give you a better mental picture of how this works in the real world, let&#8217;s look at a fictional scenario. Imagine a tech company trying to build a futuristic smartphone screen that can roll up like a piece of paper but still change colors instantly when you tap a button. Regular plastics can bend, but they don&#8217;t conduct electricity or react to magnetic fields very well.<\/p>\n<p data-path-to-node=\"43\">To solve this, materials scientists can link <strong>Ferrocene<\/strong> molecules together into long polymer chains. By embedding those iron-filled sandwiches directly into the backbone of the plastic, they create a hybrid material that can carry an electric current and change its optical properties on demand. These types of electrochromic devices, along with advanced magnetic sensors, are exactly why understanding the basic chemistry of <strong>Ferrocene<\/strong> is so incredibly valuable today.<\/p>\n<h2 data-path-to-node=\"43\"><strong>Conclusion<\/strong><\/h2>\n<p data-path-to-node=\"43\">Wrapping your head around <strong>Ferrocene<\/strong> isn&#8217;t just about ticking off a box for your IIT JAM syllabus; it\u2019s about unlocking how transition metals and organic molecules pull off incredible chemistry together. Once you move past the common exam traps\u2014like keeping its diamagnetic nature straight and mastering its electrophilic reactions\u2014you will start seeing this little iron sandwich as the predictable, high-scoring topic it actually is. Take it one concept at a time, keep practicing those electron-counting rules, and remember that our team at <a href=\"https:\/\/www.vedprep.com\/online-courses\/iit-jam\"><b data-path-to-node=\"0\" data-index-in-node=\"542\">VedPrep<\/b> <\/a>is always in your corner to help clear up the tricky parts.<\/p>\n<p data-path-to-node=\"43\">To kow more in detail from our expert faculty, watch our YouTube video:<\/p>\n<p class=\"responsive-video-wrap clr\"><iframe title=\"Stereochemistry One Shot Revision \ud83d\ude31 | CSIR NET June\/July 2026 | Chemical Sciences | VedPrep CSIR NET\" width=\"1200\" height=\"675\" src=\"https:\/\/www.youtube.com\/embed\/mHKTu9v14ps?feature=oembed\" frameborder=\"0\" allow=\"accelerometer; autoplay; clipboard-write; encrypted-media; gyroscope; picture-in-picture; web-share\" referrerpolicy=\"strict-origin-when-cross-origin\" allowfullscreen><\/iframe><\/p>\n<section class=\"vedprep-faq\">\n<h2><strong>Frequently Asked Questions<\/strong><\/h2>\n<\/section>\n<style>#sp-ea-20805 .spcollapsing { height: 0; overflow: hidden; transition-property: height;transition-duration: 300ms;}#sp-ea-20805.sp-easy-accordion>.sp-ea-single {margin-bottom: 10px; border: 1px solid #e2e2e2; }#sp-ea-20805.sp-easy-accordion>.sp-ea-single>.ea-header a {color: #444;}#sp-ea-20805.sp-easy-accordion>.sp-ea-single>.sp-collapse>.ea-body {background: #fff; color: #444;}#sp-ea-20805.sp-easy-accordion>.sp-ea-single {background: #eee;}#sp-ea-20805.sp-easy-accordion>.sp-ea-single>.ea-header a .ea-expand-icon { float: left; color: #444;font-size: 16px;}<\/style><div id=\"sp_easy_accordion-1780573105\">\n<div id=\"sp-ea-20805\" class=\"sp-ea-one sp-easy-accordion\" data-ea-active=\"ea-click\" data-ea-mode=\"vertical\" data-preloader=\"\" data-scroll-active-item=\"\" data-offset-to-scroll=\"0\">\n\n<!-- Start accordion card div. -->\n<div class=\"ea-card ea-expand sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208050\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208050\" aria-controls=\"collapse208050\" href=\"#\"  aria-expanded=\"true\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-minus\"><\/i> Is Ferrocene paramagnetic or diamagnetic?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse collapsed show\" id=\"collapse208050\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208050\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Ferrocene is strictly <b data-path-to-node=\"4\" data-index-in-node=\"22\">diamagnetic<\/b>. This is a classic exam trap! Because the cyclopentadienyl rings act as very strong-field ligands, they force all six of the <span class=\"math-inline\" data-math=\"d\" data-index-in-node=\"159\">$d$<\/span>-electrons in the <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"178\">Fe<sup>2+<\/sup><\/span>\u00a0center to pair up completely, leaving exactly zero unpaired electrons.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208051\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208051\" aria-controls=\"collapse208051\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the oxidation state of iron in Ferrocene?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208051\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208051\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>The iron atom in Ferrocene is in the <b data-path-to-node=\"6\" data-index-in-node=\"37\"><span class=\"math-inline\" data-math=\"+2\" data-index-in-node=\"37\">+2<\/span>\u00a0oxidation state<\/b> (<span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"57\">Fe<sup>2+<\/sup><\/span>). Since the overall molecule is neutral and each of the two cyclopentadienyl ligands carries a <span class=\"math-inline\" data-math=\"-1\" data-index-in-node=\"160\">-1<\/span>\u00a0charge, the math leaves iron with a <span class=\"math-inline\" data-math=\"+2\" data-index-in-node=\"199\">+2<\/span>\u00a0charge.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208052\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208052\" aria-controls=\"collapse208052\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How many valence electrons does Ferrocene have?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208052\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208052\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Ferrocene is a textbook example of a stable <b data-path-to-node=\"8\" data-index-in-node=\"44\">18-electron complex<\/b>. The <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"69\">Fe<sup>2+<\/sup><\/span>\u00a0ion provides 6 valence electrons, and each of the two \u03b7<span class=\"math-inline\" data-math=\"\\eta^5\\text{-cyclopentadienyl}\" data-index-in-node=\"131\"><sup>5<\/sup>-cyclopentadienyl<\/span>\u00a0rings donates 6 <span class=\"math-inline\" data-math=\"\\pi\" data-index-in-node=\"178\">\u03c0<\/span>-electrons (<span class=\"math-inline\" data-math=\"6 + 6 + 6 = 18\" data-index-in-node=\"193\">6 + 6 + 6 = 18<\/span>).<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208053\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208053\" aria-controls=\"collapse208053\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why is Ferrocene called a \"sandwich compound\"?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208053\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208053\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>It gets this nickname from its geometry. The central iron atom is physically located right in the middle, sandwiched perfectly between two parallel, planar cyclopentadienyl rings.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208054\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208054\" aria-controls=\"collapse208054\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Does Ferrocene show aromatic behavior?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208054\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208054\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes, it does! The cyclopentadienyl rings obey H\u00fcckel's rule (<span class=\"math-inline\" data-math=\"4n+2\" data-index-in-node=\"61\">4n+2<\/span>\u00a0<span class=\"math-inline\" data-math=\"\\pi\" data-index-in-node=\"66\">\u03c0<\/span>-electrons where <span class=\"math-inline\" data-math=\"n=1\" data-index-in-node=\"86\">n=1<\/span>), making them aromatic. Because of this, Ferrocene undergoes typical aromatic reactions like Friedel-Crafts acylation even faster than benzene.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208055\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208055\" aria-controls=\"collapse208055\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What happens when Ferrocene undergoes hapticity changes?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208055\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208055\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>In its ground state, Ferrocene features \u03b7<sup><span class=\"math-inline\" data-math=\"\\eta^5\" data-index-in-node=\"40\">5<\/span><\/sup> (pentahapto) bonding, meaning all five carbon atoms of each ring are equidistant from the iron center. While the rings can rotate, dropping to a lower hapticity (like \u03b7<sup><span class=\"math-inline\" data-math=\"\\eta^1\" data-index-in-node=\"214\">1<\/span><\/sup> or \u03b7<sup><span class=\"math-inline\" data-math=\"\\eta^3\" data-index-in-node=\"224\">3<\/span><\/sup>) is highly unfavorable because it breaks the stable 18-electron configuration.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208056\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208056\" aria-controls=\"collapse208056\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Can Ferrocene undergo direct nitration or halogenation?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208056\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208056\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>No, and this is another major pitfall to watch out for. Because strong oxidizing acids (like <span class=\"math-inline\" data-math=\"HNO_3\" data-index-in-node=\"93\">HNO<sub>3<\/sub><\/span>) or halogens will instantly oxidize the iron center from <span class=\"math-inline\" data-math=\"Fe^{2+}\" data-index-in-node=\"156\">Fe<sup>2+<\/sup><\/span><sup>\u00a0<\/sup>to the unstable <span class=\"math-inline\" data-math=\"Fe^{3+}\" data-index-in-node=\"180\">Fe<sup>3+<\/sup><\/span>\u00a0ferricenium ion, direct nitration or halogenation fails.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208057\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208057\" aria-controls=\"collapse208057\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the hapticity (\u03b7) of the ligands in Ferrocene?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208057\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208057\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>The hapticity is \u03b7<sup><span class=\"math-inline\" data-math=\"\\eta^5\" data-index-in-node=\"17\">5<\/span><\/sup>\u00a0for both rings. This means that all five carbon atoms of each cyclopentadienyl ring are actively bonding and sharing their <span class=\"math-inline\" data-math=\"\\pi\" data-index-in-node=\"147\">\u03c0<\/span>-electron cloud with the central iron atom.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208058\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208058\" aria-controls=\"collapse208058\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Is Ferrocene soluble in water?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208058\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208058\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>No, Ferrocene is highly lipophilic (fat-soluble) and practically insoluble in water. However, it dissolves easily in organic solvents like benzene, ether, and alcohol.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-208059\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse208059\" aria-controls=\"collapse208059\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What are the two main conformations of Ferrocene?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse208059\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-208059\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Ferrocene can exist in either a <b data-path-to-node=\"24\" data-index-in-node=\"32\">staggered (<span class=\"math-inline\" data-math=\"D_{5d}\" data-index-in-node=\"43\">D<sub>5d<\/sub><\/span>\u00a0symmetry)<\/b> or an <b data-path-to-node=\"24\" data-index-in-node=\"66\">eclipsed (<span class=\"math-inline\" data-math=\"D_{5h}\" data-index-in-node=\"76\">D<sub>5h<\/sub><\/span>\u00a0symmetry)<\/b> conformation. In the gas phase, the energy barrier between the two is incredibly small, but the eclipsed form is slightly more stable.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2080510\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2080510\" aria-controls=\"collapse2080510\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the Williamson reaction trap mentioned in exam prep?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2080510\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-2080510\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Students often confuse organometallic synthesis with organic ether synthesis. At <b data-path-to-node=\"26\" data-index-in-node=\"81\">VedPrep<\/b>, we remind our students that the Williamson ether synthesis is entirely unrelated to making Ferrocene; Ferrocene requires the coordination of a carbanion with a transition metal halide.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2080511\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2080511\" aria-controls=\"collapse2080511\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why is Ferrocene so thermally stable?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2080511\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-2080511\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Its stability comes down to satisfying the 18-electron rule and the extensive covalent orbital overlap between the iron's <span class=\"math-inline\" data-math=\"d\" data-index-in-node=\"122\">d<\/span>-orbitals and the aromati\u03c0-system of the rings. It can withstand temperatures up to nearly 400\u00b0C without breaking down!<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2080512\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2080512\" aria-controls=\"collapse2080512\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How does Ferrocene react to Friedel-Crafts Acylation?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2080512\" data-parent=\"#sp-ea-20805\" role=\"region\" aria-labelledby=\"ea-header-2080512\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>It reacts incredibly smoothly. Because the electron density on the rings is high, reacting Ferrocene with an acyl chloride in the presence of a Lewis acid like <span class=\"math-inline\" data-math=\"AlCl_3\" data-index-in-node=\"160\">AlCl<sub>3<\/sub><\/span>\u00a0easily yields acetylferrocene.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<\/div>\n<\/div>\n\n","protected":false},"excerpt":{"rendered":"<p>Ferrocene For IIT JAM is a crucial topic in inorganic chemistry that requires a deep understanding of its structure, properties, and applications. It is essential for CSIR NET, IIT JAM, CUET PG, and GATE aspirants to master this subject to excel in their exams.<\/p>\n","protected":false},"author":12,"featured_media":20808,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":"","rank_math_seo_score":87},"categories":[23],"tags":[2923,7638,7639,7640,7641,2922],"class_list":["post-12664","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-iit-jam","tag-competitive-exams","tag-ferrocene-for-iit-jam","tag-ferrocene-for-iit-jam-notes","tag-ferrocene-for-iit-jam-questions","tag-ferrocene-for-iit-jam-tutorials","tag-vedprep","entry","has-media"],"acf":[],"_links":{"self":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12664","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/users\/12"}],"replies":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/comments?post=12664"}],"version-history":[{"count":6,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12664\/revisions"}],"predecessor-version":[{"id":20809,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12664\/revisions\/20809"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media\/20808"}],"wp:attachment":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media?parent=12664"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/categories?post=12664"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/tags?post=12664"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}