{"id":9177,"date":"2018-02-09T11:09:52","date_gmt":"2018-02-09T05:39:52","guid":{"rendered":"http:\/\/mycbseguide.com\/blog\/?p=9177"},"modified":"2019-03-02T11:46:05","modified_gmt":"2019-03-02T06:16:05","slug":"coordination-compounds-class-12-notes-chemistry","status":"publish","type":"post","link":"https:\/\/mycbseguide.com\/blog\/coordination-compounds-class-12-notes-chemistry\/","title":{"rendered":"Coordination Compounds class 12 Notes Chemistry"},"content":{"rendered":"<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_76 counter-hierarchy ez-toc-counter ez-toc-grey ez-toc-container-direction\">\n<div class=\"ez-toc-title-container\">\n<p class=\"ez-toc-title\" style=\"cursor:inherit\">Table of Contents<\/p>\n<span class=\"ez-toc-title-toggle\"><a href=\"#\" class=\"ez-toc-pull-right ez-toc-btn ez-toc-btn-xs ez-toc-btn-default ez-toc-toggle\" aria-label=\"Toggle Table of Content\"><span class=\"ez-toc-js-icon-con\"><span class=\"\"><span class=\"eztoc-hide\" style=\"display:none;\">Toggle<\/span><span class=\"ez-toc-icon-toggle-span\"><svg style=\"fill: #999;color:#999\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" class=\"list-377408\" width=\"20px\" height=\"20px\" viewBox=\"0 0 24 24\" fill=\"none\"><path d=\"M6 6H4v2h2V6zm14 0H8v2h12V6zM4 11h2v2H4v-2zm16 0H8v2h12v-2zM4 16h2v2H4v-2zm16 0H8v2h12v-2z\" fill=\"currentColor\"><\/path><\/svg><svg style=\"fill: #999;color:#999\" class=\"arrow-unsorted-368013\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" width=\"10px\" height=\"10px\" viewBox=\"0 0 24 24\" version=\"1.2\" baseProfile=\"tiny\"><path d=\"M18.2 9.3l-6.2-6.3-6.2 6.3c-.2.2-.3.4-.3.7s.1.5.3.7c.2.2.4.3.7.3h11c.3 0 .5-.1.7-.3.2-.2.3-.5.3-.7s-.1-.5-.3-.7zM5.8 14.7l6.2 6.3 6.2-6.3c.2-.2.3-.5.3-.7s-.1-.5-.3-.7c-.2-.2-.4-.3-.7-.3h-11c-.3 0-.5.1-.7.3-.2.2-.3.5-.3.7s.1.5.3.7z\"\/><\/svg><\/span><\/span><\/span><\/a><\/span><\/div>\n<nav><ul class='ez-toc-list ez-toc-list-level-1 eztoc-toggle-hide-by-default' ><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/mycbseguide.com\/blog\/coordination-compounds-class-12-notes-chemistry\/#Class_12_Chemistry_notes_Chapter_9_Coordination_Compounds\" >Class 12 Chemistry notes Chapter 9 Coordination Compounds<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/mycbseguide.com\/blog\/coordination-compounds-class-12-notes-chemistry\/#CBSE_Class_12_Chemistry_Quick_Revision_Notes_Chapter_9_Co-ordination_Compounds\" >CBSE Class 12 Chemistry Quick Revision Notes Chapter 9 Co-ordination Compounds<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/mycbseguide.com\/blog\/coordination-compounds-class-12-notes-chemistry\/#Coordination_Compounds_class_12_Notes_Chemistry\" >Coordination Compounds class 12 Notes Chemistry<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/mycbseguide.com\/blog\/coordination-compounds-class-12-notes-chemistry\/#CBSE_Class-12_Revision_Notes_and_Key_Points\" >CBSE Class-12 Revision Notes and Key Points<\/a><\/li><\/ul><\/nav><\/div>\n<p><strong>CBSE class 12 Coordination Compounds Class 12 Notes Chemistry<\/strong> in PDF are available for free download in myCBSEguide mobile app. The best app for CBSE students now provides Coordination Compounds class 12 Notes latest chapter wise notes for quick preparation of CBSE board exams and school-based annual examinations. Class 12 Chemistry notes on chapter 9 Coordination Compounds are also available for download in CBSE Guide website.<\/p>\n<h2><span class=\"ez-toc-section\" id=\"Class_12_Chemistry_notes_Chapter_9_Coordination_Compounds\"><\/span><strong>Class 12 Chemistry notes Chapter 9 Coordination Compounds<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>Download CBSE class 12th revision notes for chapter 9 Coordination Compounds in PDF format for free. Download revision notes for Coordination Compounds class 12 Notes and score high in exams. These are the Coordination Compounds class 12 Notes prepared by team of expert teachers. The revision notes help you revise the whole chapter 9 in minutes. Revision notes in exam days is one of the best tips recommended by teachers during exam days.<\/p>\n<p style=\"text-align: center;\"><strong><a class=\"button\" href=\"https:\/\/mycbseguide.com\/downloads\/cbse-class-12-chemistry\/1267\/cbse-revision-notes\/7\/\">Download\u00a0class 12 Chemistry Revision Notes as PDF<\/a><\/strong><\/p>\n<h2><span class=\"ez-toc-section\" id=\"CBSE_Class_12_Chemistry_Quick_Revision_Notes_Chapter_9_Co-ordination_Compounds\"><\/span><strong>CBSE Class 12 Chemistry Quick Revision Notes Chapter 9 Co-ordination Compounds<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<ul>\n<li><strong>Co-ordination compounds:<\/strong><\/li>\n<\/ul>\n<ol>\n<li>A coordination compound contains a central metal atom or ion surrounded by number of oppositely charged ions or neutral molecules. These ions or molecules re bonded to the metal atom or ion by a coordinate bond.<\/li>\n<li>Example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{K_4}\\left[ {Fe{{\\left( {CN} \\right)}_6}} \\right]\" \/><\/span><\/span><\/li>\n<li>They do not dissociate into simple ions when dissolved in water.<\/li>\n<\/ol>\n<ul>\n<li><strong>Double salt <\/strong><\/li>\n<\/ul>\n<ol>\n<li>When two salts in stoichiometric ratio are crystallised together from their saturated solution they are called double salts<\/li>\n<li>Example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?FeS{O_4}.\\left( {N{H_4}} \\right)2S{O_4}.6H2O\" \/><\/span><\/span>\u00a0(Mohr\u2019s salt)<\/li>\n<li>They dissociate into simple ions when dissolved in water.<\/li>\n<\/ol>\n<ul>\n<li><strong>Coordination entity: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>A coordination entity constitutes a central metal atom or ion bonded to a fixed number of ions or molecules.<\/li>\n<li>Example: In <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{K_4}\\left[ {Fe{{\\left( {CN} \\right)}_6}} \\right],{\\text{ }}{\\left[ {Fe{{\\left( {CN} \\right)}_6}} \\right]^{4 - }}\" \/><\/span><\/span>&#8211; represents coordination entity.<\/li>\n<\/ol>\n<ul>\n<li><strong>Central atom or ion: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>In a coordination entity, the atom\/ion to which a fixed number of ions\/groups are bound in a definite geometrical arrangement around it, is called the central atom or ion.<\/li>\n<li>Example: In <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{K_4}[Fe{\\left( {CN} \\right)_6}\" \/><\/span><\/span>, <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?Fe\" \/><\/span><\/span>\u00a0<span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?^{^{^{{^ + }}}}\" \/><\/span><\/span>is the central metal ion.<\/li>\n<\/ol>\n<ul>\n<li><strong>Ligands: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>A molecule, ion or group that is bonded to the metal atom or ion in a complex or coordination compound by a coordinate bond is called ligand.<\/li>\n<li>It may be neutral, positively or negatively charged.<\/li>\n<li>Examples: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{H_2}O,{\\text{ }}C{N^ - },{\\text{ }}N{O^ + }\" \/><\/span><\/span>etc.<\/li>\n<\/ol>\n<ul>\n<li><strong>Donor atom: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>An atom of the ligand attached directly to the metal is called the donor atom.<\/li>\n<li>Example: In the complex <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{K_4}\\left[ {Fe{{\\left( {CN} \\right)}_6}} \\right]\" \/><\/span><\/span>,CN is a donor atom.<\/li>\n<\/ol>\n<ul>\n<li><strong>Coordination number: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>The coordination number (CN) of a metal ion in a complex can be defined as the number of ligand donor atoms to which the metal is directly bonded.<\/li>\n<li>Example: In the complex <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{K_4}\\left[ {Fe{{\\left( {CN} \\right)}_6}} \\right]\" \/><\/span><\/span>, the coordination number of Fe is 6.<\/li>\n<\/ol>\n<ul>\n<li><strong>Coordination sphere<\/strong>:<\/li>\n<\/ul>\n<ol>\n<li>The central atom\/ion and the ligands attached to it are enclosed in square bracket and are collectively termed as the coordination sphere.<\/li>\n<li>Example: In the complex <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{K_4}\\left[ {Fe{{\\left( {CN} \\right)}_6}} \\right],{\\text{ }}{\\left[ {Fe{{\\left( {CN} \\right)}_6}} \\right]^{4 - }}\" \/><\/span><\/span>is the coordination sphere.<\/li>\n<\/ol>\n<ul>\n<li><strong>Counter ions: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>The ions present outside the coordination sphere are called counter ions.<\/li>\n<li>Example: In the complex <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{K_4}[Fe{\\left( {CN} \\right)_6}\" \/><\/span><\/span>, K+ is the counter ion.<\/li>\n<\/ol>\n<ul>\n<li><strong>Coordination polyhedron: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>The spatial arrangement of the ligand atoms which are directly attached to the central atom\/ ion defines a coordination polyhedron about the central atom.<\/li>\n<li>The most common coordination polyhedra are octahedral, square planar and tetrahedral.<\/li>\n<li>Examples: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{\\left[ {PtC{l_4}} \\right]^{2 - }}\" \/><\/span><\/span>is square planar, <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?Ni{\\left( {CO} \\right)_4}\" \/><\/span><\/span>\u00a0is tetrahedral while [Cu(NH3)6]3+ is octahedral.<\/li>\n<\/ol>\n<ul>\n<li><strong>Charge on the complex ion: <\/strong>The charge on the complex ion is equal to the algebraic sum of the charges on all the ligands coordinated to the central metal ion.<\/li>\n<\/ul>\n<ul>\n<li><strong>Denticity: <\/strong>The number of ligating (linking) atoms present in ligand is called denticity.<\/li>\n<\/ul>\n<ul>\n<li><strong>Unidentate ligands: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>The ligands whose only one donor atom is bonded to metal atom are called unidentate ligands.<\/li>\n<li>Examples: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{H_2}O,{\\text{ }}N{H_3},{\\text{ }}CO,{\\text{ }}C{N^ - }\" \/><\/span><\/span><\/li>\n<\/ol>\n<ul>\n<li><strong>Didentate ligands: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>The ligands which contain two donor atoms or ions through which they are bonded to the metal ion.<\/li>\n<li>Examples: Ethylene diamine (<span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{H_2}NC{H_2}C{H_2}N{H_2}\" \/><\/span><\/span>) has two nitrogen atoms, oxalate ion <img decoding=\"async\" src=\"https:\/\/media-mycbseguide.s3.amazonaws.com\/images\/static\/revise\/12\/chemistry\/12_chemistry_ch09_01.PNG\" \/> has two oxygen atoms which can bind with the metal atom.<\/li>\n<\/ol>\n<ul>\n<li><strong>Polydentate ligand: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>When several donor atoms are present in a single ligand, the ligand is called polydentate ligand.<\/li>\n<li>Examples: In <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?N{\\left( {C{H_2}C{H_2}N{H_2}} \\right)_3}\" \/><\/span><\/span>, the ligand is said to be polydentate and Ethylenediaminetetraacetate ion <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left( {EDT{A^{4--}}} \\right)\" \/><\/span><\/span>\u00a0is an important hexadentate ligand. It can bind through two nitrogen and four oxygen atoms to a central metal ion.<\/li>\n<\/ol>\n<ul>\n<li><strong>Chelate: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>An inorganic metal complex in which there is a close ring of atoms caused by attachment of a ligand to a metal atom at two points.<\/li>\n<li>An example is the complex ion formed between ethylene diamine and cupric ion, <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{\\left[ {Cu{{\\left( {N{H_2}C{H_2}N{H_2}} \\right)}_2}} \\right]^{2 + }}\" \/><\/span><\/span>.<\/li>\n<\/ol>\n<ul>\n<li><strong>Ambidentate ligand: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>Ligands which can ligate (link) through two different atoms present in it are called ambidentate ligand.<\/li>\n<li>Example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?N{O^{2 - }}\" \/><\/span><\/span>and <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?SC{N^ - }\" \/><\/span><\/span>. Here, <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?N{O^{2 - }}\" \/><\/span><\/span>can link through N as well as O while <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?SC{N^ - }\" \/><\/span><\/span>\u00a0can link through S as well as N atom.<\/li>\n<\/ol>\n<ul>\n<li><strong>Werner\u2019s coordination theory: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>Werner was able to explain the nature of bonding in complexes.<\/li>\n<li>The postulates of Werner\u2019s theory are:<\/li>\n<\/ol>\n<p>a). Metal shows two different kinds of valencies: primary valence and secondary valence.<\/p>\n<p>b). The ions\/ groups bound by secondary linkages to the metal have characteristic spatial arrangements corresponding to different coordination numbers.<\/p>\n<p>c). The most common geometrical shapes in coordination compounds are octahedral, square planar and tetrahedral.<\/p>\n<ul>\n<li><strong>Primary valence <\/strong><\/li>\n<\/ul>\n<ol>\n<li>This valence is normally ionisable.<\/li>\n<li>It is equal to positive charge on central metal atom.<\/li>\n<li>These valencies are satisfied by negatively charged ions.<\/li>\n<li>Example: In <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?CrC{l_3}\" \/><\/span><\/span>, the primary valency is three. It is equal to oxidation state of central metal ion.<\/li>\n<\/ol>\n<ul>\n<li><strong>Secondary valence <\/strong><\/li>\n<\/ul>\n<ol>\n<li>This valence is non \u2013 ionisable.<\/li>\n<li>The secondary valency equals the number of ligand atoms coordinated to the metal. It is also called coordination number of the metal.<\/li>\n<li>It is commonly satisfied by neutral and negatively charged, sometimes by positively charged ligands.<\/li>\n<\/ol>\n<ul>\n<li><strong>Oxidation number of central atom: <\/strong>The oxidation number of the central atom in a complex is defined as the charge it would carry if all the ligands are removed along with the electron pairs that are shared with the central atom.<\/li>\n<\/ul>\n<ul>\n<li><strong>Homoleptic complexes: <\/strong>Those complexes in which metal or ion is coordinate bonded to only one kind of donor atoms. For example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{\\left[ {Co{{\\left( {N{H_3}} \\right)}_6}} \\right]^{3 + }}\" \/><\/span><\/span><\/li>\n<\/ul>\n<ul>\n<li><strong>Heteroleptic complexes: <\/strong>Those complexes in which metal or ion is coordinate bonded to more than one kind of donor atoms. For example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{\\left[ {CoC{l_2}{{\\left( {N{H_3}} \\right)}_4}} \\right]^ + },{\\text{ }}{\\left[ {Co{{\\left( {N{H_3}} \\right)}_5}Br} \\right]^{2 + }}\" \/><\/span><\/span><\/li>\n<\/ul>\n<ul>\n<li><strong>Isomers: <\/strong>Two or more compounds which have same chemical formula but different arrangement of atoms are called isomers.<\/li>\n<\/ul>\n<ul>\n<li><strong>Types of isomerism: <\/strong><\/li>\n<\/ul>\n<p>a). Linkage isomerism<\/p>\n<p>b). Solvate isomerism or hydrate isomerism<\/p>\n<p>c). Ionisation isomerism<\/p>\n<p>d). Coordination isomerism<\/p>\n<ol>\n<li>Structural isomerism<\/li>\n<li>Stereoisomerism<\/li>\n<\/ol>\n<p>a). Geometrical isomerism<\/p>\n<p>b). Optical isomerism<\/p>\n<ul>\n<li><strong>Structural isomerism: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>It arises due to the difference in structures of coordination compounds.<\/li>\n<li>Structural isomerism, or constitutional isomerism, is a form of isomerism in which molecules with the same molecular formula have atoms bonded together in different orders.<\/li>\n<\/ol>\n<ul>\n<li><strong>Ionisation isomerism: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>It arises when the counter ion in a complex salt is itself a potential ligand and can displace a ligand which can then become the counter ion<strong>. <\/strong><\/li>\n<li>Example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left[ {Co{{\\left( {N{H_3}} \\right)}_5}Br} \\right]{\\text{ }}S{O_4}and{\\text{ }}\\left[ {Co{{\\left( {N{H_3}} \\right)}_5}S{O_4}} \\right]{\\text{ }}Br\" \/><\/span><\/span><\/li>\n<\/ol>\n<ul>\n<li><strong>Solvate isomerism: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>It is isomerism in which solvent is involved as ligand.<\/li>\n<li>If solvent is water it is called hydrate isomerism, e.g., <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left[ {Cr{{\\left( {{H_2}O} \\right)}_6}} \\right]C{l_3}\" \/><\/span><\/span>\u00a0and <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left[ {CrC{l_2}{{\\left( {{H_2}O} \\right)}_4}} \\right]{\\text{ }}C{l_2}.{\\text{ }}2{H_2}O\" \/><\/span><\/span>.<\/li>\n<\/ol>\n<ul>\n<li><strong>Linkage isomerism: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>It arises in a coordination compound containing ambidentate ligand.<\/li>\n<li>In the isomerism, a ligand can form linkage with metal through different atoms.<\/li>\n<li>Example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left[ {Co{{\\left( {N{H_3}} \\right)}_5}ONO} \\right]C{l_2}\" \/><\/span><\/span>\u00a0and <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left[ {Co{{\\left( {N{H_3}} \\right)}_5}N{O_2}} \\right]C{l_2}\" \/><\/span><\/span>.<\/li>\n<\/ol>\n<ul>\n<li><strong>Coordination isomerism: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>This type of isomerism arises from the interchange of ligands between cationic and anionic entities of different metal ions present in a complex.<\/li>\n<li>Example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left[ {Co{{\\left( {N{H_3}} \\right)}_6}} \\right]\\left[ {Cr{{\\left( {{C_2}{O_4}} \\right)}_3}} \\right]\" \/><\/span><\/span>\u00a0and <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\left[ {Cr{{\\left( {N{H_3}} \\right)}_6}} \\right]\\left[ {Co{{\\left( {{C_2}{O_4}} \\right)}_3}} \\right]\" \/><\/span><\/span>.<\/li>\n<\/ol>\n<ul>\n<li><strong>Stereoisomerism: <\/strong>This type of isomerism arises because of different spatial arrangement.<\/li>\n<\/ul>\n<ul>\n<li><strong>Geometrical isomerism: <\/strong>It arises in heteroleptic complexes due to different possible geometrical arrangements of ligands.<\/li>\n<\/ul>\n<ul>\n<li><strong>Optical isomerism: <\/strong>Optical isomers are those isomers which are non-superimposable mirror images.<\/li>\n<\/ul>\n<ul>\n<li><strong>Valence bond theory: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>According to this theory, the metal atom or ion under the influence of ligands can use its (n-1)d, ns, np or ns, np, nd orbitals for hybridisation to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral, and square planar.<\/li>\n<li>These hybridised orbitals are allowed to overlap with ligand orbitals that can donate electron pairs for bonding.<\/li>\n<\/ol>\n<table border=\"1\" cellspacing=\"0\" cellpadding=\"3\">\n<tbody>\n<tr>\n<td>Coordination Number<\/td>\n<td>Type of hybridisation<\/td>\n<td>Shape of hybrid<\/td>\n<\/tr>\n<tr>\n<td>4<\/td>\n<td><span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?s{p^3}\" \/><\/span><\/span><\/td>\n<td>Tetrahedral<\/td>\n<\/tr>\n<tr>\n<td>4<\/td>\n<td><span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?ds{p^2}\" \/><\/span><\/span><\/td>\n<td>Square planar<\/td>\n<\/tr>\n<tr>\n<td>5<\/td>\n<td><span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?s{p^3}d\" \/><\/span><\/span><\/td>\n<td>Trigonalbipyramidal<\/td>\n<\/tr>\n<tr>\n<td>6<\/td>\n<td><span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?s{p^3}{d^2}\" \/><\/span><\/span>\u00a0(nd orbitals are involved \u2013 outer orbital complex or high spin or spin free complex)<\/td>\n<td>Octahedral<\/td>\n<\/tr>\n<tr>\n<td>6<\/td>\n<td><span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?{d^2}s{p^3}\\left( {n - 1} \\right)\" \/><\/span><\/span>\u00a0d orbitals are involved \u2013inner orbital or low spin or spin paired complex)<\/td>\n<td>Octahedral<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<ul>\n<li><strong>Magnetic properties of coordination compounds: <\/strong><\/li>\n<\/ul>\n<p>A coordination compound is paramagnetic in nature if it has unpaired electrons and diamagnetic if all the electrons in the coordination compound are paired.<\/p>\n<p>Magnetic moment <img decoding=\"async\" src=\"https:\/\/media-mycbseguide.s3.amazonaws.com\/images\/static\/revise\/12\/chemistry\/12_chemistry_ch09_02.png\" \/> where n is number of unpaired electrons.<\/p>\n<ul>\n<li><strong>Crystal Field Theory: <\/strong><\/li>\n<\/ul>\n<ol>\n<li>It assumes the ligands to be point charges and there is electrostatic force of attraction between ligands and metal atom or ion.<\/li>\n<li>It is theoretical assumption.<\/li>\n<\/ol>\n<ul>\n<li><strong>Crystal field splitting in octahedral coordination complexes: <\/strong><\/li>\n<\/ul>\n<p><img decoding=\"async\" src=\"https:\/\/media-mycbseguide.s3.amazonaws.com\/images\/static\/revise\/12\/chemistry\/12_chemistry_ch09_03.png\" \/><\/p>\n<ul>\n<li><strong>Crystal field splitting in tetrahedral coordination complexes:<\/strong><\/li>\n<\/ul>\n<p><img decoding=\"async\" src=\"https:\/\/media-mycbseguide.s3.amazonaws.com\/images\/static\/revise\/12\/chemistry\/12_chemistry_ch09_04.png\" \/><\/p>\n<ul>\n<li>For the same metal, the same ligands and metal-ligand distances, the difference in energy between eg and t2g level is <img decoding=\"async\" src=\"https:\/\/media-mycbseguide.s3.amazonaws.com\/images\/static\/revise\/12\/chemistry\/12_chemistry_ch09_05.png\" \/><\/li>\n<\/ul>\n<ul>\n<li><strong>Metal carbonyls:<\/strong><\/li>\n<\/ul>\n<ol>\n<li>Metal carbonyls are homoleptic complexes in which carbon monoxide (CO) acts as the ligand.<\/li>\n<li>Example: <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?Ni{\\left( {CO} \\right)_4}\" \/><\/span><\/span><\/li>\n<li>The metal-carbon bond in metal carbonyls possess both <em>s <\/em>and <em>p <\/em>character.<\/li>\n<li>The M\u2013C <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\sigma\" \/><\/span><\/span>\u00a0bond is formed by the donation of lone pair of electrons from the carbonyl carbon into a vacant orbital of the metal.<\/li>\n<li>The M\u2013C <span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\pi\" \/><\/span><\/span>bond is formed by the donation of a pair of electrons from a filled <em>d <\/em>orbital of metal into the vacant antibonding<span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?\\pi\" \/><\/span><\/span><span class=\"cke_widget_wrapper cke_widget_inline cke_widget_selected\"><span class=\"math-tex cke_widget_element\"><img decoding=\"async\" src=\"https:\/\/elpiscart.com\/cgi-bin\/mathtex.cgi?*\" \/><\/span><\/span>\u00a0orbital of carbon monoxide.<\/li>\n<li>The metal to ligand bonding creates a synergic effect which strengthens the bond between CO and the metal.<\/li>\n<\/ol>\n<h2><span class=\"ez-toc-section\" id=\"Coordination_Compounds_class_12_Notes_Chemistry\"><\/span>Coordination Compounds class 12 Notes Chemistry<span class=\"ez-toc-section-end\"><\/span><\/h2>\n<ul>\n<li>CBSE Revision notes (PDF Download) Free<\/li>\n<li>CBSE Revision notes for Class 12 Chemistry PDF<\/li>\n<li>Revision notes Class 12 Chemistry \u2013 CBSE<\/li>\n<li>CBSE Revisions notes and Key Points Class 12 Chemistry<\/li>\n<li>Summary of the NCERT books all chapters in Chemistry class 12<\/li>\n<li>Short notes for CBSE class 12th Chemistry<\/li>\n<li>Key notes and chapter summary of Chemistry class 12<\/li>\n<li>Quick revision notes for CBSE board exams<\/li>\n<\/ul>\n<h2><span class=\"ez-toc-section\" id=\"CBSE_Class-12_Revision_Notes_and_Key_Points\"><\/span><strong>CBSE Class-12 Revision Notes and Key Points<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>Coordination Compounds class 12 Notes Chemistry. CBSE quick revision note for class-12 Chemistry, Physics Math\u2019s, Biology and other subject are very helpful to revise the whole syllabus during exam days. The revision notes covers all important formulas and concepts given in the chapter. Even if you wish to have an overview of a chapter, quick revision notes are here to do if for you. These notes will certainly save your time during stressful exam days.<\/p>\n<ul>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-physics\/1251\/cbse-revision-notes\/7\/\">Physics<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-chemistry\/1267\/cbse-revision-notes\/7\/\">Chemistry<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-mathematics\/1284\/cbse-revision-notes\/7\/\">Mathematics<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-biology\/1298\/cbse-revision-notes\/7\/\">Biology<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-accountancy\/1315\/cbse-revision-notes\/7\/\">Accountancy<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-economics\/1327\/cbse-revision-notes\/7\/\">Economics<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-business-studies\/1727\/cbse-revision-notes\/7\/\">Business Studies<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-computer-science\/1851\/cbse-revision-notes\/7\/\">Computer Science<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-informatics-practices\/1873\/cbse-revision-notes\/7\/\">Informatics Practices<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-english-core\/1855\/cbse-revision-notes\/7\/\">English Core<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-history\/1869\/cbse-revision-notes\/7\/\">History<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-12-physical-education\/1877\/cbse-revision-notes\/7\/\">Physical Education<\/a><\/li>\n<\/ul>\n<p>To download Coordination Compounds class 12 Notes Chemistry, sample paper for class 12 Physics, Chemistry, Biology, History, Political Science, Economics, Geography, Computer Science, Home Science, Accountancy, Business Studies and Home Science; do check myCBSEguide app or website. myCBSEguide provides sample papers with solution, test papers for chapter-wise practice, NCERT Coordination Compounds, NCERT Exemplar Coordination Compounds, quick revision notes for ready reference, CBSE guess papers and CBSE important question papers. Sample Paper all are made available through\u00a0<a href=\"https:\/\/play.google.com\/store\/apps\/details?id=in.techchefs.MyCBSEGuide&amp;referrer=utm_source%3Dmycbse_bottom%26utm_medium%3Dtext%26utm_campaign%3Dmycbseads\"><strong>the best app for CBSE students<\/strong><\/a>\u00a0and myCBSEguide website.<\/p>\n<ul>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/solid-state-class-12-notes-chemistry\/\">Solid State class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/solutions-class-12-notes-chemistry\/\">Solutions class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/electrochemistry-class-12-notes-chemistry\/\">Electrochemistry class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/chemical-kinetics-class-12-notes-chemistry\/\">Chemical Kinetics class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/surface-chemistry-class-12-notes-chemistry\/\">Surface Chemistry class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/general-principles-processes-isolation-elements-class-12-notes-chemistry\/\">General Principles and Processes of Isolation of Elements class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/p-block-elements-class-12-notes-chemistry\/\">The p-Block Elements class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/d-f-block-elements-class-12-notes-chemistry\/\">The d- and f- Block Elements class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/haloalkanes-haloarenes-class-12-notes-chemistry\/\">Haloalkanes and Haloarenes class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/alcohols-phenols-ethers-class-12-notes-chemistry\/\">Alcohols Phenols and Ethers class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/aldehydes-ketones-carboxylic-acids-class-12-notes-chemistry\/\">Aldehydes Ketones and Carboxylic Acids class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/amines-class-12-notes-chemistry\/\">Amines class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/biomolecules-class-12-notes-chemistry\/\">Biomolecules class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/polymers-class-12-notes-chemistry\/\">Polymers class 12 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/chemistry-everyday-life-class-12-notes-chemistry\/\">Chemistry in Everyday Life class 12 Notes Chemistry<\/a><\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>CBSE class 12 Coordination Compounds Class 12 Notes Chemistry in PDF are available for free download in myCBSEguide mobile app. The best app for CBSE students now provides Coordination Compounds class 12 Notes latest chapter wise notes for quick preparation of CBSE board exams and school-based annual examinations. Class 12 Chemistry notes on chapter 9 &#8230; <a title=\"Coordination Compounds class 12 Notes Chemistry\" class=\"read-more\" href=\"https:\/\/mycbseguide.com\/blog\/coordination-compounds-class-12-notes-chemistry\/\" aria-label=\"More on Coordination Compounds class 12 Notes Chemistry\">Read more<\/a><\/p>\n","protected":false},"author":2,"featured_media":9086,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[48,456],"tags":[457,150,504,526,426,240],"class_list":["post-9177","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-cbse-class-12","category-revision-notes","tag-cbse-notes","tag-cbse-notes-and-key-points","tag-chemistry-notes","tag-coordination-compounds","tag-quick-revision","tag-quick-revision-notes"],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v26.0 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Coordination Compounds class 12 Notes Chemistry | myCBSEguide<\/title>\n<meta name=\"description\" content=\"Coordination Compounds class 12 Notes Chemistry chapter 9 in PDF format for free download. 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