{"id":9171,"date":"2018-02-09T11:06:35","date_gmt":"2018-02-09T05:36:35","guid":{"rendered":"http:\/\/mycbseguide.com\/blog\/?p=9171"},"modified":"2018-03-16T17:17:06","modified_gmt":"2018-03-16T11:47:06","slug":"structure-atom-class-11-notes-chemistry","status":"publish","type":"post","link":"https:\/\/mycbseguide.com\/blog\/structure-atom-class-11-notes-chemistry\/","title":{"rendered":"Structure of Atom class 11 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' ><ul class='ez-toc-list-level-2' ><li class='ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/mycbseguide.com\/blog\/structure-atom-class-11-notes-chemistry\/#CBSE_Guide_Structure_of_Atom_class_11_Notes\" >CBSE Guide Structure of Atom class 11 Notes<\/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\/structure-atom-class-11-notes-chemistry\/#Structure_of_Atom_class_11_Notes_Chemistry\" >Structure of Atom class 11 Notes Chemistry<\/a><\/li><\/ul><\/li><li class='ez-toc-page-1 ez-toc-heading-level-1'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/mycbseguide.com\/blog\/structure-atom-class-11-notes-chemistry\/#Download_Revision_Notes_as_PDF\" >Download Revision Notes as PDF<\/a><ul class='ez-toc-list-level-2' ><li class='ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/mycbseguide.com\/blog\/structure-atom-class-11-notes-chemistry\/#Structure_of_Atom_class_11_Notes\" >Structure of Atom class 11 Notes<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/mycbseguide.com\/blog\/structure-atom-class-11-notes-chemistry\/#CBSE_Class-11_Revision_Notes_and_Key_Points\" >CBSE Class-11 Revision Notes and Key Points<\/a><\/li><\/ul><\/li><\/ul><\/nav><\/div>\n<p>CBSE Chemistry Chapter 2 Structure of Atom class 11 Notes Chemistry in PDF are available for free download in myCBSEguide mobile app. The best app for CBSE students now provides Structure of Atom class 11 Notes Chemistry latest chapter wise notes for quick preparation of CBSE exams and school based annual examinations. Class 11 Chemistry notes on Chapter 2 Structure of Atom class 11 Notes Chemistry are also available for download in CBSE Guide website.<\/p>\n<h2><span class=\"ez-toc-section\" id=\"CBSE_Guide_Structure_of_Atom_class_11_Notes\"><\/span>CBSE Guide Structure of Atom class 11 Notes<span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>CBSE guide notes are the comprehensive notes which covers the latest syllabus of CBSE and NCERT. It includes all the topics given in NCERT class 11 Chemistry text book. Users can download CBSE guide quick revision notes from myCBSEguide mobile app and my CBSE guide website.<\/p>\n<h2><span class=\"ez-toc-section\" id=\"Structure_of_Atom_class_11_Notes_Chemistry\"><\/span>Structure of Atom class 11 Notes Chemistry<span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>Download CBSE class 11th revision notes for Chapter 2 Structure of Atom class 11 Notes Chemistry in PDF format for free. Download revision notes for Structure of Atom class 11 Notes Chemistry and score high in exams. These are the Structure of Atom class 11 Notes Chemistry prepared by team of expert teachers. The revision notes help you revise the whole chapter in minutes. Revising notes in exam days is on of the best tips recommended by teachers during exam days.<\/p>\n<h1 style=\"text-align: center\"><span class=\"ez-toc-section\" id=\"Download_Revision_Notes_as_PDF\"><\/span><a href=\"https:\/\/mycbseguide.com\/downloads\/cbse-class-11-chemistry\/1356\/cbse-revision-notes\/7\/\">Download Revision Notes as PDF<\/a><span class=\"ez-toc-section-end\"><\/span><\/h1>\n<p style=\"text-align: center\"><strong>CBSE Class 11 Chemistry<br \/>\nRevision Notes<br \/>\nChapter 2<br \/>\nStructure of Atom class 11 Notes Chemistry<br \/>\n<\/strong><\/p>\n<ol>\n<li><strong>Sub-atomic Particles<\/strong><\/li>\n<li><strong>Atomic Models and Their Limitations<\/strong><\/li>\n<li><strong>Quantum Mechanical Model of Atom<\/strong><\/li>\n<\/ol>\n<p>Atoms are the building blocks of elements. They are the smallest parts of an element that chemically react. The first atomic theory, proposed by John Dalton in 1808, regarded atom as the ultimate indivisible particle of matter. Towards the end of the nineteenth century it was proved experimentally that atoms are divisible and consist of three fundamental particles: electrons, protons and neutrons.<\/p>\n<p>Michael Faraday discovered electrons using cathode ray discharge tube experiment. Modified cathode ray tube experiment was carried out which led to the discovery of protons.<\/p>\n<p>Neutrons were discovered by James Chadwick by bombarding a thin sheet of beryllium by<br \/>\n<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?\\alpha\" \/><\/span><\/span>&#8211; particles. They are electrically neutral particles having a mass slightly greater than that of the protons.<\/p>\n<p>The discovery of sub-atomic particles led to the proposal of various atomic models to explain the structure of atom.<strong>Thomson<\/strong> in 1898 proposed that an atom consists of uniform sphere of positive electricity with electrons embedded into it. This model in which mass of the atom is considered to be evenly spread over the atom was proved wrong by<strong> Rutherford\u2019s<\/strong> famous alpha-particle scattering experiment in 1909. Rutherford concluded that atom is made of a tiny positively charged <strong>nucleus<\/strong>, at its centre with electrons revolving around it in circular orbits.<\/p>\n<p><strong>Rutherford model<\/strong>, which resembles the solar system, was no doubt an improvement over <strong>Thomson model<\/strong> but it could not account for the stability of the atom i.e., why the electron does not fall into the nucleus. Further, it was also silent about the electronic structure of atoms i.e., about the distribution and relative energies of electrons around the nucleus.<\/p>\n<p><strong>Planck\u2019s quantum theory<\/strong>: Max Planck proposed that atoms and molecules could emit or absorb energy only in discrete quantities and not in a continuous manner. Planck gave the name quantum, meaning \u2018fixed amount\u2019 to the smallest quantity of energy that can be emitted or absorbed in the form of electromagnetic radiation.<\/p>\n<p><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?E\\alpha\" \/><\/span><\/span>V<\/p>\n<p><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?E = hv\" \/><\/span><\/span><\/p>\n<p><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? = {hc \\ {} \\over \\lambda}\" \/><\/span><\/span><\/p>\n<p>Where:<br \/>\nE is the energy of a single quantum<br \/>\nh is Planck\u2019s constant<br \/>\n<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?\\lambda\" \/><\/span><\/span>\u00a0is the frequency of the radiation<br \/>\nh= 6.626 X 10<sup>\u201334<\/sup> Js<\/p>\n<p><strong>Photoelectric effect:<\/strong> The phenomenon of ejection of electrons from the surface of metal when light of suitable frequency strikes it is called photoelectric effect. The ejected electrons are called photoelectrons.<\/p>\n<p>The difficulties of the Rutherford model were overcome by <strong>Niels Bohr<\/strong> in 1913 in his model of the hydrogen atom. Bohr postulated that electron moves around the nucleus in circular orbits. Only certain orbits can exist and each orbit corresponds to a specific energy. Bohr calculated the energy of electron in various orbits and for each orbit predicted the distance between the electron and nucleus.<\/p>\n<p>Bohr model, though offering a satisfactory model for explaining the spectra of the hydrogen atom, could not explain the spectra of multi-electron atoms.<\/p>\n<p>The reason for this was soon discovered. In Bohr model, an electron is regarded as a charged particle moving in a well defined circular orbit about the nucleus. The wave character of the electron is ignored in Bohr\u2019s theory.<\/p>\n<p><strong>Dual behavior of matter:<\/strong> de Broglie proposed that matter exhibits dual behavior. This means matter shows both particle and wave nature. de Broglie\u2019s relation:<\/p>\n<p><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?\\lambda = {h\\ {} \\over mv}\" \/><\/span><\/span><\/p>\n<p><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 {} \\over p}\" \/><\/span><\/span><\/p>\n<p>Where:<br \/>\n<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?\\lambda\" \/><\/span><\/span>&#8211; Wavelength<br \/>\nh \u2013 Planck\u2019s constant<br \/>\np &#8211; Momentum<br \/>\nv &#8211; Velocity<\/p>\n<p>An orbit is a clearly defined path and this path can completely be defined only if both the exact position and the exact velocity of the electron at the same time are known. This is not possible according to the <strong>Heisenberg&#8217;s un<\/strong>certainty principle which states that it is impossible to determine simultaneously, the exact position and exact momentum (or velocity) of an electron. Bohr model of the hydrogen atom, therefore, not only ignores the dual behaviour of electron but also contradicts Heisenberg uncertainty principle.<\/p>\n<p><strong>Erwin Schr\u00f6dinger,<\/strong> in 1926, proposed an equation called Schr\u00f6dinger equation to describe the electron distributions in space and the allowed energy levels in atoms. This equation incorporates de Broglie\u2019s concept of wave-particle duality and is consistent with Heisenbergun uncertainty principle. When Schr\u00f6dinger equation is solved for the electron in a hydrogen atom, the solution gives the possible energy states the electron can occupy [and the corresponding wave function(s) (\u03c8) (which in fact are the mathematical functions) of the electron associated with each energy state].<\/p>\n<p>These quantized energy states and corresponding wave functions which are characterized by a set of three quantum numbers (principal quantum number n, azimuthal quantum number l and magnetic quantum number ml) arise as a natural consequence in the solution of the Schr\u00f6dinger equation. The restrictions on the values of these three quantum numbers also come naturally from this solution. The quantum mechanical model of the hydrogen atom successfully predicts all aspects of the hydrogen atom spectrum including some phenomena that could not be explained by the Bohr model.<\/p>\n<p>According to the <strong>quantum mechanical model<\/strong> of the atom, the electron distribution of an atom containing a number of electrons is divided into <strong>shells.<\/strong> The shells, in turn, are thought to consist of one or more <strong>sub-shells<\/strong> and sub-shells are assumed to be composed of one or more orbitals, which the electrons occupy. While for hydrogen and hydrogen like systems(such as <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( \\text{H}{{\\text{e}}^{+}},\\text{ L}{{\\text{i}}^{2+}}\\text{etc}\\text{. } \\right)\" \/><\/span><\/span>\u00a0all the orbitals within a given shell have same energy, the energy of the orbitals in a multi-electron atom depends upon the values of n and l: The lower the value of <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?(\\text{n }+\\text{ l}~\" \/><\/span><\/span>) for an orbital, the lower is its energy. If two orbitals have the same <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?(\\text{n }+\\text{ l}~\" \/><\/span><\/span>) value, the orbital with lower value of n has the lower energy.<\/p>\n<p>In an atom many such orbitals are possible and electrons are filled in those orbitals in order of increasing energy in accordance with <strong>Pauli exclusion principle <\/strong>(no two electrons in an atom can have the same set of four quantum numbers) and <strong>Hund\u2019s rule of maximum multiplicity<\/strong> (pairing of electrons in the orbitals belonging to the same sub shell does not take place until each orbital belonging to that sub shell has got one electron each, i.e., is singly occupied). This forms the basis of the electronic structure of atoms.<\/p>\n<p><strong>Electronic configuration of atoms:<\/strong> The electronic configuration of different atoms can be represented in two ways.<\/p>\n<p><strong>a. <\/strong>s<sup>a<\/sup> p<sup>b<\/sup> d<sup>c<\/sup> &#8230;.. notation: In the first notation, the sub-shell is represented by the respective letter symbol and the number of electrons present in the sub-shell is depicted in the form of super script, like a, b, c, &#8230; etc. The similar sub-shell for different shells is differentiated by writing the principal quantum number before the respective sub-shell.<\/p>\n<p><strong>b. <\/strong>Orbital diagram: In the second notation, each orbital of the sub-shell is represented by a box and the electron is represented by an arrow (<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?\\uparrow\" \/><\/span><\/span>) a positive spin or an arrow ( <code><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?\\downarrow\" \/><\/span><\/span><\/code>) a negative spin.<\/p>\n<h2><span class=\"ez-toc-section\" id=\"Structure_of_Atom_class_11_Notes\"><\/span>Structure of Atom class 11 Notes<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 11 Chemistry PDF<\/li>\n<li>CBSE Revision notes Class 11 Chemistry \u2013 CBSE<\/li>\n<li>CBSE Revisions notes and Key Points Class 11 Chemistry<\/li>\n<li>Summary of the NCERT books all chapters in Chemistry class 11<\/li>\n<li>Short notes for CBSE class 11th Chemistry<\/li>\n<li>Key notes and chapter summary of Chemistry class 11<\/li>\n<li>Quick revision notes for CBSE board exams<\/li>\n<\/ul>\n<h2><span class=\"ez-toc-section\" id=\"CBSE_Class-11_Revision_Notes_and_Key_Points\"><\/span><strong>CBSE Class-11 Revision Notes and Key Points<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>Structure of Atom class 11 Notes Chemistry. CBSE quick revision note for class-11 Chemistry, Physics, Maths, 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-11-physics\/1340\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Physics<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-chemistry\/1356\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Chemistry<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-mathematics\/1371\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Mathematics<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-biology\/1388\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Biology<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-accountancy\/1411\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Accountancy<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-economics\/1423\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Economics<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-business-studies\/1740\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Business Studies<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-computer-science\/1852\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Computer Science<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-informatics-practices\/1874\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Informatics Practices<\/a><\/li>\n<li><a href=\"http:\/\/mycbseguide.com\/downloads\/cbse-class-11-geography\/1864\/cbse-revision-notes\/7\/\">Revision Notes for class-11 Geography<\/a><\/li>\n<\/ul>\n<p>To download Structure of Atom class 11 Notes, sample paper for class 11 Chemistry, Physics, 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 solutions, NCERT Exemplar solutions, 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\/some-basic-concepts-of-chemistry-class-11-notes-chemistry\/\">Some Basic Concepts of Chemistry class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/structure-atom-class-11-notes-chemistry\/\">Structure of Atom class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/classification-elements-periodicity-properties-class-11-notes-chemistry\/\">Classification of Elements and Periodicity in Properties class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/chemical-bonding-and-molecular-structure-class-11-notes-chemistry\/\">Chemical Bonding and Molecular Structure class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/states-matter-class-11-notes-chemistry\/\">States of Matter class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/thermodynamics-class-11-notes-chemistry\/\">Thermodynamics class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/equilibrium-class-11-notes-chemistry\/\">Equilibrium class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/redox-reactions-class-11-notes-chemistry\/\">Redox Reactions class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/hydrogen-class-11-notes-chemistry\/\">Hydrogen class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/s-block-elements-class-11-notes-chemistry\/\">The s-Block Elements class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/the-p-block-elements-class-11-notes-chemistry\/\">The p-Block Elements class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/organic-chemistry-some-basic-principles-and-techniques-class-11-notes-chemistry\/\">Organic Chemistry \u2013 Some Basic Principles and Techniques class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/hydrocarbons-class-11-notes-chemistry\/\">Hydrocarbons class 11 Notes Chemistry<\/a><\/li>\n<li class=\"entry-title\"><a href=\"https:\/\/mycbseguide.com\/blog\/environmental-chemistry-class-11-notes-chemistry\/\">Environmental Chemistry class 11 Notes Chemistry<\/a><\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>CBSE Chemistry Chapter 2 Structure of Atom class 11 Notes Chemistry in PDF are available for free download in myCBSEguide mobile app. The best app for CBSE students now provides Structure of Atom class 11 Notes Chemistry latest chapter wise notes for quick preparation of CBSE exams and school based annual examinations. 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