{"id":4017,"date":"2026-03-30T10:44:17","date_gmt":"2026-03-30T10:44:17","guid":{"rendered":"https:\/\/ksquareinstitute.in\/blog\/?p=4017"},"modified":"2026-04-03T12:31:57","modified_gmt":"2026-04-03T12:31:57","slug":"chemical-bonding-class-11-notes","status":"publish","type":"post","link":"https:\/\/ksquareinstitute.in\/blog\/chemical-bonding-class-11-notes\/","title":{"rendered":"Chemical Bonding and Molecular Structure Class 11 Notes: The Ultimate Guide for NEET"},"content":{"rendered":"\n<!DOCTYPE html>\n<html lang=\"en\">\n<head>\n    <meta charset=\"UTF-8\">\n    <meta name=\"viewport\" content=\"width=device-width, initial-scale=1.0\">\n    <link rel=\"preconnect\" href=\"https:\/\/fonts.googleapis.com\">\n    <link rel=\"preconnect\" href=\"https:\/\/fonts.gstatic.com\" crossorigin>\n    <link href=\"https:\/\/fonts.googleapis.com\/css2?family=DM+Sans:ital,opsz,wght@0,9..40,300..600;1,9..40,300..600&#038;family=JetBrains+Mono:wght@400;500;700&#038;family=Plus+Jakarta+Sans:wght@400;600;700;800&#038;display=swap\" rel=\"stylesheet\">\n    <style>\n        :root {\n            --accent: #e8600a;\n            --accent-light: #fff3ec;\n            --accent-mid: #fde3cc;\n            --dark: #111827;\n            --text: #1a1a1a;\n            --text-muted: #4b5563;\n            --border: #e5e7eb;\n            --green-bg: #f0fdf4;\n            --green-border: #16a34a;\n            --blue-bg: #eff6ff;\n            --blue-border: #3b82f6;\n        }\n\n        * {\n            box-sizing: border-box;\n            margin: 0;\n            padding: 0;\n        }\n\n        body {\n            font-family: 'DM Sans', sans-serif;\n            color: var(--text);\n            line-height: 1.6;\n            background-color: #ffffff;\n            -webkit-font-smoothing: antialiased;\n        }\n\n        \/* Layout *\/\n        .content-wrapper {\n            width: 100%;\n            padding: 0;\n        }\n        \n        .container {\n            width: 100%;\n            padding: 0 0px;\n        }\n\n        @media (max-width: 768px) {\n            .container {\n                padding: 0 10px;\n            }\n        }\n\n        h2, h3, h4 {\n            font-family: 'Plus Jakarta Sans', sans-serif;\n            color: var(--dark);\n        }\n\n        h2 {\n            font-size: 1.85rem;\n            font-weight: 700;\n            margin: 40px 0 20px;\n            display: flex;\n            align-items: center;\n            gap: 16px;\n        }\n\n        p {\n            margin-bottom: 20px;\n            font-size: 1.05rem;\n            font-weight: 400;\n            color: var(--text-muted);\n        }\n\n        \/* Components *\/\n        .badge {\n            width: 42px;\n            height: 42px;\n            background-color: var(--accent);\n            color: white;\n            border-radius: 8px;\n            display: flex;\n            align-items: center;\n            justify-content: center;\n            font-weight: 700;\n            font-size: 1.1rem;\n            flex-shrink: 0;\n        }\n\n        .formula-dark {\n            background: var(--dark);\n            border-left: 4px solid var(--accent);\n            padding: 24px;\n            margin: 24px 0;\n            border-radius: 0 8px 8px 0;\n        }\n        .formula-dark-label {\n            font-family: 'JetBrains Mono', monospace;\n            font-size: 0.75rem;\n            color: #9ca3af;\n            text-transform: uppercase;\n            letter-spacing: 1px;\n            margin-bottom: 8px;\n            display: block;\n        }\n        .formula-dark-content {\n            font-family: 'JetBrains Mono', monospace;\n            color: var(--accent);\n            font-size: 1.1rem;\n            font-weight: 500;\n        }\n\n        .formula-orange {\n            background: var(--accent-light);\n            border: 1px solid var(--accent-mid);\n            border-left: 4px solid var(--accent);\n            padding: 24px;\n            margin: 24px 0;\n            border-radius: 0 8px 8px 0;\n        }\n        .formula-orange-content {\n            font-family: 'JetBrains Mono', monospace;\n            color: #851e00;\n            font-size: 1.1rem;\n            font-weight: 500;\n        }\n\n        .callout {\n            padding: 20px;\n            border-radius: 12px;\n            margin: 24px 0;\n            border: 1px solid;\n            position: relative;\n        }\n        .callout-pill {\n            position: absolute;\n            top: -12px;\n            left: 20px;\n            padding: 4px 12px;\n            border-radius: 50px;\n            font-size: 0.7rem;\n            font-weight: 700;\n            text-transform: uppercase;\n            letter-spacing: 0.5px;\n        }\n\n        .warning { background: #fff7ed; 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color: var(--accent); }\n        .btn-outline { border: 2px solid white; color: white; }\n\n        .internal-links {\n            background: #f9fafb;\n            border: 1px solid var(--border);\n            border-radius: 10px;\n            padding: 24px;\n            margin: 40px 0;\n        }\n        .internal-links-title {\n            color: var(--text-muted);\n            font-weight: 700;\n            font-size: 0.9rem;\n            margin-bottom: 16px;\n            display: block;\n        }\n        .internal-links a {\n            display: block;\n            color: var(--accent);\n            text-decoration: none;\n            font-weight: 600;\n            margin-bottom: 8px;\n        }\n\n        .download-btn {\n            background: var(--dark);\n            color: white;\n            display: inline-flex;\n            align-items: center;\n            gap: 10px;\n            padding: 12px 24px;\n            border-radius: 8px;\n            text-decoration: none;\n            font-weight: 600;\n            margin-top: 20px;\n        }\n    <\/style>\n<\/head>\n<body>\n\n<div class=\"content-wrapper\">\n    <div class=\"container\">\n        \n        <p>Mastering chemical bonding is critical for scoring high in the NEET Chemistry section. These <strong>chemical bonding class 11 notes<\/strong> cover everything from octet rules to Molecular Orbital Theory. Understanding how atoms combine to form molecules is the foundation for both Inorganic and Organic Chemistry preparation.<\/p>\n\n        <h2><div class=\"badge\">01<\/div>Introduction to Chemical Bonding<\/h2>\n        <p>Chemical bonding is the attractive force that holds constituent particles (atoms, ions, or molecules) together in different chemical species. Atoms combine to achieve a stable electronic configuration, specifically to attain the nearest noble gas configuration with a complete valence shell.<\/p>\n        \n        <div class=\"card-grid\">\n            <div class=\"card\">\n                <span class=\"card-title\">PRIMARY DRIVER<\/span>\n                Atoms combine to minimize potential energy and achieve maximum stability.\n            <\/div>\n            <div class=\"card\">\n                <span class=\"card-title\">OCTET RULE<\/span>\n                Most atoms tend to have eight electrons in their outermost shell (ns<sup>2<\/sup> np<sup>6<\/sup>).\n            <\/div>\n        <\/div>\n\n        <div class=\"callout tip\">\n            <div class=\"callout-pill\">TIP<\/div>\n            Remember that bonding is always an exothermic process (energy is released) because the system moves from a higher energy state to a lower, more stable energy state.\n        <\/div>\n\n        <h2><div class=\"badge\">02<\/div>Kossel\u2013Lewis Approach to Chemical Bonding<\/h2>\n        <p>According to this approach, atoms achieve the stable octet by either transferring electrons (ionic bond) or sharing electrons (covalent bond). While this rule is fundamental in <strong>chemical bonding class 11 notes<\/strong>, it has several notable exceptions that frequently appear in NEET exams.<\/p>\n\n        <div class=\"formula-dark\">\n            <span class=\"formula-dark-label\">REPRESENTATION<\/span>\n            <div class=\"formula-dark-content\">Lewis Dot Structures: Valence electrons are represented as dots around the atomic symbol.<\/div>\n        <\/div>\n\n        <h3>Limitations of the Octet Rule<\/h3>\n        <ul>\n            <li><strong>Incomplete Octet:<\/strong> BeCl<sub>2<\/sub> (Be has 4e<sup>\u2212<\/sup>), BF<sub>3<\/sub> (B has 6e<sup>\u2212<\/sup>).<\/li>\n            <li><strong>Expanded Octet:<\/strong> Elements in the 3rd period and beyond (PCl<sub>5<\/sub>, SF<sub>6<\/sub>, IF<sub>7<\/sub>).<\/li>\n            <li><strong>Odd Electron Molecules:<\/strong> NO and NO<sub>2<\/sub> have unpaired electrons.<\/li>\n        <\/ul>\n\n        <h2><div class=\"badge\">03<\/div>Ionic Bonding (Electrovalent Bond)<\/h2>\n        <p>The electrostatic force of attraction between a cation and an anion is called an ionic bond. Its formation depends on several energetic factors including lattice and ionization enthalpies.<\/p>\n        \n        <div class=\"formula-orange\">\n            <div class=\"formula-orange-content\">Factors favoring Ionic Bond: Low Ionization Enthalpy (Cation) + High Negative Electron Gain Enthalpy (Anion) + High Lattice Enthalpy.<\/div>\n        <\/div>\n\n        <div class=\"table-container\">\n            <table>\n                <thead>\n                    <tr>\n                        <th>Property<\/th>\n                        <th>Ionic Compounds<\/th>\n                        <th>Covalent Compounds<\/th>\n                    <\/tr>\n                <\/thead>\n                <tbody>\n                    <tr>\n                        <td>Physical State<\/td>\n                        <td>Crystalline Solids<\/td>\n                        <td>Gases, Liquids, or Soft Solids<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>Conductivity<\/td>\n                        <td>Only in Molten\/Aqueous State<\/td>\n                        <td>Generally Insulators<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>Boiling Point<\/td>\n                        <td>Very High<\/td>\n                        <td>Low to Moderate<\/td>\n                    <\/tr>\n                <\/tbody>\n            <\/table>\n        <\/div>\n\n        <!-- Promotional Banner 1 -->\n        <a href=\"https:\/\/courses.ksquare.co.in\/new-courses\/3-mission-180-neet-physics-rankers-batch\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" style=\"display:block; margin-bottom:40px;\">\n            <img decoding=\"async\" src=\"https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/03\/Course-Poromo-Banner-scaled.png\" alt=\"Mission 180 NEET Physics Rankers Batch - KSquare Career Institute\" style=\"width:100%; height:auto; border-radius:10px; display:block;\">\n        <\/a>\n\n        <h2><div class=\"badge\">04<\/div>Covalent Bonding and Lewis Structures<\/h2>\n        <p>In covalent bonding, atoms share electron pairs to satisfy their octets. A key concept here is the <strong>Formal Charge<\/strong>, which helps in identifying the most stable Lewis structure for a molecule.<\/p>\n\n        <div class=\"formula-dark\">\n            <span class=\"formula-dark-label\">FORMAL CHARGE CALCULATION<\/span>\n            <div class=\"formula-dark-content\">F.C. = [Total valence e<sup>\u2212<\/sup>] \u2212 [Non-bonding e<sup>\u2212<\/sup>] \u2212 1\/2[Bonding e<sup>\u2212<\/sup>]<\/div>\n        <\/div>\n\n        <div class=\"callout warning\">\n            <div class=\"callout-pill\">WARN<\/div>\n            Formal charge does not represent the real charge on the atom; it is a bookkeeping method to compare the stability of different resonance structures.\n        <\/div>\n\n        <h2><div class=\"badge\">05<\/div>Bond Parameters<\/h2>\n        <p>Quantitative values describing a bond are essential for solving theoretical NEET questions on <strong>chemical bonding class 11 notes<\/strong>.<\/p>\n        \n        <div class=\"card-grid\">\n            <div class=\"card\">\n                <span class=\"card-title\">BOND ORDER<\/span>\n                Number of bonds between two atoms. For N<sub>2<\/sub>, Bond Order = 3.\n            <\/div>\n            <div class=\"card\">\n                <span class=\"card-title\">RELATIONSHIP<\/span>\n                Bond Order \u221d 1\/Bond Length \u221d Bond Enthalpy.\n            <\/div>\n        <\/div>\n\n        <h2><div class=\"badge\">06<\/div>VSEPR Theory: Predicting Molecular Geometry<\/h2>\n        <p>Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the shape of molecules based on the repulsion between electron pairs.<\/p>\n\n        <div class=\"formula-orange\">\n            <div class=\"formula-orange-content\">Order of Repulsion: Lone Pair &#8211; Lone Pair (lp-lp) > Lone Pair &#8211; Bond Pair (lp-bp) > Bond Pair &#8211; Bond Pair (bp-bp).<\/div>\n        <\/div>\n\n        <div class=\"table-container\">\n            <table>\n                <thead>\n                    <tr>\n                        <th>Hybridization<\/th>\n                        <th>Geometry<\/th>\n                        <th>Example<\/th>\n                        <th>Bond Angle<\/th>\n                    <\/tr>\n                <\/thead>\n                <tbody>\n                    <tr>\n                        <td>sp<\/td>\n                        <td>Linear<\/td>\n                        <td>BeCl<sub>2<\/sub>, CO<sub>2<\/sub><\/td>\n                        <td>180\u00b0<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>sp<sup>2<\/sup><\/td>\n                        <td>Trigonal Planar<\/td>\n                        <td>BF<sub>3<\/sub><\/td>\n                        <td>120\u00b0<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>sp<sup>3<\/sup><\/td>\n                        <td>Tetrahedral<\/td>\n                        <td>CH<sub>4<\/sub>, NH<sub>3<\/sub> (1 lp)<\/td>\n                        <td>109.5\u00b0<\/td>\n                    <\/tr>\n                    <tr>\n                        <td>sp<sup>3<\/sup>d<\/td>\n                        <td>Trigonal Bipyramidal<\/td>\n                        <td>PCl<sub>5<\/sub><\/td>\n                        <td>90\u00b0 &#038; 120\u00b0<\/td>\n                    <\/tr>\n                <\/tbody>\n            <\/table>\n        <\/div>\n\n        <h2><div class=\"badge\">07<\/div>Valence Bond Theory (VBT) and Overlap<\/h2>\n        <p>VBT explains bonding through the overlap of atomic orbitals. Two types of bonds are formed: Sigma (\u03c3) and Pi (\u03c0). Sigma bonds result from head-on overlap, whereas Pi bonds result from lateral overlap. Sigma bonds are stronger than Pi bonds.<\/p>\n\n        <!-- Promotional Banner 2 -->\n        <a href=\"https:\/\/ksquareinstitute.in\/neet-2026-rank-predictor\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" style=\"display:block; margin-bottom:40px;\">\n            <img decoding=\"async\" src=\"https:\/\/ksquareinstitute.in\/blog\/wp-content\/uploads\/2026\/03\/neet-2026-college-and-rank-predictor-scaled.png\" alt=\"NEET 2026 Rank Predictor - KSquare Career Institute\" style=\"width:100%; height:auto; border-radius:10px; display:block;\">\n        <\/a>\n\n        <h2><div class=\"badge\">08<\/div>Hybridization<\/h2>\n        <p>Hybridization is the intermixing of atomic orbitals of slightly different energies to produce a new set of equivalent orbitals.<\/p>\n        \n        <div class=\"formula-dark\">\n            <span class=\"formula-dark-label\">STERIC NUMBER FORMULA<\/span>\n            <div class=\"formula-dark-content\">H = 1\/2 [V + M \u2212 C + A]<\/div>\n        <\/div>\n\n        <h2><div class=\"badge\">09<\/div>Molecular Orbital Theory (MOT)<\/h2>\n        <p>MOT is the most advanced concept in <strong>chemical bonding class 11 notes<\/strong>. It explains the magnetic properties of molecules (like why O<sub>2<\/sub> is paramagnetic).<\/p>\n\n        <div class=\"formula-orange\">\n            <div class=\"formula-orange-content\">Bond Order = 1\/2 [N<sub>b<\/sub> \u2212 N<sub>a<\/sub>]<\/div>\n        <\/div>\n\n        <div class=\"internal-links\">\n            <span class=\"internal-links-title\">RESOURCES FOR NEET PREPARATION<\/span>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-physics-survival-kit-2026\/\">NEET Physics Survival Kit 2026<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/organic-chemistry-strategy-neet\/\">Organic Chemistry Strategy for NEET<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-biology-tricks-for-exams\/\">Biology Mnemonics &#038; Tricks<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/blog\/score-340-in-neet-biology\/\">How to Score 340+ in Biology<\/a>\n            <a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\">Free NEET Study Material<\/a>\n        <\/div>\n\n        <div class=\"revision-box\">\n            <h3>Quick Revision Summary<\/h3>\n            <ul>\n                <li>Dipole Moment (\u03bc) = Charge (Q) \u00d7 Distance (r).<\/li>\n                <li>Polarity depends on the vector sum of individual bond moments.<\/li>\n                <li>H-bonding: Strongly electronegative elements (F, O, N) attached to Hydrogen.<\/li>\n                <li>Lattice Enthalpy \u221d (Charge 1 \u00d7 Charge 2) \/ (Radius 1 + Radius 2).<\/li>\n                <li>Paramagnetic substances have unpaired electrons in MOs.<\/li>\n                <li>Diamagnetic substances have all paired electrons.<\/li>\n                <li>% Ionic Character = 16|\u0394\u03c7| + 3.5|\u0394\u03c7|<sup>2<\/sup>.<\/li>\n                <li>VSEPR predicts Shape; Hybridization predicts Geometry.<\/li>\n            <\/ul>\n            <a href=\"#\" class=\"download-btn\" rel=\"nofollow noopener noreferrer\">\n                <span>Download Formula Sheet (PDF)<\/span>\n            <\/a>\n        <\/div>\n\n        <h2><div class=\"badge\">10<\/div>Frequently Asked Questions<\/h2>\n        <div class=\"faq-container\">\n            <details>\n                <summary>\n                    <span>Why is BF<sub>3<\/sub> non-polar despite polar B-F bonds?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">BF<sub>3<\/sub> has a symmetrical trigonal planar geometry. The vector sum of the three B-F bond dipoles is zero, making the net dipole moment \u03bc = 0.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>How does a lone pair affect the bond angle?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">Lone pairs occupy more space and exert greater repulsion on bond pairs. This causes the bond pairs to push closer together, reducing the bond angle (e.g., CH<sub>4<\/sub> is 109.5\u00b0 while NH<sub>3<\/sub> is 107\u00b0).<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>What is the bond order of O<sub>2<\/sub> and O<sub>2<\/sub><sup>+<\/sup>?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">The bond order of O<sub>2<\/sub> is 2. When it loses an electron to form O<sub>2<\/sub><sup>+<\/sup>, the electron is removed from an anti-bonding orbital, increasing the bond order to 2.5.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>What are the conditions for Hydrogen bonding?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">1. Hydrogen must be bonded to a highly electronegative atom (F, O, or N). 2. The electronegative atom must be small in size to provide concentrated charge density.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>Is every molecule with an expanded octet unstable?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">No. Molecules like SF<sub>6<\/sub> and PCl<sub>5<\/sub> are very stable because the central atom can use its d-orbitals to accommodate more than 8 electrons.<\/div>\n            <\/details>\n            <details>\n                <summary>\n                    <span>What is the main difference between Sigma and Pi bonds?<\/span>\n                    <div class=\"toggle-icon\">\n                        <svg viewBox=\"0 0 24 24\"><path class=\"plus-path\" d=\"M12 5v14M5 12h14\"\/><path class=\"minus-path\" d=\"M5 12h14\"\/><\/svg>\n                    <\/div>\n                <\/summary>\n                <div class=\"faq-answer\">Sigma bonds are formed by end-to-end overlap and allow free rotation, while Pi bonds are formed by lateral overlap and prevent rotation around the bond axis.<\/div>\n            <\/details>\n        <\/div>\n\n        <div class=\"cta-section\">\n            <h2>Ready to Ace NEET Chemistry?<\/h2>\n            <p>Join thousands of students who have transformed their preparation with KSquare Institute&#8217;s expert-led batches and rank-boosting strategies.<\/p>\n            <div class=\"cta-buttons\">\n                <a href=\"https:\/\/courses.ksquare.co.in\/new-courses\/3-mission-180-neet-physics-rankers-batch\" class=\"btn btn-white\" target=\"_blank\" rel=\"nofollow noopener noreferrer\">Join Rankers Batch<\/a>\n                <a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" class=\"btn btn-outline\" target=\"_blank\" rel=\"nofollow noopener noreferrer\">Free Practice Questions<\/a>\n            <\/div>\n        <\/div>\n    <\/div>\n<\/div>\n\n<\/body>\n<\/html>\n\n\n\n<!DOCTYPE html>\n<html lang=\"en\">\n<head>\n  <meta charset=\"UTF-8\">\n  <meta name=\"viewport\" content=\"width=device-width, initial-scale=1.0\">\n  <title>Table of Contents \u2014 Chemistry Class 11<\/title>\n  \n  <!-- Google Fonts Import -->\n  <link rel=\"preconnect\" href=\"https:\/\/fonts.googleapis.com\">\n  <link rel=\"preconnect\" href=\"https:\/\/fonts.gstatic.com\" crossorigin>\n  <link href=\"https:\/\/fonts.googleapis.com\/css2?family=DM+Sans:ital,opsz,wght@0,9..40,100..1000;1,9..40,100..1000&#038;family=Plus+Jakarta+Sans:ital,wght@0,200..800;1,200..800&#038;display=swap\" rel=\"stylesheet\">\n  \n  <style>\n    \/* Scoped wrapper using a unique ID to prevent CSS conflicts. *\/\n    #chemistry-toc-wrapper {\n      font-family: 'DM Sans', sans-serif;\n      width: 100%;\n      margin: 0;\n      padding: 60px 0;\n      color: #111;\n      background: #fff;\n      -webkit-font-smoothing: antialiased;\n    }\n\n    #chemistry-toc-wrapper .container-inner {\n      width: 100%;\n      margin: 0 auto;\n      padding: 0; \/* No left\/right padding for edge-to-edge look *\/\n    }\n\n    #chemistry-toc-wrapper h1 {\n      font-family: 'Plus Jakarta Sans', sans-serif;\n      font-size: 0.85rem;\n      font-weight: 700;\n      color: #71717a;\n      margin: 0 0 8px;\n      letter-spacing: 0.1em;\n      text-transform: uppercase;\n      padding-left: 16px; \n    }\n\n    #chemistry-toc-wrapper h2 {\n      font-family: 'Plus Jakarta Sans', sans-serif;\n      font-size: 2.25rem;\n      font-weight: 800;\n      margin: 0 0 48px;\n      letter-spacing: -0.02em;\n      color: #09090b;\n      padding-left: 16px;\n    }\n\n    #chemistry-toc-wrapper table {\n      width: 100%;\n      border-collapse: collapse;\n      border-spacing: 0;\n      border-top: 1px solid #e4e4e7;\n      border-bottom: 1px solid #e4e4e7;\n    }\n\n    #chemistry-toc-wrapper tr {\n      border-bottom: 1px solid #e4e4e7;\n      transition: all 0.2s ease;\n    }\n\n    #chemistry-toc-wrapper tr:hover {\n      background-color: #f8fafc;\n    }\n\n    #chemistry-toc-wrapper tr:last-child {\n      border-bottom: none;\n    }\n\n    #chemistry-toc-wrapper td {\n      padding: 24px 16px;\n      vertical-align: middle;\n      font-size: 1.05rem;\n      font-weight: 500;\n      border-right: 1px solid #e4e4e7;\n    }\n\n    #chemistry-toc-wrapper td:last-child {\n      border-right: none;\n    }\n\n    \/* First column (Numbers) alignment and padding *\/\n    #chemistry-toc-wrapper td:first-child {\n      color: #a1a1aa;\n      font-size: 0.9rem;\n      width: 70px;\n      font-weight: 400;\n      font-variant-numeric: tabular-nums;\n      text-align: center;\n      padding-left: 10px;\n    }\n\n    \/* Middle column (Chapter Name) alignment and padding *\/\n    #chemistry-toc-wrapper td:nth-child(2) {\n      padding-left: 24px;\n      color: #18181b;\n    }\n\n    \/* Last column (Button) alignment and padding *\/\n    #chemistry-toc-wrapper td:last-child {\n      text-align: right;\n      width: 180px;\n      padding-right: 16px;\n    }\n\n    \/* Button Styling *\/\n    #chemistry-toc-wrapper a.go {\n      display: inline-block;\n      font-family: 'Plus Jakarta Sans', sans-serif;\n      font-size: 0.75rem;\n      font-weight: 800;\n      padding: 12px 24px;\n      border: 1.5px solid #18181b;\n      border-radius: 8px;\n      color: #18181b;\n      text-decoration: none;\n      letter-spacing: 0.05em;\n      text-transform: uppercase;\n      transition: all 0.2s cubic-bezier(0.4, 0, 0.2, 1);\n      white-space: nowrap;\n    }\n\n    #chemistry-toc-wrapper a.go:hover {\n      background: #18181b;\n      color: #ffffff;\n      transform: translateY(-2px);\n      box-shadow: 0 4px 12px rgba(24, 24, 27, 0.15);\n    }\n\n    \/* Responsive adjustments *\/\n    @media (max-width: 768px) {\n      #chemistry-toc-wrapper h2 {\n        font-size: 1.75rem;\n        margin-bottom: 32px;\n      }\n      #chemistry-toc-wrapper td {\n        padding: 18px 12px;\n        font-size: 0.95rem;\n      }\n    }\n  <\/style>\n<\/head>\n<body>\n\n<div id=\"chemistry-toc-wrapper\">\n  <div class=\"container-inner\">\n    <h1>Table of Contents<\/h1>\n    <h2>Chemistry &mdash; Class 11<\/h2>\n    \n    <table>\n      <tr><td>01<\/td><td>Some Basic Concepts of Chemistry<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/some-basic-concepts-of-chemistry-class-11\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>02<\/td><td>Structure of Atom<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/structure-of-atom-class-11\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>03<\/td><td>Classification of Elements and Periodicity<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/periodic-table-class-11-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>04<\/td><td>Chemical Bonding and Molecular Structure<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/chemical-bonding-class-11-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>05<\/td><td>Thermodynamics<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/thermodynamics-chemistry-class-11-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>06<\/td><td>Equilibrium<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/equilibrium-chemistry-class-11-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>07<\/td><td>Redox Reactions<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/redox-reactions-chemistry-class-11-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>08<\/td><td>Organic Chemistry &mdash; Basic Principles<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/organic-chemistry-basic-principles-class-11\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n      <tr><td>09<\/td><td>Hydrocarbons<\/td><td><a class=\"go\" href=\"https:\/\/ksquareinstitute.in\/blog\/hydrocarbons-class-11-notes-pdf\" target=\"_blank\">Go to page<\/a><\/td><\/tr>\n    <\/table>\n  <\/div>\n<\/div>\n\n<\/body>\n<\/html>\n","protected":false},"excerpt":{"rendered":"<p>Mastering chemical bonding is critical for scoring high in the NEET Chemistry section. These chemical bonding class 11 notes cover everything from octet rules to Molecular Orbital Theory. Understanding how atoms combine to form molecules is the foundation for both Inorganic and Organic Chemistry preparation. 01 Introduction to Chemical Bonding Chemical bonding is the attractive [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[127],"tags":[311,312,315,314,313],"class_list":["post-4017","post","type-post","status-publish","format-standard","hentry","category-free-study-material","tag-chemical-bonding-class-11-notes","tag-hybridization-class-11","tag-molecular-orbital-theory-class-11","tag-molecular-structure-class-11","tag-vsepr-theory-class-11"],"blocksy_meta":{"page_structure_type":"type-1","styles_descriptor":{"styles":{"desktop":"","tablet":"","mobile":""},"google_fonts":[],"version":6}},"_links":{"self":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4017","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/comments?post=4017"}],"version-history":[{"count":2,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4017\/revisions"}],"predecessor-version":[{"id":4235,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4017\/revisions\/4235"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=4017"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=4017"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=4017"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}