Periodic Table Class 11 Notes PDF – Comprehensive NEET Study Guide<\/title>\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&family=JetBrains+Mono:wght@400;500;700&family=Plus+Jakarta+Sans:wght@400;600;700;800&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 body {\n margin: 0;\n padding: 0;\n font-family: 'DM Sans', sans-serif;\n color: var(--text);\n line-height: 1.6;\n background-color: #ffffff;\n }\n\n .content-wrapper {\n width: 100%;\n padding: 0;\n }\n\n .inner-container {\n padding: 0 0px;\n }\n\n @media (max-width: 768px) {\n .inner-container { padding: 0 10px; 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font-weight: 700; }\n .btn-outline { border: 2px solid white; color: white; padding: 10px 28px; border-radius: 6px; text-decoration: none; font-weight: 700; }\n\n .internal-links {\n background: #f9fafb;\n border: 1px solid var(--border);\n border-radius: 10px;\n padding: 20px;\n margin: 30px 0;\n }\n .internal-links span { display: block; color: var(--text-muted); font-weight: 700; margin-bottom: 10px; font-size: 0.9rem; }\n .internal-links a { color: var(--accent); text-decoration: none; font-weight: 600; display: block; margin-bottom: 5px; }\n\n .download-btn {\n background: var(--dark);\n color: white;\n text-decoration: none;\n display: inline-flex;\n align-items: center;\n gap: 10px;\n padding: 12px 24px;\n border-radius: 8px;\n font-weight: 600;\n margin: 20px 0;\n }\n <\/style>\n<\/head>\n<body>\n\n<div class=\"content-wrapper\">\n <div class=\"inner-container\">\n \n <p>Mastering the <strong>periodic table class 11 notes pdf<\/strong> is the first step toward a perfect score in Inorganic Chemistry for NEET. The chapter “Classification of Elements and Periodicity in Properties” serves as the foundation for chemical bonding, p-block, d-block, and s-block elements. In this guide, we break down the complexities of electronic configurations, periodic trends, and exceptions that frequently appear in the exam.<\/p>\n\n <div class=\"section-header\">\n <div class=\"badge\">01<\/div>\n <h2>Introduction to Classification of Elements<\/h2>\n <\/div>\n \n <p>With 118 elements known today, studying them individually is impossible. The classification organizes elements into groups and periods based on their similarities, allowing chemists to predict properties. The modern periodic table is not just a list but a logical map of atomic structure.<\/p>\n \n <div class=\"grid-cards\">\n <div class=\"mini-card\">\n <span>BASIS OF CLASSIFICATION<\/span>\n <p>The fundamental shift happened from using Atomic Mass (Mendeleev) to Atomic Number (Moseley).<\/p>\n <\/div>\n <div class=\"mini-card\">\n <span>WHY IT MATTERS<\/span>\n <p>It explains the physical and chemical behavior of elements based on their electron configurations.<\/p>\n <\/div>\n <\/div>\n\n <div class=\"section-header\">\n <div class=\"badge 02\">02<\/div>\n <h2>Early Classifications of Elements<\/h2>\n <\/div>\n\n <h3>Dobereiner\u2019s Triads<\/h3>\n <p>In 1817, Johann Dobereiner arranged elements in groups of three (triads). The atomic mass of the middle element was approximately the arithmetic mean of the other two.<\/p>\n \n <div class=\"formula-orange\">\n <p>Example: Li (7), Na (23), K (39) <br> Mean: (7 + 39) \/ 2 = 23<\/p>\n <\/div>\n\n <h3>Newlands\u2019 Law of Octaves<\/h3>\n <p>John Newlands proposed that when elements are arranged in increasing order of atomic masses, every eighth element has properties similar to the first, similar to musical notes. However, this law only worked up to Calcium (Ca).<\/p>\n\n <h3>Mendeleev\u2019s Periodic Table<\/h3>\n <p>Dmitri Mendeleev formulated the Periodic Law: “The properties of elements are periodic functions of their atomic masses.”<\/p>\n <ul>\n <li><strong>Achievements:<\/strong> He left gaps for undiscovered elements like Eka-boron (Scandium), Eka-aluminium (Gallium), and Eka-silicon (Germanium).<\/li>\n <li><strong>Limitations:<\/strong> It could not explain the position of isotopes, the placement of Hydrogen, or the anomalous pairs like Cobalt (58.9) before Nickel (58.7).<\/li>\n <\/ul>\n\n <div class=\"section-header\">\n <div class=\"badge\">03<\/div>\n <h2>Modern Periodic Law and Structure<\/h2>\n <\/div>\n\n <p>The <strong>Modern Periodic Law<\/strong>, proposed by Henry Moseley, states that the physical and chemical properties of elements are periodic functions of their <strong>atomic number (Z)<\/strong>. This resolved the discrepancies found in Mendeleev’s mass-based table.<\/p>\n\n <div class=\"callout-tip\">\n <div class=\"pill-tip\">TIP<\/div>\n <p>Always remember: It is the electronic configuration of an atom that determines its position in the modern periodic table, not its mass!<\/p>\n <\/div>\n\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:20px;\">\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 <div class=\"section-header\">\n <div class=\"badge\">04<\/div>\n <h2>Electronic Configuration and Periodic Table<\/h2>\n <\/div>\n\n <p>The table is divided into four main blocks based on the orbital being filled by the last electron:<\/p>\n \n <table>\n <thead>\n <tr>\n <th>Block<\/th>\n <th>Groups<\/th>\n <th>General Configuration<\/th>\n <th>Properties<\/th>\n <\/tr>\n <\/thead>\n <tbody>\n <tr>\n <td>s-block<\/td>\n <td>1 & 2<\/td>\n <td>ns<sup>1-2<\/sup><\/td>\n <td>Highly reactive metals, low IE<\/td>\n <\/tr>\n <tr>\n <td>p-block<\/td>\n <td>13 to 18<\/td>\n <td>ns<sup>2<\/sup>np<sup>1-6<\/sup><\/td>\n <td>Contains metals, non-metals, metalloids<\/td>\n <\/tr>\n <tr>\n <td>d-block<\/td>\n <td>3 to 12<\/td>\n <td>(n-1)d<sup>1-10<\/sup>ns<sup>1-2<\/sup><\/td>\n <td>Transition metals, colored ions<\/td>\n <\/tr>\n <tr>\n <td>f-block<\/td>\n <td>Bottom Rows<\/td>\n <td>(n-2)f<sup>1-14<\/sup>(n-1)d<sup>0-1<\/sup>ns<sup>2<\/sup><\/td>\n <td>Inner transition elements (Lanthanoids\/Actinoids)<\/td>\n <\/tr>\n <\/tbody>\n <\/table>\n\n <div class=\"section-header\">\n <div class=\"badge\">05<\/div>\n <h2>Periodic Trends in Properties (NEET High-Weightage)<\/h2>\n <\/div>\n\n <p>Understanding trends is crucial for solving conceptual questions in your <strong>periodic table class 11 notes pdf<\/strong>. These trends are governed by Effective Nuclear Charge (Z<sub>eff<\/sub>) and Shielding Effect.<\/p>\n\n <h3>1. Atomic Radius<\/h3>\n <p>Atomic radius generally decreases across a period due to increased Z<sub>eff<\/sub> pulling electrons closer. It increases down a group as new shells are added.<\/p>\n \n <div class=\"callout-warning\">\n <div class=\"pill-warn\">WARN<\/div>\n <p>Van der Waals radius is always larger than Metallic or Covalent radius for the same element because it involves non-bonded distances.<\/p>\n <\/div>\n\n <h3>2. Ionization Enthalpy (\u0394<sub>i<\/sub>H)<\/h3>\n <p>The energy required to remove an electron from an isolated gaseous atom.<\/p>\n \n <div class=\"formula-dark\">\n <span>Factors Affecting \u0394<sub>i<\/sub>H<\/span>\n <p>\u0394<sub>i<\/sub>H \u221d (Nuclear Charge \/ Atomic Size)<\/p>\n <\/div>\n\n <div class=\"grid-cards\">\n <div class=\"mini-card\">\n <span>EXCEPTION: N vs O<\/span>\n <p>Nitrogen (half-filled 2p<sup>3<\/sup>) has higher IE than Oxygen (2p<sup>4<\/sup>) due to extra stability.<\/p>\n <\/div>\n <div class=\"mini-card\">\n <span>EXCEPTION: Be vs B<\/span>\n <p>Beryllium (full-filled 2s<sup>2<\/sup>) has higher IE than Boron (2p<sup>1<\/sup>).<\/p>\n <\/div>\n <\/div>\n\n <h3>3. Electron Gain Enthalpy (\u0394<sub>eg<\/sub>H)<\/h3>\n <p>Across a period, \u0394<sub>eg<\/sub>H becomes more negative (except noble gases which are positive). Down a group, it usually becomes less negative.<\/p>\n \n <div class=\"callout-tip\">\n <div class=\"pill-tip\">TIP<\/div>\n <p>Chlorine (Cl) has a more negative electron gain enthalpy than Fluorine (F) because F is so small that inter-electronic repulsions hinder the incoming electron.<\/p>\n <\/div>\n\n <div class=\"section-header\">\n <div class=\"badge\">06<\/div>\n <h2>Periodic Trends in Chemical Properties<\/h2>\n <\/div>\n\n <p>Trends in chemical reactivity are also predictable. Metallic character increases down the group while non-metallic character increases across the period.<\/p>\n \n <ul>\n <li><strong>Oxide Nature:<\/strong> Basic oxides (e.g., Na<sub>2<\/sub>O) are formed by metals on the left. Acidic oxides (e.g., Cl<sub>2<\/sub>O<sub>7<\/sub>) are formed by non-metals on the right. Amphoteric oxides include Al<sub>2<\/sub>O<sub>3<\/sub>.<\/li>\n <li><strong>Valency:<\/strong> Across a period, it increases from 1 to 4 and then decreases to 0 (for noble gases) with respect to hydrogen.<\/li>\n <\/ul>\n\n <div class=\"section-header\">\n <div class=\"badge\">07<\/div>\n <h2>Anomalous Properties and Diagonal Relationship<\/h2>\n <\/div>\n\n <p>The first element of each group (Li, Be, B) shows different behavior than its peers due to extremely small size, high IE, and absence of d-orbitals. Furthermore, some second-period elements show similarities with third-period elements placed diagonally.<\/p>\n \n <div class=\"grid-cards\">\n <div class=\"mini-card\">\n <span>DIAGONAL PAIRS<\/span>\n <p>Li & Mg, Be & Al, B & Si<\/p>\n <\/div>\n <div class=\"mini-card\">\n <span>REASON<\/span>\n <p>Similar ionic size and polarizing power (Charge\/Radius ratio).<\/p>\n <\/div>\n <\/div>\n\n <a href=\"https:\/\/ksquareinstitute.in\/neet-2026-rank-predictor\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" style=\"display:block; margin-bottom:20px;\">\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 <div class=\"section-header\">\n <div class=\"badge\">08<\/div>\n <h2>Summary of Periodic Trends (Quick Revision)<\/h2>\n <\/div>\n\n <div class=\"revision-box\">\n <h3>Key Revision Points<\/h3>\n <ul>\n <li>Atomic Radius: Decreases \u2192 (Period), Increases \u2193 (Group)<\/li>\n <li>Ionization Energy: Increases \u2192 (Period), Decreases \u2193 (Group)<\/li>\n <li>Electronegativity: Increases \u2192 (Period), Decreases \u2193 (Group)<\/li>\n <li>Electron Affinity: More Negative \u2192 (Period), Less Negative \u2193 (Group)<\/li>\n <li>Non-metallic Character: Increases \u2192 (Period), Decreases \u2193 (Group)<\/li>\n <li>Metallic Character: Decreases \u2192 (Period), Increases \u2193 (Group)<\/li>\n <li>Effective Nuclear Charge (Z<sub>eff<\/sub>): Increases across a period<\/li>\n <li>Screening Effect: Increases down a group<\/li>\n <li>Oxidizing Power: Increases across a period<\/li>\n <li>Reducing Power: Increases down a group<\/li>\n <\/ul>\n <\/div>\n\n <a href=\"#\" rel=\"nofollow noopener noreferrer\" class=\"download-btn\">\n Download Periodic Table Notes PDF\n <\/a>\n\n <div class=\"section-header\">\n <div class=\"badge\">09<\/div>\n <h2>Important Exam Focus & Exceptions<\/h2>\n <\/div>\n\n <p>NEET focuses heavily on exceptions. Ensure you have these noted down in your <strong>periodic table class 11 notes pdf<\/strong>:<\/p>\n \n <div class=\"formula-orange\">\n <p>Electronegativity Order: F > O > Cl > N <br> (Note: Cl and N have similar values but Cl is often considered more electronegative in certain scales).<\/p>\n <\/div>\n\n <div class=\"callout-warning\">\n <div class=\"pill-warn\">WARN<\/div>\n <p>Noble gases have the highest Ionization Enthalpy in their respective periods due to their stable ns<sup>2<\/sup>np<sup>6<\/sup> configuration.<\/p>\n <\/div>\n\n <div class=\"section-header\">\n <div class=\"badge\">10<\/div>\n <h2>Frequently Asked Questions (FAQs)<\/h2>\n <\/div>\n\n <details>\n <summary>Why does Chlorine have more negative electron gain enthalpy than Fluorine?<\/summary>\n <div class=\"faq-answer\">Fluorine is very small. When an electron is added, it experiences significant repulsion from the existing 7 electrons in its compact 2p subshell. Chlorine has a larger 3p subshell, accommodating the extra electron more easily.<\/div>\n <\/details>\n\n <details>\n <summary>What is the main difference between Mendeleev and Modern Periodic Law?<\/summary>\n <div class=\"faq-answer\">Mendeleev’s Law is based on atomic mass, whereas the Modern Periodic Law is based on the atomic number, which is a more fundamental property of an element.<\/div>\n <\/details>\n\n <details>\n <summary>What are isoelectronic species?<\/summary>\n <div class=\"faq-answer\">These are atoms or ions that have the same number of electrons (e.g., O<sup>2-<\/sup>, F<sup>–<\/sup>, Ne, Na<sup>+<\/sup>, Mg<sup>2+<\/sup>). For these, the radius decreases as nuclear charge increases.<\/div>\n <\/details>\n\n <details>\n <summary>What is the diagonal relationship?<\/summary>\n <div class=\"faq-answer\">It is the similarity in properties between certain elements of the second period and the elements of the third period that are diagonally opposite to them, such as Lithium and Magnesium.<\/div>\n <\/details>\n\n <details>\n <summary>Which element has the highest electronegativity?<\/summary>\n <div class=\"faq-answer\">Fluorine (F) has the highest electronegativity with a value of 4.0 on the Pauling scale.<\/div>\n <\/details>\n\n <div class=\"internal-links\">\n <span>RELATED STUDY GUIDES<\/span>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-physics-survival-kit-2026\/\" target=\"_blank\">NEET Physics Survival Kit 2026<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/organic-chemistry-strategy-neet\/\" target=\"_blank\">Organic Chemistry Strategy for NEET<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-biology-tricks-for-exams\/\" target=\"_blank\">NEET Biology Memory Tricks<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/score-340-in-neet-biology\/\" target=\"_blank\">How to Score 340+ in NEET Biology<\/a>\n <\/div>\n\n <div class=\"cta-section\">\n <h2>Ready to Crack NEET 2026?<\/h2>\n <p>Join our Mission 180 Rankers Batch and get access to premium study materials, periodic table class 11 notes pdf, and expert mentorship to secure your medical seat.<\/p>\n <div class=\"cta-btns\">\n <a href=\"https:\/\/courses.ksquare.co.in\/new-courses\/3-mission-180-neet-physics-rankers-batch\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" class=\"btn-white\">Join Mission 180<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" class=\"btn-outline\">Free Study Material<\/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 \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&family=Plus+Jakarta+Sans:ital,wght@0,200..800;1,200..800&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 — 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 — 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>Periodic Table Class 11 Notes PDF – Comprehensive NEET Study Guide Mastering the periodic table class 11 notes pdf is the first step toward a perfect score in Inorganic Chemistry for NEET. The chapter “Classification of Elements and Periodicity in Properties” serves as the foundation for chemical bonding, p-block, d-block, and s-block elements. In this […]<\/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":[308,309,306,310,307],"class_list":["post-4012","post","type-post","status-publish","format-standard","hentry","category-free-study-material","tag-chemistry-class-11-notes-pdf","tag-classification-of-elements-notes","tag-periodic-table-class-11-notes-pdf","tag-periodic-table-revision-notes","tag-periodicity-trends-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\/4012","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=4012"}],"version-history":[{"count":4,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4012\/revisions"}],"predecessor-version":[{"id":4234,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4012\/revisions\/4234"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=4012"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=4012"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=4012"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}

{"id":4012,"date":"2026-03-30T08:44:02","date_gmt":"2026-03-30T08:44:02","guid":{"rendered":"https:\/\/ksquareinstitute.in\/blog\/?p=4012"},"modified":"2026-04-03T12:31:20","modified_gmt":"2026-04-03T12:31:20","slug":"periodic-table-class-11-notes-pdf","status":"publish","type":"post","link":"https:\/\/ksquareinstitute.in\/blog\/periodic-table-class-11-notes-pdf\/","title":{"rendered":"Periodic Table Class 11 Notes PDF: Comprehensive Guide for NEET Preparation"},"content":{"rendered":"\n\n\n\n \n \n Periodic Table Class 11 Notes PDF – Comprehensive NEET Study Guide<\/title>\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&family=JetBrains+Mono:wght@400;500;700&family=Plus+Jakarta+Sans:wght@400;600;700;800&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 body {\n margin: 0;\n padding: 0;\n font-family: 'DM Sans', sans-serif;\n color: var(--text);\n line-height: 1.6;\n background-color: #ffffff;\n }\n\n .content-wrapper {\n width: 100%;\n padding: 0;\n }\n\n .inner-container {\n padding: 0 0px;\n }\n\n @media (max-width: 768px) {\n .inner-container { padding: 0 10px; }\n }\n\n h1, h2, h3, h4 {\n font-family: 'Plus Jakarta Sans', sans-serif;\n font-weight: 700;\n color: var(--dark);\n }\n\n h1 { font-size: 2.5rem; margin-bottom: 1.5rem; padding: 0 20px; }\n\n .section-header {\n display: flex;\n align-items: center;\n gap: 15px;\n margin-top: 40px;\n margin-bottom: 20px;\n }\n\n .badge {\n width: 42px;\n height: 42px;\n background-color: var(--accent);\n color: white;\n display: flex;\n align-items: center;\n justify-content: center;\n border-radius: 8px;\n font-family: 'Plus Jakarta Sans', sans-serif;\n font-weight: 800;\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: 20px;\n margin: 20px 0;\n border-radius: 0 8px 8px 0;\n }\n .formula-dark span {\n display: block;\n font-size: 0.75rem;\n color: #9ca3af;\n text-transform: uppercase;\n margin-bottom: 8px;\n font-family: 'Plus Jakarta Sans', sans-serif;\n }\n .formula-dark p {\n color: var(--accent);\n font-family: 'JetBrains Mono', monospace;\n margin: 0;\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: 20px;\n margin: 20px 0;\n border-radius: 0 8px 8px 0;\n }\n .formula-orange p {\n color: #922b05;\n font-family: 'JetBrains Mono', monospace;\n margin: 0;\n font-weight: 500;\n }\n\n .callout-warning {\n background: #fff7ed;\n border: 1px solid #fed7aa;\n padding: 20px;\n border-radius: 10px;\n margin: 20px 0;\n position: relative;\n }\n .pill-warn {\n background: var(--accent);\n color: white;\n padding: 2px 10px;\n border-radius: 20px;\n font-size: 0.7rem;\n font-weight: 700;\n margin-bottom: 10px;\n display: inline-block;\n }\n\n .callout-tip {\n background: var(--blue-bg);\n border: 1px solid #bfdbfe;\n padding: 20px;\n border-radius: 10px;\n margin: 20px 0;\n }\n .pill-tip {\n background: #3b82f6;\n color: white;\n padding: 2px 10px;\n border-radius: 20px;\n font-size: 0.7rem;\n font-weight: 700;\n margin-bottom: 10px;\n display: inline-block;\n }\n\n table {\n width: 100%;\n border-collapse: collapse;\n margin: 20px 0;\n }\n th {\n background: var(--dark);\n color: white;\n text-align: left;\n padding: 14px;\n font-family: 'Plus Jakarta Sans', sans-serif;\n font-weight: 700;\n }\n td {\n padding: 14px;\n border-bottom: 1px solid var(--border);\n background: white;\n }\n tr:hover td { background: #fafafa; 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color: var(--accent); }\n details[open] summary::after { content: '\u2212'; }\n .faq-answer { padding: 16px 20px; background: white; color: var(--text-muted); }\n\n .revision-box {\n background: var(--green-bg);\n border: 2px solid var(--green-border);\n border-radius: 12px;\n padding: 25px;\n margin: 30px 0;\n }\n .revision-box h3 { color: var(--green-border); margin-top: 0; }\n .revision-box ul { padding-left: 20px; }\n .revision-box li { color: #166534; margin-bottom: 8px; font-weight: 500; }\n\n .cta-section {\n background: linear-gradient(135deg, #e8600a, #c2410c, #9a3412);\n padding: 60px 20px;\n text-align: center;\n margin-top: 50px;\n }\n .cta-section h2 { color: white; font-size: 2.2rem; }\n .cta-section p { color: rgba(255,255,255,0.85); max-width: 700px; margin: 0 auto 30px; }\n .cta-btns { display: flex; gap: 15px; justify-content: center; flex-wrap: wrap; }\n .btn-white { background: white; color: var(--accent); padding: 12px 30px; border-radius: 6px; text-decoration: none; font-weight: 700; }\n .btn-outline { border: 2px solid white; color: white; padding: 10px 28px; border-radius: 6px; text-decoration: none; font-weight: 700; }\n\n .internal-links {\n background: #f9fafb;\n border: 1px solid var(--border);\n border-radius: 10px;\n padding: 20px;\n margin: 30px 0;\n }\n .internal-links span { display: block; color: var(--text-muted); font-weight: 700; margin-bottom: 10px; font-size: 0.9rem; }\n .internal-links a { color: var(--accent); text-decoration: none; font-weight: 600; display: block; margin-bottom: 5px; }\n\n .download-btn {\n background: var(--dark);\n color: white;\n text-decoration: none;\n display: inline-flex;\n align-items: center;\n gap: 10px;\n padding: 12px 24px;\n border-radius: 8px;\n font-weight: 600;\n margin: 20px 0;\n }\n <\/style>\n<\/head>\n<body>\n\n<div class=\"content-wrapper\">\n <div class=\"inner-container\">\n \n <p>Mastering the <strong>periodic table class 11 notes pdf<\/strong> is the first step toward a perfect score in Inorganic Chemistry for NEET. The chapter “Classification of Elements and Periodicity in Properties” serves as the foundation for chemical bonding, p-block, d-block, and s-block elements. In this guide, we break down the complexities of electronic configurations, periodic trends, and exceptions that frequently appear in the exam.<\/p>\n\n <div class=\"section-header\">\n <div class=\"badge\">01<\/div>\n <h2>Introduction to Classification of Elements<\/h2>\n <\/div>\n \n <p>With 118 elements known today, studying them individually is impossible. The classification organizes elements into groups and periods based on their similarities, allowing chemists to predict properties. The modern periodic table is not just a list but a logical map of atomic structure.<\/p>\n \n <div class=\"grid-cards\">\n <div class=\"mini-card\">\n <span>BASIS OF CLASSIFICATION<\/span>\n <p>The fundamental shift happened from using Atomic Mass (Mendeleev) to Atomic Number (Moseley).<\/p>\n <\/div>\n <div class=\"mini-card\">\n <span>WHY IT MATTERS<\/span>\n <p>It explains the physical and chemical behavior of elements based on their electron configurations.<\/p>\n <\/div>\n <\/div>\n\n <div class=\"section-header\">\n <div class=\"badge 02\">02<\/div>\n <h2>Early Classifications of Elements<\/h2>\n <\/div>\n\n <h3>Dobereiner\u2019s Triads<\/h3>\n <p>In 1817, Johann Dobereiner arranged elements in groups of three (triads). The atomic mass of the middle element was approximately the arithmetic mean of the other two.<\/p>\n \n <div class=\"formula-orange\">\n <p>Example: Li (7), Na (23), K (39) <br> Mean: (7 + 39) \/ 2 = 23<\/p>\n <\/div>\n\n <h3>Newlands\u2019 Law of Octaves<\/h3>\n <p>John Newlands proposed that when elements are arranged in increasing order of atomic masses, every eighth element has properties similar to the first, similar to musical notes. However, this law only worked up to Calcium (Ca).<\/p>\n\n <h3>Mendeleev\u2019s Periodic Table<\/h3>\n <p>Dmitri Mendeleev formulated the Periodic Law: “The properties of elements are periodic functions of their atomic masses.”<\/p>\n <ul>\n <li><strong>Achievements:<\/strong> He left gaps for undiscovered elements like Eka-boron (Scandium), Eka-aluminium (Gallium), and Eka-silicon (Germanium).<\/li>\n <li><strong>Limitations:<\/strong> It could not explain the position of isotopes, the placement of Hydrogen, or the anomalous pairs like Cobalt (58.9) before Nickel (58.7).<\/li>\n <\/ul>\n\n <div class=\"section-header\">\n <div class=\"badge\">03<\/div>\n <h2>Modern Periodic Law and Structure<\/h2>\n <\/div>\n\n <p>The <strong>Modern Periodic Law<\/strong>, proposed by Henry Moseley, states that the physical and chemical properties of elements are periodic functions of their <strong>atomic number (Z)<\/strong>. This resolved the discrepancies found in Mendeleev’s mass-based table.<\/p>\n\n <div class=\"callout-tip\">\n <div class=\"pill-tip\">TIP<\/div>\n <p>Always remember: It is the electronic configuration of an atom that determines its position in the modern periodic table, not its mass!<\/p>\n <\/div>\n\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:20px;\">\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 <div class=\"section-header\">\n <div class=\"badge\">04<\/div>\n <h2>Electronic Configuration and Periodic Table<\/h2>\n <\/div>\n\n <p>The table is divided into four main blocks based on the orbital being filled by the last electron:<\/p>\n \n <table>\n <thead>\n <tr>\n <th>Block<\/th>\n <th>Groups<\/th>\n <th>General Configuration<\/th>\n <th>Properties<\/th>\n <\/tr>\n <\/thead>\n <tbody>\n <tr>\n <td>s-block<\/td>\n <td>1 & 2<\/td>\n <td>ns<sup>1-2<\/sup><\/td>\n <td>Highly reactive metals, low IE<\/td>\n <\/tr>\n <tr>\n <td>p-block<\/td>\n <td>13 to 18<\/td>\n <td>ns<sup>2<\/sup>np<sup>1-6<\/sup><\/td>\n <td>Contains metals, non-metals, metalloids<\/td>\n <\/tr>\n <tr>\n <td>d-block<\/td>\n <td>3 to 12<\/td>\n <td>(n-1)d<sup>1-10<\/sup>ns<sup>1-2<\/sup><\/td>\n <td>Transition metals, colored ions<\/td>\n <\/tr>\n <tr>\n <td>f-block<\/td>\n <td>Bottom Rows<\/td>\n <td>(n-2)f<sup>1-14<\/sup>(n-1)d<sup>0-1<\/sup>ns<sup>2<\/sup><\/td>\n <td>Inner transition elements (Lanthanoids\/Actinoids)<\/td>\n <\/tr>\n <\/tbody>\n <\/table>\n\n <div class=\"section-header\">\n <div class=\"badge\">05<\/div>\n <h2>Periodic Trends in Properties (NEET High-Weightage)<\/h2>\n <\/div>\n\n <p>Understanding trends is crucial for solving conceptual questions in your <strong>periodic table class 11 notes pdf<\/strong>. These trends are governed by Effective Nuclear Charge (Z<sub>eff<\/sub>) and Shielding Effect.<\/p>\n\n <h3>1. Atomic Radius<\/h3>\n <p>Atomic radius generally decreases across a period due to increased Z<sub>eff<\/sub> pulling electrons closer. It increases down a group as new shells are added.<\/p>\n \n <div class=\"callout-warning\">\n <div class=\"pill-warn\">WARN<\/div>\n <p>Van der Waals radius is always larger than Metallic or Covalent radius for the same element because it involves non-bonded distances.<\/p>\n <\/div>\n\n <h3>2. Ionization Enthalpy (\u0394<sub>i<\/sub>H)<\/h3>\n <p>The energy required to remove an electron from an isolated gaseous atom.<\/p>\n \n <div class=\"formula-dark\">\n <span>Factors Affecting \u0394<sub>i<\/sub>H<\/span>\n <p>\u0394<sub>i<\/sub>H \u221d (Nuclear Charge \/ Atomic Size)<\/p>\n <\/div>\n\n <div class=\"grid-cards\">\n <div class=\"mini-card\">\n <span>EXCEPTION: N vs O<\/span>\n <p>Nitrogen (half-filled 2p<sup>3<\/sup>) has higher IE than Oxygen (2p<sup>4<\/sup>) due to extra stability.<\/p>\n <\/div>\n <div class=\"mini-card\">\n <span>EXCEPTION: Be vs B<\/span>\n <p>Beryllium (full-filled 2s<sup>2<\/sup>) has higher IE than Boron (2p<sup>1<\/sup>).<\/p>\n <\/div>\n <\/div>\n\n <h3>3. Electron Gain Enthalpy (\u0394<sub>eg<\/sub>H)<\/h3>\n <p>Across a period, \u0394<sub>eg<\/sub>H becomes more negative (except noble gases which are positive). Down a group, it usually becomes less negative.<\/p>\n \n <div class=\"callout-tip\">\n <div class=\"pill-tip\">TIP<\/div>\n <p>Chlorine (Cl) has a more negative electron gain enthalpy than Fluorine (F) because F is so small that inter-electronic repulsions hinder the incoming electron.<\/p>\n <\/div>\n\n <div class=\"section-header\">\n <div class=\"badge\">06<\/div>\n <h2>Periodic Trends in Chemical Properties<\/h2>\n <\/div>\n\n <p>Trends in chemical reactivity are also predictable. Metallic character increases down the group while non-metallic character increases across the period.<\/p>\n \n <ul>\n <li><strong>Oxide Nature:<\/strong> Basic oxides (e.g., Na<sub>2<\/sub>O) are formed by metals on the left. Acidic oxides (e.g., Cl<sub>2<\/sub>O<sub>7<\/sub>) are formed by non-metals on the right. Amphoteric oxides include Al<sub>2<\/sub>O<sub>3<\/sub>.<\/li>\n <li><strong>Valency:<\/strong> Across a period, it increases from 1 to 4 and then decreases to 0 (for noble gases) with respect to hydrogen.<\/li>\n <\/ul>\n\n <div class=\"section-header\">\n <div class=\"badge\">07<\/div>\n <h2>Anomalous Properties and Diagonal Relationship<\/h2>\n <\/div>\n\n <p>The first element of each group (Li, Be, B) shows different behavior than its peers due to extremely small size, high IE, and absence of d-orbitals. Furthermore, some second-period elements show similarities with third-period elements placed diagonally.<\/p>\n \n <div class=\"grid-cards\">\n <div class=\"mini-card\">\n <span>DIAGONAL PAIRS<\/span>\n <p>Li & Mg, Be & Al, B & Si<\/p>\n <\/div>\n <div class=\"mini-card\">\n <span>REASON<\/span>\n <p>Similar ionic size and polarizing power (Charge\/Radius ratio).<\/p>\n <\/div>\n <\/div>\n\n <a href=\"https:\/\/ksquareinstitute.in\/neet-2026-rank-predictor\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" style=\"display:block; margin-bottom:20px;\">\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 <div class=\"section-header\">\n <div class=\"badge\">08<\/div>\n <h2>Summary of Periodic Trends (Quick Revision)<\/h2>\n <\/div>\n\n <div class=\"revision-box\">\n <h3>Key Revision Points<\/h3>\n <ul>\n <li>Atomic Radius: Decreases \u2192 (Period), Increases \u2193 (Group)<\/li>\n <li>Ionization Energy: Increases \u2192 (Period), Decreases \u2193 (Group)<\/li>\n <li>Electronegativity: Increases \u2192 (Period), Decreases \u2193 (Group)<\/li>\n <li>Electron Affinity: More Negative \u2192 (Period), Less Negative \u2193 (Group)<\/li>\n <li>Non-metallic Character: Increases \u2192 (Period), Decreases \u2193 (Group)<\/li>\n <li>Metallic Character: Decreases \u2192 (Period), Increases \u2193 (Group)<\/li>\n <li>Effective Nuclear Charge (Z<sub>eff<\/sub>): Increases across a period<\/li>\n <li>Screening Effect: Increases down a group<\/li>\n <li>Oxidizing Power: Increases across a period<\/li>\n <li>Reducing Power: Increases down a group<\/li>\n <\/ul>\n <\/div>\n\n <a href=\"#\" rel=\"nofollow noopener noreferrer\" class=\"download-btn\">\n Download Periodic Table Notes PDF\n <\/a>\n\n <div class=\"section-header\">\n <div class=\"badge\">09<\/div>\n <h2>Important Exam Focus & Exceptions<\/h2>\n <\/div>\n\n <p>NEET focuses heavily on exceptions. Ensure you have these noted down in your <strong>periodic table class 11 notes pdf<\/strong>:<\/p>\n \n <div class=\"formula-orange\">\n <p>Electronegativity Order: F > O > Cl > N <br> (Note: Cl and N have similar values but Cl is often considered more electronegative in certain scales).<\/p>\n <\/div>\n\n <div class=\"callout-warning\">\n <div class=\"pill-warn\">WARN<\/div>\n <p>Noble gases have the highest Ionization Enthalpy in their respective periods due to their stable ns<sup>2<\/sup>np<sup>6<\/sup> configuration.<\/p>\n <\/div>\n\n <div class=\"section-header\">\n <div class=\"badge\">10<\/div>\n <h2>Frequently Asked Questions (FAQs)<\/h2>\n <\/div>\n\n <details>\n <summary>Why does Chlorine have more negative electron gain enthalpy than Fluorine?<\/summary>\n <div class=\"faq-answer\">Fluorine is very small. When an electron is added, it experiences significant repulsion from the existing 7 electrons in its compact 2p subshell. Chlorine has a larger 3p subshell, accommodating the extra electron more easily.<\/div>\n <\/details>\n\n <details>\n <summary>What is the main difference between Mendeleev and Modern Periodic Law?<\/summary>\n <div class=\"faq-answer\">Mendeleev’s Law is based on atomic mass, whereas the Modern Periodic Law is based on the atomic number, which is a more fundamental property of an element.<\/div>\n <\/details>\n\n <details>\n <summary>What are isoelectronic species?<\/summary>\n <div class=\"faq-answer\">These are atoms or ions that have the same number of electrons (e.g., O<sup>2-<\/sup>, F<sup>–<\/sup>, Ne, Na<sup>+<\/sup>, Mg<sup>2+<\/sup>). For these, the radius decreases as nuclear charge increases.<\/div>\n <\/details>\n\n <details>\n <summary>What is the diagonal relationship?<\/summary>\n <div class=\"faq-answer\">It is the similarity in properties between certain elements of the second period and the elements of the third period that are diagonally opposite to them, such as Lithium and Magnesium.<\/div>\n <\/details>\n\n <details>\n <summary>Which element has the highest electronegativity?<\/summary>\n <div class=\"faq-answer\">Fluorine (F) has the highest electronegativity with a value of 4.0 on the Pauling scale.<\/div>\n <\/details>\n\n <div class=\"internal-links\">\n <span>RELATED STUDY GUIDES<\/span>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-physics-survival-kit-2026\/\" target=\"_blank\">NEET Physics Survival Kit 2026<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/organic-chemistry-strategy-neet\/\" target=\"_blank\">Organic Chemistry Strategy for NEET<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/neet-biology-tricks-for-exams\/\" target=\"_blank\">NEET Biology Memory Tricks<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/blog\/score-340-in-neet-biology\/\" target=\"_blank\">How to Score 340+ in NEET Biology<\/a>\n <\/div>\n\n <div class=\"cta-section\">\n <h2>Ready to Crack NEET 2026?<\/h2>\n <p>Join our Mission 180 Rankers Batch and get access to premium study materials, periodic table class 11 notes pdf, and expert mentorship to secure your medical seat.<\/p>\n <div class=\"cta-btns\">\n <a href=\"https:\/\/courses.ksquare.co.in\/new-courses\/3-mission-180-neet-physics-rankers-batch\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" class=\"btn-white\">Join Mission 180<\/a>\n <a href=\"https:\/\/ksquareinstitute.in\/free-study-material\/\" target=\"_blank\" rel=\"nofollow noopener noreferrer\" class=\"btn-outline\">Free Study Material<\/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 \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&family=Plus+Jakarta+Sans:ital,wght@0,200..800;1,200..800&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 — 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 — 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>Periodic Table Class 11 Notes PDF – Comprehensive NEET Study Guide Mastering the periodic table class 11 notes pdf is the first step toward a perfect score in Inorganic Chemistry for NEET. The chapter “Classification of Elements and Periodicity in Properties” serves as the foundation for chemical bonding, p-block, d-block, and s-block elements. In this […]<\/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":[308,309,306,310,307],"class_list":["post-4012","post","type-post","status-publish","format-standard","hentry","category-free-study-material","tag-chemistry-class-11-notes-pdf","tag-classification-of-elements-notes","tag-periodic-table-class-11-notes-pdf","tag-periodic-table-revision-notes","tag-periodicity-trends-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\/4012","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=4012"}],"version-history":[{"count":4,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4012\/revisions"}],"predecessor-version":[{"id":4234,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/posts\/4012\/revisions\/4234"}],"wp:attachment":[{"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/media?parent=4012"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/categories?post=4012"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ksquareinstitute.in\/blog\/wp-json\/wp\/v2\/tags?post=4012"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}