Students of Bihar Board Class 11 can find complete details about the Bihar Board 11th Chemistry Book 2026 PDF Download on this page. The Chemistry textbook prescribed by the Bihar Board is important for building a strong base in chemical concepts for higher classes.
| Details | Information |
|---|---|
| Board | Bihar Board (BSEB) |
| Class | 11th |
| Subject | Chemistry |
| Academic Year | 2025–26 |
| Material Type | Textbook / Study Material |
| Syllabus | Latest Bihar Board Syllabus |
| Format | |
| Availability | PDF Download Links Available |
This page provides Chemistry study materials (books) in PDF format with direct download links, prepared according to the latest Bihar Board syllabus and useful for exam-oriented preparation.
Bihar Board 11th Chemistry Book Chemistry 2026 PDF Download (रसायनशास्त्र)
इस पेज पर बिहार बोर्ड के छात्रों के लिए “Class XI: Chemistry (रसायनशास्त्र)” दिया गया है | जिसे आप अपने फ़ोन में Free Download कर सकते हैं |
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Bihar Board 12th Chemistry Book in Hindi
अध्याय 1: रसायन विज्ञान की कुछ मूल अवधारणाएँ
अध्याय 1: रसायन विज्ञान की कुछ मूल अवधारणाएँ – PDF Download
अध्याय 2: परमाणु की संरचना
अध्याय 2: परमाणु की संरचना – PDF Download
अध्याय 3: तत्वों का वर्गीकरण एवं गुणधर्मों में आवर्तिता
अध्याय 3: तत्वों का वर्गीकरण एवं गुणधर्मों में आवर्तिता – PDF Download
अध्याय 4: रासायनिक आबंधन तथा आण्विक संरचना
अध्याय 4: रासायनिक आबंधन तथा आण्विक संरचना – PDF Download
अध्याय 5: द्रव्य के अवस्थाएँ
अध्याय 5: द्रव्य के अवस्थाएँ – PDF Download
अध्याय 6: उष्मागतिकी
अध्याय 6: उष्मागतिकी – PDF Download
अध्याय 7: साम्यावस्था
अध्याय 7: साम्यावस्था – PDF Download
अध्याय 8: अपचयोपचय अभिक्रियाएँ
अध्याय 8: अपचयोपचय अभिक्रियाएँ – PDF Download
अध्याय 9: हाइड्रोजन
अध्याय 9: हाइड्रोजन – PDF Download
अध्याय 10: s – बलॉक तत्व
अध्याय 10: s – बलॉक तत्व – PDF Download
अध्याय 11: p – बलॉक तत्व
अध्याय 11: p – बलॉक तत्व – PDF Download
अध्याय 12: कार्बनिक रसायन: कुछ आधारभूत सिद्धांत तथा तकनीकें
अध्याय 12: कार्बनिक रसायन: कुछ आधारभूत सिद्धांत तथा तकनीकें – PDF Download
अध्याय 13: हाइड्रोकार्बन
अध्याय 13: हाइड्रोकार्बन – PDF Download
अध्याय 14: पर्यावरणीय रसायन
अध्याय 14: पर्यावरणीय रसायन – PDF Download
Bihar Board 12th Chemistry Book in English
Chapter 1: Some Basic Concepts of Chemistry
This chapter, ‘Some Basic Concepts of Chemistry’, provides a foundational overview of chemistry, starting with its historical development in India as Rasayan Shastra, where ancient scientists practiced metallurgy and medicine. It defines chemistry as the study of atoms and molecules and explores its vital role in meeting human needs like healthcare, agriculture, and environmental protection.
The text explains the nature of matter, classifying it by physical states—solid, liquid, and gas—and chemical composition, distinguishing between mixtures and pure substances like elements and compounds. It introduces the International System of Units (SI) and emphasizes the importance of precision, accuracy, and scientific notation in measurements.
Fundamental laws of chemical combination, such as the Law of Conservation of Mass, Law of Definite Proportions, and Avogadro’s Law, are discussed as the basis for Dalton’s Atomic Theory. Detailed explanations are provided for atomic and molecular masses, leading to the crucial mole concept, where one mole is defined as 6.022 x 10^23 entities.
The chapter concludes with stoichiometry, detailing how to calculate reactants and products in balanced chemical equations, and methods for expressing solution concentration, including mass percent, molarity, and molality. This unit establishes the essential quantitative framework required to understand chemical transformations.
Chapter 1: Some Basic Concepts of Chemistry – PDF Download
Chapter 2: Structure of Atom
The chapter ‘Structure of Atom’ explores the evolution of atomic theory from Dalton’s indivisible atom to the sophisticated quantum mechanical model. It chronicles the discovery of fundamental subatomic particles—electrons, protons, and neutrons—through landmark experiments such as J.J. Thomson’s cathode ray studies and Rutherford’s gold foil scattering.
These discoveries led to the proposal of various atomic models, including the Thomson and Rutherford models, which eventually gave way to Bohr’s quantized model for hydrogen. The text addresses the limitations of these early theories, particularly their inability to explain the stability of multi-electron atoms and the wave-particle duality of matter. Central to the modern understanding is the quantum mechanical model, grounded in de Broglie’s hypothesis and Heisenberg’s uncertainty principle.
It introduces the Schrödinger wave equation, which defines atomic orbitals as regions of high electron probability rather than fixed paths. These orbitals are characterized by four quantum numbers—principal, azimuthal, magnetic, and spin—which determine their size, shape, and orientation. The chapter concludes by detailing the rules for electronic configuration, such as the Aufbau principle and Hund’s rule, and explaining the exceptional stability of half-filled and fully-filled subshells, which is crucial for understanding the chemical properties of elements.
Overall, it provides a comprehensive foundation for studying the internal structure of matter.
Chapter 2: Structure of Atom – PDF Download
Chapter 3: Classification of Elements and Periodicity in Properties
This chapter explores the historical development and modern structure of the Periodic Table, a fundamental tool in chemistry. It details the journey from early attempts by scientists like Dobereiner, Newlands, and Mendeleev to organize elements based on atomic weights, to the Modern Periodic Law, which uses atomic number as the basis for classification. The Modern Periodic Table organizes elements into periods and groups reflecting their electronic configurations.
The unit classifies elements into s, p, d, and f blocks. It highlights periodic trends in physical properties such as atomic and ionic radii, ionization enthalpy, electron gain enthalpy, and electronegativity. Generally, atomic size decreases across a period and increases down a group, while ionization enthalpy and electronegativity increase across a period.
The chapter also discusses periodic variations in chemical properties, including valence and oxidation states. It notes that elements at the extremes of the table are highly reactive, forming basic and acidic oxides, while central elements often form amphoteric oxides. Additionally, it addresses the unique position of hydrogen and the anomalous behavior of second-period elements due to their small size and high electronegativity.
This systematic organization allows for predicting the properties of elements and understanding the underlying building blocks of matter.
Chapter 3: Classification of Elements and Periodicity in Properties – PDF Download
Chapter 4: Chemical Bonding and Molecular Structure
The chapter ‘Chemical Bonding and Molecular Structure’ explores the fundamental forces and theories that explain how atoms combine to form molecules. It begins with the Kössel-Lewis approach, introducing the octet rule which states that atoms achieve stability by attaining eight electrons in their valence shells through electron transfer or sharing. The text explains Lewis symbols and the formation of ionic and covalent bonds.
It further delves into VSEPR theory, which predicts molecular geometries based on electron pair repulsions, explaining why molecules like water and ammonia have specific bent or pyramidal shapes. The chapter also discusses Valence Bond (VB) Theory, focusing on orbital overlap and the concept of hybridization to explain the directional properties and bond angles in polyatomic molecules. Furthermore, it introduces Molecular Orbital (MO) Theory, describing how atomic orbitals combine to form bonding and antibonding molecular orbitals, which determines a molecule’s stability, bond order, and magnetic properties.
Key bond parameters such as bond length, angle, enthalpy, and polarity are analyzed. Finally, it covers hydrogen bonding, emphasizing its role in determining the physical properties of substances. This comprehensive study provides the theoretical foundation for understanding the architecture and behavior of chemical species.
Chapter 4: Chemical Bonding and Molecular Structure – PDF Download
Chapter 5: States of Matter
The chapter ‘States of Matter’ explores the physical properties of gases and liquids, emphasizing the balance between intermolecular forces and thermal energy. Intermolecular forces like London forces, dipole-dipole, and hydrogen bonding tend to keep particles together, while thermal energy promotes motion and keeps them apart. The gaseous state, the simplest form of matter, is characterized by high compressibility and lack of fixed volume.
Key gas laws are discussed: Boyle’s Law (P-V relationship), Charles’ Law (V-T relationship), Gay Lussac’s Law (P-T relationship), and Avogadro’s Law (V-n relationship). These are combined into the Ideal Gas Equation (PV=nRT). The chapter explains that real gases deviate from ideal behavior at high pressure and low temperature due to molecular interactions and the non-negligible volume of molecules, modeled by the van der Waals equation.
It also covers the kinetic molecular theory, providing a microscopic view of gas behavior. For liquids, properties such as vapour pressure, surface tension, and viscosity are examined, all of which are governed by strong intermolecular attractions. The concept of critical temperature is introduced, marking the threshold for gas liquefaction.
Overall, the unit provides a fundamental understanding of how molecular interactions determine the macroscopic behavior of substances in different physical states.
Chapter 5: States of Matter – PDF Download
Chapter 6: Thermodynamics
Thermodynamics, as detailed in Unit 6, is the branch of science that explores energy transformations in macroscopic systems, focusing on initial and final states rather than microscopic details. It distinguishes between the ‘system’—the portion under observation—and the ‘surroundings.’ Systems are further classified as open, closed, or isolated based on their interaction with the environment. The First Law of Thermodynamics, represented by the equation ΔU = q + w, defines internal energy change as the sum of heat and work, emphasizing the fundamental conservation of energy.
Enthalpy (H) is introduced as a state function for processes at constant pressure, where ΔH equals the heat change. The text also covers Hess’s Law, which states that enthalpy change is independent of the reaction path. Spontaneity is linked to entropy (S), representing molecular disorder, and Gibbs Energy (G).
The Second Law dictates that spontaneous processes increase the total entropy of the universe, while the primary criterion for spontaneity at constant temperature and pressure is a negative ΔG (ΔG = ΔH – TΔS). The Third Law establishes that the entropy of a pure crystalline substance is zero at absolute zero (0 K). Finally, the relationship between standard Gibbs energy change and the equilibrium constant is established.
Chapter 6: Thermodynamics – PDF Download
Chapter 7: Equilibrium
This chapter, titled ‘Redox Reactions’, provides a comprehensive study of chemical processes involving the simultaneous occurrence of oxidation and reduction. It explores the evolution of redox concepts from classical definitions—focusing on the addition or removal of oxygen and hydrogen—to the modern electronic theory, where oxidation is defined as the loss of electrons and reduction as the gain of electrons. The text introduces the ‘oxidation number’ as a vital book-keeping tool to track electron shifts, especially in covalent compounds, and outlines specific rules for its determination.
The chapter classifies redox reactions into four main types: combination, decomposition, displacement (both metal and non-metal), and disproportionation. It addresses the paradox of fractional oxidation numbers, explaining them as averages of different whole-number oxidation states revealed by molecular structures. Furthermore, it details two systematic methods for balancing redox equations: the oxidation number method and the half-reaction (ion-electron) method.
Practical applications are highlighted through redox titrations using indicators like permanganate and starch. Finally, the text explains electrode processes, the construction of the Daniell cell, and the significance of standard electrode potentials in measuring the relative oxidizing or reducing strength of various species. This fundamental knowledge lays the groundwork for understanding electrochemical cells and broader chemical transformations in biological and industrial systems.
Chapter 7: Equilibrium – PDF Download
Chapter 8: Redox Reactions
The chapter ‘Redox Reactions’ from the NCERT Chemistry textbook (Unit 8) explores the fundamental concepts of oxidation and reduction, which occur simultaneously in chemical processes. It traces the evolution of these concepts from classical ideas—focusing on the addition/removal of oxygen or hydrogen—to modern electronic and oxidation number theories. The unit defines oxidation as the loss of electrons and reduction as the gain of electrons.
It introduces the ‘oxidation number’ method as a practical tool for keeping track of electron shifts, especially in covalent compounds, using a specific set of rules. Redox reactions are classified into four main types: combination, decomposition, displacement (including metal and non-metal displacement), and disproportionation reactions. Additionally, the chapter discusses competitive electron transfer reactions and develops the concept of the electrochemical series.
It explains the design and operation of the Daniell cell, introducing electrode potential and standard electrode potential. The text also covers the application of redox reactions in titrations (using self-indicators like KMnO4) and acknowledges the limitations of the oxidation number concept, suggesting a more modern view involving electron density changes. Finally, it provides various solved problems and exercises to reinforce balancing equations via the oxidation number and half-reaction methods.
Chapter 8: Redox Reactions – PDF Download
Chapter 9: Hydrogen
This chapter from the NCERT Chemistry textbook focuses extensively on Hydrogen, the most abundant element in the universe. It begins by examining the unique position of hydrogen in the periodic table, noting how its electronic configuration (1s¹) allows it to resemble both alkali metals and halogens, though it is ultimately placed separately.
The text describes the three isotopes of hydrogen—protium, deuterium, and radioactive tritium—and the preparation of dihydrogen through laboratory and commercial methods like electrolysis, coal gasification, and water-gas shift reactions. A significant portion of the unit is dedicated to the physical and chemical properties of dihydrogen, highlighting its exceptionally high bond dissociation enthalpy and its reactions with halogens, dioxygen, dinitrogen, and various metals.
The chapter also categorizes hydrides into ionic, covalent, and metallic types, providing specific examples like diborane and methane. It further investigates the vital properties of water, including its bent structure, extensive hydrogen bonding, and the chemical causes and removal techniques for water hardness.
Detailed accounts of hydrogen peroxide (H2O2), its non-planar structure, and its dual role as an oxidising and reducing agent are provided. The unit concludes with the innovative concept of ‘Hydrogen Economy,’ suggesting dihydrogen as a clean, pollution-free energy carrier that could eventually revolutionize power generation and transportation globally.
Chapter 9: Hydrogen – PDF Download
Chapter 10: The s – Block Elements
The s-block elements of the Periodic Table comprise Group 1 (alkali metals) and Group 2 (alkaline earth metals), where the last electron enters the s-orbital. Group 1 elements like lithium and sodium are soft, silvery-white, and highly reactive, forming strong alkaline hydroxides.
They exhibit low ionization enthalpies and increasing atomic sizes down the group. Group 2 elements, including magnesium and calcium, are also reactive but denser and harder than alkali metals.
Both groups display systematic property trends, although lithium and beryllium show anomalous behavior and ‘diagonal relationships’ with magnesium and aluminum. The text details the industrial production of essential compounds such as sodium carbonate (washing soda) via the Solvay process, sodium hydroxide (caustic soda), and calcium-based materials like quicklime, slaked lime, and Portland cement.
Furthermore, the biological significance of these ions is highlighted: sodium and potassium are vital for nerve impulse conduction and maintaining ion balance, while magnesium and calcium are indispensable for enzyme activity, bone integrity, and blood coagulation. In conclusion, the chapter provides a thorough chemical analysis of s-block elements, bridging their fundamental atomic properties with their practical industrial applications and critical physiological roles in living organisms.
Chapter 10: The s – Block Elements – PDF Download
Chapter 11: The p – Block Elements
The p-block elements occupy groups 13 to 18 of the periodic table, where the last electron enters the outermost p-orbital. This unit specifically focuses on Group 13 (The Boron Family) and Group 14 (The Carbon Family). Group 13 elements, ranging from boron to thallium, exhibit a general electronic configuration of ns²np¹.
Boron is a unique non-metal, while others like aluminium, gallium, indium, and thallium are metallic. Key compounds discussed include borax, orthoboric acid, and diborane. Group 14 elements, comprising carbon, silicon, germanium, tin, and lead, have an ns²np² configuration.
Carbon is renowned for its versatility, exhibiting allotropes like diamond, graphite, and fullerenes. It also shows the unique property of catenation, forming stable chains and rings. The chapter details periodic trends such as atomic radii, ionization enthalpy, and oxidation states, highlighting the ‘inert pair effect’ where lower oxidation states become progressively more stable for heavier elements.
Chemical reactivity towards air, acids, alkalies, and halogens is thoroughly explored. Additionally, the unit examines the industrial and domestic importance of compounds like silicates, silicones, and oxides of carbon. The presence of d and f orbitals in heavier elements significantly influences their chemical behavior and physical properties, distinguishing them from the lighter members.
This comprehensive study provides a foundational understanding of p-block chemistry and its diverse applications in science and industry.
Chapter 11: The p – Block Elements – PDF Download
Chapter 12: Organic Chemistry – Some Basic Principles and Techniques
This unit covers the foundational principles and methods of organic chemistry, starting with carbon’s tetravalence and the resulting molecular shapes like sp3, sp2, and sp hybridizations. It explains various ways to represent structures, such as bond-line and 3D formulas, and classifies compounds into acyclic, cyclic, and aromatic categories.
The text details the systematic IUPAC nomenclature for naming complex organic molecules and describes isomerism, where compounds share molecular formulas but differ in structure or spatial arrangement. It explores reaction mechanisms, detailing bond fission like homolytic and heterolytic and the behavior of reactive intermediates like carbocations and free radicals.
Electronic effects, including inductive, resonance, electromeric, and hyperconjugation, are analyzed for their impact on chemical properties. Additionally, the chapter presents purification techniques like distillation, crystallization, and chromatography, along with qualitative and quantitative analytical methods for identifying elements like nitrogen, sulfur, and halogens.
This comprehensive overview provides the essential toolkit for understanding the formation, identification, and reactivity of organic substances.
Chapter 12: Organic Chemistry – Some Basic Principles and Techniques – PDF Download
Chapter 13: Hydrocarbons
The chapter ‘Hydrocarbons’ offers a detailed and systematic study of organic compounds composed entirely of carbon and hydrogen. It begins by classifying these substances into three main groups based on the nature of carbon-carbon bonds: saturated (alkanes), unsaturated (alkenes and alkynes), and aromatic hydrocarbons (arenes). The unit extensively discusses alkanes, covering their IUPAC nomenclature, structural isomerism, and conformations, with a specific focus on the energy differences and stability of staggered and eclipsed forms.
Their chemical reactivity is explored through free radical substitution, combustion, and aromatization processes. For unsaturated hydrocarbons, the text emphasizes electrophilic addition reactions, clearly explaining critical principles such as Markovnikov’s rule and the anti-Markovnikov peroxide effect. Furthermore, industrial processes like polymerization and ozonolysis are detailed to highlight their practical utility.
The aromatic section focuses on benzene, explaining its unique electronic structure and stability through resonance and Hückel’s rule. It details electrophilic substitution reactions, including nitration and Friedel-Crafts alkylation, while also explaining the directive influence of substituents in disubstituted benzenes. Ultimately, the chapter underscores the vital role of hydrocarbons as energy sources such as LPG and CNG, while concluding with a warning about the toxicity and carcinogenicity of certain fused benzene ring systems produced during incomplete combustion.
Chapter 13: Hydrocarbons – PDF Download
Chapter 14: Environmental Chemistry
This chapter explores the origins, transport, reactions, and effects of chemical species in the environment. It defines environmental pollution as undesirable changes in our surroundings that have harmful effects on plants, animals, and human beings. Atmospheric pollution is categorized into tropospheric and stratospheric pollution.
Tropospheric pollutants, such as oxides of sulphur, nitrogen, and carbon, alongside hydrocarbons and particulates, contribute significantly to acid rain and the enhanced greenhouse effect, which leads to global warming. The text explains how gases like carbon dioxide and methane trap heat, while stratospheric pollution focuses on the depletion of the protective ozone layer by chlorofluorocarbons (CFCs), resulting in increased UV radiation exposure. Water pollution is analyzed through pathogens, organic wastes (measured by Biochemical Oxygen Demand), and chemical pollutants, emphasizing International Standards for drinking water and the process of eutrophication.
Soil pollution is primarily attributed to the excessive use of synthetic pesticides and herbicides. The chapter also addresses industrial waste management and recycling strategies. Finally, it introduces Green Chemistry as a sustainable philosophy aimed at minimizing waste and environmental deterioration through innovative, environment-friendly chemical processes.
It concludes that collective responsibility and the adoption of green practices are essential for preserving the environment for future generations.
Chapter 14: Environmental Chemistry – PDF Download
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⚠️ अगर उपर दी गयी कोई भी बुक डाउनलोड करने में किसी प्रकार की समस्या हो रही हो तो कमेंट करके हमें बताएं | 
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⚠️ इस पेज पर दी गयी बुक्स “Bihar Education Project” द्वारा पब्लिश की गई हैं | ऑफिसियल साईट से इन बुक्स को डाउनलोड करने के लिए – यहाँ क्लिक करें
chemistry book ka bdf
hey @Tannu, PDF Links are already given on this page.
chemistry class 11th ka book bdf live
EK SATH EK BOOK DAUNLOD NHI HORAHA HAI B’S EK CHEPTER DAUNLOD HO RHA HAI
hey @Asas, you can’t download the whole book in a single file. Every chapter is given separately.