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CBSE 11th
Understand the concepts and topics of class eleventh chemistry
Overview of the CBSE Class 11 Chemistry Course
Understanding the ideas and themes of class eleven chemistry is a complex endeavor. It requires thorough knowledge of the material. Some students may benefit by studying for CBSE eleven-standard chemistry exams while others could use CBSE study notes to study for it. Chemistry classes eleven–12 will learn what they need to study, how many marks each unit receives, and how long it takes to complete it by studying for reviews like these. It is based on this that they can arrange their study time more efficiently. Exam questions will understand topics that pupils learn in CBSE Class 11 Chemistry standards; thus, pupils should adhere to the curriculum provided by reviews like these.
Course Curriculum and Topics Covered in CBSE Class 11 Chemistry
- Encourage awareness of fundamental chemical facts and ideas.
- Prepare to face a variety of challenges in agriculture, industry, population, environment, and health.
- Improve your problem-solving abilities.
- Expose the various industrial processes and their technological applications.
- Develop an interest in pursuing a career in chemistry.
Course Content
- Importance and scope of Chemistry
- Laws of chemical combination
- Dalton’s atomic theory
- Atoms and molecules
- Atomic and molecular masses
- Mole concept
- Molar mass
- Percentage composition
- Empirical and molecular formula
- Chemical reactions
- Stoichiometry
- Calculations based on stoichiometry
- Discovery of Electron
- Proton and Neutron
- Atomic number
- Isotopes and isobars
- Thomson’s model and its limitations
- Rutherford’s model and its limitations
- Bohr’s model and its limitations
- de Broglie’s relationship
- Heisenberg uncertainty principle
- Concept of orbitals
- Quantum numbers
- Shapes of s, p, and d orbitals
- Rules for filling electrons in orbitals
- Aufbau principle
- Pauli’s exclusion principle
- Hund’s rule
- Electronic configuration of atoms
- Stability of half-filled and completely filled orbitals
- Significance and development of the periodic table
- Modern periodic law and the present form of the periodic table
- Periodic trends in properties of elements
- Atomic radii
- Ionic radii
- Inert gas radii
- Ionization enthalpy
- Electrons gain enthalpy
- Electronegativity
- Valency
- Nomenclature of elements with atomic number greater than 100
- Valence electrons
- Ionic bond
- Covalent bond
- Bond parameters
- Lewis structure
- The polar character of covalent bond
- The covalent character of ionic bond
- Valence bond theory
- Resonance
- The geometry of covalent molecules
- VSEPR theory
- Concept of hybridization
- S, p, and d orbitals and shapes of some simple molecules
- Molecular orbital theory
- Hydrogen bond
- Three states of matter
- Intermolecular interactions
- Types of bonding
- Melting and boiling points
- Role of gas laws in elucidating the concept of the molecule
- Boyle’s law
- Charles law
- Gay Lussac’s law
- Avogadro’s law
- Ideal behavior
- Empirical derivation of gas equation
- Ideal gas equation
- Deviation from ideal behavior
- Liquefaction of gases
- Critical temperature
- Kinetic energy and molecular speeds (elementary idea)
- Liquid State – vapor pressure
- Viscosity and surface tension
- Concepts of System and types of systems, surroundings, work, heat, energy,
- Extensive and intensive properties
- State functions
- The first law of thermodynamics
- Internal energy
- Enthalpy
- Heat capacity
- Specific heat
- Measurement of ?U and ?H
- Hess’s law of constant heat summation
- Enthalpy of bond dissociation
- Combustion, formation, atomization
- Sublimation, phase transition, ionization
- Solution and dilution
- The second law of Thermodynamics (brief introduction)
- Introduction of entropy
- State function
- Gibb’s energy change for spontaneous and non-spontaneous processes
- Criteria for equilibrium
- Third law of thermodynamics (brief introduction)
- Equilibrium in physical and chemical processes
- Dynamic nature of equilibrium
- Law of mass action
- Equilibrium constant, factors affecting equilibrium
- Le Chatelier’s principle
- Ionic equilibrium –
- Ionization of acids and bases
- Strong and weak electrolytes
- Degree of ionization
- Ionization of polybasic acids
- Acid strength
- Concept of pH
- Hydrolysis of salts (elementary idea)
- Buffer solution
- Henderson Equation
- Solubility product
- Common ion effect (with illustrative examples)
- Concept of oxidation and reduction
- Redox reactions
- Oxidation number
- Balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number
- Applications of redox reactions
- Position of hydrogen in the periodic table
- Occurrence
- Isotopes
- Preparation, properties of hydrogen
- Uses of hydrogen
- Hydrides – ionic covalent and interstitial
- Physical and chemical properties of water
- Heavy water
- Hydrogen peroxide – preparation, reactions and structure, and use
- Hydrogen as a fuel
- Group 1 and Group 2 Elements General introduction
- Electronic configuration
- Occurrence, anomalous properties of the first element of each group, diagonal relationship, Trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii)
- Trends in chemical reactivity with oxygen, water, hydrogen, and halogens, uses.
Preparation and Properties of Some Important Compounds:
- Sodium Carbonate
- Sodium Chloride
- Sodium Hydroxide
- Sodium Hydrogen carbonate
- Biological importance of Sodium and Potassium
- Calcium Oxide
- Calcium Carbonate and their industrial uses
- Biological importance of Magnesium and Calcium
- General Introduction to p -Block Elements
- Group 13 Elements:
- Boron – physical and chemical properties
Some important compounds:
- Borax, Boric acid, Boron Hydrides, Aluminium: Reactions with acids and alkalis,
- Group 14 Elements:
- Carbon-catenation
- Allotropic forms
- Physical and chemical properties
- Uses of some important compounds: Oxides
Important compounds of Silicon and a few uses
- Silicon Tetrachloride, Silicones, Silicates and Zeolites, their uses
- General introduction
- Methods of purification
- Qualitative analysis
- Classification and IUPAC nomenclature of organic compounds
- Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyperconjugation.
- Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles
- Types of organic reactions
- Classification of Hydrocarbons
- Aliphatic Hydrocarbons:
- Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion, and pyrolysis.
- Alkenes – Nomenclature, Structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.
- Alkynes – Nomenclature, the structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of – hydrogen, halogens, hydrogen halides, and water.
Aromatic Hydrocarbons:
- Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Crafts alkylation and acylation, directive influence of the functional group in monosubstituted benzene. Carcinogenicity and toxicity
- Environmental pollution – air, water, and soil pollution, chemical reactions in the atmosphere, smog, major atmospheric pollutants, acid rain, ozone and its reactions, effects of depletion of the ozone layer, greenhouse effect, and global warming – pollution due to industrial wastes, green chemistry as an alternative tool for reducing pollution, strategies for control of environmental pollution.
Course Details & Descriptions
The Chemistry Class 11 syllabus has been the talk of the class for a while now. Everyone is wondering what new topics will be taught this year, or will there even be any changes to the course content? Bob Smith has officially released the details of the course on his blog. Download it for free in chunks based on your schedule with Chemistry 11 Syllabus pdf.
Class 11 Chemistry is an important stage in higher education.
It is at this stage that they are introduced to the notion of streams, which include several topic combinations from which they must pick. This choice will have a significant influence on their future employment prospects. It is also vital for students to perform well in Class 11 since it demonstrates that they understand the courses they have chosen and will be able to continue them in Class 12.
Chemistry in Class 11 introduces some new subjects.
All of these subjects are necessary for students who wish to pursue a profession in disciplines linked to chemistry to have a strong foundation in the subject for higher study in institutions. The study is primarily concerned with the makeup of the many non-living objects that exist in our environment. It covers the existence of matter in many states, including solids, gases, and liquids. Many chapters in class 11 will assist students comprehend the chemical compositions and reactions that occur when various elements combine.
Course Structure
1
Unit I: Some Basic Concepts of Chemistry
General Introduction: Importance and scope of Chemistry.
Nature of matter, laws of chemical combination, Dalton's atomic theory: the concept of elements, atoms, and molecules.
Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry, and calculations based on stoichiometry
2
Unit II: Structure of Atom
Discovery of Electron, Proton, Neutron, atomic number, isotopes, and isobars. Thomson's model and its limitations. Rutherford's model and its limitations, Bohr's model and its limitations, the concept of shells and subshells, the dual nature of matter and light, de Broglie's relationship, Heisenberg uncertainty principle, the concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals - Aufbau principle, Pauli's exclusion principle and Hund's rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.
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Unit III: Classification of Elements and Periodicity in Properties
Significance of classification, a brief history of the development of the periodic table, modern periodic law and the present form of the periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100.
Course Instructor
Shruti Koli
It facilitates student learning through interactive classrooms, question and answer sessions, and individual attention to each student.
Ravikant Sharma
It is an useful website for test preparation, whether technical or non-technical. It includes simulated examinations and previous year papers to help with knowledge and preparation.
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- Course videos and readings
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- Shareable Certificate upon completion
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Frequently Asked Questions
Matter is made up of atoms and molecules, and the arrangement of these building blocks determines the shape and structure of matter. The physical properties of matter are determined by the force of interaction between its molecules. This force is known as an intermolecular force. The intermolecular force is greatest in solids and least in gases.
Carbon dioxide and water vapor in the atmosphere absorb infrared light. Part of these rays are also reflected on the earth's surface, causing it to heat. Global warming, often known as the Greenhouse Effect, refers to the heating of the earth's surface. This phenomenon arose primarily as a result of deforestation, which increased CO2 levels in the atmosphere.
If you are seeking Class 11 Chemistry notes that can help you better comprehend the numerous topics included in the curriculum, Vedantu's e-platform is the place to go. Students may access and download CBSE Notes for Class 11 Chemistry chapter-by-chapter from the Vedantu website or app. These notes are free to download. Subject specialists prepared these notes to assist students with the greatest resource available for better and stronger preparation for their Class 11 Chemistry exam. These solutions are based on the most recent CBSE standards and exam patterns, thus they are completely dependable and correct.
- Preparation of Class 11 CBSE Chemistry Sections following the CBSE Syllabus
- Examining past year's question papers
- Last-minute Notes revision
Class 11 Chemistry has a lengthy syllabus that spans two volumes. Matriye Academy Revision Notes for Class 11 Chemistry helps students by presenting all pertinent material in simple and concise terms. When you don't have time to go over every line in the textbook before the tests, these notes are an excellent revision aid. If you write personalized notes, you may compare them to our experienced specialists' notes for a more complete picture.
CBSE curriculum preparation is required for Class 11 CBSE Chemistry examinations. It is also recommended to solve sample question papers.
Class 11 Chemistry Notes cover the following chapters:
- Chapter 1 - Some Basic Concepts of Chemistry
- Chapter 2 - Structure of Atom
- Chapter 3 - Classification of Elements and Periodicity in Properties
- Chapter 4 - Chemical Bonding and Molecular Structure
- Chapter 5 - States of Matter
- Chapter 6 - Thermodynamics
- Chapter 7 - Equilibrium
- Chapter 8 - Redox Reactions
- Chapter 9 - Hydrogen
- Chapter 10 - The s-Block Elements
- Chapter 11 - The p-Block Elements
- Chapter 12 - Organic Chemistry - Some Basic Principles and Techniques
- Chapter 13 - Hydrocarbons
- Chapter 14 - Environmental Chemistry
CBSE Class 11 Chemistry is regarded to be simpler, however significant preparation is essential to achieve top scores.
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