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The IIT JEE Main Chemistry syllabus 2023 has been made available in PDF format online by the National Testing Agency (NTA) on its official website (jeemain.nta.nic.in), along with a brochure. On the official website, candidates should review the chemistry syllabus for the Joint Entrance Examination Main 2023 Exam.
The exam conducting authority will base their questions on the topics covered in the IIT JEE Main 2023 chemistry syllabus in the JEE Main Chemistry section. It should be noted that the JEE Main Chemistry 2023 syllabus will cover the same subjects that are covered in the 11th and 12th grades. Physical, Inorganic, and Organic Chemistry make up the three sections of the JEE Main Chemistry curriculum. Before beginning the preparation process, candidates are advised to review the JEE Main Chemistry syllabus so that they can plan their study time accordingly.
We have attempted to cover a variety of JEE Main Chemistry Syllabus topics in this article, including topical weighting, video lectures, mock exams, reference materials, analysis of difficulty level, tips for passing the chemistry section, and preparation methods.
Table of Contents
The NCERT books should be used by candidates to complete the IIT JEE chemistry syllabus. The topics of physical, inorganic, and organic chemistry are provided below. To effectively prepare, review the JEE Main syllabus and weightage.
Section A: Physical Chemistry | ||
---|---|---|
Unit Number | Topic | Sub-topics |
1. | Some Basic Concepts of Chemistry |
Matter and its nature, Dalton’s atomic theory, the concept of the atom, molecule, element, and compound; Physical quantities and their measurements in Chemistry, precision, and accuracy, significant figures, S.I. Units, dimensional analysis; Laws of chemical combination; Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae; Chemical equations and stoichiometry. |
2. | States of Matter |
Classification of matter into solid, liquid, and gaseous states; Gaseous State: Measurable properties of gases; Gas laws – Boyle’s law, Charles’s law, Graham’s law of diffusion, Avogadro’s law, Dalton’s law of partial pressure; The concept of the Absolute scale of temperature; Ideal gas equation, Kinetic theory of gases (only postulates); The concept of average, root mean square, and most probable velocities; Real gases, deviation from Ideal behavior, compressibility factor, van der Waals equation, liquefaction of gases, critical constants; Liquid State: Properties of liquids – vapor pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only); Solid State: Classification of solids-molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea); Bragg’s Law and its applications; Unit cell and lattices, packing in solids (fcc, bcc, and hcp lattices), voids, calculations involving unit cell parameters, an imperfection in solids; Electrical, magnetic, and dielectric properties. |
3. | Atomic Structure |
Discovery of subatomic particles (electron, proton, and neutron); Thomson and Rutherford’s atomic models and their limitations; Nature of electromagnetic radiation, photoelectric effect; The spectrum of the hydrogen atom, Bohr model of a hydrogen atom – its postulates, derivation of the relations for the energy of the electron and radii of the different orbits, limitations of Bohr’s model; Dual nature of matter, de-Broglie relationship, Heisenberg uncertainty principle; Elementary ideas of quantum mechanics, the quantum mechanical model of an atom, its important features, the concept of atomic orbitals as one-electron wave functions; Variation of Ψ1 and Ψ2 with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum, and magnetic quantum numbers), and their significance; Shapes of s, p, and d – orbitals, electron spin, and spin quantum number; Rules for filling electrons in orbitals – Aufbau principle, Pauli exclusion principle, and Hund’s rule, electronic configuration of elements, the extra stability of half-filled, and completely filled orbitals. |
4. | Chemical Bonding and Molecular Structure |
Kossel – Lewis approach to chemical bond formation, the concept of ionic and covalent bonds; Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy; Covalent Bonding: Concept of electronegativity, Fagan’s rule, dipole moment; Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules; Quantum mechanical approach to covalent bonding: Valence bond theory, Its important features, the concept of hybridization involving s, p, and d orbitals; Resonance; Molecular Orbital Theory: Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, the concept of bond order, bond length, and bond energy; Elementary idea of metallic bonding, Hydrogen bonding, and its applications. |
5. | Chemical Thermodynamics |
Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes; The first law of thermodynamics: Concept of work, heat internal energy, and enthalpy, heat capacity, molar heat capacity; Hess’s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization, and solution; The second law of thermodynamics: Spontaneity of processes; Delta S of the universe and Delta G of the system as criteria for spontaneity, Delta Go (Standard Gibbs energy change) and equilibrium constant. |
6. | Solutions |
Different methods for expressing the concentration of a solution: molality, molarity, mole fraction, percentage (by volume and mass both), the vapor pressure of solutions, and Raoult’s Law; Ideal and non-ideal solutions, vapor pressure – composition, plots for ideal and non-ideal solutions; Colligative properties of dilute solutions, relative lowering of vapor pressure, depression of freezing point, the elevation of boiling point, and osmotic pressure; Determination of molecular mass using colligative properties; Abnormal value of molar mass, Hoff factor, and its significance. |
7. | Equilibrium |
Meaning of equilibrium, the concept of dynamic equilibrium; Equilibria involving physical processes: Solid-liquid, liquid – gas, and solid-gas equilibria, Henry’s law, a general characteristic of equilibrium involving physical processes; Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of Delta G and Delta Go in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, the effect of the catalyst; Le Chatelier’s principle; Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted-Lowry, and Lewis) and their ionization, acid-base equilibria (including multistage ionization) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, the solubility of sparingly soluble salts and solubility products, buffer solutions. |
8. | Redox Reactions and Electrochemistry |
Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions; Electrolytic and metallic conduction, conductance in electrolytic solutions, specific and molar conductivities and their variation with concentration; Kohlrausch’s law and its applications; Electrochemical cells: Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half–cell and cell reactions, emf of a Galvanic cell and its measurement; Nernst equation and its applications; Relationship between cell potential and Gibbs’ energy change; Dry cell and lead accumulator, Fuel cells; Corrosion and its prevention. |
9. | Chemical Kinetics |
The rate of a chemical reaction, factors affecting the rate of reactions: concentration, temperature, pressure, and catalyst. Elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first-order reactions, their characteristics and half-lives, and the effect of temperature on the rate of reactions. Arrhenius theory, activation energy, and its calculation, collision theory of bimolecular gaseous reactions (no derivation). |
10. | Surface Chemistry |
Adsorption: Physisorption and chemisorption and their characteristics, factors affecting the adsorption of gases on solids: Freundlich and Langmuir adsorption isotherms, adsorption from solutions. Catalysis: Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis, and its mechanism. Colloidal state: Distinction among true solutions, colloids, and suspensions, classification of colloids: lyophilic, lyophobic. Multimolecular, macromolecular and associated colloids (micelles), preparation, and properties of colloids: Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation, and flocculation. Emulsions and their characteristics. |
Section B: Inorganic Chemistry | ||
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Unit Number | Topic | Sub-topics |
11. | Classification of Elements and Periodicity in Properties |
Modern periodic law and the present form of the periodic table. s, p, d, and f block elements. Periodic trends in properties of elements atomic and ionic radii, ionization enthalpy. Electron gain enthalpy, valence, oxidation states, and chemical reactivity. |
12. | General Principles and Process of Isolation of Metals |
Modes of occurrence of elements in nature, minerals, ores. Steps involved in the extraction of metals: concentration, reduction (chemical and electrolytic methods), and refining with special reference to the extraction of Al, Cu, Zn, and Fe. Thermodynamic and electrochemical principles are involved in the extraction of metals. |
13. | Hydrogen |
The position of hydrogen in the periodic table, isotopes, preparation, properties, and uses of hydrogen. Physical and chemical properties of water and heavy water. Structure, preparation, reactions, and uses of hydrogen peroxide. Classification of hydrides: ionic, covalent, and interstitial. Hydrogen as a fuel. |
14. | S Block Elements (Alkali and Alkaline Earth Metals) |
Group 1 and Group 2 Elements: General introduction, electronic configuration and general trends in physical and chemical properties of elements, anomalous properties of the first element of each group, diagonal relationships. Preparation and properties of some important compounds: sodium carbonate, sodium chloride, sodium hydroxide, and sodium hydrogen carbonate. Industrial uses of lime, limestone, Plaster of Paris, and cement. The biological significance of Na, K, Mg and Ca. |
15. | P Block Elements |
Group 13 to Group 18 Elements: General Introduction, Electronic configuration, and general trends in physical and chemical properties of elements across the periods and down the groups; unique behavior of the first element in each group. Groupwise study of the p block elements. Group 13: Preparation, properties, and uses of boron and aluminum; Structure, properties, and uses of borax, boric acid, diborane, boron trifluoride, aluminum chloride, and alums. Group 14: Tendency for catenation; Structure, properties, and uses of allotropes and oxides of carbon, silicon tetrachloride, silicates, zeolites, and silicones. Group 15: Properties and uses of nitrogen and phosphorus; Allotropic forms of phosphorus; Preparation, properties, structure, and uses of ammonia, nitric acid, phosphine, and phosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of nitrogen and phosphorus. Group 16: Preparation, properties, structures, and uses of dioxygen and ozone; Allotropic forms of sulfur; Preparation, properties, structures, and uses of sulfur dioxide, sulphuric acid (including its industrial preparation); Structures of oxoacids of sulfur. Group 17: Preparation, properties, and uses of chlorine and hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxyacids of halogens. Group 18: Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon. |
16. | D and F Block Elements |
Transition Elements: General introduction, electronic configuration, occurrence and characteristics, general trends in properties of the first-row transition elements: physical properties, ionization enthalpy, oxidation states, atomic radii, color, catalytic behavior, magnetic properties, complex formation, interstitial compounds, alloy formation. Preparation, properties, and uses of K2Cr2O7 and KMnO4. Inner Transition Elements: Lanthanides, Electronic configuration, oxidation states, chemical reactivity, and lanthanoid contraction, and Actinoids: Electronic configuration and oxidation states. |
17. | Coordination Compounds |
Introduction to coordination compounds, Werner’s theory. ligands, coordination number, denticity, chelation. IUPAC nomenclature of mononuclear coordination compounds, isomerism. Bonding-Valence bond approach and basic ideas of Crystal field theory, color, and magnetic properties. Importance of coordination compounds (in qualitative analysis, extraction of metals, and biological systems). |
18. | Environmental Chemistry |
Environmental pollution: Atmospheric, water, and soil. Atmospheric pollution: Tropospheric and stratospheric. Gaseous pollutants: Oxides of carbon, nitrogen, and sulfur, hydrocarbons; their sources, harmful effects, and prevention. Greenhouse effect and Global warming, acid rain. Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects, and prevention. Stratospheric pollution: Formation and breakdown of ozone, depletion of ozone layer its mechanism and effects. Water Pollution: Major pollutants such as pathogens, organic wastes, and chemical pollutants; their harmful effects and prevention. Soil pollution: Major pollutants such as Pesticides (insecticides, herbicides and fungicides) their harmful effects and prevention. Strategies to control environmental pollution. |
Section C: Organic Chemistry | ||
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Unit Number | Topic | Sub-topics |
19. |
Purification and Characterisation of Organic Compounds |
Purification: Crystallization, sublimation, distillation, differential extraction, and chromatography principles and their applications. Qualitative analysis: Detection of nitrogen, sulfur, phosphorus, and halogens. Quantitative analysis (basic principles only): Estimation of carbon, hydrogen, nitrogen, halogens, sulfur, phosphorus. Calculations of empirical formula and molecular formulae; Numerical problems in organic quantitative analysis. |
20. |
Some Basic Principles of Organic Chemistry |
Tetravalency of carbon; Shapes of simple molecules – hybridization (s and p). Classification of organic compounds based on functional groups: -C = C- and those containing halogens, oxygen, nitrogen, and sulfur; Homologous series. Isomerism: structural and stereoisomerism. Nomenclature (Trivial and IUPAC): Covalent bond fission Homolytic and heterolytic: free radicals, carbocations, and carbanions; stability of carbocations and free radicals, electrophiles and nucleophiles. Electronic displacement in a covalent bond: Inductive effect, electromeric effect, resonance, and hyperconjugation. Common types of organic reactions: Substitution, addition, elimination, and rearrangement. |
21. |
Hydrocarbons |
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and reactions. Alkanes: Conformations; Sawhorse and Newman projections (of ethane); Mechanism of halogenation of alkanes. Alkenes: Geometrical isomerism. Mechanism of electrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff’s and peroxide effect); Ozonolysis, oxidation, and polymerization. Alkynes: Acidic character; Addition of hydrogen, halogens, water and hydrogen halides; Polymerization. Aromatic hydrocarbons: Nomenclature, benzene structure and aromaticity. Mechanism of electrophilic substitution: halogenation, nitration, Friedel Crafts alkylation and acylation, directive influence of the functional group in monosubstituted benzene. |
22. |
Organic Compounds Containing Halogens |
General methods of preparation, properties, and reactions. Nature of C-X bond. Mechanisms of substitution reactions. Uses, Environmental effects of chloroform, iodoform, freons, and DDT. |
23. |
Organic Compounds Containing Oxygen |
General methods of preparation, properties, reactions, and uses. Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration. Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration, and sulphonation, Reimer Tiemann reaction. Ethers: Structure. Aldehyde and Ketones: Nature of carbonyl group; Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones. Important reactions such as Nucleophilic addition reactions (addition of HCN, NH3 and its derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); the acidity of hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction. Chemical tests to distinguish between aldehydes and Ketones. Carboxylic Acids: Acidic strength and factors affecting it. |
24. |
Organic Compounds Containing Nitrogen |
General methods of preparation, properties, reactions, and uses. Amines: Nomenclature, classification, structure, basic character and identification of primary, secondary and tertiary amines and their basic character. Diazonium Salts: Importance in synthetic organic chemistry. |
25. |
Polymers |
General introduction and classification of polymers, general methods of polymerization addition and condensation, co-polymerization. Natural and synthetic rubber and vulcanization. Some important polymers with emphasis on their monomers and uses, polyethene, nylon, polyester, and bakelite. |
26. |
Biomolecules |
General introduction and importance of biomolecules. Carbohydrates: Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides or oligosaccharides (sucrose, lactose, maltose), and polysaccharides (starch, cellulose, glycogen). Proteins: Elementary Idea of amino acids, peptide bond, polypeptides; Proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes. Vitamins: Classification and functions. B Chemical constitution of DNA and RNA. Biological functions of nucleic acids. |
27. |
Chemistry in Everyday Life |
Chemicals in medicines: Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamines their meaning and common examples. Chemicals in food: Preservatives, artificial sweetening agents common examples. Cleansing agents: Soaps and detergents, cleansing action. |
28. |
Principles Related to Practical Chemistry |
Detection of extra elements (N, S, halogens) in organic compounds. Detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds. The chemistry involved in the preparation of the following: Inorganic compounds: Mohr’s salt, potash alum, and Organic compounds: Acetanilide, p-nitro acetanilide, aniline yellow, iodoform. The chemistry involved in the titrimetric exercises: Acids bases and the use of indicators, oxalic-acid vs KMnO4, Mohr’s salt vs KMnO4. Chemical principles involved in the qualitative salt analysis: Cations: Pb2+, Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+, and Anions: CO32-, S2-, SO42-, NO2-, NO3-, CI-, Br, I. (Insoluble salts excluded). Chemical principles involved in the following experiments: Enthalpy of solution of CuSO4, Enthalpy of neutralization of strong acid and strong base, Preparation of lyophilic and lyophobic sols, and Kinetic study of the reaction of iodide ion with hydrogen peroxide at room temperature. |
The topic-wise weightage of chemistry questions with regard to number of questions and marks is as follows:
Topics | Number of Questions | Marks |
---|---|---|
Transition Elements and Coordination Chemistry | 3 | 12 |
Periodic table and Representative Elements | 3 | 12 |
Thermodynamics And Gaseous State | 2 | 8 |
Atomic Structure | 2 | 8 |
Chemical Bonding | 2 | 8 |
Chemical And Ionic Equilibrium | 2 | 8 |
Solid State And Surface Chemistry | 2 | 8 |
Nuclear Chemistry And Environment | 2 | 8 |
Mole Concept | 1 | 4 |
Redox Reaction | 1 | 4 |
Electrochemistry | 1 | 4 |
Chemical Kinetics | 1 | 4 |
Solution and Colligative Properties | 1 | 4 |
General Organic Chemistry | 1 | 4 |
Stereochemistry | 1 | 4 |
Hydrocarbon | 1 | 4 |
Alkyl Halides | 1 | 4 |
Carboxylic Acid and their Derivatives | 1 | 4 |
Carbohydrates,amino acid and Polymers | 1 | 4 |
Aromatic Compounds | 1 | 4 |
One of the most essential components of preparation is analyzing your exam strategy. Using mock exams, one must continuously assess the accuracy of their exam preparation strategies and the degree to which they understand various concepts.
NTA helps candidates by offering official practice exams. The NTA’s official website, nta.ac.in, is where the official mock tests can be found. On the NTA’s official website, a total of 18 mock exams have been made available, 15 of which are for Paper 1 and 3 for Paper 2. You can access mock exams in Gujarati, Hindi, and English.
For the preparation of the JEE Main Chemistry section, NTA has made available online video lectures by IIT faculty and experts. The following are the steps to access the video lectures:
During different sessions, the JEE Main Chemistry section’s level of difficulty changes. The following table provides a basic breakdown of the number of questions on the B.E./ B. Tech paper for the JEE Main 2020 January session for the candidates’ understanding:
Sections | Tough | Medium | Easy |
---|---|---|---|
Chemistry | 4 | 11 | 10 |
Mathematics | 2 | 10 | 13 |
Physics | 2 | 7 | 16 |
Although chemistry appears to be the most difficult section in the B.E./B.Tech paper based on the analysis above, candidates must remember that level of difficulty is a subjective issue and chemistry still ranks among the easiest sections to attempt and score well in.
For Physical Chemistry
Since practice is the key to success in physical chemistry, books with quality questions become crucial. Read NCERT textbooks and class notes (from school or coaching) only for theory preparation because side books contain additional topics that are not on any exam syllabus. Refer to these books for practice questions:
For Organic Chemistry
For Inorganic Chemistry
Chemistry, the most highly scored section, frequently proves to be a significant rank-raiser for one’s overall JEE Main performance. However, candidates find that chemistry can be challenging when it comes to preparation. The following advice can help candidates with their JEE Main Chemistry preparation:
Utilize precise, constrained resources: Don’t try to cover the syllabus from several different sources; instead, concentrate on mastering NCERT. Apart from that, you can read various ideas from a few reliable sources. Write down or record notes, then review them frequently.
Solve Questions Everyday: Retention is one of the factors that contribute to a successful attempt in the chemistry section, and retention can only be ensured through practice. Candidates should establish a daily habit of answering 40–50 questions. It is entirely up to you whether you mix questions from different topics or deal with questions from a single topic every day. Making sure that your memorization and analytical abilities are in balance will help you to get the best possible grade in Chemistry.
Identify answers through approximations: It is not a good idea to test your mathematical prowess while answering chemistry questions. Instead, find answers through approximations. You must keep in mind that there is a time limit and find solutions accordingly. Unless the choices are extremely close to one another, candidates can obtain a rough answer and select the option that comes the closest to it.
Practice with past year’s test questions and mock exams: According to all experts, practicing is the most important part of your preparation. To determine the effectiveness of your current plan, continuously practice and evaluate your performance.
Invest your time wisely: Candidates can use the time they save on direct questions to spend on questions that will take longer to complete. Time management is crucial for the chemistry paper.
While the class XI and XII NCERT textbooks are recommended as the best preparation for the JEE Main Chemistry Section because so many direct questions are drawn from them, the following list of additional books may be useful to applicants:
Authors/Publishers | Books |
---|---|
P Bahadur | Concept of Physical Chemistry for JEE Main & Advanced |
N Awasthi | Physical Chemistry |
Solomons and Fryhle | Organic Chemistry |
Morrison and Boyd | Organic Chemistry |
R.K Gupta | Arihant’s Practice Book Chemistry for JEE Main And Advanced |
J D Lee | Concise Inorganic Chemistry |
Freedman and Young | University Chemistry |
MS Chauhan | Elementary problems in Organic Chemistry |
O.P. Tandon | Physical Chemistry; Organic Chemistry |
P.W.Atkins | Physical Chemistry |
R.C. Mukherjee | Modern Approach to Chemical Calculations |
Ans. For JEE Mains Chemistry preparation, NCERT books are extremely helpful. But it is not enough.
The part with the highest scores is inorganic chemistry. And NCERT books are a requirement for this section. In previous years, NCERT-approved questions were included. But you should also read your textbooks and class notes.
NCERT is insufficient for Physical and Inorganic Chemistry. In order to have a strong command of these sections, you must practice a lot. Go through the NCERT for these sections, make notes for key passages, and complete practice exercises.
Ans. You must use wise preparation methods if you want to achieve a JEE Main score of 250 or higher. Utilize your time wisely and revise each section thoroughly. For a thorough understanding of the subject, you must solve two papers per day.
For the JEE Mains, chemistry scores quite well. You must strive for a 90–100 overall score.
NCERT is sufficient for Physical Chemistry.
You must practice in order to perform well in math. You can easily achieve a high grade if you put in the extra effort. For JEE Mains, the coordinate geometry section has a high passing rate.
It can be challenging to achieve a physics score of 70 to 90. Learn to use shortcuts and tricks to finish the task faster. You can study NCERT to understand physics concepts, and books like HCV can help you solve problems.
Browse through the last two months’ exam papers to see how various topics were weighted. To solve issues faster, use shortcuts and tricks.
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