AP Inter 1st year Chemistry Textbook & Study Material 2022 – Download Question Papers, Syllabus Here

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AP Inter 1st Year Chemistry Textbook & Study Material 2022:

AP Inter 1st Year Chemistry Textbook & Study Material 2022 are your primary source of information as you prepare for the 2022 Intermediate Board Exam.  The AP Intermediate Board (Board of Intermediate Education) (BIEAP) has announced the AP Inter 1st Year  Chemistry Text Book, Syllabus, Examination Time Table, Previous Papers, and Examination Pattern. The timetable for the 11th Class general and vocational examinations has been made public by the Board of Intermediate Education. Candidates must refer to the AP Board of Intermediate Education’s official website to obtain a complete examination schedule, detailed syllabus, and detailed examination pattern for each subject (www.bieap.gov.in). The AP Board of Intermediate Education AP Inter 1st year Chemistry Textbook 2022 will publish the timetable.

Candidates must obtain the PDF Document published by the AP Intermediate board or get the Chemistry Syllabus from our article. In this article, we are providing direct links to download the Textbook, Examination Timetable, Examination Pattern, and Detailed Syllabus of Chemistry Subjects. Here are direct links to the PDF documents for download. For the convenience of candidates, previous test questions on different topics are also made available. Please feel free to download the Chemistry Subject textbook and whole syllabus and get ready for the upcoming test. Candidates should carefully mark the crucial questions and finish reading them before focusing on the syllabus material that carries a lower weight. We provide all the information about Subject right here on our website questionspapers.co.in.

AP Textbooks Download PDF – Overview

Name of the Organizations AP Intermediate Board (Board of Intermediate Education) (BIEAP)
Name of the Website in which textbooks got published NCERT
Subjects Telugu, Hindi, English, Maths, Science, Social Studies
Available Information Textbook
Classes Intermediate 1st Year
Official Website bie.ap.gov.in


About Board of Intermediate Education, AP:

  • The Andhra Pradesh Board of Intermediate Education or BIEAP board is the governing and regulating authority for intermediate education in the state for classes 11 and 12. Intermediate I refers to the 11th grade course, while Intermediate II refers to the 12th-grade course. The Intermediate Public Exams, on the other hand, are significant exams that are administered in a systematic manner. When it comes to tests, the AP BIEAP is stricter, and this is done to test the student’s entire potential and knowledge of the many courses. Find information about the Board of Intermediate Education of Andhra Pradesh in this article, as well as links to numerous resources for preparing for board exams.
  • For the academic year 2021-2022, the Board of Intermediate Education of Andhra Pradesh has issued Intermediate Textbooks for Junior and Senior Inter MPC, BIPC, CEC, MEC, and all other Group Students. BIEAP provides Digital Format eBooks and Pdf Books to all government and private college Telugu Medium (TM), English Medium (EM), Urdu Medium (UM), and Hindi Medium (HM) students.

AP Inter 1st year Textbook & Study Material 2022 – All Subjects

  • Mathematics 1A
  • Mathematics 1B
  • Botany
  • Zoology
  • Physics
  • Chemistry
  • Economics
  • Civics
  • History
  • Commerce
  • English
  • Hindi
  • Urdu
  • Telugu

AP Inter 1st Year Textbook & Study Material Details 2022 – Overview

Name of the Board Board of Intermediate Education, AP
Examination Name  Inter First Year Public Examinations 2022 (Inter 1st Year)
Groups Arts, Science and Commerce
Subjects Telugu, English, Hindi, Urdu, Sanskrit, Mathematics, Physics, Chemistry, Botany, Zoology and etc.
Date of Exams 6th May 2022 to 23rd May 2022
Official Website bie.ap.gov.in
Status Available
Category Andhra Pradesh (AP), Intermediate, Textbook


AP Inter 1st Year Chemistry Syllabus 2022:

AP 11th Class / Inter 1st Year mostly consists of the following courses: (Sanskrit, English, Hindi, Telugu). Candidates are free to select any Language Group. We describe the Chemistry Syllabus in this article. All of the Intermediate groups have access to the Chemistry syllabus. Below is a description of the Chemistry subject’s comprehensive syllabus.

Detailed Chemistry Unit Wise Syllabus:

1.1 Sub- atomic particles
1.2 Atomic models- Rutherford’s Nuclear model of atom
1.3 Developments to the Bohr’s model of atom
1.3.1 Nature of electromagnetic radiation.
1.3.2 Particle nature of electromagnetic radiation- Planck’s
quantum theory.
1.4 Bohr’s model for Hydrogen atom.
1.4.1 Explanation of line spectrum of hydrogen.
1.4.2 Limitations of Bohr’s model
1.5Quantum mechanical considerations of sub atomic particles.
1.5.1 Dual behaviour of matter.
1.5.2 Heisenberg’s uncertainty principle.
1.6 Quantum mechanical model of an atom. Important
features of Quantum mechanical model of atom.
1.6.1 Orbitals and quantum numbers.
1.6.2 Shapes of atomic orbitals.
1.6.3 Energies of orbitals.
1.6.4 Filling of orbitals in atoms. Aufbau Principle, Pauli’s exclusion Principle and Hund’s rule of maximum multiplicity.
1.6.5 Electronic configurations of atoms.
1.6.6 Stability of half filled and completely filled orbitals.

2.1 Need to classify elements
2.2 Genesis of periodic classification.
2.3 Modern periodic law and present form of the periodic table.
2.4 Nomenclature of elements with atomic number greater than 100
2.5 Electronic configuration of elements and the periodic
2.6 Electronic configuration and types of elements s,p,d.and f blocks.
2.7.1 Trends in physical properties:
(a) Atomic radius
(b) Ionic radius
(c)Variation of size in inner transition elements.
(d)Ionization enthalpy.
(e) Electron gain enthalpy
(f) Electro negativity.
2.7.2 Periodic trends in chemical properties:
(a) Valence or Oxidation states.
(b) Anomalous properties of second period elements – diagonal relationship.
2.7.3 Periodic trends and chemical reactivity

3.1 Kossel – Lewis approach to chemical bonding.
3.2 Ionic or electrovalent bond – Factors favourable for the formation of ionic compounds-Crystal structure of sodium chloride-General properties of ionic compounds.
3.3 Bond Parameters – bond length, bond angle, and bond enthalpy, bond order, resonance-Polarity of bonds dipole moment
3.4 Valence Shell Electron Pair Repulsion (VSEPR) theories. Predicting the geometry of simple molecules.
3.5 Valence bond theory-Orbital overlap concept-Directional properties of bonds-overlapping of atomic orbitals
strength of sigma and pi bonds-Factors favouring the formation of covalent bonds
3.6 Hybridisation- different types of hybridization involving s, p and d orbitals- shapes of simple covalent molecules.
3.7 Coordinate bond –definition with examples.
3.8 Molecular orbital theory – Formation of molecular orbitals,Linear combination of atomic orbitals (LCAO)-conditions forcombination of atomic orbitals – Energy level diagrams for molecular orbitals -Bonding in some homo nuclear diatomic molecules- HЇ,HeЇ,LiЇ,BЇ,CЇ,NЇ,and OЇ
3.9 Hydrogen bonding-cause of formation of hydrogen bond-Types of hydrogen bonds-inter and intra molecular-Generalproperties of hydrogen bonds.

4.1 Intermolecular forces
4.2 Thermal Energy
4.3 Intermolecular forces Vs Thermal interactions.
4.4 The Gaseous State.
4.5 The Gas Laws
4.6 Ideal gas equation.
4.7 Graham’s law of diffusion – Dalton’s Law of partialpressures.
4.8 Kinetic molecular theory of gases.
4.9 Kinetic gas equation of an ideal gas (No derivation) deduction of gas laws from Kinetic gas equation.
4.10 Distribution of molecular speeds – rms, average and most probable speeds-Kinetic energy of gas molecules.
4.11 Behaviour of real gases – Deviation from Ideal gas behaviour – Compressibility factor Vs Pressure diagrams of real gases.
4.12 Liquefaction of gases
4.13 Liquid State – Properties of Liquids in terms of Inter molecular interactions – Vapour pressure, Viscosity and
Surface tension (Qualitative idea only. No mathematical derivation)

5.1 Some Basic Concepts – Properties of matter – uncertainty in Measurement-significant figures, dimensional analysis.
5.2 Laws of Chemical Combinations – Law of Conservation of Mass, Law of Definite Proportions, Law of Multiple Proportions, Gay Lussac’s Law of Gaseous Volumes, Dalton’s Atomic Theory, Avogadro Law, Principles,Examples.
5.3 Atomic and molecular masses- mole concept and molar mass concept of equivalent weight.
5.4 Percentage composition of compounds and calculations of empirical and molecular formulae of compounds.
5.5 Stoichiometry and stoichiometric calculations.
5.6 Methods of Expressing concentrations of solutions-mass percent, mole fraction, molarity, molality and normality.
5.7 Redox reactions-classical idea of redox reactions, oxidation and reduction reactions-redox reactions in terms of electron transfer.
5.8 Oxidation number concept.
5.9 Types of Redox reactions-combination, decomposition, displacement. and disproportionation reactions
5.10 Balancing of redox reactions – oxidation number method Half reaction (ion-electron) method.
5.11 Redox reactions in Titrimetry.

6.1 Thermodynamic Terms.
6.1.1 The system and the surroundings.
6.1.2. Types of systems and surroundings.
6.1.3 The state of the system.
6.1.4 The Internal Energy as a State Function.
(a) Work (b) Heat (c) The general case, the first law of Thermodynamics.
6.2 Applications.
6.2.1 Work
6.2.2 Enthalpy, H- a useful new state function
6.2.3 Extensive and intensive properties.
6.2.4 Heat capacity
6.2.5 The relationship between CP and Cv.
6.3 Measurement of ̈U and ̈ H: Calorimetry
6.4 Enthalpy change, ̈r H of reactions – reaction Enthalpy
(a) Standard enthalpy of reactions.
(b) Enthalpy changes during transformations.
(c) Standard enthalpy of formation.
(d) Thermo chemical equations.
(e) Hess’s law of constant Heat summation.
6.5 Enthalpies for different types of reactions.
(a) Standard enthalpy of combustion ( ̈c HO )
(b) Enthalpy of atomization ( ̈a Hø), phase transition, sublimation and ionization.
(c) Bond Enthalpy ( ̈bond Hø )
(d) Enthalpy of solution ( ̈sol Hø ) and dilution.
6.6 Spontaneity.
(a) Is decrease in enthalpy a criterion for spontaneity?
(b) Entropy and spontaneity, *the second law of thermodynamics.
(c) Gibbs Energy and spontaneity.
6.7 Gibbs Energy change and equilibrium.
6.8 Absolute entropy and the third law of thermodynamics.

7.1 Equilibrium in Physical process.
7.2 Equilibrium in chemical process – Dynamic Equilibrium
7.3 Law of chemical Equilibrium – Law of mass action and Equilibrium constant.
7.4 Homogeneous Equilibria, Equilibrium constant in gaseous systems. Relationship between KP and Kc
7.5 Heterogeneous Equilibria.
7.6 Applications of Equilibrium constant.
7.7 Relationship between Equilibrium constant K, reaction quotient Q and Gibbs energy G.
7.8 Factors affecting Equilibria.-Le-chatlieprinciple application to industrial synthesis of Ammonia and Sulphur trioxide.
7.9 Ionic Equilibrium in solutions.
7.10 Acids, bases and salts- Arrhenius, Bronsted-Lowry and Lewis concepts of acids and bases.
7.11 Ionisation of Acids and Bases –Ionisation constant of water and it’s ionic product- pH scale-ionisation constants of weak acids-ionisation of weak bases-relation between Ka and Kb-Di and poly basic acids and di and poly acidic Bases-Factors affecting acid strength-Common ion effect in the ionization of acids and bases-Hydrolysis of salts and pH of their solutions.
7.12 Buffer solutions-designing of buffer solution-Preparation of Acidic buffer
7.13 Solubility Equilibria of sparingly soluble salts. Solubility product constant Common ion effect on solubility of Ionic salts.

8.1 Position of hydrogen in the periodic table.
8.2 Dihydrogen-Occurance and Isotopes.
8.3 Preparation of Dihydrogen
8.4 Properties of Dihydrogen
8.5 Hydrides: Ionic, covalent, and non-stiochiometric hydrides.
8.6 Water: Physical properties; structure of water, ice. Chemical properties of water; hard and soft water Temporary and permanent hardness of water
8.7 Hydrogen peroxide: Preparation; Physical properties; structure and chemical properties; storage and uses.
8.8 Heavy Water
8.9 Hydrogen as a fuel.

9.1 Alkali metals; Electronic configurations; Atomic and Ionic radii; Ionization enthalpy; Hydration enthalpy; Physical properties; Chemical properties; Uses
9.2 General characteristics of the compounds of the alkali metals: Oxides; Halides; Salts of Oxy Acids.
9.3 Anomalous properties of Lithium: Differences and similarities with other alkali metals. Diagonal relationship; similarities between Lithium and Magnesium.
9.4 Some important compounds of Sodium: Sodium Carbonate; Sodium Chloride; Sodium Hydroxide; Sodium hydrogen carbonate.
9.5 Biological importance of Sodium and Potassium. Group 2 Elements:
9.6 Alkaline earth elements; Electronic configuration; Ionizationenthalpy; Hydration enthalpy; Physical properties,
Chemical properties; Uses.
9.7 General characteristics of compounds of the Alkaline Earth Metals: Oxides, hydroxides, halides, salts of Oxyacids
(Carbonates; Sulphates and Nitrates).
9.8 Anomalous behavior of Beryllium; its diagonal relationshipwith Aluminum.
9.9 Some important compounds of calcium: Preparation and uses of Calcium Oxide ; Calcium Hydroxide; Calcium Carbonate;Plaster of Paris; Cement.
9.10 Biological importance of Calcium and Magnesium.

10.1 General introduction – Electronic configuration, Atomic radii, Ionization enthalpy, Electro negativity; Physical & Chemical properties.
10.2 Important trends and anomalous properties of boron.
10.3 Some important compounds of boron – Borax, Ortho boric acid,diborane.
10.4 Uses of boron, aluminium and their compounds.

11.1 General introduction – Electronic configuration, Atomic radii, Ionization enthalpy, Electro negativity; Physical & Chemical properties.
11.2 Important trends and anomalous properties of carbon.
11.3 Allotropes of carbon.
11.4 Uses of carbon.
11.5 Some important compounds of carbon and silicon – carbonmonoxide, carbon dioxide,Silica, silicones, silicates and zeolites.

12.1 Definition of terms: Air, Water and Soil Pollutions.
12.2 Environmental Pollution
12.3 Atmospheric pollution; Tropospheric Pollution; GaseousAir Pollutants (Oxides of Sulphur; Oxides of Nitrogen; Hydro Carbons; Oxides of Carbon (CO; CO2). Global warming and Green house effect.
12.4 Acid Rain- Particulate Pollutants- Smog.
12.5 Stratospheric Pollution: Formation and breakdown of Ozone- Ozone hole- effects of depletion of the Ozone layer.
12.6 Water Pollution: Causes of Water Pollution; International standards for drinking water.
12.7 Soil Pollution: Pesticides, Industrial Wastes.
12.8 Strategies to control environmental pollution- waste Management- collection and disposal.
12.9 Green Chemistry: Green chemistry in day-to-day life; Dry cleaning of clothes; Bleaching of paper; Synthesis of chemicals

13.1 General introduction.
13.2 Tetravalency of Carbon: shapes of organic compounds.
13.3 Structural representations of organic compounds.
13.4 Classification of organic compounds.
13.5 Nomenclature of organic compounds.
13.6 Isomerism.
13.7 Fundamental concepts in organic reaction mechanisms.
13.7.1 Fission of covalent bond.
13.7.2 Nucleophiles and electrophiles.
13.7.3 Electron movements in organic reactions.
13.7.4 Electron displacement effects in covalent bonds.
13.7.5 Types of Organic reactions.
13.8 Methods of purification of organic compounds.
13.9 Qualitative elemental analysis of organic compounds.
13.10 Quantitative elemental analysis of organic compounds. HYDROCARBONS
13.11 Classification of Hydrocarbons.
13.12 Alkanes – Nomenclature, isomerism (structural and conformations of ethane only)
13.12.1 Preparation of alkanes
13.12.2 Properties – Physical properties and chemical Reactivity, Substitution reactions – Halogenation(free radical mechanism), Combustion, Controlled Oxidation, Isomerisation, Aromatization, reaction with steam and Pyrolysis.

13.13 Alkenes- Nomenclature, structure of ethane, Isomerism (structural and geometrical).
13.13.1 Methods of preparation.
13.13.2 Properties- Physical and chemical reactions: Additio=of Hydrogen, halogen, water, sulphuric acid, Hydrogen halides (Mechanism- ionic and peroxide effect, Markovnikov’s , antiMarkovnikov’s or Kharasch effect). Oxidation, Ozonolysis and Polymerization.
13.14 Alkynes – Nomenclature and isomerism, structure of acetylene. Methods of preparation of acetylene.
13.14.1 Physical properties, Chemical reactions- acidiccharacter of acetylene, addition reactions- of hydrogen, Halogen, Hydrogen halides and water. Polymerization.
13.15 Aromatic Hydrocarbons: Nomenclature and isomerism.Structure of benzene, Resonance and aromaticity.
13.15.1 Preparation of benzene. Physical properties. Chemicalproperties: Mechanism of electrophilic substitution. Electrophilic substitution reactions- Nitration, Sulphonation, Halogenation, Friedel-Craft’ alkylation and acylation.
13.15.2 Directive influence of functional groups in mono substituted benzene, Carcinogenicity and toxicity.

AP Inter 1st Year / 11th Class Chemistry Question Papers 2022:

  • BIEAP has created a structured collection of thorough and educational curriculum for intermediate first-year students.
  • Students can ask their friends and neighbours for further information by passing along these AP Inter 1st Year Question Paper 2022.
  • The most urgent educational needs of the students were also taken into consideration when developing the AP Inter Question Paper 2022.
  • The preceding exam’s question paper will be thoroughly understood by AP Intermediate first-year students.
  • The BIEAP’s rules were followed in the preparation of these AP Inter 1st Year Previous Question Papers.

AP Inter First Year 2022 Chemistry Previous Question Papers

Name of the Subject Download PDF (English Medium) Download PDF (Urdu Medium) Download PDF (Telugu Medium)
Chemistry Paper-I [September 2021] Click Here Click Here
Chemistry Paper-I [March 2020] Click Here Click Here Click Here
Chemistry Paper-I [May 2019] Click Here Click Here Click Here
Chemistry Paper-I [March 2019] Click Here Click Here Click Here
Chemistry Paper-I [May 2018] Click Here Click Here
Chemistry Paper-I [March 2018] Click Here Click Here


AP Intermediate Exam Pattern:

  • The marks distribution, exam duration, and mode are all included in the AP Intermediate Exam pattern. As a result, students should be informed of the entire AP Intermediate 2022 exam pattern. Please see the information below for more information.
  • Students must study six subjects for the BIEAP Intermediate Exam 2022, which will be held in a set manner. Students must choose six subjects.
  • There will be three language papers among the six topics, with the remaining three being General Science, Social Studies, and Mathematics.
  • There will be eleven papers in each of these six disciplines, with the exception of a second language paper, each subject having two papers.
  • Each AP Intermediate 2022 exam paper will be worth 100 points. The summative evaluation (board exam) accounts for 80 of the 100 points, while the formative test accounts for 20.
    The minimal passing score for each paper is 35, which you can achieve rapidly if you use Andhra Pradesh Inter First-year & Second-year Syllabus Copies to study.

AP Intermediate  Eligibility Criteria

The minimal qualifications that students must fulfil before submitting their applications are the AP Intermediate 2022 eligibility standards. The prerequisites for Andhra Pradesh Intermediate 2022 are as follows:

For Intermediate, students must be enrolled in a college that is accredited with the Andhra Pradesh Board.
The Andhra Pradesh Board or a board that has been approved by the Andhra Pradesh Board must have awarded the student’s class 10 diploma.
The minimum age requirement for Intermediate AP Inter 1st year Chemistry Textbook should be carefully considered since age plays such a significant role in a student’s career.

AP Inter 1st year Textbook & Study Material 2022 – All Subjects Work Book

S.No Resource Material/ Work Book Year Month Subject Download Link
1 Work Book 2020 November English Paper-I Click Here
3 Work Book 2020 January Urdu Paper-I Click Here
5 Work Book 2020 February Civics Paper-I (TM) Click Here
7 Work Book 2020 February Botany Paper-I (EM) Click Here
8 Work Book 2020 February Chemistry Paper-I Click Here
9 Work Book 2020 February Commerce Paper-I Click Here
11 Work Book 2020 February Mathematics-I (B) Click Here


AP Inter 1st year Textbook & Study Material 2022 – All Subjects

Subject-wise SCERT AP Intermediate 1st Year Books 2021 (English Medium) Pdf Download

BIEAP 1st Year Intermediate Textbooks 2021 Pdf Download (Hindi Medium)

Click here for Board of Intermediate Education AP (BIEAP) Official website

Click Here to Download AP Inter 1st Year Chemistry Syllabus

Click Here to Download AP Inter 1st Year Textbook & Study Material

FAQs regarding AP 1st year Inter Chemistry Textbook & Study Material 2022

In which Group, English Subjects will be present in the Intermediate Board?

English Subject is present in all most all the Intermediate Groups (MPC, HEC, CEC, MEC, Bi. P.C)

Who will conduct the Intermediate Education in Andhra Pradesh State?

Board of Intermediate Education, AP (BIEAP)

What is the full form of BIEAP?

Board of Intermediate Education, AP (BIEAP)

What is the Official Website of BIEAP?


What is the minimum pass mark out of 75 in Intermediate in AP?

Students can get minimum of 30 marks to qualify for the examination.

What is the first language in Intermediate in AP?

What are the Subjects in MPC?
MPC subjects or commonly known as PCM subjects consist of Mathematics, Physics, Chemistry, and English. Along with these mandatory subjects, candidates choose a fifth subject that is elective.

How many subjects are there in Intermediate 1st Year AP?
Students must study six subjects for the BIEAP Intermediate Exam 2022, which will be held in a set manner. Students must choose six subjects. There will be three language papers among the six topics, with the remaining three being General Science, Social Studies, and Mathematics AP Inter 1st year Chemistry Textbook.

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