NCERT Exemplar Solutions-Organic Chemistry Some Basic Principles and Techniques for Class 11

NCERT Exemplar Solutions-Organic Chemistry Some Basic Principles and Techniques for Class 11

I. Multiple-choice Questions (Type-I)

1. Which of the following is the correct IUPAC name?

(i) 3-Ethyl-4, 4-dimethylheptane

(ii) 4,4-Dimethyl-3-ethylheptane

(iii) 5-Ethyl-4, 4-dimethylheptane

(iv) 4,4-Bis(methyl)-3-ethylheptane

Solution:

Option (i) the answer.

2. The IUPAC name is ________ for

I. Multiple-choice Questions (Type-I)

(i) 1-hydroxypentane-1,4-dione

(ii) 1,4-dioxopentanol

(iii) 1-carboxybutan-3-one

(iv) 4-oxopentanoic acid

Solution:

Option (iv) is the answer.

3. The IUPAC name for

I. Multiple-choice Questions (Type-I)

(i) 1-Chloro-2-nitro-4-methylbenzene

(ii) 1-Chloro-4-methyl-2-nitrobenzene

(iii) 2-Chloro-1-nitro-5-methylbenzene

(iv) m-Nitro-p-chlorotoluene

Solution:

Option (ii) is the answer.

4. Electronegativity of carbon atoms depends upon their state of hybridisation.

In which of the following compounds, the carbon marked with an asterisk is

most electronegative?

(i) CH3 – CH2 – *CH2 –CH3

(ii) CH3 – *CH = CH – CH3

(iii) CH3 – CH2 – C ≡ *CH

(iv) CH3 – CH2 – CH = *CH2

Solution:

Option (iii) is the answer.

5. In which of the following, functional group isomerism is not possible?

(i) Alcohols

(ii) Aldehydes

(iii) Alkyl halides

(iv) Cyanides

Solution:

Option (iii) is the answer.

6. The fragrance of flowers is due to the presence of some steam volatile organic

compounds called essential oils. These are generally insoluble in water at

room temperature but are miscible with water vapour in the vapour phase. A

a suitable method for the extraction of these oils from the flowers is:

(i) Distillation

(ii) Crystallisation

(iii) Distillation under reduced pressure

(iv) Steam distillation

Solution:

Option (iv) is the answer.

7. During the hearing of a court case, the judge suspected that some changes in the

documents had been carried out. He asked the forensic department to check

the ink used at two different places. According to you, which technique can

give the best results?

(i) Column chromatography

(ii) Solvent extraction

(iii) Distillation

(iv) Thin-layer chromatography

Solution:

Option (iv) is the answer.

8. The principle involved in paper chromatography is

(i) Adsorption

(ii) Partition

(iii) Solubility

(iv) Volatility

Solution:

Option (ii) is the answer.

9. What is the correct order of decreasing stability of the following cations?

I. Multiple-choice Questions (Type-I)

(i) II > I > III

(ii) II > III > I

(iii) III > I > II

(iv) I > II > III

Solution:

Option (i) is the answer.

10. Correct IUPAC name for is ___________.

I. Multiple-choice Questions (Type-I)

(i) 2- ethyl-3-methylpentane

(ii) 3,4- dimethylhexane

(iii) 2-sec-butylbutane

(iv) 2, 3-dimethylbutane

Solution:

Option (ii) is the answer.

11. In which of the following compounds the carbon marked with an asterisk is

expected to have the greatest positive charge?

(i) *CH3—CH2—Cl

(ii) *CH3—CH2—Mg+Cl–

(iii) *CH3—CH2—Br

(iv) *CH3—CH2—CH3

Solution:

Option (i) is the answer.

12. Ionic species are stabilised by the dispersal of charge. Which of the

following carboxylate ion is the most stable?

I. Multiple-choice Questions (Type-I)

Solution:

Option (iv) is the answer.

13. Electrophilic addition reactions proceed in two steps. The first step

involves the addition of an electrophile. Name the type of intermediate

formed in the first step of the following addition reaction.

H3

C—HC = CH2 + H+ →?

(i) 2° Carbanion

(ii) 1° Carbocation

(iii) 2° Carbocation

(iv) 1° Carbanion

Solution:

Option (iii) is the answer.

14. A covalent bond can undergo fission in two different ways. The correct

representation involving heterolytic fission of CH3—Br is

I. Multiple-choice Questions (Type-I)

Solution:

Option (ii) is the answer.

15. The addition of HCl to alkene proceeds in two steps. The first step is the

attack of H+ ion C=C to a portion which can be shown as

Solution:

Option (ii) is the answer.

II. Multiple Choice Questions (Type-II)

In the following questions, two or more options may be correct.

16. Which of the following compounds contains all the carbon atoms in the same

hybridisation state?

(i) H—C ≡ C—C ≡ C—H

(ii) CH3—C ≡ C—CH3

(iii) CH2 = C = CH2

(iv) CH2 = CH—CH = CH2

Solution:

Option (i) and (iv) are the answers.

17. In which of the following representations given below spatial arrangement of

group/ atom different from that given in structure ‘A’?

I. Multiple-choice Questions (Type-I)

Solution:

Option (i), (iii) and (iv) are the answers.

18. Electrophiles are electron-seeking species. Which of the following groups contain only electrophiles?

(i) BF3, NH3, H2O

(ii) AlCl3, SO3 , + NO2

(iii) NO2+ , CH3+ , CH3 –C+ = O

(iv) C2H-5, C2H5, CH5+

Solution:

Option (ii) and (iii) are the answers.

Note: Consider the following four compounds for answering question 19

and 20.

I. Multiple-choice Questions (Type-I)

19. Which of the following pairs are position isomers?

(i) I and II

(ii) II and III

(iii) II and IV

(iv) III and IV

Solution:

Option (ii) is the answer.

20. Which of the following pairs are not functional group isomers?

(i) II and III

(ii) II and IV

(iii) I and IV

(iv) I and II

Solution:

Option (i) and (iii) are the answers.

21. A nucleophile is a species that should have

(i) a pair of electrons to donate

(ii) positive charge

(iii) negative charge

(iv) electron-deficient speciesSolution:

Option (i) and (iii) are the answers.

22. Hyperconjugation involves the delocalisation of ___________.

(i) electrons of the carbon-hydrogen σ bond of an alkyl group directly attached

to an atom of the unsaturated system.

(ii) electrons of carbon-hydrogen σ bond of alkyl group directly attached to

the positively charged carbon atom.

(iii) π-electrons of carbon-carbon bond

(iv) lone pair of electrons

Solution:

Option (i) and (ii) are the answers.

III. Short Answer Type

Note: Consider structures I to VII and answer questions 23–26.

I. Multiple-choice Questions (Type-I)

23. Which of the above compounds form pairs of metamers?

Solution:

V and VI form pairs of metamers. (metamers of ethers). Here in compounds V and VI, the chain length is the same, but the distribution of carbons is different around oxygen atom.

24. Identify the pairs of compounds which are functional group isomers.

Solution:

I and V, I and VI, I and VII, II and V, II and VI, II and VII, III and V, III and VI, III and VII, IV and V, IV and VI, IV and VII. Alcholol is the function group of each ether in the given seven compounds.

25. Identify the pairs of compounds that represent position isomerism.

Solution:

I and II, III and IV, V and VI are the compounds which represent the position isomerism.

Position isomerism means where the length of the parent chain and functional group is the same, but the position of the functional group is different; then it is called position isomer.

26. Identify the pairs of compounds that represent chain isomerism.

Solution:

I and III, I and IV, II and III, II and IV, II and IV, V and VII, VI and VII are the compounds which represent chain isomerism. Compounds having the same molecular formula but varying in the length of the parent chain(as they are branched) is called chain isomerism.

27. For testing halogens in an organic compound with AgNO3 solution, sodium extract (Lassaigne’s test) is acidified with dilute HNO3. What will happen if a student acidifies the extract with dilute H2 SO4 in place of dilute HNO3?

Solution:

If dilute H2 SO4is added, then sodium sulphide and sodium cyanine are not decomposed thereby, we will not get the correct result if halides are also present.

28. What is the hybridisation of each carbon in H2C = C = CH2?

Solution:

The terminal carbons are sp2 hybridised as they form 3 (2 with H and 1 with C) sigma bonds and 1 pi bond(between carbons) while the centre carbon is sp hybridised (as it forms 2 sigma bonds, 1 with each carbon and 2 pi bonds, one with each carbon).

29. Explain how is the electronegativity of carbon atoms related to their state of hybridisation in an organic compound?

Solution:

Hybridization for carbon in organic compounds is of three types, sp, sp2 and sp3. The more the ‘s’ character, the more is the electronegativity of the carbon as ‘s’ orbitals are closer to the nucleus; hence electrons held more closely.

30. Show the polarisation of the carbon-magnesium bond in the following structure.

CH3—CH2—CH2—CH2—Mg—X

Solution:

CH3—CH2—CH2—δ-CH2—δ+Mg+ X-

Carbon is more electronegative than Mg because of the electronegativity difference in the bond between C-Mg is highly polarised. C being more electronegative the electron density is towards C hence Mg readily loses its electron to form C-( carbanion).

31. Compounds with same molecular formula but differing in their structures are

said to be structural isomers. What type of structural isomerism is shown by

I. Multiple-choice Questions (Type-I)

Solution:

In the above structures, both have the same functional group (thioether/sulphide), but there is a difference in the arrangement of atoms in the main chain. So they can exhibit chain isomerism.

32. Which of the following selected chains is correct to name the given compound according to the IUPAC system.

I. Multiple-choice Questions (Type-I)

a. The main(parent) chain should be the longest possible carbon chain with all the carbons with the functional groups included in them. The above selection is the only possible one with both the functional groups in the main chain.

b. Out of carboxylic acid and alcohol acid gets the priority hence the numbering starts from carboxylic carbon.

c. There is a branched alkyl group substitution at second carbon

d. There is a hydroxyl group at 4th carbon therefore it can be named as 2-(2-methyl butyl)-4-hydroxybutanoic acid.

33. In DNA and RNA, the nitrogen atom is present in the ring system. Can the Kjeldahl method be used for the estimation of nitrogen present in these? Give reasons.

Solution:

The Kjeldahl method cannot be used for the estimation of nitrogen present in DNA and RNA because nitrogen cannot be converted into ammonium sulphate in the conditions provided in this method. The difficulty in decomposing ring structures limits this test for DNA and RNA.

34. If a liquid compound decomposes at its boiling point, which method(s) can you choose for its purification. It is known that the compound is stable at low pressure, steam volatile and insoluble in water.

Solution:

As the liquid compound decomposes at its boiling point, which means that the compound is heat-sensitive, hence we use “Steam distillation” for its purification. It is done for temperature-sensitive materials.

Note: Answer questions 35 to 38 based on the information given below:

“Stability of carbocations depends upon the electron releasing inductive effect

of groups adjacent to positively charged carbon atom involvement of

neighbouring groups in hyperconjugation and resonance.”

35. Draw the possible resonance structures for and predict which of the structures is more stable. Give the reason for your answer.

Solution:

I. Multiple-choice Questions (Type-I)

Structure C is more stable than that of structure A because, in structure C, the octet of all the atoms is complete, whereas, in structure A, C-atom having a positive charge is not having 8 electrons in its valence shell.

36. Which of the following ions is more stable? Use resonance to explain your answer.

I. Multiple-choice Questions (Type-I)

Solution:

I. Multiple-choice Questions (Type-I)

The stability of carbocation is decided by inductive effect, hyperconjugation, resonance etc.

As structure A has a carbocation, which is primary and allylic carbocation, whereas the carbocation in structure B has secondary and allylic carbocation.

Hence, structure B is more stable.

37. The structure of triphenylmethylcation is given below. This is very stable, and some of its salts can be stored for months. Explain the cause of the high stability of this cation.

I. Multiple-choice Questions (Type-I)

Solution:

Triphenylcarbocation is tertiary carbocation and the positive charge is on the carbon atom, which is stabilised by the three phenyl group by resonance. Due to the resonance, the stability increases.

38. Write structures of various carbocation that can be obtained from 2-methyl butane. Arrange these carbocations in the order of increasing stability.

Solution:

I. Multiple-choice Questions (Type-I)

the stability order is found to be:

(III) > (II) > (I) > (IV)

This is because (III) is tertiary carbocation, (II) is secondary carbocation, (I) and (IV) are primary,

39. Three students, Manish, Ramesh and Rajni were determining the extra

elements present in an organic compound given by their teacher. They

prepared the Lassaigne’s extract (L.E.) independently by the fusion of the

compound with sodium metal. Then they added solid FeSO4 and dilute

sulphuric acid to a part of Lassaigne’s extract. Manish and Rajni obtained

Prussian blue colour, but Ramesh got a red colour. Ramesh repeated the test

with the same Lassaigne’s extract but again got red colour only. They were

surprised and went to their teacher and told him about their observation.

A teacher asked them to think over the reason for this. Can you help them by

giving the reason for this observation? Also, write the chemical equations to

explain the formation of compounds of different colours

Solution:

3NaCNS + FeSO4 + dilute sulphuric→ Fe(CNS)3 (Blood red colour) + 3Na+

Ramesh has Nitrogen as well as Sulphur present in his organic compound, so he observed the Blood-red colour of Fe(CNS)3 and Manish and Rajni had only Nitrogen in their compound; hence they got Prussian blue colour.

40. Name the compounds whose line formulae are given below:

I. Multiple-choice Questions (Type-I)

Solution:

(i) The name of the compound is 3-ethyl-4-methyl-5-heptane-2-one.

(ii) The name of the compound is; 1-nitro-cyclohexane-2-ene.

41. Write structural formulae for compounds named as-

(a) 1-Bromoheptane

(b) 5-Bromoheptanoic acid

Solution:

(a)

I. Multiple-choice Questions (Type-I)

(b)

I. Multiple-choice Questions (Type-I)

42. Draw the resonance structures of the following compounds;

I. Multiple-choice Questions (Type-I)

Solution:

I. Multiple-choice Questions (Type-I)
I. Multiple-choice Questions (Type-I)
I. Multiple-choice Questions (Type-I)

43. Identify the most stable species in the following set of ions giving reasons:

I. Multiple-choice Questions (Type-I)

Solution:

(i) C+H3 will be more stable as the bromine atom destabilizes the positive charge on a carbon atom. Bromine atom is an electron-withdrawing group and has a lone pair of electrons.

(ii) CCl3 will be most stable because chlorine is more electron-withdrawing atom and the negative charge on carbon will be stabilized by the chlorine atom. As the number of chlorine atom attached to carbocation increases the stability also increases.

44. Give three points of differences between the inductive effect and resonance effect.

Solution:

1. In the inductive effect, the transmission of the electron is only from sigma bond whereas in resonance effect the transmission occurs from both sigma and pi bond.

2. It is possible when the polarization of bond takes place whereas the resonance effect is possible only if the system is conjugated.

3. Electronegativity plays role in inductive effect whereas in resonance effect more number of an alternative double bond will lead to more resonating structure and hence more stability.

45. Which of the following compounds will not exist as a resonance hybrid. Give the reason for your answer:

Solution:

Conjugation is only possible when an atom has any of the charge or alternative position of the double bond. Here CH3OH will not exist as resonance hybrid because of the reason.

46. Why does SO3 act as an electrophile?

Solution:

Oxygen is more electronegative than sulphur and the electron density at S in SO3 is reduced and they need more electrons to suppress the partial positive charge and hence they act as an electrophile.

47. Resonance structures of propenal are given below. Which of these resonating structures is more stable? Give a reason for your answer.

I. Multiple-choice Questions (Type-I)

Solution:

The structure I will be more stable than structure II because all the atoms have a complete octet in structure I, and the carbon atom having a positive charge don’t have a complete octet in structure II.

48. By mistake, an alcohol (boiling point 97°C) was mixed with a hydrocarbon (boiling point 68°C). Suggest a suitable method to separate the two compounds. Explain the reason for your choice.

Solution:

We can separate the mixture by steam distillation. Both alcohol and hydrocarbon don’t have much difference in the boiling point. Steam distillation is particularly used for the purification of temperature-sensitive material.

49. Which of the two structures (A) and (B) given below is more stabilised by resonance? Explain.

(A) CH3COOH (B) CH3COO-

Solution:

The two resonating structures in compound A are not equivalent, whereas compound B, having a negative charge on the oxygen atom, has the two equivalent structures; hence compound B is more stable.

IV. Matching Type

In the following questions, more than one correlation is possible between

options of Column I and Column II. Make as many correlations as you can.

50. Match the type of mixture of compounds in Column I with the technique of

separation/purification given in Column II.

Column I (i) Two solids which have different solubilities in a solvent and which do not undergo a reaction when dissolved in it. (ii) The liquid that decomposes at its boiling point (iii) Steam volatile liquid (iv) Two liquids which have boiling points close to each other (v) Two liquids with the large difference in boiling points.Column II (a) Steam distillation (b) Fractional distillation (c) Simple distillation (d) Distillation under reduced pressure (e) Crystallisation

Solution:

(i) is e

(ii) is d

(iii) is a

(iv) is b

(v) is c

51. Match the terms mentioned in Column I with the terms in Column II.

Column I (i) Carbocation (ii) Nucleophile (iii) Hyperconjugation (iv) Isomers (v) sp hybridisation (vi) ElectrophileColumn II (a) Cyclohexane and 1- hexene (b) Conjugation of electrons of C–Hσ bond with empty p-orbital present at adjacent positively charged carbon. (c) sp2 hybridised carbon with empty p-orbital (d) Ethyne (e) Species that can receive a pair of electrons (f) Species that can supply a pair of electrons.

Solution:

(i) is c

(ii) is f

(iii) is b

(iv) is a

(v) is d

(vi) is e

52. Match Column I with Column II.

Column I (i) Dumas method (ii) Kjeldahl’s method (iii) Carius method (iv) ChromatographyColumn II (a) AgNO3 (b) Silica gel (c) Nitrogen gas (d) Free radicals (e) Ammonium sulphate

Solution:

(i) is c

(ii) is e

(iii) is a

(iv) is b

(v) is d

53. Match the intermediates given in Column I with their probable structure in

Column II.

Column I (i) Free radical (ii) Carbocation (iii) CarbanionColumn II (a) Trigonal planar (b) Pyramidal (c) Linear

Solution:

(i) is a

(ii) is a

(iii) is b

54. Match the ions given in Column I with their nature given in Column II.

I. Multiple-choice Questions (Type-I)

Solution:

(i) is a, b and d

(ii) is b

(iii) is b

(iv) are c and d


Subtopics of Chapter 12 Organic Chemistry Some Basic Principles and Techniques

  1. General Introduction
  2. Tetravalence of Carbon: Shapes of Organic Compounds
  3. Structural Representations of Organic Compounds
    1. Complete, Condensed and Bond-line Structural Formulas
    2. Three-dimensional Representation of Organic Molecules
  4. Classification of Organic Compounds
  5. Nomenclature of Organic Compounds
    1. The Iupac System of Nomenclature
    2. Iupac Nomenclature of Alkanes
    3. Nomenclature of Organic Compounds Having Functional Group(S)
    4. Nomenclature of Substituted Benzene Compounds
  6. Isomerism
    1. Structural Isomerism
    2. Stereoisomerism
  7. Fundamental Concepts in Organic Reaction Mechanism
    1. Fission of a Covalent Bond
    2. Nucleophiles and Electrophiles
    3. Electron Movement in Organic Reactions
    4. Electron Displacement Effects in Covalent Bonds
    5. Inductive Effect
    6. Resonance Structure
    7. Resonance Effect
    8. Electromeric Effect (E Effect)
    9. Hyperconjugation
    10. Types of Organic Reactions and Mechanisms
  8. Methods of Purification Of Organic Compounds
    1. Sublimation
    2. Crystallisation
    3. Distillation
    4. Differential Extraction
    5. Chromatography
  9. Qualitative Analysis of Organic Compounds
    1. Detection of Carbon and Hydrogen
    2. Detection of Other Elements
  10. Quantitative Analysis
    1. Carbon and Hydrogen
    2. Nitrogen
    3. Halogens
    4. Sulphur
    5. Phosphorus
    6. Oxygen.

To learn the concepts of Organic Chemistry, students should solve NCERT Exemplar Class 11 Chemistry Chapter 12.

Frequently Asked Questions on NCERT Exemplar Solutions for Class 11 Chemistry Chapter 12

Q1

Which are the important topics I should learn from Chapter 12 of NCERT Exemplar Solutions for Class 11 Chemistry?

The important topics you should learn from Chapter 12 of NCERT Exemplar Solutions for Class 11 Chemistry are listed below:
General Introduction
Tetravalence of Carbon: Shapes of Organic Compounds
Structural Representations of Organic Compounds
Complete, Condensed and Bond-line Structural Formulas
Three-dimensional Representation of Organic Molecules
Classification of Organic Compounds
Nomenclature of Organic Compounds
The Iupac System of Nomenclature
Iupac Nomenclature of Alkanes
Nomenclature of Organic Compounds Having Functional Group(s)
Nomenclature of Substituted Benzene Compounds
Isomerism
Structural Isomerism
Stereoisomerism
Fundamental Concepts in Organic Reaction Mechanism
Fission of a Covalent Bond
Nucleophiles and Electrophiles
Electron Movement in Organic Reactions
Electron Displacement Effects in Covalent Bonds
Inductive Effect
Resonance Structure
Resonance Effect
Electromeric Effect (E Effect)
Hyperconjugation
Types of Organic Reactions and Mechanisms

Q2

Give three points of differences between the inductive effect and resonance effect in Chapter 12 of NCERT Exemplar Solutions for Class 11 Chemistry.

1. In the inductive effect, the transmission of the electron is only from the sigma bond, whereas in the resonance effect, the transmission occurs from both the sigma and pi bonds.
2. It is possible when the polarization of the bond takes place, whereas the resonance effect is possible only if the system is conjugated.
3. Electronegativity plays a role in the inductive effect, whereas in the resonance effect, more number of alternative double bonds will lead to a more resonating structure and hence more stability.

Q3

Why should I download the NCERT Exemplar Solutions for Class 11 Chemistry Chapter 12 from ANAND CLASSES (A School Of Competitions)?

Students who aspire to score good marks in the annual exams and other competitive exams should download the NCERT Exemplar Solutions from ANAND CLASSES (A School Of Competitions) website and practise them regularly, which will help them in getting their doubts cleared instantly. Besides, they will obtain comprehensive knowledge of all the topics covered in this chapter from the solutions PDF available at ANAND CLASSES (A School Of Competitions). While answering the textbook questions, they can cross-check their answers with the solutions and understand the areas in which they are lagging behind.

Er. Neeraj K.Anand is a freelance mentor and writer who specializes in Engineering & Science subjects. Neeraj Anand received a B.Tech degree in Electronics and Communication Engineering from N.I.T Warangal & M.Tech Post Graduation from IETE, New Delhi. He has over 30 years of teaching experience and serves as the Head of Department of ANAND CLASSES. He concentrated all his energy and experiences in academics and subsequently grew up as one of the best mentors in the country for students aspiring for success in competitive examinations. In parallel, he started a Technical Publication "ANAND TECHNICAL PUBLISHERS" in 2002 and Educational Newspaper "NATIONAL EDUCATION NEWS" in 2014 at Jalandhar. Now he is a Director of leading publication "ANAND TECHNICAL PUBLISHERS", "ANAND CLASSES" and "NATIONAL EDUCATION NEWS". He has published more than hundred books in the field of Physics, Mathematics, Computers and Information Technology. Besides this he has written many books to help students prepare for IIT-JEE and AIPMT entrance exams. He is an executive member of the IEEE (Institute of Electrical & Electronics Engineers. USA) and honorary member of many Indian scientific societies such as Institution of Electronics & Telecommunication Engineers, Aeronautical Society of India, Bioinformatics Institute of India, Institution of Engineers. He has got award from American Biographical Institute Board of International Research in the year 2005.

CBSE Class 11 Chemistry Syllabus

CBSE Class 11 Chemistry Syllabus is a vast which needs a clear understanding of the concepts and topics. Knowing CBSE Class 11 Chemistry syllabus helps students to understand the course structure of Chemistry.

Unit-wise CBSE Class 11 Syllabus for Chemistry

Below is a list of detailed information on each unit for Class 11 Students.

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: 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.

UNIT II – Structure of Atom

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, concept of shells and subshells, dual nature of matter and light, 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 and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.

UNIT III – Classification of Elements and Periodicity in Properties

Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of 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.

UNIT IV – Chemical Bonding and Molecular Structure

Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.

UNIT V – Chemical Thermodynamics

Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics – internal energy and enthalpy, 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. Second law of Thermodynamics (brief introduction)
Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes.
Third law of thermodynamics (brief introduction).

UNIT VI – Equilibrium

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 poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).

UNIT VII – Redox Reactions

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.

UNIT VIII – Organic Chemistry: Some basic Principles and Techniques

General introduction, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.

UNIT IX – Hydrocarbons

Classification of Hydrocarbons
Aliphatic Hydrocarbons:
Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions.
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, 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 Craft’s alkylation and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.

To know the CBSE Syllabus for all the classes from 1 to 12, visit the Syllabus page of CBSE. Meanwhile, to get the Practical Syllabus of Class 11 Chemistry, read on to find out more about the syllabus and related information in this page.

CBSE Class 11 Chemistry Practical Syllabus with Marking Scheme

In Chemistry subject, practical also plays a vital role in improving their academic scores in the subject. The overall weightage of Chemistry practical mentioned in the CBSE Class 11 Chemistry syllabus is 30 marks. So, students must try their best to score well in practicals along with theory. It will help in increasing their overall academic score.

CBSE Class 11 Chemistry Practical Syllabus

The experiments will be conducted under the supervision of subject teacher. CBSE Chemistry Practicals is for 30 marks. This contribute to the overall practical marks for the subject.

The table below consists of evaluation scheme of practical exams.

Evaluation SchemeMarks
Volumetric Analysis08
Salt Analysis08
Content Based Experiment06
Project Work04
Class record and viva04
Total30

CBSE Syllabus for Class 11 Chemistry Practical

Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used.

A. Basic Laboratory Techniques
1. Cutting glass tube and glass rod
2. Bending a glass tube
3. Drawing out a glass jet
4. Boring a cork

B. Characterization and Purification of Chemical Substances
1. Determination of melting point of an organic compound.
2. Determination of boiling point of an organic compound.
3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.

C. Experiments based on pH

1. Any one of the following experiments:

  • Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
  • Comparing the pH of solutions of strong and weak acids of same concentration.
  • Study the pH change in the titration of a strong base using universal indicator.

2. Study the pH change by common-ion in case of weak acids and weak bases.

D. Chemical Equilibrium
One of the following experiments:

1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
2. Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.

E. Quantitative Estimation
i. Using a mechanical balance/electronic balance.
ii. Preparation of standard solution of Oxalic acid.
iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid.
iv. Preparation of standard solution of Sodium carbonate.
v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonatesolution.

F. Qualitative Analysis
1) Determination of one anion and one cation in a given salt
Cations‐ Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4 +
Anions – (CO3)2‐ , S2‐, NO2 , SO32‐, SO2‐ , NO , Cl , Br, I‐, PO43‐ , C2O2‐ ,CH3COO
(Note: Insoluble salts excluded)

2) Detection of ‐ Nitrogen, Sulphur, Chlorine in organic compounds.

G) PROJECTS
Scientific investigations involving laboratory testing and collecting information from other sources.

A few suggested projects are as follows:

  • Checking the bacterial contamination in drinking water by testing sulphide ion
  • Study of the methods of purification of water.
  • Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional
    variation in drinking water and study of causes of presence of these ions above permissible
    limit (if any).
  • Investigation of the foaming capacity of different washing soaps and the effect of addition of
    Sodium carbonate on it.
  • Study the acidity of different samples of tea leaves.
  • Determination of the rate of evaporation of different liquids Study the effect of acids and
    bases on the tensile strength of fibres.
  • Study of acidity of fruit and vegetable juices.

Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with the approval of the teacher.

Practical Examination for Visually Impaired Students of Class 11

Below is a list of practicals for the visually impaired students.

A. List of apparatus for identification for assessment in practicals (All experiments)
Beaker, tripod stand, wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand,
dropper, test tube holder, ignition tube, china dish, tongs, standard flask, pipette, burette, conical flask, clamp
stand, dropper, wash bottle
• Odour detection in qualitative analysis
• Procedure/Setup of the apparatus

B. List of Experiments A. Characterization and Purification of Chemical Substances
1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid
B. Experiments based on pH
1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied
concentrations of acids, bases and salts using pH paper
2. Comparing the pH of solutions of strong and weak acids of same concentration.

C. Chemical Equilibrium
1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing
the concentration of eitherions.
2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the
concentration of either of the ions.

D. Quantitative estimation
1. Preparation of standard solution of oxalic acid.
2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard
solution of oxalic acid.

E. Qualitative Analysis
1. Determination of one anion and one cation in a given salt
2. Cations – NH+4
Anions – (CO3)2-, S2-, (SO3)2-, Cl-, CH3COO-
(Note: insoluble salts excluded)
3. Detection of Nitrogen in the given organic compound.
4. Detection of Halogen in the given organic compound.

Note: The above practicals may be carried out in an experiential manner rather than recording observations.

We hope students must have found this information on CBSE Syllabus useful for their studying Chemistry. Learn Maths & Science in interactive and fun loving ways with ANAND CLASSES (A School Of Competitions) App/Tablet.

Frequently Asked Questions on CBSE Class 11 Chemistry Syllabus

Q1

How many units are in the CBSE Class 11 Chemistry Syllabus?

There are 9 units in the CBSE Class 11 Chemistry Syllabus. Students can access various study materials for the chapters mentioned in this article for free at ANAND CLASSES (A School Of Competitions).

Q2

What is the total marks for practicals examination as per the CBSE Class 11 Chemistry Syllabus?

The total marks for the practicals as per the CBSE Class 11 Chemistry Syllabus is 30. It includes volumetric analysis, content-based experiment, salt analysis, class record, project work and viva.

Q3

Which chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry?

The organic chemistry chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry.