CBSE Class 12 Chemistry Question Paper 2026 (Set 3 - 56/2/3) with Solutions is now available here for download. CBSE conducted the Class 12 Chemistry examination on February 28, 2026, from 10:30 AM to 1:30 PM.
CBSE Class 12 Chemistry paper is of total 100 marks out of which 70 marks are allocated to the theory paper and 30 marks are for practical examination.
Also Check: CBSE Class 12 Question Paper 2026 (All Subjects)
The theory paper consists of 33 questions divided into five sections:
- Section A contains Multiple Choice Questions (MCQs),
- Section B contains Very Short Answer Type (VSA) Questions,
- Section C contains Short Answer Type (SA) Questions,
- Section D contains Case-Study based Questions,
- Section E contains Long Answer (LA) Type Questions.
All sections are compulsory.
CBSE Class 12 Chemistry Question Paper 2026 (Set 3 - 56/2/3) with Solution PDF
| CBSE Official PDF | CD PDF | CD PDF with Solutions |
|---|---|---|
| Download official PDF 0.79 MB | Download Collegedunia PDF 0.43 MB | Download solutions PDF 0.52 MB |
CBSE Class 12 Chemistry 2026 Set 3 (56/2/3) Questions with Solutions
Identify the correct statement:
Consider the following reaction:
\(Zn_{(s)} + Ag_2O_{(s)} + H_2O_{(l)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)} + 2OH^-_{(aq)}\)
Given: \(E^\circ_{Ag^+/Ag} = 0.80~V\), \(E^\circ_{Zn^{2+}/Zn} = -0.76~V\), \(1~F = 96500~C~mol^{-1}\). \(\Delta_r G^\circ\) for the above reaction is:
Electronic configuration of chromium is:
The order for the given reaction is:
\(A + 2B \rightarrow Products\)
\(Rate = k[A]^{\frac{1}{2}}[B]^1\)
Which of the following is heteroleptic complex?
The correct IUPAC name of the complex \([Pt(NH_3)_2Cl_2]\) is:
Identify the correct increasing order of boiling points of the given compounds:
Which of the following molecules is chiral in nature?
The base which is present in DNA but not in RNA is:
Identify the compound produced by the reduction of Ethanenitrile with Lithium aluminium hydride:
Which of the following reactions is not explained by the open chain structure of glucose?
Proteins are polymers of \(\alpha\)-amino acids which are joined to each other by:
Assertion (A): Zinc, cadmium and mercury are not considered as transition elements.
Reason (R): These elements have completely filled orbitals in their ground state as well as in their common oxidation states.
Assertion (A): The molecularity of the given reaction is 2
\(2HI \longrightarrow H_2 + I_2\)
Reason (R): Two molecules of the reactants are involved in simultaneous collision between them.
Assertion (A): Glucose gets oxidized to six carbon gluconic acid on reaction with bromine water.
Reason (R): The carbonyl group is absent in the open chain structure of glucose.
Assertion (A): Aromatic primary amines can be prepared by Gabriel Phthalimide synthesis.
Reason (R): Aryl halides do not undergo nucleophilic substitution with the anion formed by phthalimide.
Indicate the type of isomerism exhibited by the following complex: \([Co(en)_3]Cl_3\)
Define coordination number.
Write the unit of (i) second order reaction and (ii) zero order reaction.
Define Effective collision.
Why second ionization enthalpies of chromium and copper are exceptionally higher than those of their neighbouring elements?
Why transition elements form interstitial compounds?
The concentration of the reactant is reduced from 0.6 mol \(L^{-1}\) to 0.2 mol \(L^{-1}\) in 5 minutes in a first order reaction. Calculate rate constant of the reaction. \((\log 3 = 0.48)\)
Rate constant k for the first order reaction is \(2.54 \times 10^{-3} s^{-1}\). Calculate the time required for three-fourth of the reactant to decompose. \((\log 4 = 0.60)\)
What happens when 2-Bromobutane is made to react with alcoholic potassium hydroxide?
Write the major product in the following reaction:
\( \mathrm{C_6H_5Cl} \) (structure shown below) \( + \ \mathrm{CH_3-Cl} \ \xrightarrow[\text{dry ether}]{\mathrm{Na}} \ ? \)
60 g of glucose is dissolved in 250 g of water. Calculate the freezing point of this solution.
(molar mass of glucose = \(180~g~mol^{-1}\), \(K_f\) for water = \(1.86~K~kg~mol^{-1}\))
Calculate emf of the following cell at 298 K:
\(Sn | Sn^{2+}(0.001~M) || H^+(0.01~M) | H_{2(g)}(1~bar) | Pt_{(s)}\)
Given: \(E^\circ_{Sn^{2+}/Sn} = -0.14~V\), \(E^\circ_{H^+/H_2} = 0.00~V [\log 10 = 1]\)
Complete and balance the following equations:
(i) \(2Na_2CrO_4 + 2H^+ \longrightarrow\)
(ii) \(5S^{2-} + 2MnO_4^- + 16H^+ \longrightarrow\)
Why is chemistry of actinoids complicated as compared to lanthanoids?
On the basis of crystal field theory, write the electronic configuration for \(d^5\) ion for which \(\Delta_o \lt P\)
Explain why \([Fe(H_2O)_6]^{3+}\) is strongly paramagnetic whereas \([Fe(CN)_6]^{3-}\) is weakly paramagnetic. [Atomic number of Fe = 26]
The boiling points of the alkyl halides with the same alkyl group decrease in the given order: \(RI \gt RBr \gt RCl \gt RF\). Explain the above statement.
Define Racemisation.
Write the IUPAC name of the given compound: \(CH_3CH(CH_3)CH(Br)CH_3\)
Write the reaction involved in: Rosenmund's reduction
Write the reaction involved in: Cannizzaro's reaction
Write the reaction involved in: Hell-Volhard-Zelinsky reaction
(a) Define the following terms:
(i) Invert Sugar
(ii) Polysaccharides
(b) On the basis of structure differentiate between fibrous and globular proteins.
(a) Why is glycogen known as animal starch?
(b) Differentiate between essential amino acids and non-essential amino acids.
(c) What is the effect of denaturation on the structure of proteins?
Osmosis is a process by which the molecules of a solvent pass from a
solution of low solute concentration to a solution of high solute
concentration through a semi-permeable membrane. Osmotic pressure is
a colligative property. When the applied pressure on a solution exceeds its
osmotic pressure, reverse osmosis occurs. When two solutions are
separated by a semipermeable membrane and they have same osmotic
pressure they are said to be isotonic. Of the two solutions separated by a
semipermeable membrane, if one is a lower osmotic pressure, it is said to
be hypotonic relative to the second solution. If it has a higher osmotic
pressure, than the second solution, it is said to be hypertonic relative to
the second solution. The osmotic pressure associated with the fluid inside
the blood cell is equivalent to that of 0.9% (mass/volume) sodium chloride
solution called normal saline solution and it is safe to inject intravenously.
Osmotic pressure is vital in daily life and nature. It helps in explain, why
IV fluids match blood’s osmotic pressure, its also the principle behind food
preservation using salt or sugar.
(a) Calculate the amount of \(CaCl_2\) (\(i = 2.59\)) dissolved in 2.46 litre of water such that its osmotic pressure is 0.70 atm at \(27^\circ C\).
\([\)Given: \(R = 0.082~L~atm~K^{-1}mol^{-1}\), molar mass of \(CaCl_2 = 111~g~mol^{-1}]\)
When raisins are kept in water, they get swollen. Name the phenomenon involved in this process.
Why osmotic pressure is more advantageous than other colligative properties?
Which phenomenon is responsible for desalination of sea water?
Why primary amines have higher boiling points than tertiary amines?
Out of Butan-1-amine and Butan-1-ol, which is more soluble in water?
Like \( \mathrm{NH_3} \), nitrogen atom of amine is trivalent and carries an unshared pair of electrons. Nitrogen orbitals in amines are therefore \( sp^3 \) hybridised and the geometry of amines is pyramidal. Lower aliphatic amines are soluble in water due to the formation of hydrogen bond with water molecules. The solubility decreases as the molar mass of amines increases due to increase in size of hydrophobic part. Higher amines are insoluble in water. However amines are less soluble in water than alcohols because of low electronegativity of nitrogen as compared to oxygen. Boiling points of isomeric amines follow the order \( 1^{\circ} > 2^{\circ} > 3^{\circ} \). It is due to the fact the amines are held together due to hydrogen bonding. Extent of hydrogen bonding is more in primary amines than in secondary amines as two hydrogen atoms are available for hydrogen bond formation. Tertiary amines do not show hydrogen bonding because of the absence of hydrogen atom attached to nitrogen. Amines can be prepared from, nitro compounds, nitriles, amides etc.
Complete the following equations:
(i) \( \mathrm{CH_3CONH_2} \xrightarrow[\mathrm{(ii)\ H_2O}]{\mathrm{(i)\ LiAlH_4}} \)
(ii) The compound shown in the figure below (a benzene ring carrying \( \mathrm{NO_2} \) and \( \mathrm{CH_3} \) at opposite positions) \( \xrightarrow{\mathrm{Fe + HCl}} \)
Like \( \mathrm{NH_3} \), nitrogen atom of amine is trivalent and carries an unshared pair of electrons. Nitrogen orbitals in amines are therefore \( sp^3 \) hybridised and the geometry of amines is pyramidal. Lower aliphatic amines are soluble in water due to the formation of hydrogen bond with water molecules. The solubility decreases as the molar mass of amines increases due to increase in size of hydrophobic part. Higher amines are insoluble in water. However amines are less soluble in water than alcohols because of low electronegativity of nitrogen as compared to oxygen. Boiling points of isomeric amines follow the order \( 1^{\circ} > 2^{\circ} > 3^{\circ} \). It is due to the fact the amines are held together due to hydrogen bonding. Extent of hydrogen bonding is more in primary amines than in secondary amines as two hydrogen atoms are available for hydrogen bond formation. Tertiary amines do not show hydrogen bonding because of the absence of hydrogen atom attached to nitrogen. Amines can be prepared from, nitro compounds, nitriles, amides etc.
Classify the following amines as primary, secondary or tertiary:
(i) A naphthalene ring carrying the group \( \mathrm{N(CH_3)_2} \) (shown in the figure below)
(ii) The same naphthalene ring carrying the group \( \mathrm{NH_2} \) in place of \( \mathrm{N(CH_3)_2} \)
The conductivity of \(0.1\) mol \(L^{-1}\) solution of NaCl is \(1.06 \times 10^{-2}\) S \(cm^{-1}\). Calculate its molar conductivity and degree of dissociation. (\(\lambda^\circ_{Na^+} = 50.1, \lambda^\circ_{Cl^-} = 76.5\) S \(cm^2\) \(mol^{-1}\)). (b) (i) Predict current flow direction for \(2Ag^+ + Zn \rightarrow 2Ag + Zn^{2+}\). (ii) Differentiate between primary and secondary battery.
(a) Resistance of a conductivity cell filled with 0.1 M KCl solution is 100 \(\Omega\). If the resistance of the same cell when filled with 0.01 mol L\(^{-1}\) KCl solution is 300 \(\Omega\), calculate the conductivity and molar conductivity of 0.01 mol L\(^{-1}\) KCl solution. The conductivity of 0.1 M KCl solution is \(1.29 \times 10^{-2}\) S cm\(^{-1}\).
(b) (i) Write any two advantages of \( \mathrm{H_2 - O_2} \) fuel cell.
(ii) Why does the cell potential of mercury cell remain constant throughout the life ?
An organic compound 'A', with molecular formula \(C_2H_6O\) reacts with active metals such as sodium to give compound 'B' and hydrogen gas. 'A' on treatment with iodine and sodium hydroxide gives 'C' and in presence of \(H_2SO_4\) at \(413~K\) gives 'D' (\(C_4H_{10}O\)). 'D' on reaction with excess of HI gives 'E'. Identify 'A', 'B', 'C', 'D' and 'E' and write all the reactions involved.
(a) Write the reagents which are used in the given conversions :
(i) Phenol to 2, 4, 6 - tribromophenol
(ii) Propene to propan-1-ol
(iii) Butan-2-one to butan-2-ol
(b) Explain the mechanism of acid catalyzed hydration of alkene to form corresponding alcohol.
(a) How will you convert the following:
(i) Propanone to Propene
(ii) Benzoic acid to Benzaldehyde
(iii) Benzene to m-Nitroacetophenone
(b) (i) Arrange the following compounds in increasing order of their reactivity towards HCN:
\( \mathrm{(CH_3)_2C=O} \), \( \mathrm{(CH_3)_3C{-}CO{-}C(CH_3)_3} \), \( \mathrm{CH_3CHO} \)
(ii) Identify the compounds, which would undergo Aldol condensation:
\( \mathrm{HCHO} \), \( \mathrm{C_6H_5CHO} \), \( \mathrm{CH_3CHO} \), and the cyclic ketone (a six-membered carbon ring with one C=O) shown in the figure below
(a) Give chemical tests to distinguish between the following pairs of compounds:
(i) Acetophenone and Benzophenone
(ii) Propanal and Propanone
(iii) Pentan-2-one and Pentan-3-one
(b) (i) Which of the following acids is stronger and why?
\( \mathrm{CH_2FCOOH} \), \( \mathrm{CH_3COOH} \)
(ii) Arrange the following compounds in the increasing order of their boiling points:
\( \mathrm{CH_3OCH_3} \), \( \mathrm{CH_3CH_2CH_3} \), \( \mathrm{CH_3CH_2OH} \), \( \mathrm{CH_3CHO} \)
CBSE Class 12 Chemistry Question Paper Pattern and Marking Scheme
The CBSE Class 12 Chemistry 2026 question paper is of 70 marks and has 33 questions in five sections, A to E, all compulsory. The tables below give the section-wise paper pattern and the marking rules from the official CBSE marking scheme.
CBSE Class 12 Chemistry Question Paper Pattern 2026
| Section | Questions | Question Type | Marks per Question | Marks |
|---|---|---|---|---|
| A | Q1 - Q16 | Multiple choice questions | 1 | 16 |
| B | Q17 - Q21 | Very short answer type | 2 | 10 |
| C | Q22 - Q28 | Short answer type | 3 | 21 |
| D | Q29 - Q30 | Case-based questions | 4 | 8 |
| E | Q31 - Q33 | Long answer type | 5 | 15 |
| Total | 33 questions | 70 |
CBSE Class 12 Chemistry Marking Scheme 2026
| Marking point | How it is applied |
|---|---|
| Value-point marking | Marks are awarded against the value points (steps) given in the official marking scheme; the marks of an answer are split across its steps. |
| Own expression | The marking scheme carries suggested value points only. A correct answer in the student's own words is awarded due marks. |
| Competency-based questions | If a competency-based answer is not from the marking scheme but shows the correct competency, due marks are awarded. |
| Errors | An error is penalised only once; no marks are deducted for its cumulative effect. |
| Incorrect answer | A totally incorrect answer is awarded zero (0) marks. |
| Choice (OR) questions | If both options of a question with internal choice are attempted, marks are awarded for both and the higher score is taken; if only one option is attempted, the other is marked NA (not attempted). |
| Scale of marks | The full scale of 0 to 70 marks is used and full marks are awarded whenever the answer deserves them. |
CBSE Class 12 Chemistry Unit-Wise Weightage
| Unit No. | Unit Name | Marks |
|---|---|---|
| 1 | Solutions | 7 |
| 2 | Electrochemistry | 9 |
| 3 | Chemical Kinetics | 7 |
| 4 | d- and f-Block Elements | 7 |
| 5 | Coordination Compounds | 7 |
| 6 | Haloalkanes and Haloarenes | 6 |
| 7 | Alcohols, Phenols and Ethers | 6 |
| 8 | Aldehydes, Ketones and Carboxylic Acids | 8 |
| 9 | Amines | 6 |
| 10 | Biomolecules | 7 |
| Total | — | 70 |
Comments