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Chemistry · Class 11 Science

Rajasthan Rbse Class 11 Chemistry — Real Previous-Year Papers

with complete answers

Real previous-year board papers, year by year — the official exam pattern, the full question paper, and every question solved the concept-first way. Distinct from the chapter-wise textbook bank.

2017–2026
Years of papers
5
Total Papers
5
Real Board Papers
0
Sample papers
183
Real-paper Q & A
0
Sample-paper Q & A

Real board-paper questions available, by year

51 Q2026complete
—2025Paper not yet available
—2024Paper not yet available
34 Q2023complete
38 Q2022complete
—2021Exam not held (COVID-19)
—2020Paper not yet available
—2019Paper not yet available
30 Q2018complete
30 Q2017complete

2025 — Paper not yet available: This year’s RBSE Class-11 exam was presumably held, but no verified question paper for this subject has been published by any source we check — the official rajeduboard.rajasthan.gov.in and the public past-paper archives. We publish only a paper we can verify against a real printed original — this one will appear here once it is.

2024 — Paper not yet available: This year’s RBSE Class-11 exam was presumably held, but no verified question paper for this subject has been published by any source we check — the official rajeduboard.rajasthan.gov.in and the public past-paper archives. We publish only a paper we can verify against a real printed original — this one will appear here once it is.

2021 — Exam not held (COVID-19): RBSE did not conduct the Class-11 (Senior Secondary Part-I) examination in 2021 at all — students were promoted without sitting any exam (a Rajasthan government decision, COVID-19 2nd wave). No question paper exists for this year because none was ever administered.

2020 — Paper not yet available: This year’s RBSE Class-11 exam was presumably held, but no verified question paper for this subject has been published by any source we check — the official rajeduboard.rajasthan.gov.in and the public past-paper archives. We publish only a paper we can verify against a real printed original — this one will appear here once it is.

2019 — Paper not yet available: This year’s RBSE Class-11 exam was presumably held, but no verified question paper for this subject has been published by any source we check — the official rajeduboard.rajasthan.gov.in and the public past-paper archives. We publish only a paper we can verify against a real printed original — this one will appear here once it is.

Rajasthan Board Senior Secondary Part-I Examination 2026 · Set ANNUAL

Real board examination

About this paper

The real Class-12 board examination held in 2026. Every question below is solved the concept-first way. Sample papers are labelled honestly — never shown as a past exam.

Total marks
70
Questions
51
Duration
195 min
Sections
6

The marks / questions / duration above are the official exam pattern. We currently have 51 of this paper’s questions (100% of the full paper), with 51 fully solved. Questions we couldn’t yet extract or verify are held — never shown as complete.

Sections & marks

SectionTypeQuestionsMarks eachTotal
ASection Amcq10110
ASection Asubjective19119
ASection Asubjective121.518
ASection Asubjective8216
ASection Asubjective133
ASection Asubjective144
Total5170

The question paper

The questions we hold for this paper, laid out by section. Solutions are on the Answers tab.

Board Examination

Chemistry

Rajasthan Board Senior Secondary Part-I Examination 2026 · Set ANNUAL

Series/Set: ANNUALRoll No. ________
Time Allowed: 3 hr 15 minMaximum Marks: 70

General Instructions

  1. This question paper contains 51 questions divided into 6 sections — A, A, A, A, A, A.
  2. Section A comprises 10 questions of 1 mark each (mcq).
  3. Section A comprises 19 questions of 1 mark each (subjective).
  4. Section A comprises 12 questions of 1.5 marks each (subjective).
  5. Section A comprises 8 questions of 2 marks each (subjective).
  6. Section A comprises 1 question of 3 marks each (subjective).
  7. Section A comprises 1 question of 4 marks each (subjective).

Above is the official exam pattern. The questions printed below are those we currently hold for this paper.

Section A

mcq · 1 mark each · 51 of 10 shown

Q1.
How many significant figures are there in 0.0052?
  • (a) 4
  • (b) 1
  • (c) 3
  • (d) 2
[1]
Q2.
In 7d orbitals, 7 denotes -
  • (a) Principal quantum number
  • (b) Azimuthal quantum number
  • (c) Magnetic quantum number
  • (d) Spin quantum number
[1]
Q3.
Example of Sp3d2 hybridization is -
  • (a) CH4
  • (b) PCl5
  • (c) NH3
  • (d) SF6
[1]
Q4.
The correct sequence of Ionization Enthalpy for Li, Be, B, C is -
  • (a) C > B > Be > Li
  • (b) C > Be > B > Li
  • (c) B > C > Be > Li
  • (d) C > B > Li > Be
[1]
Q5.
Substance with minimum Entropy is -
  • (a) Water
  • (b) Ice
  • (c) Water vapour
  • (d) None of these
[1]
Q6.
The pH value of gastric juice is -
  • (a) -3
  • (b) -1.2
  • (c) -2
  • (d) -4
[1]
Q7.
IUPAC name of Neopentane is -
  • (a) 2,2-dimethylpropane
  • (b) 2-Methylbutane
  • (c) 3-Methylbutane
  • (d) 2-Ethylbutane
[1]
Page 1 of 33
Q8.
Most stable Carbocation is - (a) (CH3)3C+ (b) CH3CH2+ (c) (CH3)2CH+ (d) CH3+
[1]
Q9.
Oxidation number of oxygen in H2O2 is - (a) -1 (b) -2 (c) -1/2 (d) +1
[1]
Q10.
Which of the following is an example of Homocyclic compound? (a) Cyclopropane (b) Benzene (c) Furan (d) Toluene
[1]
Q11.
In ⁸⁰₃₅Br, the number of neutrons is ___.
[1]
Q12.
The value of change in Gibbs energy (ΔG) for the spontaneous process is always ___.
[1]
Q13.
The solutions which resist change in their pH on dilution are called ___ solution.
[1]
Q14.
___ block elements are called transition elements.
[1]
Q15.
In propyne, ___ sigma (σ) and ___ pi (π) bonds are present.
[1]
Q16.
Oxidation number of Fe in Fe2O3 is ___.
[1]
Q17.
Free radical species are product of ___ bond cleavage.
[1]
Q18.
For n = 1, the value of l is ___.
[1]
Page 2 of 33
Q19.
Write the relation between Cp and Cv for an ideal gas.
[1]
Q20.
Write Mendeleev's Periodic Law.
[1]
Q21.
Write the electronic configuration of Mn (Z=25).
[1]
Q22.
Write the formula to calculate formal charge.
[1]
Q23.
Draw the molecular orbital diagram of Ethane.
[1]
Q24.
Write Pauli's Exclusion Principle.
[1]
Q25.
In an adiabatic process, is change in heat possible or not?
[1]
Q26.
Write the isomers of pentane.
[1]
Q27.
Write the conjugate base of HClO4.
[1]
Q28.
Identify [A] in the reaction: CH3Br + 2Na + BrCH3 --(dry ether)--> [A] + 2NaBr
[1]
Q29.
Write Markownikoff's rule.
[1]
Page 3 of 33
Q30.
Explain disproportionation reaction with example.
[2]
Q31.
Identify the Lewis acid and Lewis base in the following: HO-, F-, H+, BCl3
[2]
Q32.
A solution is prepared by adding 2g of a substance 'A' to 18g of water. Calculate the mass percent of the solute 'A'.
[2]
Q33.
Calculate the pH of 0.005M NaOH solution.
[2]
Q34.
Define Shielding Effect.
[2]
Q35.
Draw resonating structures of CO3²- (carbonate ion).
[2]
Q36.
What is the wave nature of electromagnetic radiation? Draw the spectrum of electromagnetic radiation.
[2]
Q37.
Draw the labelled diagram of Daniel cell and write its equation.
[2]
Q38.
Derive the relation between Kp and Kc.
[2]
Page 4 of 33
Q39.
Explain why the Ionisation Enthalpy of Be is higher than B.
[2]
Q40.
H2S is a gas while H2O is liquid, why?
[2]
Q41.
Identify the oxidizing and reducing agent in the reaction: N2H4(l) + 2H2O2(l) -> N2(g) + 4H2O(l)
[2]
Q42.
What is fractional distillation? Explain with a diagram.
[2]
Q43.
How is Lassaigne's solution prepared?
[2]
Q44.
Explain the addition of HBr on propene with the help of Markownikoff's rule.
[2]
Q45.
Complete the reaction - CH≡CH --(Red hot Fe tube)--> ? CH3COO-Na+ --(CaO, NaOH, Δ)--> ? **OR** Complete the reaction - (Benzene ring) + 3Cl2 --(UV, 500)--> ? CH3-CH=CH2 + O3 --> ? --(Zn + H2O)--> ?
[2]
Q46.
Explain the following: Friedel Craft reaction **OR** Explain the following: β-elimination reaction of Ethyl chloride in the presence of alcoholic KOH
[2]
Q47.
Explain the following: Inductive effect **OR** Explain the following: Hyper-Conjugation
[2]
Page 5 of 33
Q48.
Explain the following: Acidic nature of Alkyne **OR** Explain the following: Anti-Markownikoff rule
[2]
Q49.
Explain the following: Structural isomerism in Hydrocarbons **OR** Explain the following: Nucleophilic species
[2]
Q50.
Balance the given reaction by the oxidation number method: P4(s) + OH-(aq) -> PH3(g) + HPO2-(aq)
[3]
Q51.
Write the IUPAC names of the following compounds - (a) CH3-CH2-C(CH3)=CH-CH3 (a clearly drawn C=C double bond, with a methyl branch on the double-bond carbon) (b) CH3CH2-C(=O)-OH (c) CH3CH2-CH(OH)-CH2CH3 (d) Toluene (a benzene ring with a -CH3 substituent) **OR** Write the IUPAC names of the following compounds - (a) CH3-CH-C≡CH, printed with a -CH2-CH3 (ethyl) branch shown attached below the CH carbon (exact attachment point not fully legible in the scan) (b) CH3CH2-C(=O)-H (c) (CH3)?C-CH2-CH3, printed with a subscript on the methyl count that is not fully legible in the scan (appears as 5, which would be an invalid valence, so this digit is uncertain and transcribed as printed rather than silently corrected) (d) Phenol (a benzene ring with an -OH substituent)
[4]
Section A

mcq · 1 mark each · 51 of 10 shown

Q1.
How many significant figures are there in 0.0052? (a) 4 (b) 1 (c) 3 (d) 2
[1]
Q2.
In 7d orbitals, 7 denotes - (a) Principal quantum number (b) Azimuthal quantum number (c) Magnetic quantum number (d) Spin quantum number
[1]
Q3.
Example of Sp3d2 hybridization is - (a) CH4 (b) PCl5 (c) NH3 (d) SF6
[1]
Q4.
The correct sequence of Ionization Enthalpy for Li, Be, B, C is - (a) C > B > Be > Li (b) C > Be > B > Li (c) B > C > Be > Li (d) C > B > Li > Be
[1]
Page 6 of 33
Q5.
Substance with minimum Entropy is - (a) Water (b) Ice (c) Water vapour (d) None of these
[1]
Q6.
The pH value of gastric juice is - (a) -3 (b) -1.2 (c) -2 (d) -4
[1]
Q7.
IUPAC name of Neopentane is - (a) 2,2-dimethylpropane (b) 2-Methylbutane (c) 3-Methylbutane (d) 2-Ethylbutane
[1]
Q8.
Most stable Carbocation is - (a) (CH3)3C+ (b) CH3CH2+ (c) (CH3)2CH+ (d) CH3+
[1]
Q9.
Oxidation number of oxygen in H2O2 is - (a) -1 (b) -2 (c) -1/2 (d) +1
[1]
Q10.
Which of the following is an example of Homocyclic compound? (a) Cyclopropane (b) Benzene (c) Furan (d) Toluene
[1]
Q11.
In ⁸⁰₃₅Br, the number of neutrons is ___.
[1]
Q12.
The value of change in Gibbs energy (ΔG) for the spontaneous process is always ___.
[1]
Q13.
The solutions which resist change in their pH on dilution are called ___ solution.
[1]
Q14.
___ block elements are called transition elements.
[1]
Q15.
In propyne, ___ sigma (σ) and ___ pi (π) bonds are present.
[1]
Page 7 of 33
Q16.
Oxidation number of Fe in Fe2O3 is ___.
[1]
Q17.
Free radical species are product of ___ bond cleavage.
[1]
Q18.
For n = 1, the value of l is ___.
[1]
Q19.
Write the relation between Cp and Cv for an ideal gas.
[1]
Q20.
Write Mendeleev's Periodic Law.
[1]
Q21.
Write the electronic configuration of Mn (Z=25).
[1]
Q22.
Write the formula to calculate formal charge.
[1]
Q23.
Draw the molecular orbital diagram of Ethane.
[1]
Q24.
Write Pauli's Exclusion Principle.
[1]
Q25.
In an adiabatic process, is change in heat possible or not?
[1]
Q26.
Write the isomers of pentane.
[1]
Page 8 of 33
Q27.
Write the conjugate base of HClO4.
[1]
Q28.
Identify [A] in the reaction: CH3Br + 2Na + BrCH3 --(dry ether)--> [A] + 2NaBr
[1]
Q29.
Write Markownikoff's rule.
[1]
Q30.
Explain disproportionation reaction with example.
[2]
Q31.
Identify the Lewis acid and Lewis base in the following: HO-, F-, H+, BCl3
[2]
Q32.
A solution is prepared by adding 2g of a substance 'A' to 18g of water. Calculate the mass percent of the solute 'A'.
[2]
Q33.
Calculate the pH of 0.005M NaOH solution.
[2]
Q34.
Define Shielding Effect.
[2]
Q35.
Draw resonating structures of CO3²- (carbonate ion).
[2]
Page 9 of 33
Q36.
What is the wave nature of electromagnetic radiation? Draw the spectrum of electromagnetic radiation.
[2]
Q37.
Draw the labelled diagram of Daniel cell and write its equation.
[2]
Q38.
Derive the relation between Kp and Kc.
[2]
Q39.
Explain why the Ionisation Enthalpy of Be is higher than B.
[2]
Q40.
H2S is a gas while H2O is liquid, why?
[2]
Q41.
Identify the oxidizing and reducing agent in the reaction: N2H4(l) + 2H2O2(l) -> N2(g) + 4H2O(l)
[2]
Q42.
What is fractional distillation? Explain with a diagram.
[2]
Q43.
How is Lassaigne's solution prepared?
[2]
Q44.
Explain the addition of HBr on propene with the help of Markownikoff's rule.
[2]
Page 10 of 33
Q45.
Complete the reaction - CH≡CH --(Red hot Fe tube)--> ? CH3COO-Na+ --(CaO, NaOH, Δ)--> ? **OR** Complete the reaction - (Benzene ring) + 3Cl2 --(UV, 500)--> ? CH3-CH=CH2 + O3 --> ? --(Zn + H2O)--> ?
[2]
Q46.
Explain the following: Friedel Craft reaction **OR** Explain the following: β-elimination reaction of Ethyl chloride in the presence of alcoholic KOH
[2]
Q47.
Explain the following: Inductive effect **OR** Explain the following: Hyper-Conjugation
[2]
Q48.
Explain the following: Acidic nature of Alkyne **OR** Explain the following: Anti-Markownikoff rule
[2]
Q49.
Explain the following: Structural isomerism in Hydrocarbons **OR** Explain the following: Nucleophilic species
[2]
Q50.
Balance the given reaction by the oxidation number method: P4(s) + OH-(aq) -> PH3(g) + HPO2-(aq)
[3]
Q51.
Write the IUPAC names of the following compounds - (a) CH3-CH2-C(CH3)=CH-CH3 (a clearly drawn C=C double bond, with a methyl branch on the double-bond carbon) (b) CH3CH2-C(=O)-OH (c) CH3CH2-CH(OH)-CH2CH3 (d) Toluene (a benzene ring with a -CH3 substituent) **OR** Write the IUPAC names of the following compounds - (a) CH3-CH-C≡CH, printed with a -CH2-CH3 (ethyl) branch shown attached below the CH carbon (exact attachment point not fully legible in the scan) (b) CH3CH2-C(=O)-H (c) (CH3)?C-CH2-CH3, printed with a subscript on the methyl count that is not fully legible in the scan (appears as 5, which would be an invalid valence, so this digit is uncertain and transcribed as printed rather than silently corrected) (d) Phenol (a benzene ring with an -OH substituent)
[4]
Page 11 of 33
Section A

mcq · 1 mark each · 51 of 10 shown

Q1.
How many significant figures are there in 0.0052? (a) 4 (b) 1 (c) 3 (d) 2
[1]
Q2.
In 7d orbitals, 7 denotes - (a) Principal quantum number (b) Azimuthal quantum number (c) Magnetic quantum number (d) Spin quantum number
[1]
Q3.
Example of Sp3d2 hybridization is - (a) CH4 (b) PCl5 (c) NH3 (d) SF6
[1]
Q4.
The correct sequence of Ionization Enthalpy for Li, Be, B, C is - (a) C > B > Be > Li (b) C > Be > B > Li (c) B > C > Be > Li (d) C > B > Li > Be
[1]
Q5.
Substance with minimum Entropy is - (a) Water (b) Ice (c) Water vapour (d) None of these
[1]
Q6.
The pH value of gastric juice is - (a) -3 (b) -1.2 (c) -2 (d) -4
[1]
Q7.
IUPAC name of Neopentane is - (a) 2,2-dimethylpropane (b) 2-Methylbutane (c) 3-Methylbutane (d) 2-Ethylbutane
[1]
Q8.
Most stable Carbocation is - (a) (CH3)3C+ (b) CH3CH2+ (c) (CH3)2CH+ (d) CH3+
[1]
Q9.
Oxidation number of oxygen in H2O2 is - (a) -1 (b) -2 (c) -1/2 (d) +1
[1]
Q10.
Which of the following is an example of Homocyclic compound? (a) Cyclopropane (b) Benzene (c) Furan (d) Toluene
[1]
Page 12 of 33
Q11.
In ⁸⁰₃₅Br, the number of neutrons is ___.
[1]
Q12.
The value of change in Gibbs energy (ΔG) for the spontaneous process is always ___.
[1]
Q13.
The solutions which resist change in their pH on dilution are called ___ solution.
[1]
Q14.
___ block elements are called transition elements.
[1]
Q15.
In propyne, ___ sigma (σ) and ___ pi (π) bonds are present.
[1]
Q16.
Oxidation number of Fe in Fe2O3 is ___.
[1]
Q17.
Free radical species are product of ___ bond cleavage.
[1]
Q18.
For n = 1, the value of l is ___.
[1]
Q19.
Write the relation between Cp and Cv for an ideal gas.
[1]
Q20.
Write Mendeleev's Periodic Law.
[1]
Q21.
Write the electronic configuration of Mn (Z=25).
[1]
Page 13 of 33
Q22.
Write the formula to calculate formal charge.
[1]
Q23.
Draw the molecular orbital diagram of Ethane.
[1]
Q24.
Write Pauli's Exclusion Principle.
[1]
Q25.
In an adiabatic process, is change in heat possible or not?
[1]
Q26.
Write the isomers of pentane.
[1]
Q27.
Write the conjugate base of HClO4.
[1]
Q28.
Identify [A] in the reaction: CH3Br + 2Na + BrCH3 --(dry ether)--> [A] + 2NaBr
[1]
Q29.
Write Markownikoff's rule.
[1]
Q30.
Explain disproportionation reaction with example.
[2]
Q31.
Identify the Lewis acid and Lewis base in the following: HO-, F-, H+, BCl3
[2]
Page 14 of 33
Q32.
A solution is prepared by adding 2g of a substance 'A' to 18g of water. Calculate the mass percent of the solute 'A'.
[2]
Q33.
Calculate the pH of 0.005M NaOH solution.
[2]
Q34.
Define Shielding Effect.
[2]
Q35.
Draw resonating structures of CO3²- (carbonate ion).
[2]
Q36.
What is the wave nature of electromagnetic radiation? Draw the spectrum of electromagnetic radiation.
[2]
Q37.
Draw the labelled diagram of Daniel cell and write its equation.
[2]
Q38.
Derive the relation between Kp and Kc.
[2]
Q39.
Explain why the Ionisation Enthalpy of Be is higher than B.
[2]
Q40.
H2S is a gas while H2O is liquid, why?
[2]
Page 15 of 33
Q41.
Identify the oxidizing and reducing agent in the reaction: N2H4(l) + 2H2O2(l) -> N2(g) + 4H2O(l)
[2]
Q42.
What is fractional distillation? Explain with a diagram.
[2]
Q43.
How is Lassaigne's solution prepared?
[2]
Q44.
Explain the addition of HBr on propene with the help of Markownikoff's rule.
[2]
Q45.
Complete the reaction - CH≡CH --(Red hot Fe tube)--> ? CH3COO-Na+ --(CaO, NaOH, Δ)--> ? **OR** Complete the reaction - (Benzene ring) + 3Cl2 --(UV, 500)--> ? CH3-CH=CH2 + O3 --> ? --(Zn + H2O)--> ?
[2]
Q46.
Explain the following: Friedel Craft reaction **OR** Explain the following: β-elimination reaction of Ethyl chloride in the presence of alcoholic KOH
[2]
Q47.
Explain the following: Inductive effect **OR** Explain the following: Hyper-Conjugation
[2]
Q48.
Explain the following: Acidic nature of Alkyne **OR** Explain the following: Anti-Markownikoff rule
[2]
Q49.
Explain the following: Structural isomerism in Hydrocarbons **OR** Explain the following: Nucleophilic species
[2]
Page 16 of 33
Q50.
Balance the given reaction by the oxidation number method: P4(s) + OH-(aq) -> PH3(g) + HPO2-(aq)
[3]
Q51.
Write the IUPAC names of the following compounds - (a) CH3-CH2-C(CH3)=CH-CH3 (a clearly drawn C=C double bond, with a methyl branch on the double-bond carbon) (b) CH3CH2-C(=O)-OH (c) CH3CH2-CH(OH)-CH2CH3 (d) Toluene (a benzene ring with a -CH3 substituent) **OR** Write the IUPAC names of the following compounds - (a) CH3-CH-C≡CH, printed with a -CH2-CH3 (ethyl) branch shown attached below the CH carbon (exact attachment point not fully legible in the scan) (b) CH3CH2-C(=O)-H (c) (CH3)?C-CH2-CH3, printed with a subscript on the methyl count that is not fully legible in the scan (appears as 5, which would be an invalid valence, so this digit is uncertain and transcribed as printed rather than silently corrected) (d) Phenol (a benzene ring with an -OH substituent)
[4]
Section A

mcq · 1 mark each · 51 of 10 shown

Q1.
How many significant figures are there in 0.0052? (a) 4 (b) 1 (c) 3 (d) 2
[1]
Q2.
In 7d orbitals, 7 denotes - (a) Principal quantum number (b) Azimuthal quantum number (c) Magnetic quantum number (d) Spin quantum number
[1]
Q3.
Example of Sp3d2 hybridization is - (a) CH4 (b) PCl5 (c) NH3 (d) SF6
[1]
Q4.
The correct sequence of Ionization Enthalpy for Li, Be, B, C is - (a) C > B > Be > Li (b) C > Be > B > Li (c) B > C > Be > Li (d) C > B > Li > Be
[1]
Q5.
Substance with minimum Entropy is - (a) Water (b) Ice (c) Water vapour (d) None of these
[1]
Q6.
The pH value of gastric juice is - (a) -3 (b) -1.2 (c) -2 (d) -4
[1]
Page 17 of 33
Q7.
IUPAC name of Neopentane is - (a) 2,2-dimethylpropane (b) 2-Methylbutane (c) 3-Methylbutane (d) 2-Ethylbutane
[1]
Q8.
Most stable Carbocation is - (a) (CH3)3C+ (b) CH3CH2+ (c) (CH3)2CH+ (d) CH3+
[1]
Q9.
Oxidation number of oxygen in H2O2 is - (a) -1 (b) -2 (c) -1/2 (d) +1
[1]
Q10.
Which of the following is an example of Homocyclic compound? (a) Cyclopropane (b) Benzene (c) Furan (d) Toluene
[1]
Q11.
In ⁸⁰₃₅Br, the number of neutrons is ___.
[1]
Q12.
The value of change in Gibbs energy (ΔG) for the spontaneous process is always ___.
[1]
Q13.
The solutions which resist change in their pH on dilution are called ___ solution.
[1]
Q14.
___ block elements are called transition elements.
[1]
Q15.
In propyne, ___ sigma (σ) and ___ pi (π) bonds are present.
[1]
Q16.
Oxidation number of Fe in Fe2O3 is ___.
[1]
Q17.
Free radical species are product of ___ bond cleavage.
[1]
Page 18 of 33
Q18.
For n = 1, the value of l is ___.
[1]
Q19.
Write the relation between Cp and Cv for an ideal gas.
[1]
Q20.
Write Mendeleev's Periodic Law.
[1]
Q21.
Write the electronic configuration of Mn (Z=25).
[1]
Q22.
Write the formula to calculate formal charge.
[1]
Q23.
Draw the molecular orbital diagram of Ethane.
[1]
Q24.
Write Pauli's Exclusion Principle.
[1]
Q25.
In an adiabatic process, is change in heat possible or not?
[1]
Q26.
Write the isomers of pentane.
[1]
Q27.
Write the conjugate base of HClO4.
[1]
Q28.
Identify [A] in the reaction: CH3Br + 2Na + BrCH3 --(dry ether)--> [A] + 2NaBr
[1]
Page 19 of 33
Q29.
Write Markownikoff's rule.
[1]
Q30.
Explain disproportionation reaction with example.
[2]
Q31.
Identify the Lewis acid and Lewis base in the following: HO-, F-, H+, BCl3
[2]
Q32.
A solution is prepared by adding 2g of a substance 'A' to 18g of water. Calculate the mass percent of the solute 'A'.
[2]
Q33.
Calculate the pH of 0.005M NaOH solution.
[2]
Q34.
Define Shielding Effect.
[2]
Q35.
Draw resonating structures of CO3²- (carbonate ion).
[2]
Q36.
What is the wave nature of electromagnetic radiation? Draw the spectrum of electromagnetic radiation.
[2]
Q37.
Draw the labelled diagram of Daniel cell and write its equation.
[2]
Page 20 of 33
Q38.
Derive the relation between Kp and Kc.
[2]
Q39.
Explain why the Ionisation Enthalpy of Be is higher than B.
[2]
Q40.
H2S is a gas while H2O is liquid, why?
[2]
Q41.
Identify the oxidizing and reducing agent in the reaction: N2H4(l) + 2H2O2(l) -> N2(g) + 4H2O(l)
[2]
Q42.
What is fractional distillation? Explain with a diagram.
[2]
Q43.
How is Lassaigne's solution prepared?
[2]
Q44.
Explain the addition of HBr on propene with the help of Markownikoff's rule.
[2]
Q45.
Complete the reaction - CH≡CH --(Red hot Fe tube)--> ? CH3COO-Na+ --(CaO, NaOH, Δ)--> ? **OR** Complete the reaction - (Benzene ring) + 3Cl2 --(UV, 500)--> ? CH3-CH=CH2 + O3 --> ? --(Zn + H2O)--> ?
[2]
Q46.
Explain the following: Friedel Craft reaction **OR** Explain the following: β-elimination reaction of Ethyl chloride in the presence of alcoholic KOH
[2]
Page 21 of 33
Q47.
Explain the following: Inductive effect **OR** Explain the following: Hyper-Conjugation
[2]
Q48.
Explain the following: Acidic nature of Alkyne **OR** Explain the following: Anti-Markownikoff rule
[2]
Q49.
Explain the following: Structural isomerism in Hydrocarbons **OR** Explain the following: Nucleophilic species
[2]
Q50.
Balance the given reaction by the oxidation number method: P4(s) + OH-(aq) -> PH3(g) + HPO2-(aq)
[3]
Q51.
Write the IUPAC names of the following compounds - (a) CH3-CH2-C(CH3)=CH-CH3 (a clearly drawn C=C double bond, with a methyl branch on the double-bond carbon) (b) CH3CH2-C(=O)-OH (c) CH3CH2-CH(OH)-CH2CH3 (d) Toluene (a benzene ring with a -CH3 substituent) **OR** Write the IUPAC names of the following compounds - (a) CH3-CH-C≡CH, printed with a -CH2-CH3 (ethyl) branch shown attached below the CH carbon (exact attachment point not fully legible in the scan) (b) CH3CH2-C(=O)-H (c) (CH3)?C-CH2-CH3, printed with a subscript on the methyl count that is not fully legible in the scan (appears as 5, which would be an invalid valence, so this digit is uncertain and transcribed as printed rather than silently corrected) (d) Phenol (a benzene ring with an -OH substituent)
[4]
Section A

mcq · 1 mark each · 51 of 10 shown

Q1.
How many significant figures are there in 0.0052? (a) 4 (b) 1 (c) 3 (d) 2
[1]
Q2.
In 7d orbitals, 7 denotes - (a) Principal quantum number (b) Azimuthal quantum number (c) Magnetic quantum number (d) Spin quantum number
[1]
Q3.
Example of Sp3d2 hybridization is - (a) CH4 (b) PCl5 (c) NH3 (d) SF6
[1]
Page 22 of 33
Q4.
The correct sequence of Ionization Enthalpy for Li, Be, B, C is - (a) C > B > Be > Li (b) C > Be > B > Li (c) B > C > Be > Li (d) C > B > Li > Be
[1]
Q5.
Substance with minimum Entropy is - (a) Water (b) Ice (c) Water vapour (d) None of these
[1]
Q6.
The pH value of gastric juice is - (a) -3 (b) -1.2 (c) -2 (d) -4
[1]
Q7.
IUPAC name of Neopentane is - (a) 2,2-dimethylpropane (b) 2-Methylbutane (c) 3-Methylbutane (d) 2-Ethylbutane
[1]
Q8.
Most stable Carbocation is - (a) (CH3)3C+ (b) CH3CH2+ (c) (CH3)2CH+ (d) CH3+
[1]
Q9.
Oxidation number of oxygen in H2O2 is - (a) -1 (b) -2 (c) -1/2 (d) +1
[1]
Q10.
Which of the following is an example of Homocyclic compound? (a) Cyclopropane (b) Benzene (c) Furan (d) Toluene
[1]
Q11.
In ⁸⁰₃₅Br, the number of neutrons is ___.
[1]
Q12.
The value of change in Gibbs energy (ΔG) for the spontaneous process is always ___.
[1]
Q13.
The solutions which resist change in their pH on dilution are called ___ solution.
[1]
Q14.
___ block elements are called transition elements.
[1]
Page 23 of 33
Q15.
In propyne, ___ sigma (σ) and ___ pi (π) bonds are present.
[1]
Q16.
Oxidation number of Fe in Fe2O3 is ___.
[1]
Q17.
Free radical species are product of ___ bond cleavage.
[1]
Q18.
For n = 1, the value of l is ___.
[1]
Q19.
Write the relation between Cp and Cv for an ideal gas.
[1]
Q20.
Write Mendeleev's Periodic Law.
[1]
Q21.
Write the electronic configuration of Mn (Z=25).
[1]
Q22.
Write the formula to calculate formal charge.
[1]
Q23.
Draw the molecular orbital diagram of Ethane.
[1]
Q24.
Write Pauli's Exclusion Principle.
[1]
Q25.
In an adiabatic process, is change in heat possible or not?
[1]
Page 24 of 33
Q26.
Write the isomers of pentane.
[1]
Q27.
Write the conjugate base of HClO4.
[1]
Q28.
Identify [A] in the reaction: CH3Br + 2Na + BrCH3 --(dry ether)--> [A] + 2NaBr
[1]
Q29.
Write Markownikoff's rule.
[1]
Q30.
Explain disproportionation reaction with example.
[2]
Q31.
Identify the Lewis acid and Lewis base in the following: HO-, F-, H+, BCl3
[2]
Q32.
A solution is prepared by adding 2g of a substance 'A' to 18g of water. Calculate the mass percent of the solute 'A'.
[2]
Q33.
Calculate the pH of 0.005M NaOH solution.
[2]
Q34.
Define Shielding Effect.
[2]
Q35.
Draw resonating structures of CO3²- (carbonate ion).
[2]
Page 25 of 33
Q36.
What is the wave nature of electromagnetic radiation? Draw the spectrum of electromagnetic radiation.
[2]
Q37.
Draw the labelled diagram of Daniel cell and write its equation.
[2]
Q38.
Derive the relation between Kp and Kc.
[2]
Q39.
Explain why the Ionisation Enthalpy of Be is higher than B.
[2]
Q40.
H2S is a gas while H2O is liquid, why?
[2]
Q41.
Identify the oxidizing and reducing agent in the reaction: N2H4(l) + 2H2O2(l) -> N2(g) + 4H2O(l)
[2]
Q42.
What is fractional distillation? Explain with a diagram.
[2]
Q43.
How is Lassaigne's solution prepared?
[2]
Q44.
Explain the addition of HBr on propene with the help of Markownikoff's rule.
[2]
Page 26 of 33
Q45.
Complete the reaction - CH≡CH --(Red hot Fe tube)--> ? CH3COO-Na+ --(CaO, NaOH, Δ)--> ? **OR** Complete the reaction - (Benzene ring) + 3Cl2 --(UV, 500)--> ? CH3-CH=CH2 + O3 --> ? --(Zn + H2O)--> ?
[2]
Q46.
Explain the following: Friedel Craft reaction **OR** Explain the following: β-elimination reaction of Ethyl chloride in the presence of alcoholic KOH
[2]
Q47.
Explain the following: Inductive effect **OR** Explain the following: Hyper-Conjugation
[2]
Q48.
Explain the following: Acidic nature of Alkyne **OR** Explain the following: Anti-Markownikoff rule
[2]
Q49.
Explain the following: Structural isomerism in Hydrocarbons **OR** Explain the following: Nucleophilic species
[2]
Q50.
Balance the given reaction by the oxidation number method: P4(s) + OH-(aq) -> PH3(g) + HPO2-(aq)
[3]
Q51.
Write the IUPAC names of the following compounds - (a) CH3-CH2-C(CH3)=CH-CH3 (a clearly drawn C=C double bond, with a methyl branch on the double-bond carbon) (b) CH3CH2-C(=O)-OH (c) CH3CH2-CH(OH)-CH2CH3 (d) Toluene (a benzene ring with a -CH3 substituent) **OR** Write the IUPAC names of the following compounds - (a) CH3-CH-C≡CH, printed with a -CH2-CH3 (ethyl) branch shown attached below the CH carbon (exact attachment point not fully legible in the scan) (b) CH3CH2-C(=O)-H (c) (CH3)?C-CH2-CH3, printed with a subscript on the methyl count that is not fully legible in the scan (appears as 5, which would be an invalid valence, so this digit is uncertain and transcribed as printed rather than silently corrected) (d) Phenol (a benzene ring with an -OH substituent)
[4]
Page 27 of 33
Section A

mcq · 1 mark each · 51 of 10 shown

Q1.
How many significant figures are there in 0.0052? (a) 4 (b) 1 (c) 3 (d) 2
[1]
Q2.
In 7d orbitals, 7 denotes - (a) Principal quantum number (b) Azimuthal quantum number (c) Magnetic quantum number (d) Spin quantum number
[1]
Q3.
Example of Sp3d2 hybridization is - (a) CH4 (b) PCl5 (c) NH3 (d) SF6
[1]
Q4.
The correct sequence of Ionization Enthalpy for Li, Be, B, C is - (a) C > B > Be > Li (b) C > Be > B > Li (c) B > C > Be > Li (d) C > B > Li > Be
[1]
Q5.
Substance with minimum Entropy is - (a) Water (b) Ice (c) Water vapour (d) None of these
[1]
Q6.
The pH value of gastric juice is - (a) -3 (b) -1.2 (c) -2 (d) -4
[1]
Q7.
IUPAC name of Neopentane is - (a) 2,2-dimethylpropane (b) 2-Methylbutane (c) 3-Methylbutane (d) 2-Ethylbutane
[1]
Q8.
Most stable Carbocation is - (a) (CH3)3C+ (b) CH3CH2+ (c) (CH3)2CH+ (d) CH3+
[1]
Q9.
Oxidation number of oxygen in H2O2 is - (a) -1 (b) -2 (c) -1/2 (d) +1
[1]
Q10.
Which of the following is an example of Homocyclic compound? (a) Cyclopropane (b) Benzene (c) Furan (d) Toluene
[1]
Page 28 of 33
Q11.
In ⁸⁰₃₅Br, the number of neutrons is ___.
[1]
Q12.
The value of change in Gibbs energy (ΔG) for the spontaneous process is always ___.
[1]
Q13.
The solutions which resist change in their pH on dilution are called ___ solution.
[1]
Q14.
___ block elements are called transition elements.
[1]
Q15.
In propyne, ___ sigma (σ) and ___ pi (π) bonds are present.
[1]
Q16.
Oxidation number of Fe in Fe2O3 is ___.
[1]
Q17.
Free radical species are product of ___ bond cleavage.
[1]
Q18.
For n = 1, the value of l is ___.
[1]
Q19.
Write the relation between Cp and Cv for an ideal gas.
[1]
Q20.
Write Mendeleev's Periodic Law.
[1]
Q21.
Write the electronic configuration of Mn (Z=25).
[1]
Page 29 of 33
Q22.
Write the formula to calculate formal charge.
[1]
Q23.
Draw the molecular orbital diagram of Ethane.
[1]
Q24.
Write Pauli's Exclusion Principle.
[1]
Q25.
In an adiabatic process, is change in heat possible or not?
[1]
Q26.
Write the isomers of pentane.
[1]
Q27.
Write the conjugate base of HClO4.
[1]
Q28.
Identify [A] in the reaction: CH3Br + 2Na + BrCH3 --(dry ether)--> [A] + 2NaBr
[1]
Q29.
Write Markownikoff's rule.
[1]
Q30.
Explain disproportionation reaction with example.
[2]
Q31.
Identify the Lewis acid and Lewis base in the following: HO-, F-, H+, BCl3
[2]
Page 30 of 33
Q32.
A solution is prepared by adding 2g of a substance 'A' to 18g of water. Calculate the mass percent of the solute 'A'.
[2]
Q33.
Calculate the pH of 0.005M NaOH solution.
[2]
Q34.
Define Shielding Effect.
[2]
Q35.
Draw resonating structures of CO3²- (carbonate ion).
[2]
Q36.
What is the wave nature of electromagnetic radiation? Draw the spectrum of electromagnetic radiation.
[2]
Q37.
Draw the labelled diagram of Daniel cell and write its equation.
[2]
Q38.
Derive the relation between Kp and Kc.
[2]
Q39.
Explain why the Ionisation Enthalpy of Be is higher than B.
[2]
Q40.
H2S is a gas while H2O is liquid, why?
[2]
Page 31 of 33
Q41.
Identify the oxidizing and reducing agent in the reaction: N2H4(l) + 2H2O2(l) -> N2(g) + 4H2O(l)
[2]
Q42.
What is fractional distillation? Explain with a diagram.
[2]
Q43.
How is Lassaigne's solution prepared?
[2]
Q44.
Explain the addition of HBr on propene with the help of Markownikoff's rule.
[2]
Q45.
Complete the reaction - CH≡CH --(Red hot Fe tube)--> ? CH3COO-Na+ --(CaO, NaOH, Δ)--> ? **OR** Complete the reaction - (Benzene ring) + 3Cl2 --(UV, 500)--> ? CH3-CH=CH2 + O3 --> ? --(Zn + H2O)--> ?
[2]
Q46.
Explain the following: Friedel Craft reaction **OR** Explain the following: β-elimination reaction of Ethyl chloride in the presence of alcoholic KOH
[2]
Q47.
Explain the following: Inductive effect **OR** Explain the following: Hyper-Conjugation
[2]
Q48.
Explain the following: Acidic nature of Alkyne **OR** Explain the following: Anti-Markownikoff rule
[2]
Q49.
Explain the following: Structural isomerism in Hydrocarbons **OR** Explain the following: Nucleophilic species
[2]
Page 32 of 33
Q50.
Balance the given reaction by the oxidation number method: P4(s) + OH-(aq) -> PH3(g) + HPO2-(aq)
[3]
Q51.
Write the IUPAC names of the following compounds - (a) CH3-CH2-C(CH3)=CH-CH3 (a clearly drawn C=C double bond, with a methyl branch on the double-bond carbon) (b) CH3CH2-C(=O)-OH (c) CH3CH2-CH(OH)-CH2CH3 (d) Toluene (a benzene ring with a -CH3 substituent) **OR** Write the IUPAC names of the following compounds - (a) CH3-CH-C≡CH, printed with a -CH2-CH3 (ethyl) branch shown attached below the CH carbon (exact attachment point not fully legible in the scan) (b) CH3CH2-C(=O)-H (c) (CH3)?C-CH2-CH3, printed with a subscript on the methyl count that is not fully legible in the scan (appears as 5, which would be an invalid valence, so this digit is uncertain and transcribed as printed rather than silently corrected) (d) Phenol (a benzene ring with an -OH substituent)
[4]
Page 33 of 33