Goa Board Class 12 Sample Paper 2024 Chemistry

Sample Paper
&
Question Paper Pattern
2023
2024

GOA BOARD

GOA BOARD OF SECONDARY AND HIGHER SECONDARY EDUCATION
CLASS: XII SUBJECT: CHEMISTRY
Syllabus-2023-2024
CLASS XII (THEORY)
Total Periods 180

Unit I: Solid State (Periods 12)
Classification of solids based on different binding forces :molecular, ionic covalent and metallic solids,
amorphous and crystalline solids(elementary idea),unit cell in two dimensional and three dimensional lattices,
calculation of density of unit cell, packing in solids, packing efficiency (excluding derivations), voids ,
number of atoms per unit cell in a cubic unit cell, point defects, magnetic properties.

Unit II : Solutions (Periods 12)
Types of solutions, expression of concentration of solutions of solids in liquids, solubility of gases in
liquids, vapour pressure of liquid solutions, Raoult’s law ,Ideal solutions & Non ideal solutions, colligative
properties – relative lowering of vapour pressure, elevation of B.P., depression of freezing point, osmosis ,reverse
osmosis & osmotic pressure, determination of molecular masses using colligative properties, abnormal molecular
mass, Vant Hoff factor(excluding numericals using vant Hoff factor).

Unit III: Electrochemistry (Periods 14)
Redox reactions; conductance in electrolytic solutions(excluding measurement of conductivity of
ionic solutions), specific and molar conductivity, variations of conductivity with concentration,
Kohlrausch’s Law, electrolysis and laws of electrolysis (elementary idea), – Electrochemical cells &
electrolytic cells; Galvanic cells EMF of a cell, measurement of standard electrode potential ,Nernst
equation and its application to chemical cells. Relation between Gibbs energy change and EMF of a cell .
Batteries (only Leclanche cell & lead accumulator), fuel cells; corrosion.

Unit IV: Chemical Kinetics (Periods 12)
Rate of a reaction (average and instantaneous), factors affecting rates of reaction: concentration,
temperature, catalyst; order and molecularity of a reaction; rate law and specific rate constant, integrated
rate equations and half-life (only for zero and first order reactions); Temperature dependence of rate of
reaction, effect of catalyst on rate of reaction ,Activation energy& Arrhenious equation.

Unit V: Surface Chemistry (Periods 8)
Adsorption – physisorption and chemisorption; Adsorption Isotherms Adsorption from solution phase, catalysis
:homogeneous and heterogeneous, activity and selectivity: enzyme catalysis; colloidal state: distinction between
true solutions, colloids and suspensions; lyophillic, lyophobic multimolecular and macromolecular colloids,
Associated colloids; Preparation of colloids( only Bredig’s arc method) properties of colloids; Tyndall effect,
Brownian movement, charge on colloids(only examples of positively and negatively charged colloids)
electrophoresis, coagulation; emulsions – types of emulsions.

Unit VI: General Principles and Processes of Isolation of Elements (Periods 8 )
Occurrence of metals, Concentration of ores, Extraction of crude metal from concentrated
ore(excluding diagram of reverberatory furnace &Blast furnace),Thermodynamic principles of
metallurgy(excluding Ellingham diagram),Extraction of iron from it’s oxides ,Extraction of copper from
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cuprous oxide, Extraction of Zinc from zinc oxide. Electrochemical principles of metallurgy -Extraction
of Aluminium. Refining- Distillation, Liquation, Electrolytic refining, Zone refining, Vapour phase
refining.
Unit VII: The p-Block Elements (Periods 16)
Group 15 elements: General introduction, electronic configuration, occurrence, oxidation states,
trends in physical and chemical properties; nitrogen – preparation, properties and uses; compounds
of nitrogen: preparation and properties of ammonia and nitric acid, oxides of nitrogen (only
formulas); Phosphorous-allotropic forms; compounds of phosphorous: preparation and properties of
phosphine .
Group 16 elements: General introduction, electronic configuration, oxidation states, occurrence,
trends in physical and chemical properties; dioxygen: preparation, properties and uses, Sulphur –
allotropic forms; compounds of sulphur: preparation, properties and uses of sulphur dioxide; sulphuric
acid: properties and uses, oxoacids of sulphur (structures only).
Group 17 elements: General introduction, electronic configuration, oxidation states, occurrence,
trends in physical and chemical properties; compounds of halogens: preparation, properties and uses
of chlorine and hydrochloric acid, interhalogen compounds, oxoacids of halogens (structures only).
Group 18 elements: General introduction, electronic configuration, occurrence, trends in
physical and chemical properties, Preparation, properties &structures of Xenon Fluorine compounds
& Xenon Oxygen compounds.

Unit VIII: The d and f Block Elements (Periods 12)
General introduction ,electronic configuration, occurrence and characteristics of transition metals,
general trends in properties of the first row transition metals – metallic character, ionization enthalpy,
oxidation states, ionic radii, colour, catalytic property, magnetic properties, interstitial compounds,
alloy formation. Preparation and properties of K 2Cr2 O 7 and KM nO.4
Lanthanoids – electronic configuration, oxidation states, chemical reactivity and lanthanoid
contraction and its consequences.
Actinoids – , Ionic sizes, oxidation states and comparison with lanthanoids .

Unit IX Coordination Compounds (Periods 12)

Coordination compounds: Introduction, ligands, coordination number, colour, magnetic properties
and shapes, IUPAC nomenclature of mononuclear coordination compounds, bonding, Werner’s
theory, VBT,CFT; isomerism (structural and stereo)importance of coordination compounds (in
qualitative analysis, extraction of metals and biological systems).

Unit X: Haloalkanes and Haloarenes (Periods 12)

Haloalkanes: Nomenclature, nature of C-X bond, physical and chemical properties, mechanism of
substitution reactions. Optical rotation.

Haloarenes: Nature of C-X bond, substitution reactions(directive influence of halogen for
monosubstituted compounds only). Reaction with metals.

Unit XI: Alcohols, Phenols and Ethers (Periods 12)
Alcohols: Nomenclature, methods of preparation, physical and chemical properties ; identification

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of primary, secondary and tertiary alcohols.
Phenols : Nomenclature, methods of preparation, physical and chemical properties, acidic nature
of phenol, electrophilic substitution reactions, kolbes reaction ,Reimer Tiemann reaction, reaction
with zinc dust, oxidation.
Ethers : Nomenclature, methods of preparation, physical and chemical properties.

Unit XII: Aldehydes, Ketones and Carboxylic Acids (Periods 14)
Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of preparation,
physical and chemical properties, nucleophilic addition(with respect to HCN , Ammonia, Hydrazine &
2,4 DNP ), reduction, oxidation and reactivity of alpha and no alpha hydrogen in aldehydes,
electrophilic substitution reaction.
Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical and chemical
properties.

Unit XIII: Amines (Periods 10)
Amines: Nomenclature, classification, structure, methods of preparation, physical and chemical
properties, identification of primary secondary and tertiary amines.
Diazonium salts: Preparation, chemical reactions .
Unit XIV: Biomolecules (Periods 10)
Carbohydrates – Classification (aldoses and ketoses), monosaccharide (glucose and fructose),
D-L configuration, oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose,
glycogen excluding structures)
Proteins - Elementary idea of a - amino acids classification, peptide bond, polypeptides, proteins,
primary structure, secondary structure, tertiary structure and quaternary structure (qualitative idea only),
denaturation of proteins.
Vitamins – Classification and functions.
Nucleic Acids: DNA and RNA(excluding structures).

Unit XV: Polymers (Periods 8)
Classification based on source, structure, molecular forces and mode of polymerization, Preparation of
polymers (natural and synthetic) like polythene, Teflon, PAN ,nylon, polyesters(dacron).Melamine &
bakelite(excluding structures), and rubber(excluding structures for natural and vulcanized), copolymerization.:
Biodegradable and non-biodegradable polymers.

Unit XVI: Chemistry in Everyday Life (Periods 8)
1. Chemicals in medicines – analgesics, tranquilizers, antiseptics, disinfectants,
antimicrobials, antifertility drugs, antibiotics, antacids, antihistamines.
2. Chemicals in food – preservatives, artificial sweetening agents.
3. Cleansing agents – soaps, types of soaps & detergents, cleansing action.(excluding equations)

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GOA BOARD OF SECONDARY AND HIGHER SECONDARY EDUCATION
CLASS: XII SUBJECT: CHEMISTRY

SCHEME OF EXAMINATION AND MARKS DISTRIBUTION (2023- 24)

1st 2nd Innovative
Board
No Unit Formativ Formative Exam,
e testing
Test March
Test,
Oct,
Aug.
1 THE SOLID STATE 4± 1
2 SOLUTIONS 5±1 5±1
3 ELECTROCHEMISTRY 5±1 5±1
4 CHEMICAL KINETICS 5±1 5±1
5 SURFACE CHEMISTRY 4±1
6 GENERAL PRINCIPLES AND 4±1 4±1
PROCESSESOF ISOLATION OF
ELEMENTS
7 THE P-BLOCK ELEMENTS 6±1
8 THE d-& f-BLOCK ELEMENTS 5±1
5±1
9 COORDINATION COMPOUNDS 4±1
10 HALOALKANES& HALOARENES 6±1 5±1
11 ALCOHOLS,PHENOLS AND ETHERS 6±1 5±1
12 ALDEHYDES, KETONES AND 6±1
CARBOXYLIC ACIDS
13 AMINES 4±1
14 BIOMOLECULES 4±1 4±1
15 POLYMERS 2±1
16 CHEMISTRY IN EVERDAY LIFE 2±1
INNOVATIVE TESTING 10
PRACTICAL-FIRST TERM 10
MAXIMUM MARKS 20 20 20 70
DURATION IN MINUTES 60 60 150
NUMBER OF QUESTIONS 10 10 35
MULTIPLE CHOICE QUESTION (1MARK) 2 2
VERY SHORT ANSWER VSA (1 MARK) 2 2
SHORT ANSWER I (SA I)—2 MARKS 3 3
SHORT ANSWER (SA II)—3 MARKS 2 2
LONG ANSWER (LA) —4 MARKS 1 1
KNOWLEDGE % 30 ±5 30 ±5
UNDERSTANDING % 40±5 40±5
SKILL % 10±5 10±5
APPLICATION % 20 ±5 20 ±5
DIFFICULTY EASY 30±5 30±5
LEVEL % AVERAGE 50±5 50±5
DIFFICULT 20±5 20±5

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FIRST TERM PRACTICAL EXAMINATION

VOLUMETRIC ANALYSIS 06 Marks

DETECTION OF FUNCTIONAL GROUP 02 Marks

JOURNAL + VIVA 02 Marks

TOTAL 10 Marks

DURATION 90 Minutes

FINAL HSSC PRACTICAL EXAMINATION

VOLUMETRIC ANALYSIS 08 Marks

JOURNAL + VIVA 02 Marks (01+01)

ANALYSIS OF SALT 10 Marks

TOTAL 20 Marks

DURATION 180 Minutes(Three Hours)

COMPUTATION OF INTERNAL MARKS

Examination Max Marks Duration
A. Formative -I Examination 20 Marks 60 Minutes
B. Formative -II Examination 20 Marks 60 Minutes
C. First term Practical examination 10 Marks 90 Minutes
D. Innovative Test 10 Marks
TOTAL=(A+B+C+D) 60 Marks
HSSC Internal Marks=Average=60/6 = MAX=10 10 Marks

COMPUTATION OF CHEMISTRY MARKS FOR FINAL HSSC EXAMINATION

HSSC Theory examination 70 Marks 150 Minutes
HSSC Practical examination 20 Marks 180 Minutes
HSSC Internal Marks 10 Marks
Total 100 Marks

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Goa Board of Secondary & Higher Secondary Education
Alto, Betim-Goa

Model Paper for First term Practical Examination-2023
CHEMISTRY
Date: Duration: 90 Minutes
Session: Max. Marks: 10

N. B.
1) On your answer books write your Examination Seat number and your Laboratory
table number.
2) Get the burette reading and confirmatory tests initialed by the Examiner.
3) Check if the number on (i) your table (ii) answer script and (iii) the containers A, B,
and F are the same. If not, report immediately to the Examiner.
4) Use of non - programmable calculator is allowed.
Atomic Masses:- H=1, C=12, N=14, O=16, S=32, K=39, Mn=55, Fe= 56.

SECTION – I
Q .1 You are provided with two solutions as follows:-
Container A: N/M stock solution of hydrated Oxalic acid / Mohr’s salt.
Container B: KMnO4 Solution
Using the stock solution from Container A, prepare 100 mL of N/M hydrated
Oxalic acid /Mohr’s salt in the given Standard Measuring flask C.
Using the solution prepared in flask C, determine N/M of the solution in container B.
Also calculate. ( any one)
• The strength of the solution in container B in terms of grams per mL.
• The percentage purity of the solution in container B, g of which have been dissolved
per mL. (6 Marks)

Q.2. Determine the functional group of the organic compound supplied to you in Container F bearing
your table number. Give a complete report of all the tests performed. (2 Marks)

Q.3. Journal + Viva (1+1 Marks)

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Marking Scheme

Scheme for allotment of marks for First term practical examination

1. Volumetric analysis ........................................................................................ 6 marks
a. Calculation of correct volume .............................................. 1 mark
b. Titre reading .............................................. 3 marks
c. Calculations .......................................... 1 + 1 mark (2 Marks)

2. Functional group ............................................................................................. 2 marks
(Distribution of marks same as for the board examination)

3. Journal + Viva ............................................................. 1+ 1 mark

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SEAT NO:- TABLE NO:-
Goa Board of Secondary & Higher Secondary Education
Alto, Betim-Goa

HSSC Practical Examination –March/April 2024
CHEMISTRY
Date: Duration: 3 Hours
Session: Max. Marks: 20

N. B.1) Write your Examination Seat number and your Laboratory table number on your
answer book.
2) Get the burette reading and confirmatory tests initialed by one of theExaminer.
3) Check if the number on (i) your table (ii) answer book and (iii) the containersA, B ,C and D
are the same. If not, report immediately to the Examiners.
4) Use of non - programmable calculator is allowed.
Atomic Masses:- H=1, C=12, N=14, O=16, S=32, K=39, Mn=55, Fe= 56.

SECTION – I
Q.1 You are provided with two solutions as follows:-

Container A: N/M stock solution of hydrated Oxalic acid / Mohr’s salt.
Container B: KMnO4 Solution
Using the stock solution from Container A, prepare 100 mL of N/M hydrated
Oxalic acid /Mohr’s salt in the given Standard Measuring flask C.
Using the solution prepared in flask C, determine N/M of the solution in container B.
Also calculate.(any one)
• The strength of the solution in container B in terms of grams per mL.
• The percentage purity of the solution in container B, g of which have been dissolved
per mL. (08 Marks)

Q.2 Journal + Viva (1+1 Marks)

SECTION – II

Q.3 Analyse the inorganic salt given in container D bearing your table number qualitatively
and detect the cation and anion present. Give a complete report of all the tests performed.
Write the formula of the compound detected. (10 Marks)
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GOA BOARD OF SECONDARY & HIGHER SECONDARY
EDUCATION Alto, Betim – Goa
HIGHER SECONDARY SCHOOL CERTIFICATE EXAMINATION
GUIDELINES FOR CONDUCT OF THE H.S.S.C. PRACTICALS IN CHEMISTRY -2024
1 .Student should report in journal:
(a) Minimum of 4 volumetric exercises.
(b) Minimum 12 inorganic qualitative analysis.
(c) Four Physical experiments
• To prepare lyophilic sol of starch.
• To determine enthalpy of Neutralization.
• To study the effect of concentration on the rate of reaction.
• To study the role of emulsifying agents in stabilizing the emulsion of different
oils.
(d) Minimum Five Organic compounds from the following list covering all five functional
groups
(Oxalic acid, Acetic acid, Benzoic acid ,β-Napthol, Aniline, Benzaldehyde, Acetone ,Ehanol)

2 List of the compounds.

COMPOUND COMPOUND
NH4Cl Zn(NO3)2
NH4Br ZnCl2
(NH4)3PO4
CoCl2
(NH4)2CO3
CoSO4
Pb(NO3)2
Pb(CH3COO)2 Co(NO3)2
CuSO4 CaCl2
CuCl2
Ca(NO3)2
Cu(NO3)2
AlCl3 Sr(NO3)2
Al2(SO4)3 SrCl2
Al(NO3)3 BaCl2
FeCl3 Ba(NO3)2
Fe(NO3)3
MgSO4
MnCl2 MgCl2
MnSO4 KCl
NiSO4 KI
NiCl2 KBr
Ni(NO3)2 K2SO4
ZnSO4 K2CO3
K3PO4
K2C2O4

1. Scheme for allotment of marks.

Q1. In organic Volumetric Analysis (Redox titration) (8 marks)

(a) Correct observations (burette solution, solution in the flask, indicator and colour change) (1 mark)

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(b) Calculation of correct volume .............................................. (1 mark)
(c) Range of titre reading for allotment of marks is as follows: (Maximum 4 marks)
Error in titre reading Marks
+0.2mL 4
+0.3mL 3
+0.4mL 2
+0.5mL 1
Pilot reading and a set of three concordant reading shall be recorded in the observation table and thus
the concordant reading should be taken as the correct reading for assigning the marks for accuracy in the
reading.

(d) Calculations:- (2 marks)
(1) Calculation of N/M of solution in container B,by using
(1)N1V1=N2V2 (2)N=aM
a1M1V1=a2M2V2formula/e, (a= number of electrons lost or gained per molecule )….…
(1 mark)
(2) Calculate the following…………. (1 mark)
Strength of the solution in container B in terms of g/ mL
Or % purity of solution in container B

N.B. In case the titre reading is not within the range of error then for calculations (correct formula) ½
mark to be allotted out of the 1 mark allotted for each calculation.

Q 2. JOURNAL+Viva (2 Mark)
The marks are to be allotted as follows:
I. For the experiments performed and recorded during the year. (1 mark)
II. Viva on Physical expts (Two questions ½ marks each) (1 mark)

Q 3. Qualitative analysis of Inorganic Compound (10 marks)

Dry/PreliminaryTests ......... (4 marks) WET TESTS FOR CATION…..(3 marks)
Colour .............................(½ mark) 1) Group separation ...................... (1 mark)
Heating in a dry test tube……..(½ mark) 2) Identification of cation …..…(1 mark)
Flame test ……………..…(½ mark) 3)C.T. for cation………………(1 mark)
Test for NH + ………. ………(½ mark)
4
WET TESTS FOR ANION AND
Dil HCI test .................... (½ mark)
RESULT........................ (2 marks)
Conc H2SO4 ....................... (½ mark)
Phosphate test ………..…(½ mark) (1) Identification of anion……..(1 mark)
KMnO4test…………...……(½ mark) (2) C.T. for anion……………. (1 mark)
If no anion is detected and if it is SO -2, it need (3) CORRECT FORMULA OF SALT
4
…………………………………. (1 mark)
not be reported as given in the chart.

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GOA BOARD OF SECONDARY AND HIGHER SECONDARY
EDUCATIONALTO - PORVORIM , GOA.

BLUEPRINT OF FIRST FORMATIVE EXAM ( 2023 - 2024 )

STD : XII SCIENCE SUBJECT : CHEMISTRY MARKS : 20 DURATION : 60 min

OBJECTIVES DIFFICULTY LEVEL
K U S A Eas Average Difficul
y (Av) t
(E) (D)
Percentage 30% 40% 10% 20% 30% 50% 20%
Marks 6 8 2 4 6 10 4

Variation of ± 5 % is permitted in the above Objectives and Difficulty Level

Type of questions Marks Number of Total marks
questions
MCQ 1 2 2
VSA 1 2 2
SA – I 2 3 6
SA – II 3 2 6
LA 4 1 4
Total ….. 10 20

MCQ = Multiple Choice Question
VSA = Very Short Answer
SA – I = Short Answer – I
SA –II = Short Answer –II
LA =Long Answer.

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BLUEPRINT OF FIRST FORMATIVE EXAM (2023 - 2024)

Q. No. Type Unit No. and Name Objectives Difficulty Duration Marks
level (min)

1 MCQ 2.SOLUTIONS U E 2 1

2 MCQ 4. CHEMICAL K E 2 1
KINETICS

3 VSA 4. CHEMICAL K E 2 1
KINETICS
4 VSA 6.GENERAL S Av 2 1
PRINCIPLES &
PROCESSES OF
ISOLATION OF
ELEMENTS
5 SA-1 2.SOLUTIONS A D 5 2

6* SA-I 2.SOLUTIONS K/S Av 4 1+1=2
OR

6* SA-I 2.SOLUTIONS K/S Av 4 1+1=2

7 SA-I 10. HALOALKANES A D 5 2
AND
HALOARENES
8 SA-II 6.GENERAL K E 8 3
PRINCIPLES &
PROCESSES OF
ISOLATION OF
ELEMENTS
9 SA-II 4.CHEMICAL U Av 8 3
KINETICS
10* LA 10. HALOALKANES U Av 12 4
AND
HALOARENES
OR
10* LA 10. HALOALKANES U Av 12 4
AND
HALOARENES
TOTAL DURATION IN MINUTES AND 50 min 20mks
MARKS

*Internal choice

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BLUEPRINT OF SECOND FORMATIVE EXAM (2023 – 2024)
STD : XII SCIENCE SUBJECT : CHEMISTRY MAXIMUM MARKS : 20
DURATION : 60 Min

OBJECTIVES DIFFICULTY LEVEL

K U S A EASY AVERAGE( DIFFICULT
(E) Av) (D)

Percentage 30 40 10 20% 30% 50% 20%
% % %

Marks 6 8 2 4 6 10 4

Variation of ± 5% is permitted in the above Objectives and Difficulty Level.

TYPE OF MARKS NUMBER OF TOTAL
QUESTIONS QUESTIONS MARKS

MCQ 1 2 2

VSA 1 2 2

SA - I 2 3 6

SA – II 3 2 6

LA 4 1 4

TOTAL ------------- 10 20
-

MCQ = Multiple Choice Question
VSA = Very Short Answer
SA – 1 = Short Answer type I
SA- II = Short Answer type II
LA = Long Answer.

*Internal choice

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.BLUEPRINT OF SECOND FORMATIVE EXAM (2023-2024)

DURATION
Q.No. TYPE UNIT NUMBER AND OBJECTIVES DIFFICULTY IN MARKS
NAME LEVEL Min

1 MCQ I4. BIOMOLECULES K E 2 1
11. ALCOHOLS, PHENOLS
2 MCQ AND ETHERS K E 2 1

3 VSA 14. BIOMOLECULES K E 2 1
11. ALCOHOLS, PHENOLS
4 VSA AND ETHERS K E 2 1

5 SA-1 8. d-AND f-BLOCK A D 5 2
ELEMENTS

6 SA- 1 14. BIOMOLECULES U E 4 2

7* SA-1 A D 5 2
3 ELECTROCHEMISTRY

OR

7* SA- 1 3. A D 5 2
ELECTROCHEMISTRY

8 SA-II 3. S+U Av 8 1+2
ELECTROCHEMISTRY

9 SA-II 8. d-AND f-BLOCK S+K Av 8 1+2
ELEMENTS
11. ALCOHOLS, PHENOLS
10* LA AND ETHERS U Av 12 4

OR
11. ALCOHOLS, PHENOLS
10* LA AND ETHERS. U Av 12 4

TOTAL DURATION IN MINUTES AND 50 min 20mks
MARKS

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Blue Print of HSSC Final Examination March-2024

Q. Objective Difficulty Q-Type Duration Marks
No. Unit No. and Name Level (min)

1 1. THE SOLID STATE A D MCQ 3 1
2 4. CHEMICAL KINETICS K E MCQ 1 1
3 10. HALOALKANES AND HALOARENES U A MCQ 2 1
4 11. ALCOHOLS, PHENOLS AND ETHERS U A MCQ 2 1
5 8. The d-& f-block elements K E MCQ 1 1
6 2. SOLUTIONS A D MCQ 3 1
7 13.AMINES A D MCQ 3 1
8 14. BIOMOLECULES U A MCQ 1 1
9 6.GENERAL PRINCIPLES & PROCESSES OF ISOLATION
S A VSA 3 1
OF ELEMENTS
10 11. ALCOHOLS, PHENOLS AND ETHERS U A VSA 3 1
11 9.COORDINATION COMPOUNDS S A VSA 3 1
12 5. SURFACE CHEMISTRY K E VSA 2 1
13 3.ELECTROCHEMISTRY K E VSA 2 1
14 15.POLYMERS K E SA-I 3 2
15 7. THE P-BLOCK ELEMENTS U A SA-I 4 2
16 16. CHEMISTRY IN EVERYDAY LIFE K E SA-I 2 2
17 3.ELECTROCHEMISTRY S A SA-I 4 2
18 4. CHEMICAL KINETICS U A SA-I 3 2
19 12. ALDEHYDES, KETONES AND CARBOXYLIC ACIDS U A SA-I 3 2
20 8. The d-& f-block elements U A SA-I 3 2
21 10. HALOALKANES AND HALOARENES U A SA-I 4 2
22 3.ELECTROCHEMISTRY SA-I
A D 6 2
OR
22 3.ELECTROCHEMISTRY A D SA-I 6 2
23 8. The d-& f-block elements K E SA-I 2 2
24 10. HALOALKANES AND HALOARENES A D SA-I 5 2
25 4. CHEMICAL KINETICS K E SA-I 3 2
26 6.GENERAL PRINCIPLES & PROCESSES OF ISOLATION
K E SA-II 5 3
OF ELEMENTS
27 5. SURFACE CHEMISTRY S+U A SA-II 8 1+2
28 9.COORDINATION COMPOUNDS K E SA-II 4 3
29 14. BIOMOLECULES K E SA-II 4 3
30 1. THE SOLID STATE S+U A SA-II 8 1+2
31 11. ALCOHOLS, PHENOLS AND ETHERS SA-II
A D 8 3
OR
31 11. ALCOHOLS, PHENOLS AND ETHERS A D SA-II 8 3
32 13.AMINES U A SA-II 7 3
33 2. SOLUTIONS
S+U A LA 8 1+3
OR
33 2. SOLUTIONS S+U A LA 8 1+3
34 7. THE P-BLOCK ELEMENTS LA
OR U A 8 4
34 7. THE P-BLOCK ELEMENTS U A LA 8 4
35 12. ALDEHYDES, KETONES AND CARBOXYLIC ACIDS LA
A D 9 4
OR
35 12. ALDEHYDES, KETONES AND CARBOXYLIC ACIDS A D LA 9 4
TOTAL DURATION (min) & Marks 140 70

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MODEL QUESTION PAPER - FINAL EXAMINATION ( 2023 - 2024)

STD : XII SCIENCE SUBJECT : CHEMISTRY MAXIMUM MARKS : 70
NUMBER OF QUESTIONS : 35 DURATION : 2 ½ hours.

INSTRUCTIONS : (i) All questions are compulsory. However Q. Nos . 22, 31, 33, 34 & 35 have
Internal choice
(ii) Answer each question only once.
(iii) Do not use calculators. Logarithmic tables shall be supplied on request.
(iv) Question Nos . 1 to 13 carry one mark each.
(v) Question Nos.14 to 25 carry two marks each.
(vi) Question Nos. 26 to 32 carry three marks each .
(vii) Question Nos 33, 34 & 35 carry four marks each.
Atomic mass: Na=23,Cl=35.5 u

Q. 1 The number of unit cells in 58.5 g of NaCl is nearly 1
● 6 × 1020
● 3 × 1022
● 1.5 × 1023
● 0.5 × 1024
Q.2 Activation energy for a chemical reaction with rate constants k 1 and k2 at 1
temperatures T1 and T2 respectively is calculated using the equation………….

Q.3 The correct order of boiling points for the given sets of compounds is . 1
● 1-iodopropane < 1-bromopropane <1-chloropropane < propane.
● 1-chloropropane > 1-bromopropane > 1-iodopropane > propane.
● Propane < 1-chloropropane < 1-bromopropane < 1-iodopropane.
● Propane > 1-iodopropane > 1-bromopropane > 1-chloropropane.

Q.4 Hydroboration – oxidation of propene in presence of NaOH and hydrogen 1
peroxide gives —--
● propan-1-ol
● propan- 2-ol
● 2- methylpropanol
● 2- methylpropan-2-ol
Q.5 Colour of transition metal ions are due to absorption of some wavelength. This 1
is due to .

● d-f transition
● d-d transition
● s-d transition
● f-f transition

Q.6 An unripe mango placed in a concentrated salt solution to prepare pickles 1
shrivels because .
● It gains water due to osmosis
● It loses water due to reverse osmosis
● It gains water due to reverse osmosis
● It loses water due to osmosis

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Q.7 Among the following amines,the one that will exhibit acidic nature on reaction 1
with Hinsberg’s reagent is—--------------------------
● Dimethyl amine
● Methyl amine
● Diethylamine
● Trimethylamine
Q.8 The non-reducing sugar among the following is………………. 1
● Lactose
● Maltose
● Glucose
● Sucrose
Q.9 Draw a neat labeled diagram showing the zone refining process. 1

Q.10 Why does the boiling point of alcohols decrease with increase in branching? 1

Q.11 Draw the structure of Ethylenediaminetetraacetate ion. 1

Q.12 Write the mathematical expression for Freundlich adsorption isotherm. 1

Q.13 What are the products of electrolysis of molten Sodium chloride? 1

Q,14 Name the type of polythene used in manufacturing buckets and flexible pipes. 2
Also write the names of monomers used in the preparation of Buna-N.
Q.15 Write the formulas of hydrides of Group 16 elements and arrange them in 2
decreasing order of their stability.
Q.16 Mention the action of Aspirin and Chloramphenicol on the human body in 2
bringing relief from a disease.
Q.17 Draw a neat diagram of the Dry Cell and label the composition of anode, 2
cathode and electrolyte used in it.
Q.18 The rate constant for first order reaction is 4 x 10-2 min-1 . The initial 2
concentration of the reactant is 0.12 mol/L. Calculate the time required by the
reactant to attain the concentration of 0.03 mol/L. ( Given : log 4 = 0.6021)
Q.19 Write chemical equations for the Clemmensen reduction of Acetophenone and 2
Hell Volhard Zelinsky reaction of Ethanoic acid.
Q.20 What is Actinoid contraction? Why is it greater from element to element than 2
lanthanoid contraction?
Q.21 Identify the structures and names of Compounds X and Y in the following 2
Sequence.

Benzene diazonium salt +KI → Compound X which on → Compound Y
treatment with Na /ether

Q.22 Two metals E1 and E2 have their standard Reduction Potentials as – 0.25 V and 2

– 2.36 V respectively .Which of the metal will spontaneously liberate bubbles of
Hydrogen gas when placed in dil. Sulphuric acid ? Also calculate the emf of the
cell in case the two metals were used as electrodes to build an Electrochemical
cell.

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OR

Q.22 Rusting of underground iron pipe lines can be prevented by joining it with a 2
piece of a suitable metal.Select the most suitable metal from the following for
this purpose.
Aluminium, Copper, Silver.
Also calculate the emf obtained in case Iron and Aluminium are used as
electrodes in an Electrochemical cell..
(Given : Standard Reduction potentials of Fe, Al and Cu are –0.44 V, –1.66 V
& 0.34 V respectively )
Q.23 Name the element of the 3d transition series that exhibits the largest number of 2
oxidation states and why?
Q.24 Compound P with molecular formula C4 H9 Br is treated with aq. KOH 2
solution.
The rate of this reaction depends on the concentration of Compound P
only.When another optically active isomer Q of this compound was treated
with
aq. KOH the rate of reaction was found to be dependent on concentration of
both Compound Q and KOH .
Identify the Compounds P and Q. Out of the two compounds which one will be
converted to a product with total inversion in configuration?
Q.25 Derive the Integrated rate equation for the Zero Order Reaction. 2

Q.26 During the visit to the Iron and Copper industry following observations were 3
made.
● Iron obtained from blast furnace was cast into a variety of shapes.
● Copper was produced in the form of copper matte.
Name the type of iron obtained from the blast furnace and also write the % of
carbon present in it.
Write the formulae of the two types of metal sulphides present in copper matte
and name the gas evolved and the type of copper formed during the extraction
of copper.
Q.27 Draw a neat labeled diagram of Bredig’s arc method used for the preparation of 3
sol. Write one point of difference between homogeneous and heterogeneous
catalysis. Why is a lyophilic colloid more stable than lyophobic colloid?
Q.28 The outer orbital complex [ CoF6]3- shows octahedral geometry and has four 3
unpaired electrons in the hybridized state. Comment on its type of hybridisation
and magnetic property. Identify the type of isomerism in [Cr(en) 3]Cl3.Write the
name of the ligand, Coordination number and oxidation number of Chromium
in the complex.

Q.29 What is a peptide linkage? Name the vitamins whose deficiency causes night 3
blindness and rickets. Give one example each of fibrous & Globular proteins.
Q.30 Draw the structure of the fcc unit cell and calculate the total number of atoms 3
per unit cell in it.
Q.31 An organic compound A having molecular formula C3H8O on treatment with 3
chromic anhydride gave compound B. Compound B on treatment with
Methyl magnesium bromide gives compound C ,When compound C is passed
through a copper tube heated at 573K gives 2-Methyl propene. Identify A, B, C
and also write the sequence of reactions involved.

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OR

Q.31 An aromatic hydrocarbon M having molecular formula C6H6on treatment 3
with oleum and gave compound N . Compound N on treatment with Sodium
hydroxide and acid gave compound O. Compound O on treatment with Zn
dust gave compound M. Identify M,N & O and also write the sequence of
reactions involved.
Q.32 Write chemical equations to convert Propanamide to Ethanamine, Benzene 3
diazonium chloride to Orange dye.
Why are aromatic amines weaker bases than ammonia?
Q.33 Show graphically the effect on the boiling point of water when a non-volatile 4
solute is added into it.
18 grams of glucose ( C6H12O6 ) is dissolved in one Kilogram of water in a
saucepan.Calculate the molality and the boiling point of the solution.
(Given : Kb for water = 0.52 K /m , At. Mass of C=12, H=1 , O=16 )

OR

Q.33 Show graphically the type of solution formed ( ideal or nonideal) when ethanol 4
and methanol are mixed together.
The Vapour pressure of pure ethanol and methanol are 44.5mm and 88.7 mm of
Hg respectively. A solution is prepared by mixing 60 gms of ethanol and 40
gms of methanol. Calculate the Vapour Pressure of the solution.

(Given : At. mass of C = 12, H= 1, O=16)
Q.34 Write the general trend of group 15 elements with respect to Atomic/ionic radii 4
and Ionization enthalpy and also write the general trend of group 17 elements
with respect to electronegativity and electron gain enthalpy.

OR

Q.34 Write the formula of oleum and name the gas that is dissolved in sulphuric acid 4

to get the oleum and write the reaction for the same. Also write the formula of
Xenon hexafluoride and write its reaction showing complete hydrolysis.

Q.35 Write the sequence of reactions involved and name the compounds W,X,Y and 4
Z

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OR

Q.35 Write the sequence of reactions involved and name the compounds E,F,G and H 4

ALTO - PORVORIM GOA.

ANSWER KEY TO MODEL QUESTION PAPER OF FINAL EXAMINATION (2023 - 2024)

STD : XII SCIENCE SUBJECT : CHEMISTRY MAXIMUM MARKS : 70
DURATION : 2 ½ hours

Q.1 1mk

23
Correct answer:1.5 × 10

Q.2 1mk

Q.3 ● Propane < 1-chloropropane < 1-bromopropane < 1-iodopropane 1mk

Q.4 Propan-1-ol 1mk

Q.5 Correct answer: d-d transition 1mk

Q.6 ● It loses water due to osmosis. 1mk

Q.7 Methyl amine 1mk

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Q.8 sucrose 1mk

Q.9 1mk

Q.10 Due to increase in branching there is decrease in surface area. 1mk

Q.11 1mk

Q.12 x/m =k.p1/n(n >1) 1mk

Q.13 Sodium metal and Chlorine gas ( ½ mk for each ) 1mk

Q.14 Buckets- high density polythene …..(½ mk ) 2mks
Flexible pipes- low density polythene ……( ½ mk)
Monomers used in preparation of Buna -N are 1,3-Butadiene and
Acrylonitrile ...................... ( ½ mk for each )

Q.15 Hydrides of group 16 elements are H2O, H2S , H2Se , H2Te & H2Po 2 mks
Thermal stability decreases down the group
Hence, we have order of thermal stability as H2O > H2S > H2Se > H2Te > H2Po

Q.16 Aspirin is used as an analgesic as well as antipyretic. It is also used in prevention of 1 mk
heart attack. each
Chloramphenicol is a broad spectrum antibiotic. It is rapidly absorbed from the
gastrointestinal tract and hence can be given orally in case of typhoid, dysentery, acute
fever, certain form of urinary infections, meningitis and pneumonia.(any one)

Q.17 Dry Cell/ Leclanche Cell:

Diagram = ½ mk
Anode = Zinc ( ½ mk) , cathode = Carbon (½ mk) ,
Electrolyte = paste of ammonium chloride and Zinc chloride (½ mk.)

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Q.18
……………………..(½ mk ) 2mks
4x10-2 = 2.303 log 0.12
t 0.03..................................... (½ mk)
t = 2.303 log4
4x10-2
= 2.303 x 0.6021 x 102 = 34.665 min…( 1mk for ans with units)
4

Q.19

1mk

1mk

Q.20 Actinoid contraction refers to the gradual decrease in the ionic radii with 1mk
increase in atomic number of actinoids.It ismore as compared to lanthanoid
contraction because 5f electrons have more poor shielding effect as compared
to 4f electrons. Therefore, the effect of increased nuclear charge leading to
contraction in size is more incase of actinoid elements.
1mk

Q.21 Compound X = Iodobenzene ( naming ½ mk + structure ½ mk) 2 mks
Compound Y = Biphenyl ( naming ½ mk + structure ½ mk)

Q.22 E2 will liberate Hydrogen gas…… ( 1 mk) EMF 2mks
= E(higher reduction ) - E(lesser reduction)
=[ ( – 0.25 V) – ( – 2.36 V)]
= 2.11V ...................( 1mk)

OR

Q.22 Suitable metal for prevention of corrosion = Aluminium (1mk)EMF = 2mks
E(higher reduction ) - E (lesser reduction )
= [– 0.44 V – ( – 1.66 V) ]
= 1.22 V .................(1mk)

Q.23 Manganese (Z = 25) shows maximum number of O.S. This is because itsouter 2mks
EC is 3d 4s . As 3d and 4s are close in energy, it has a maximum number of e s
5 2 -1

to lose or share (participation of both 3d and 4s electrons). Hence, it shows O.S.
from +2 to +7 which is the maximum number.

Q.24 Compound P = 2-bromo-2-methylpropane or tert-butyl bromide 2mks
(either structure or name =½ mk)
Compound Q = 2-bromobutane or sec-butyl bromide
(either structure or name = ½ mk)
Compound Q or 2-bromobutane or sec-butyl bromide will be converted to a product withtotal
inversion in configuration…….1 mk

Q.25
Let [R] be the concentration of the reaction. For zero order reaction the rate
of the reaction is independent of concentration of R. Thus,

(½)

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(½)

(½)

(½)

Q.26 Pig iron (½ mk) 2mks
4% (½mk)
Cu2S and FeS (½ mk each)
Sulphur dioxide gas and blister copper (½mk each)

Q.27

3 mks

Diagram1/2mk any 2 labelings ½ mk

In homogeneous catalysis, the catalyst and reactants are in the same phase, usually a gasor
liquid. In heterogeneous catalysis, the catalyst and reactants are in different phases . 1mk

Lyophilic sols are more stable than lyophobic sols because lyophilic sols are extensively
solvated.They are covered by a sheath of liquid in which they are dispersed.
1mk

Q.28
Hybridisation: sp3d2 …………..½ mk 3mks
Magnetic property: Paramagnetic ....................... ½ mk
Optical isomerism ……………..½ mk
Ethylenediamine/ Ethane-1,2-diamine ................... ½ mk
Coordination no. of Cr : +6 ...................... ½ mk
Oxidation No. of Cr : +3 ....................... ½ mk

Q.29 It is an amide linkage formed between the -COOH group of one amino acid & NH2 groupof 3mks
the other amino acid by loss of water molecule. .......................... 1mk
Deficiency of Vitamin D causes rickets and deficiency of Vitamin A causes night blindness.
…………………….(½ mk + ½ mk)

Examples of Fibrous protein: keratin /myosin (any one) ..................... ½ mk
Examples of Globular protein:Insulin /albumins(any one) ......................½ mk

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Q.30 1+2

Q.31 each
equati
on ½
mark
(½×3=
1½mks)
each
label
½mark.
(½×3=
1½marks)
1½+1½
=
Total
3 Mks

M=Propan-2-ol N= Propanone/Dimethyl ketone/Acetone O=Tert-butyl alcohol

OR

Q.31

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Q.32
1 mk

1mk

1 mk

Aromatic amines are weaker bases than ammonia due to the electronwithdrawing
nature of the aryl group.

Q.33 4
mks

Graph .............. 1mk

Molality = mass of solute / Molar mass of solute x mass of solvent in Kg
( ½ mk)
= 18/180 x 1 = 0.1 m ……( ½ mk)

ᐃTb = Kb x W 2 x 1000/ M2 x W1 ................ (½ mk formula )
= 0.52 x 18 x 1000 / 180 x 1000 .......... ( ½ mk substitution)
= 0.052 K ............... ( ½ mk )
ᐃTb = Tb – Tᐤ b = Tb – 373 K = 0.052
i.e. Tb =373 + 0.052 = 373.052 K or 100.052⁰ C ….( ½ mk )

OR

Q.33

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Graph ……. 1 mk.

Moles of methanol i.e n(methanol) = mass of methanol / Molar mass
= 40 / 32 = 1.25 mole
Moles of ethanol i.e n (ethanol) = mass of ethanol / Molar mass
= 60 / 46 = 1.30 mole

Mole fraction of methanol (ϰ) = n (methanol) / n (methanol) + n(ethanol)
= 1.25 / 1.25 + 1.30 = 0.49 …….( ½ mk)
Mole fraction of ethanol (ϰ) = n(ethanol) / n (methanol) + n (ethanol)
= 1.30 / 1.25 + 1.30 = 0.51 ........... ( ½ mk)

Partial V. P of methanol …P(methanol) = Pᐤ ϰ(methanol) = 88.7 x 0.49
= 43.46 mm …( ½ mk)Partial
V.P of ethanol …P(ethanol) = Pᐤ ϰ(ethanol) = 44.5 x 0.51
= 22.70 mm…( ½ mk)

Total vapour Pressure of solution =P(methanol) + P(ethanol)
= 43.46 + 22.70
= 66.16 mm ……( 1 mk)

Q.34 Covalent and ionic (in a particular state) radii of group 15 increase in size down 1mk
the group. There is a considerable increase in covalent radius from N to P. However, for
from As to Bi only a small increase in covalent radius is observed. each
Ionisation enthalpy decreases down the group due togradual increase in atomic size. trend
Halogens have maximum negative electron gain enthalpy in the corresponding periods
Electron gain enthalpy of the elements of the group 16 becomes less negative down the
group. They have very high electronegativity. The electronegativity decreasesdown the
group.

OR

Q.34 Formula of Oleum: H2S2O7 Form
Gas used:Sulphur trioxide ula ½
mk &
eqn
1mk
Equation: 1/2
Formula of Xenon hexafluoride: XeF6 mk
each
Complete hydrolysis reaction:

Q.35

½ mk

W- Benzene X-Benzaldehyde
1mk

Y- Benzyl alcohol Z- Sodium benzoate

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½ mk

W- Benzene X-Benzaldehyde
Y- Benzyl alcohol Z- Sodium benzoate ½ mk each

OR

Q.35

½ mk

E= Propanoic acid F=Propan-1-ol
½ mk

G= Propanal

½ mk

H-3-Hydroxy -2-methylpentanal

½ mk

+ H2O

½
E-Propanoic acid/Propionic acid
mk
F- Propan-1-ol/n-propyl alcohol each
G- Propanal /Propionaldehyde
H-3-Hydroxy -2-methylpentanal

Note: Teachers kindly set the papers as per the pattern of questions given in the Model paper of XII for all the examinations
of both XI and XII so that students get some idea about the Board paper pattern.

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