ICSE Class 10 Chemistry Sample Paper 2025 - 4 | Chemistry Class 10 ICSE PDF Download

 Page 1


Time Allowed: 2 hours Maximum Marks: 80 
General Instructions:
Answers to this Paper must be written on the paper provided separately.
You will not be allowed to write during the first 15 minutes.
This time is to be spent reading the question paper.
The time given at the head of this Paper is the time allowed for writing the answers.
Section A is compulsory. Attempt any four questions from Section B.
The intended marks for questions or parts of questions are given in brackets [ ].
Section A
1. Question 1 Choose one correct answer to the questions from the given options: [15]
a) Beryllium b) Potassium
c) Sodium d) Magnesium
Amongst the following, select the element with highest ionisation enthalpy. [1] (a)
a) Neon b) Argon
c) Sulphur d) Sodium
An element in period-3 whose electron affinity is zero ________. [1] (b)
a) electrovalent b) ionic
c) molecular d) covalent
Compound X consists of molecules. The type of bonding in X will be [1] (c)
a) Hg b) Al
c) Cu d) Ag
Which of the following metals can displace hydrogen from the aqueous solution of NaOH? [1] (d)
a) Copper (II) oxide b) Zinc oxide
c) Barium oxide d) Calcium oxide
Identify the metallic oxide which is amphoteric in nature: [1] (e)
a) Silver oxide b) Calcium oxide
c) Copper(II) oxide d) Aluminium oxide
The metal oxide which can react with acid as well as alkali is: [1] (f)
The empirical formula of the compound is CH. Its molecular weight is 78. The molecular formula of [1] (g)
 Chemistry
Page 2


Time Allowed: 2 hours Maximum Marks: 80 
General Instructions:
Answers to this Paper must be written on the paper provided separately.
You will not be allowed to write during the first 15 minutes.
This time is to be spent reading the question paper.
The time given at the head of this Paper is the time allowed for writing the answers.
Section A is compulsory. Attempt any four questions from Section B.
The intended marks for questions or parts of questions are given in brackets [ ].
Section A
1. Question 1 Choose one correct answer to the questions from the given options: [15]
a) Beryllium b) Potassium
c) Sodium d) Magnesium
Amongst the following, select the element with highest ionisation enthalpy. [1] (a)
a) Neon b) Argon
c) Sulphur d) Sodium
An element in period-3 whose electron affinity is zero ________. [1] (b)
a) electrovalent b) ionic
c) molecular d) covalent
Compound X consists of molecules. The type of bonding in X will be [1] (c)
a) Hg b) Al
c) Cu d) Ag
Which of the following metals can displace hydrogen from the aqueous solution of NaOH? [1] (d)
a) Copper (II) oxide b) Zinc oxide
c) Barium oxide d) Calcium oxide
Identify the metallic oxide which is amphoteric in nature: [1] (e)
a) Silver oxide b) Calcium oxide
c) Copper(II) oxide d) Aluminium oxide
The metal oxide which can react with acid as well as alkali is: [1] (f)
The empirical formula of the compound is CH. Its molecular weight is 78. The molecular formula of [1] (g)
 Chemistry
a) C
4
H
4
b) C
3
H
3
c) C
2
H
2
d) C
6
H
6
the compound will be:
a) 40 b) 36
c) 48 d) 30
Percentage of calcium in calcium carbonate (CaCO
3
) is [1] (h)
a) Two moles of aluminium ions b) Three moles of oxide ions
c) Five moles of hydroxide ions d) Six moles of hydrogen ions
Which of the following requires the least number of electrons for discharge to take place? [1] (i)
a) adsorption b) coagulation
c) sedimentation d) absorption
Froth floatation process for the concentration of ores is an illustration of the practical application of [1] (j)
a) aqua-regia b) aqua fortis
c) oil of vitriol d) muriatic acid
The name of aqueous solution of HCl is [1] (k)
a) Hydrogen chloride gas b) Sulphuric acid
c) Chlorine d) Ammonia
Name the gas produced when ammonium sulphate is heated with sodium hydroxide solution. [1] (l)
a) CH
3
OH b) C
3
H
7
OH
c) C
4
H
9
OH d) C
2
H
5
OH
The molecular formula of propyl alcohol is [1] (m)
a) Isoheptane b) Isohexane
c) Isopentane d) Neopentane
Which of the following will give only one monochloro derivative on halogenation? [1] (n)
a) CH
3
CH
2
CH
2
COOH b)
c) (CH
3
)
2
CH-COOH d) CH
3
(CH
2
)
3
COOH
Which of the following is iso-butyric acid? [1] (o)
- C H 3 C | H C H 2 C O O H C H 3 2. Question 2 [25]
Ammonia is manufactured by Haber's process.
i. Under what conditions do the reactants combine to form ammonia? Give a balanced equation for
the reaction.
ii. In what ratio by volume, are the above gases used?
iii. What is the function of:
a. Finely divided iron,
[5] (a)
Page 3


Time Allowed: 2 hours Maximum Marks: 80 
General Instructions:
Answers to this Paper must be written on the paper provided separately.
You will not be allowed to write during the first 15 minutes.
This time is to be spent reading the question paper.
The time given at the head of this Paper is the time allowed for writing the answers.
Section A is compulsory. Attempt any four questions from Section B.
The intended marks for questions or parts of questions are given in brackets [ ].
Section A
1. Question 1 Choose one correct answer to the questions from the given options: [15]
a) Beryllium b) Potassium
c) Sodium d) Magnesium
Amongst the following, select the element with highest ionisation enthalpy. [1] (a)
a) Neon b) Argon
c) Sulphur d) Sodium
An element in period-3 whose electron affinity is zero ________. [1] (b)
a) electrovalent b) ionic
c) molecular d) covalent
Compound X consists of molecules. The type of bonding in X will be [1] (c)
a) Hg b) Al
c) Cu d) Ag
Which of the following metals can displace hydrogen from the aqueous solution of NaOH? [1] (d)
a) Copper (II) oxide b) Zinc oxide
c) Barium oxide d) Calcium oxide
Identify the metallic oxide which is amphoteric in nature: [1] (e)
a) Silver oxide b) Calcium oxide
c) Copper(II) oxide d) Aluminium oxide
The metal oxide which can react with acid as well as alkali is: [1] (f)
The empirical formula of the compound is CH. Its molecular weight is 78. The molecular formula of [1] (g)
 Chemistry
a) C
4
H
4
b) C
3
H
3
c) C
2
H
2
d) C
6
H
6
the compound will be:
a) 40 b) 36
c) 48 d) 30
Percentage of calcium in calcium carbonate (CaCO
3
) is [1] (h)
a) Two moles of aluminium ions b) Three moles of oxide ions
c) Five moles of hydroxide ions d) Six moles of hydrogen ions
Which of the following requires the least number of electrons for discharge to take place? [1] (i)
a) adsorption b) coagulation
c) sedimentation d) absorption
Froth floatation process for the concentration of ores is an illustration of the practical application of [1] (j)
a) aqua-regia b) aqua fortis
c) oil of vitriol d) muriatic acid
The name of aqueous solution of HCl is [1] (k)
a) Hydrogen chloride gas b) Sulphuric acid
c) Chlorine d) Ammonia
Name the gas produced when ammonium sulphate is heated with sodium hydroxide solution. [1] (l)
a) CH
3
OH b) C
3
H
7
OH
c) C
4
H
9
OH d) C
2
H
5
OH
The molecular formula of propyl alcohol is [1] (m)
a) Isoheptane b) Isohexane
c) Isopentane d) Neopentane
Which of the following will give only one monochloro derivative on halogenation? [1] (n)
a) CH
3
CH
2
CH
2
COOH b)
c) (CH
3
)
2
CH-COOH d) CH
3
(CH
2
)
3
COOH
Which of the following is iso-butyric acid? [1] (o)
- C H 3 C | H C H 2 C O O H C H 3 2. Question 2 [25]
Ammonia is manufactured by Haber's process.
i. Under what conditions do the reactants combine to form ammonia? Give a balanced equation for
the reaction.
ii. In what ratio by volume, are the above gases used?
iii. What is the function of:
a. Finely divided iron,
[5] (a)
Section B
Attempt any 4 questions
b. Molybdenum in the above process?
iv. Mention two possible ways by which ammonia produced is removed from unchanged gases.
Match the following:
Column A Column B
(a) Acid salt (i) Sodium potassium carbonate
(b) Mixed salt (ii) Alum
(c) Complex salt (iii) Sodium hydrogen carbonate
(d) Double salt (iv) Sodium zincate
[5] (b)
Complete the following by choosing the correct answers from the bracket:
i. In Period 3, the most metallic element is ________. (sodium/magnesium/aluminium) [1]
ii. The hydroxides which can act as weak bases as well as weak acids are ________ (neutral,
acidic, amphoteric) in nature.
[1]
iii. ________ is defined as the amount of substance which contains same number of units as the
number of atoms in 12 g of carbon-12.
[1]
iv. We can expect that pure water ________ normally conduct electricity. [1]
v. Hot, concentrated nitric acid reacts with sulphur to form ________. (sulphur dioxide/sulphuric
acid)
[1]
(c)
Identify the following:
i. The covalent compounds of carbon and hydrogen. [1]
ii. The gas evolved when hydrochloric acid is added to manganese(IV) oxide. [1]
iii. The particle that move when electric current is passed through metal wire. [1]
iv. Ice like crystals formed on cooling an organic acid sufficiently. [1]
v. ________ have maximum electron affinity in their respective periods. (halogens/inert gases) [1]
(d)
i. A gaseous hydrocarbon contains 82.76% of carbon. Given that its vapour density is 29, find its
molecular formula. [C = 12, H = 1].
[2]
ii. Draw the electron dot structure of:
i. Nitrogen molecule [N = 7]
ii. Sodium chloride [Na = 11, Cl = 17]
iii. Ammonium ion [N = 7, H = 1]
[3]
(e)
3. Question 3 [10]
Sulphur trioxide  Sulphuric acid 
In manufacturing of sulphuric acid by contact process. Sulphur trioxide is not converted to sulphuric
acid by reacting it with water. Instead a two step procedure is used. Write the equations for the two
steps involved in A. 
[2] (a)
? A Write the products and balance the equation.
i. Lead sulphate from lead carbonate. [1]
ii. Copper carbonate. [1]
(b)
Page 4


Time Allowed: 2 hours Maximum Marks: 80 
General Instructions:
Answers to this Paper must be written on the paper provided separately.
You will not be allowed to write during the first 15 minutes.
This time is to be spent reading the question paper.
The time given at the head of this Paper is the time allowed for writing the answers.
Section A is compulsory. Attempt any four questions from Section B.
The intended marks for questions or parts of questions are given in brackets [ ].
Section A
1. Question 1 Choose one correct answer to the questions from the given options: [15]
a) Beryllium b) Potassium
c) Sodium d) Magnesium
Amongst the following, select the element with highest ionisation enthalpy. [1] (a)
a) Neon b) Argon
c) Sulphur d) Sodium
An element in period-3 whose electron affinity is zero ________. [1] (b)
a) electrovalent b) ionic
c) molecular d) covalent
Compound X consists of molecules. The type of bonding in X will be [1] (c)
a) Hg b) Al
c) Cu d) Ag
Which of the following metals can displace hydrogen from the aqueous solution of NaOH? [1] (d)
a) Copper (II) oxide b) Zinc oxide
c) Barium oxide d) Calcium oxide
Identify the metallic oxide which is amphoteric in nature: [1] (e)
a) Silver oxide b) Calcium oxide
c) Copper(II) oxide d) Aluminium oxide
The metal oxide which can react with acid as well as alkali is: [1] (f)
The empirical formula of the compound is CH. Its molecular weight is 78. The molecular formula of [1] (g)
 Chemistry
a) C
4
H
4
b) C
3
H
3
c) C
2
H
2
d) C
6
H
6
the compound will be:
a) 40 b) 36
c) 48 d) 30
Percentage of calcium in calcium carbonate (CaCO
3
) is [1] (h)
a) Two moles of aluminium ions b) Three moles of oxide ions
c) Five moles of hydroxide ions d) Six moles of hydrogen ions
Which of the following requires the least number of electrons for discharge to take place? [1] (i)
a) adsorption b) coagulation
c) sedimentation d) absorption
Froth floatation process for the concentration of ores is an illustration of the practical application of [1] (j)
a) aqua-regia b) aqua fortis
c) oil of vitriol d) muriatic acid
The name of aqueous solution of HCl is [1] (k)
a) Hydrogen chloride gas b) Sulphuric acid
c) Chlorine d) Ammonia
Name the gas produced when ammonium sulphate is heated with sodium hydroxide solution. [1] (l)
a) CH
3
OH b) C
3
H
7
OH
c) C
4
H
9
OH d) C
2
H
5
OH
The molecular formula of propyl alcohol is [1] (m)
a) Isoheptane b) Isohexane
c) Isopentane d) Neopentane
Which of the following will give only one monochloro derivative on halogenation? [1] (n)
a) CH
3
CH
2
CH
2
COOH b)
c) (CH
3
)
2
CH-COOH d) CH
3
(CH
2
)
3
COOH
Which of the following is iso-butyric acid? [1] (o)
- C H 3 C | H C H 2 C O O H C H 3 2. Question 2 [25]
Ammonia is manufactured by Haber's process.
i. Under what conditions do the reactants combine to form ammonia? Give a balanced equation for
the reaction.
ii. In what ratio by volume, are the above gases used?
iii. What is the function of:
a. Finely divided iron,
[5] (a)
Section B
Attempt any 4 questions
b. Molybdenum in the above process?
iv. Mention two possible ways by which ammonia produced is removed from unchanged gases.
Match the following:
Column A Column B
(a) Acid salt (i) Sodium potassium carbonate
(b) Mixed salt (ii) Alum
(c) Complex salt (iii) Sodium hydrogen carbonate
(d) Double salt (iv) Sodium zincate
[5] (b)
Complete the following by choosing the correct answers from the bracket:
i. In Period 3, the most metallic element is ________. (sodium/magnesium/aluminium) [1]
ii. The hydroxides which can act as weak bases as well as weak acids are ________ (neutral,
acidic, amphoteric) in nature.
[1]
iii. ________ is defined as the amount of substance which contains same number of units as the
number of atoms in 12 g of carbon-12.
[1]
iv. We can expect that pure water ________ normally conduct electricity. [1]
v. Hot, concentrated nitric acid reacts with sulphur to form ________. (sulphur dioxide/sulphuric
acid)
[1]
(c)
Identify the following:
i. The covalent compounds of carbon and hydrogen. [1]
ii. The gas evolved when hydrochloric acid is added to manganese(IV) oxide. [1]
iii. The particle that move when electric current is passed through metal wire. [1]
iv. Ice like crystals formed on cooling an organic acid sufficiently. [1]
v. ________ have maximum electron affinity in their respective periods. (halogens/inert gases) [1]
(d)
i. A gaseous hydrocarbon contains 82.76% of carbon. Given that its vapour density is 29, find its
molecular formula. [C = 12, H = 1].
[2]
ii. Draw the electron dot structure of:
i. Nitrogen molecule [N = 7]
ii. Sodium chloride [Na = 11, Cl = 17]
iii. Ammonium ion [N = 7, H = 1]
[3]
(e)
3. Question 3 [10]
Sulphur trioxide  Sulphuric acid 
In manufacturing of sulphuric acid by contact process. Sulphur trioxide is not converted to sulphuric
acid by reacting it with water. Instead a two step procedure is used. Write the equations for the two
steps involved in A. 
[2] (a)
? A Write the products and balance the equation.
i. Lead sulphate from lead carbonate. [1]
ii. Copper carbonate. [1]
(b)
Arrange the following as per the instruction given in the brackets:
i. Cs, Na, Li, K, Rb (increasing order of metallic character) [1]
ii. Li, F, N [increasing order of electronegativity] [1]
iii. He, Ar, Ne (Increasing order of the number of shells) [1]
(c)
Fill in the blanks by selecting the appropriate word from the given choice:
i. One carbon atom in a hydrocarbon contain the root word as ________. [1]
ii. -COOH group represents an ________. [1]
iii. 1 mole = ________ L at STP if substance is a gas. [1]
(d)
4. Question 4 [10]
What are the terms defined in (i) and (ii) below?
i. A bond formed by a shared pair of electrons, each bonding atom contributing one electron to the
pair.
ii. A bond formed by a shared paired of electrons with both electrons coming from the same atom.
[2] (a)
If 112 cm
3
 of hydrogen sulphide is mixed with 120 cm
3
 of chlorine at STP what mass of sulphur is
formed? 
H
2
S + Cl
2
  2HCl + S
[2] (b)
? For each of the substance listed below, describe the role played in the extraction of aluminium:
i. Cryolite
ii. Sodium hydroxide
iii. Graphite
[3] (c)
Explain the following:
i. Aluminium is more abundant than gold in the earth's crust, yet it is gold and not aluminium
that has been known to man since ancient times.
[1]
ii. Farmers spread slaked lime on the fields. [1]
iii. Direct current should be used during electroplating. [1]
(d)
5. Question 5 [10]
i. Gas used as illuminating country houses. Identify the gas. [1]
ii. Complete the chemical equation: 
[1]
(a)
O H + C O O H C 2 H 5 C H 3 Conc. H
2 S O 4 ? Compare the compounds carbon tetrachloride and sodium chloride with regard to solubility in water
and electrical conductivity.
[2] (b)
Give balanced chemical equation for the following:
i. Action of concentrated sulphuric acid on carbon [1]
ii. Action of dilute sulphuric acid on sodium hydroxide [1]
iii. Lead nitrate is heated in a dry test tube [1]
(c)
State one relevant observation for each of the following reactions:
i. Barium chloride solution is slowly added to sodium sulphate solution. [1]
ii. Sodium hydroxide solution is added to ferric chloride solution at first a little and then in
excess.
[1]
iii. In the electrolyte during the electrolysis of copper sulphate solutions with inert electrodes. [1]
(d)
6. Question 6 [10]
Page 5


Time Allowed: 2 hours Maximum Marks: 80 
General Instructions:
Answers to this Paper must be written on the paper provided separately.
You will not be allowed to write during the first 15 minutes.
This time is to be spent reading the question paper.
The time given at the head of this Paper is the time allowed for writing the answers.
Section A is compulsory. Attempt any four questions from Section B.
The intended marks for questions or parts of questions are given in brackets [ ].
Section A
1. Question 1 Choose one correct answer to the questions from the given options: [15]
a) Beryllium b) Potassium
c) Sodium d) Magnesium
Amongst the following, select the element with highest ionisation enthalpy. [1] (a)
a) Neon b) Argon
c) Sulphur d) Sodium
An element in period-3 whose electron affinity is zero ________. [1] (b)
a) electrovalent b) ionic
c) molecular d) covalent
Compound X consists of molecules. The type of bonding in X will be [1] (c)
a) Hg b) Al
c) Cu d) Ag
Which of the following metals can displace hydrogen from the aqueous solution of NaOH? [1] (d)
a) Copper (II) oxide b) Zinc oxide
c) Barium oxide d) Calcium oxide
Identify the metallic oxide which is amphoteric in nature: [1] (e)
a) Silver oxide b) Calcium oxide
c) Copper(II) oxide d) Aluminium oxide
The metal oxide which can react with acid as well as alkali is: [1] (f)
The empirical formula of the compound is CH. Its molecular weight is 78. The molecular formula of [1] (g)
 Chemistry
a) C
4
H
4
b) C
3
H
3
c) C
2
H
2
d) C
6
H
6
the compound will be:
a) 40 b) 36
c) 48 d) 30
Percentage of calcium in calcium carbonate (CaCO
3
) is [1] (h)
a) Two moles of aluminium ions b) Three moles of oxide ions
c) Five moles of hydroxide ions d) Six moles of hydrogen ions
Which of the following requires the least number of electrons for discharge to take place? [1] (i)
a) adsorption b) coagulation
c) sedimentation d) absorption
Froth floatation process for the concentration of ores is an illustration of the practical application of [1] (j)
a) aqua-regia b) aqua fortis
c) oil of vitriol d) muriatic acid
The name of aqueous solution of HCl is [1] (k)
a) Hydrogen chloride gas b) Sulphuric acid
c) Chlorine d) Ammonia
Name the gas produced when ammonium sulphate is heated with sodium hydroxide solution. [1] (l)
a) CH
3
OH b) C
3
H
7
OH
c) C
4
H
9
OH d) C
2
H
5
OH
The molecular formula of propyl alcohol is [1] (m)
a) Isoheptane b) Isohexane
c) Isopentane d) Neopentane
Which of the following will give only one monochloro derivative on halogenation? [1] (n)
a) CH
3
CH
2
CH
2
COOH b)
c) (CH
3
)
2
CH-COOH d) CH
3
(CH
2
)
3
COOH
Which of the following is iso-butyric acid? [1] (o)
- C H 3 C | H C H 2 C O O H C H 3 2. Question 2 [25]
Ammonia is manufactured by Haber's process.
i. Under what conditions do the reactants combine to form ammonia? Give a balanced equation for
the reaction.
ii. In what ratio by volume, are the above gases used?
iii. What is the function of:
a. Finely divided iron,
[5] (a)
Section B
Attempt any 4 questions
b. Molybdenum in the above process?
iv. Mention two possible ways by which ammonia produced is removed from unchanged gases.
Match the following:
Column A Column B
(a) Acid salt (i) Sodium potassium carbonate
(b) Mixed salt (ii) Alum
(c) Complex salt (iii) Sodium hydrogen carbonate
(d) Double salt (iv) Sodium zincate
[5] (b)
Complete the following by choosing the correct answers from the bracket:
i. In Period 3, the most metallic element is ________. (sodium/magnesium/aluminium) [1]
ii. The hydroxides which can act as weak bases as well as weak acids are ________ (neutral,
acidic, amphoteric) in nature.
[1]
iii. ________ is defined as the amount of substance which contains same number of units as the
number of atoms in 12 g of carbon-12.
[1]
iv. We can expect that pure water ________ normally conduct electricity. [1]
v. Hot, concentrated nitric acid reacts with sulphur to form ________. (sulphur dioxide/sulphuric
acid)
[1]
(c)
Identify the following:
i. The covalent compounds of carbon and hydrogen. [1]
ii. The gas evolved when hydrochloric acid is added to manganese(IV) oxide. [1]
iii. The particle that move when electric current is passed through metal wire. [1]
iv. Ice like crystals formed on cooling an organic acid sufficiently. [1]
v. ________ have maximum electron affinity in their respective periods. (halogens/inert gases) [1]
(d)
i. A gaseous hydrocarbon contains 82.76% of carbon. Given that its vapour density is 29, find its
molecular formula. [C = 12, H = 1].
[2]
ii. Draw the electron dot structure of:
i. Nitrogen molecule [N = 7]
ii. Sodium chloride [Na = 11, Cl = 17]
iii. Ammonium ion [N = 7, H = 1]
[3]
(e)
3. Question 3 [10]
Sulphur trioxide  Sulphuric acid 
In manufacturing of sulphuric acid by contact process. Sulphur trioxide is not converted to sulphuric
acid by reacting it with water. Instead a two step procedure is used. Write the equations for the two
steps involved in A. 
[2] (a)
? A Write the products and balance the equation.
i. Lead sulphate from lead carbonate. [1]
ii. Copper carbonate. [1]
(b)
Arrange the following as per the instruction given in the brackets:
i. Cs, Na, Li, K, Rb (increasing order of metallic character) [1]
ii. Li, F, N [increasing order of electronegativity] [1]
iii. He, Ar, Ne (Increasing order of the number of shells) [1]
(c)
Fill in the blanks by selecting the appropriate word from the given choice:
i. One carbon atom in a hydrocarbon contain the root word as ________. [1]
ii. -COOH group represents an ________. [1]
iii. 1 mole = ________ L at STP if substance is a gas. [1]
(d)
4. Question 4 [10]
What are the terms defined in (i) and (ii) below?
i. A bond formed by a shared pair of electrons, each bonding atom contributing one electron to the
pair.
ii. A bond formed by a shared paired of electrons with both electrons coming from the same atom.
[2] (a)
If 112 cm
3
 of hydrogen sulphide is mixed with 120 cm
3
 of chlorine at STP what mass of sulphur is
formed? 
H
2
S + Cl
2
  2HCl + S
[2] (b)
? For each of the substance listed below, describe the role played in the extraction of aluminium:
i. Cryolite
ii. Sodium hydroxide
iii. Graphite
[3] (c)
Explain the following:
i. Aluminium is more abundant than gold in the earth's crust, yet it is gold and not aluminium
that has been known to man since ancient times.
[1]
ii. Farmers spread slaked lime on the fields. [1]
iii. Direct current should be used during electroplating. [1]
(d)
5. Question 5 [10]
i. Gas used as illuminating country houses. Identify the gas. [1]
ii. Complete the chemical equation: 
[1]
(a)
O H + C O O H C 2 H 5 C H 3 Conc. H
2 S O 4 ? Compare the compounds carbon tetrachloride and sodium chloride with regard to solubility in water
and electrical conductivity.
[2] (b)
Give balanced chemical equation for the following:
i. Action of concentrated sulphuric acid on carbon [1]
ii. Action of dilute sulphuric acid on sodium hydroxide [1]
iii. Lead nitrate is heated in a dry test tube [1]
(c)
State one relevant observation for each of the following reactions:
i. Barium chloride solution is slowly added to sodium sulphate solution. [1]
ii. Sodium hydroxide solution is added to ferric chloride solution at first a little and then in
excess.
[1]
iii. In the electrolyte during the electrolysis of copper sulphate solutions with inert electrodes. [1]
(d)
6. Question 6 [10]
An element has atomic number 11. Where would you expect this element in the periodic table and
why?
[2] (a)
a. What do you understand by Avogadro’s number?
b. Write the symbol which is used to denote it.
[2] (b)
Which of the following represents the correct IUPAC name for the compounds concerned?
i. 2,2-dimethylpentane or 2-dimethylpentane
ii. 2,4,7-trimethyloctane or 2,5,7-trimethyl octane
iii. 2-chloro-4-methylpentane or 4-chloro-2-methylpentane
[3] (c)
Distinguish between the following pairs of compounds using a reagent as a chemical test:
i. Calcium nitrate and Zinc nitrate solution.
ii. Ammonium sulphate crystals and Sodium sulphate crystals.
iii. Magnesium chloride and Magnesium nitrate solution.
[3] (d)
7. Question 7 [10]
How many covalent bonds and coordinate bonds are present in
i. Hydronium ion
ii. Ammonium ion
[2] (a)
A gas cylinder contains 12  10
24
 molecules of oxygen gas. If Avogadro's number is 6  10
23
;
molecules. Calculate.
i. The mass of oxygen present in the cylinder.
ii. The volume of oxygen at STP present in the cylinder.
[2] (b)
× × With reference, to the electrolysis of acidulated water, answer the following:
i. Explain why distilled water is a non-electrolyte.
ii. What is the electrolytic cell called?
iii. State what you would observe at the:
a. Anode
b. Cathode
[3] (c)
Draw the structural formula for each of the following:
i. 2, 3 - dimethyl butane
ii. diethyl ether
iii. propanoic acid
[3] (d)
8. Question 8 [10]
Draw an electron dot diagram to show the formation of each of the following compounds:
i. Methane
ii. Magnesium chloride 
[H = 1, C = 6, Mg = 12, Cl = 17]
[2] (a)
The vapour density of a gas is 8. What would be the volume occupied by 24.0 g of the gas at STP? [2] (b)
Write balanced chemical equations, for the preparation of the given salts (i) to (iii) by using the
methods A to C respectively: 
A. Neutralization, B. Precipitation, C. Titration
i. Copper sulphate
[3] (c)