Students can refer to the following Sample Paper ICSE Class 10 Chemistry Set A with Answers provided below based on the latest syllabus and examination guidelines issued for ICSE Chemistry. All specimen papers have been prepared covering all chapters given in ICSE Chemistry book for Class 10. You should also refer to ICSE Class 10 Chemistry Solutions.
Sample Paper ICSE Class 10 Chemistry Set A with Answers
Class : X
Marks : 80
Sub: Chemistry Time : 2 Hrs.
Sample Paper ICSE Class 10 Chemistry Set A
Section – A (40 Marks)
Q 1. (a). Choose the correct answer from the options given below. (5)
(i). The element with highest ionization potential is:
A. Hydrogen
B. Caesium
C. Radon
D. Helium
(ii). The inert electrode used in the electrolysis of acidified water is:
A. Nickel
B. Platinum
C. Copper
D. Silver
(iii). A compound with low boiling point is:
A. Sodium Chloride
B. Calcium Chloride
C. Potassium Chloride
D. Carbon tetrachloride
(iv). The acid which can produce carbon from cane sugar is:
A. Conc H2SO4
B. Conc HNO3
C. Conc HCl
D. Conc CH3COOH
(v). The dehydrating nature can be exhibited by conc. H2SO4 in its reaction with:
A. Sulphur
B. NaNO3
C. NaCl
D. Hydrated Copper Sulphide
(b). State one relevant observation for each of the following reactions: (5)
(i). Action of concentrated HNo3 on copper.
(ii).Action of excess NH4OH into CuSO4 solution.
(iii). Zinc nitrate solution is treated with NaOH solution drop wise till in excess.
(iv). Blue litmus solution is added to NaHso4 solution.
(v). At the anode during the electrolysis of acidified water using platinum electrodes.
(c). Write a balanced chemical equation for each of the following: (5)
(i). Reaction of carbon powder and Conc HNO3
(ii). Reaction of excess NH3 with chlorine.
(iii). Reaction of lead nitrated solution with NH4OH
(iv). Reaction of Zinc with potassium Hydroxide solution.
(d). State one relevant reason for each of the following: (5).
(i). Graphite anode is preferred to platinum in the electrolysis of molten lead bromide.
(ii). Inert gases do not form ions.
(iii). Ionisation potential increases across a period, from left to right.
(iv). Concentrate HNO3 appears yellow when it is left for a while in a glass bottle.
(v). Alkali metals are good reducing agents.
(e). Give one word or a phrase for the following statements. (5).
(i). The chemical bond formed by a shared pair of electrons each bonding atom contributing one electron to a pair.
(ii). Electrode used as cathode in electrorefining of impure copper.
(iii). The tendency of an atom to attract electrons to itself when combined in a compound.
(iv). Electrolytic reduction of pure alumina to aluminium.
(v). The energy released when an electron is added to a neutral gaseous isolated atom to form anion.
(f). Fill in the blanks from the choices given in brackets : (5).
(i). The polar covalent compound in gaseous state that does not conduct electricity is _ (Carbon tetrachloride, ammonia, Methane)
(ii). An alkali which completely dissociates into ions is ___ (ammonium Hydroxide, Calcium Hydoxide, Lithium Hydoxide)
(iii). Reddish brown precipitate is formed when NH4OH reacts with (FeCl3 , FeSO4 , CuSO4)
(iv). Ionic or electrovalent compounds do not conduct electricity in their _ state. (fused/ solution/ solid)
(v). Ammonium salt which is not used in the preparation of NH3 gas is __ (NH4Cl, NH4NO3, NH4So4)
(g). Answer the following: (5)
a) (i). The process of conversion of chloride ion to chlorine atom.
(ii). Define Periodicity.
b). (i). What do you understand by lone pair of electrons?
(ii). Draw the electron dot diagram of Hydronium ion: (H = 1 ; O = 8).
c). (i). Three solutions P, Q, R and S have pH value of 3.5, 5.2, 7 and 12.2 respectively. (3)
Which one of these is a:
A). Weak acid
B). Strong alkali
C). Neutral.
(ii). What is the type of salt formed when the reactants are heated at a suitable temperature for the preparation of Nitric acid? (1).
(iii). State why for the preparation of Nitric acid the complete apparatus is made up of glass. (1)
Sample Paper ICSE Class 10 Chemistry Set A
Section – B (40 Marks)
Attempt any four questions from this section.
Q. 2. (a). The following table represent the elements and the atomic number. With reference to this, answer the following using only the alphabets given in the table:
Element At. No.
P 13
Q 7
R 10
(i). Which element combines with Hydrogen to form a basic gas?
(ii). Which element has an electron affinity zero?
(iii). Name the element which forms an ionic compound with Chlorine.
(b). Draw the electron dot diagram for the compounds given below. Represent the electrons by (.) and (x) in the diagrams. (3)
(i). Calcium Oxide
(ii). Chlorine molecule
(iii). Water molecule
(c). Choose the correct word which refers to the process of electrolysis from A to E. to match the description (i) to (iv). A. Oxidation B. Cathode C. Anode D. An electrolyte E. Reduction (4)
(i). Conducts electricity in aquaeous or in molten state.
(ii). Loss of electron takes place at anode.
(iii). A reducing electrode
(iv). Electrode connected to the positive end or terminal of the battery.
Q3. (a). Baeyer’s process is used to concentrate bauxite Ore to alumina. Give balanced chemical equation for the reaction taking place for its conversion from bauxite to alumina. (3)
(b). Complete the following by selecting the correct option from the choices given: (3)
(i). pH of acetic acid is greater than dilute Sulphuric acid. So acetic contains concentration of H+ ions. (greater, same, low)
(ii). The indicator which does not change colour on passage of HCl gas is ___ (Methyl orange, moist blue litmus, phenolphthalein)
(iii). The acid which cannot act as an oxidizing agent is _ (Conc H2SO4, Conc HNO3, Conc HCl)
(c). Match the gases given in column I to the identification of the gases mentioned in column II. (4)
Q 4. (a). Differentiate between the following pairs based on the information given in the brackets: (3)
(i). Ionic and covalent compounds (solubility)
(ii). Cations and anions (formation from an atom)
(iii). Acid and Alkali ( Formation of type of ions)
(b). Hydrogen Chloride gas is prepared in the laboratory using concentrated H2So4 and Nacl. (4)
Answer the questions that follow based on this reaction.
(i). Give the balanced chemical equation for the reaction with suitable conditions if any.
(ii). Why is concentrated H2So4 used instead of concentrated HNO3?
(iii). How is the gas collected?
(iv). Name the drying agent not used for drying the gas.
(c). Name the following elements. (3)
(i). An alkaline earth metal present in group 2 and period 3.
(ii). A trivalent metal used to make light tools.
(iii). A monovalent non-metal present in fluorspar.
Q 5. (a). Distinguish between the following pairs of compounds using a reagent as a chemical test: (3)
(i). Calcium nitrate and Zinc nitrate solution.
(ii). Carbon dioxide and Sulphur dioxide.
(iii). Hydrochloric acid and Sulphuric acid.
(b). Identify the substance underlined in each of the following: (3)
(i). The electrode that increases in mass during the electrorefining of copper.
(ii). The acid that is a dehydrating as well as a drying agent.
(iii). The catalyst used to oxidize ammonia into nitric oxide.
(c). An aqueous solution of Nickel (II) Sulphate was electrolyzed using nickel electrodes. (4)
(i). What do you observe at the cathode and anode respectively?
(ii). Which ions are present in the solution?
(iii). Write the equation for the reaction at the anode?
Q 6. (a). (i). Define mineral and ore (2)
(ii). Write the equation for the formation of aluminium at the cathode during the electrolysis of alumina. (1)
(b). Name the gases released when: (4)
(i). Pb + Conc NaOH →
(ii). S + Conc H2SO4 →
(iii). Gas released at anode electrolytic Reduction of pure alumina.
(iv). Cu + Cold dil HNO3 →
(c). In the preparation of Ammonia : (3)
(i). Name the drying agent?
(ii). What is the method of collection?
(iii). How do you know that gas jar is full?
Q 7. (a). Answer the following : (3)
(i). Why do metallic character decreases across the period?
(ii). Why do noble gases have larger atomic size than the elements in the same period?
(iii). Arrange the following elements in the increasing order of non-metallic character: F, Br, I, Cl
(b). Write the balanced equation for the conversion with the condition if: (3)
(i). NH3 → N2
(ii). Na2Co3 → Na2So4
(iii). H2 → NH3
(c). Name the following: (4)
(i). The catalyst used in Haber’s process.
(ii). Gas released at the anode in the electrolysis of PbBr2
(iii). Bases which are soluble in water.
(iv). Metals which reacts with both acids as well as bases.