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ICSE Class X Sample / Model Paper 2026 : Chemistry

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Pujaa Chaudhary
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ICSE 2026 EXAMINATION Sample Question Paper - 1 Chemistry 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: (a) (b) (c) The element with the highest ionisation potential in the periodic table is ________. a) He b) Ne c) Xe d) Ar Which one of the following is the correct order of the size of ions? a) Mg2+ > Na+ > F- > O2- b) O2- > F- > Na+ > Na+ c) Na+ > Mg2+ > F- > O2- d) O2- > F- > Na+ > Mg2+ Ionic compounds in general possess both a) directional bonds and low boiling points [15] [1] [1] [1] b) high melting point and low boiling points c) high melting point and non-directional d) high solubilities in polar and non-polar bonds (d) (e) (f) compounds Dilute sulphuric acid will produce a white precipitate when added to a solution of ________. a) Lead nitrate b) Zinc nitrate c) Sodium nitrate d) Copper nitrate In laboratory copper sulphate is prepared by: [1] a) Displacement b) Direct combination c) Decomposition by acid d) Synthesis Which of the following analysis deals with the identification of unknown substance? a) Both qualitative and quantitative [1] b) Qualitative analysis Page 1 of 12 [1] analysis c) chemical analysis (g) (h) (i) (j) d) Quantitative analysis In defining Charle's law volume is directly proportional to: a) Pressure b) Moles c) Atoms d) Temperature Percentage of calcium in calcium carbonate (CaCO3) is a) 36 b) 30 c) 48 d) 40 The electrolyte used for electroplating an article with silver is: a) Silver cyanide solution b) Sodium argentocyanide solution c) Nickel sulphate solution d) Silver nitrate solution [1] [1] [1] Heating an ore in a limited supply of air or in the absence of air at a temperature just below its melting [1] point is known as: (k) (l) a) Ore dressing b) Bessemerisation c) Smelting d) Calcination Hydrogen chloride can be obtained by adding concentrated sulphuric acid to: a) Na2SO4 b) NaNO3 c) NaCl d) Na2CO3 Which of the following statements is incorrect about ammonia? a) It gives white fumes with HCI b) It gives black precipitate with calomel c) It is oxidised by oxygen at 700oC in the d) It can be dried by P2O5, H2SO4 and presence of platinum. (m) (n) (o) 2. [1] CaCI2. The property of carbon to form chains and rings is called: a) Catenation b) Polymerization c) Hydrogenation d) Cracking How many acids are possible for the compound with molecular formula, C4H8O2? a) Three acids b) Four acids c) Two acids d) One acid Among the following, which alkane is expected to have lowest boiling point. a) 2-methylpentane b) 3-methylpentane c) Hexane d) 2,2-dimethyl butane Question 2 (a) [1] [1] [1] [1] [25] Complete and balance the following equations. 200 C i. KNO3 + H2SO4 (conc.) ________ + ________ Page 2 of 12 [5] ii. 2Cu(NO3)2 ________ + ________ + ________ iii. KOH + HNO3 ________ + ________ iv. P + 5HNO3 ________ + ________ + ________ v. C + 4HNO3 ________ + ________ + ________ (b) The diagram below is to prepare iron (III) chloride in the laboratory. [5] i. What is substance B? ii. What is the purpose of B? iii. Why is iron (III) chloride to be stored in a closed container? iv. Write the equation for the between iron and chlorine. (c) Complete the following by choosing the correct answers from the bracket: i. The energy required to remove an electron from a neutral isolated gaseous atom and convert it [1] into a positively charged gaseous ion is called ________. (electron affinity/ionisation potential/electronegativity) ii. Soluble salts are prepared by ________ whereas insoluble salts are generally prepared by [1] ________. iii. Complete the following, n = iv. ________ is an electrically charged atom. [1] v. ________ and conc. H2SO4 are the reactants used during the preparation of nitric acid in [1] Molecular mass ________ [1] laboratory. (d) Identify the following: i. Identify and name the following: [1] Ice like crystals formed on cooling on organic acid sufficient. ii. Identify and name the following: [1] The gas produced by the action of concentrated sulphuric acid on sodium chloride. iii. Identify and name the following: [1] The name of that process by which impurities from metals are removed electrolytically. iv. Identify and name the following: [1] Name the aqueous salt solution used for testing sulphate radical. v. Fill in the blanks: [1] In Period 3, the most metallic element is ________. (sodium/magnesium/aluminium) (e) i. Calculate the percentage of: [2] i. Fluorine ii. Sodium and iii. Aluminium in sodium aluminium fluoride [Na3AlF6], to the nearest whole number. [Atomic mass: Na = 23, Al = 27, F = 19] Page 3 of 12 ii. i. Name the charged particles, which attract one another to form electrovalent compounds. [3] ii. In the formation of electrovalent compounds, electrons are transferred from one element to another. How are electrons involved in the formation of a covalent compound? iii. The electronic configuration of nitrogen is 2, 5. How many electrons in the outer shell of a nitrogen atom are not involved in the formation of a nitrogen molecule? Section B Attempt any 4 questions 3. Question 3 (a) [10] Distinguish between the following pairs of compounds using the reagent given in the bracket. [2] Manganese dioxide and Copper (II) oxide, (using concentrated HCl). (b) (c) (d) Write the products and balance the equation. i. Reaction of zinc with potassium hydroxide solution. [1] ii. Calcium bicarbonate reacts with nitric acid. [1] Arrange the following as per the instruction given in the brackets: i. Li, K, Na, H (In the decreasing order of their ionization potential) [1] ii. Na, K, Li (increasing chemical reactivity) [1] iii. Mg, Cl, Na, S, Si (decreasing order of atomic size) [1] Fill in the blanks by selecting the appropriate word from the given choice: i. The name of organic compound consists of three types such as ________, ________ and [1] ________. ii. The name of carboxylic acid is derived by the combination of ________ group and the [1] ________ group. The number of molecules present in 35.5 g of chlorine is ________ 1023. (3.01/6.02) iii. 4. Question 4 (a) [1] [10] Element X is a metal with a valency 2, Y is a non-metal with a valency 3. [2] i. Write an equation to show how Y forms on ion. ii. If Y is a diatomic gas write an equation for the direct combination of X and Y to form a compound. (b) Calculate the mass of iron which will be converted into its oxide (Fe3O4) by the action of 36 g steam [2] on it. (c) Answer the following questions based on the extraction of aluminium from alumina by Hall-Heroult's [3] Process: i. What is the function of cryolite used along with alumina as the electrolyte? ii. Why is powdered coke sprinkled in top of electrolyte? iii. Name the electrode, from which aluminium is collected. (d) Explain the following: i. Zinc oxide can be reduced to zinc by using carbon monoxide, but aluminium oxide cannot be [1] reduced by a reducing agent. 5. ii. Zinc chloride is stored in air-tight bottles. [1] iii. Sea water is a strong electrolyte. [1] Question 5 [10] Page 4 of 12 (a) What are the main types (groups) of aliphatic hydrocarbons? [1] ii. Give an example of isomer shown by triple bond hydrocarbon and write its IUPAC name. [1] (b) Why hydrogen chloride can be termed as a polar covalent compound? (c) Give balanced chemical equation for the following: (d) 6. i. i. Ammonium chloride is warmed with concentrated sulphuric acid [1] ii. Concentrated nitric acid is heated [1] iii. Concentrated hydrochloric acid and potassium permanganate solution [1] State one relevant observation for each of the following reactions: i. Copper sulphide is heated with dilute hydrochloric acid. [1] ii. NaOH solution is added to calcium nitrate solution. [1] iii. At the anode when aqueous copper sulphate solution is electrolysed using copper electrodes. [1] Question 6 (a) [2] [10] Give the number of the group and the period, of the element having three shells with three electrons in [2] valence shell. (b) Commercial sodium hydroxide weighing 30 g has same sodium chloride in it. The mixture on [2] dissolving in water and subsequent treatment with excess silver nitrate solution formed a precipitate weighing 14.3 g. What is the percentage of sodium chloride in the commercial sample of sodium hydroxide? The equation for the reaction is NaCl + AgNO3 AgCl + NaNO3 (Relative molecular mass of NaCl = 58 and AgCl = 143) (c) i. Give two tests to identify acetic acid. [3] ii. How vinegar is prepared in industries? (d) Write the product of the following reactions. [3] i. Ca(NO3)2 + 2NaOH ii. FeSO4 + NaOH iii. FeCl3 + 3NaOH iv. CuSO4 + NaOH v. ZnSO4 + NaOH vi. Pb(NO3) + 2NaOH 7. Question 7 (a) [10] Use Lewis symbols to show electron transfer between the following. atoms to form cations and [2] anions: i. K and S ii. Al and N (b) Calculate the mass of: [2] i. 1022 atoms of sulphur ii. 0.1 mole of carbon dioxide. (c) Write the three different conditions to be maintained during electroplating. [3] (d) Give the structural formulae of each of the following: [3] i. 2-methyl propane Page 5 of 12 ii. Ethanoic acid iii. Butan-2-ol 8. Question 8 [10] (a) Why an aqueous solution of sodium chloride conducts electricity? [2] (b) Ethane burns in oxygen to form CO2 and H2O according to the equation: [2] 2C2H6 + 7O2 4CO2 + 6H2O. If 1250 cc of oxygen is burnt with 300 cc of ethane. Calculate: i. The volume of CO2 formed. ii. The volume of unused O2. (c) Define the term: [3] i. Acid ii. pH scale iii. Neutralisation (d) Give examples of the use of sulphuric acid: i. As an electrolyte in everyday use ii. As non-volatile acid iii. As an oxidising agent. Page 6 of 12 [3] Solution Section A 1. Question 1 Choose one correct answer to the questions from the given options: (i) (a) He Explanation: He (ii) (d) O2- > F- > Na+ > Mg2+ Explanation: Ionic size = (p/e) value can be calculated by where, p = number of protons e = number of electrons and ionic size 1/p/e i.e, more be the value of Ionic size for Na+ = Mg2+ = F- = 9 10 e = 11 10 e , smaller be the ionic size and vice versa. = 1.1 = 1.2 = 0.9 10 O2- = 12 p p 8 10 = 0.8 Hence, correct order is O2- > F- > Na+ > Mg2+ (iii) (c) high melting point and non-directional bonds Explanation: high melting point and non-directional bonds (iv) (a) Lead nitrate Explanation: Lead nitrate (v) (c) Decomposition by acid Explanation: Decomposition by acid (vi) (b) Qualitative analysis Explanation: Qualitative analysis (vii) (d) Temperature Explanation: Temperature (viii) (d) 40 Explanation: 40 (ix) (b) Sodium argentocyanide solution Explanation: Sodium argentocyanide solution (x) (d) Calcination Explanation: Calcination (xi) (c) NaCl Explanation: NaCl Page 7 of 12 (xii) (d) It can be dried by P2O5, H2SO4 and CaCI2. Explanation: Ammonia gas is basic and cone. H2SO4 is an acid thus it will react to form white fumes of (NH 4 ) 2 SO4 P2 O5 and also react with ammonia, hence cannot be used for drying it. + H SO (NH ) SO + 6NH + 3H O 2(NH ) PO CaCl2 2NH 3 P2 O5 2 4 3 4 2 4 2 4 4 3 CaCl2 + 8NH 3 CaCl2 .8NH 3 (xiii) (a) Catenation Explanation: Catenation (xiv) (c) Two acids Explanation: Twp acids are possible for the compound with molecular formula, C4H8O2 (xv) (d) 2,2-dimethyl butane Explanation: A straight chain alkane will have a boiling point higher than a branched-chain alkane, due to the greater surface area in contact, thus the greater van der waals forces between adjacent molecules. Hence, 2,2-dimethyl butane have lowest boiling point. 2. Question 2 (i) Complete reaction are as follows: i. KHSO4 + HNO3 ii. 2CuO + 4NO2 + O2 iii. KNO3 + H2O iv. H3PO4 + 5NO2 + H2O v. CO2 + 4NO2 + 2H2O (ii) i. Substance B is anhydrous calcium chloride CaCl2. ii. Anhydrous calcium chloride is a drying agent which does not allow the moisture to enter into the receiver. iii. Iron (III) chloride is highly deliquescent. So, it should be kept dry by storing in a closed container. iv. 2Fe + 3Cl 2FeCl 2 heated 3 dry (iii)Complete the following by choosing the correct answers from the bracket: i. 1. ionisation potential ii. 1. neutralisation, precipitation reactions iii. 1. Empirical formula mass iv. 1. Ion v. 1. Potassium nitrate (iv)Identify the following: i. 1. Glacial acetic acid ii. 1. Hydrogen chloride iii. 1. Electrolytic refining iv. 1. Barium chloride solution 2. Barium chloride v. 1. Sodium (v) i. Molar mass of sodium aluminium fluoride [Na3AlF6] = 3 23 + 27 + 6 19 [Atomic mass: Na = 23, Al = 27, F = 19] Page 8 of 12 = 69 + 27 + 114 = 210 gm. i. Percentage of fluorine = = Mass of fluorine Molecular mass of Na 3 AlF6 19 6 210 100 100 = 54.3% It has to be rounded up to nearest whole number so 54%. ii. Percentage of sodium = = Mass of aluminium Molecular mass of Na 3 AlF6 23 3 210 100 100 = 32.8% It has to be rounded up to nearest whole number so 33%. iii. Percentage of aluminium = = Mass of the aluminium Molecular mass of Na 3 AlF6 27 210 100 100 = 12.86% It has to be rounded up to nearest whole number so 13%. ii. i. Cations are positively charged ions and anions are negatively charged ions. ii. In the formation of a covalent compound sharing of one, two or three pairs of electrons between two atoms takes place. iii. Two electrons. Section B 3. Question 3 (i) On adding concentrated hydrochloric acid if a greenish yellow gas is evolved it is Manganese dioxide. If no gas is evolved it is CuO. (ii) Write the products and balance the equation. i. Zn + 2KOH K2ZnO2 + H2 ii. Ca(HCO 3 )2 + 2HCl Calcium bicarbonate ( dil ) Hydrochloric acid CaCl2 + 2H2 O + Calcium Water 2CO2 Carbon dioxide Chloride (iii)Arrange the following as per the instruction given in the brackets: i. H, Li, Na, K ii. Li < Na < K iii. Na > Mg > Si > S > Cl (decreasing order of atomic size) (iv)Fill in the blanks by selecting the appropriate word from the given choice: i. 1. root word, suffix, prefix ii. 1. carbonyl, hydroxyl iii. 1. 3.01 4. Question 4 (i) i. Y + 3e- Y3ii. 3X + Y2 X3Y2 (ii) The balanced chemical equation representing the reaction is - 3Fe 3 moles + 4H2 O(g) Fe3 O4 + 4H2 (g) 4 moles 4 18 = 72 3 56 = 168 72 g of steam will react with = 168 g of iron 36 g of steam will react with = 36 168 172 = 84 g of iron Mass of iron = 84 g (iii) i. Cryolite reduces the fusion temperature of the mixture/Cryolite increases the mobility of the ions/increases the conductivity of the electrolyte/acts as solvent for alumina. Page 9 of 12 ii. Powdered coke protects the graphite rods of the anode from oxidation by oxygen released at the anode/Powdered coke prevents the loss of heat from the electrolyte. iii. Cathode. (iv)Explain the following: i. This is because of the fact that aluminium has great affinity towards oxygen and so, it cannot be reduced by reducing agents such as carbon monoxide, carbon or hydrogen. ii. Zinc chloride is a deliquescent substance. It absorbs moisture from the atmosphere and turns into solution. In order to prevent this, it is stored in air tight bottles. iii. Sea water is not a pure water, it contains NaCl which dissociates completely into free mobile ions and behave as strong electrolyte. NaCl Na + + Cl 5. Question 5 (i) i. i. Saturated aliphatic hydrocarbons e.g., Methane and ethane. ii. Unsaturated aliphatic hydrocarbons e.g., Ethene and ethyne. ii. C H3 C H2 C CH (IU P AC name: But 1 yne) , CH 3 C C C H3 (IU P AC name: But 2 yne) (ii) In hydrogen chloride, chlorine is more electronegative than that of hydrogen. So it attracts the shared electron pair towards itself. Due to this, Cl acquires partial negative charge and H acquires partial positive charge. Therefore, a polar covalent bond is formed. (iii)Give balanced chemical equation for the following: i. 2NH4Cl + H 2 SO4 (NH4)2SO4 + 2HCl (conc) 2H2O + 4NO2 + O2 ii. 4HNO3 iii. 2KMnO4 + 16HCl conc. 2KCl + 2MnCl2 + 8H2O + 5Cl2 (iv)State one relevant observation for each of the following reactions: i. H2S gas with rotten egg smell is evolved. ii. A white precipitate of Ca(OH)2 is obtained which is insoluble in excess of NaOH. iii. The copper of the anode dissolves and therefore it becomes thin or consumed gradually. 6. Question 6 (i) No of shells = 3 No of electron in valence shell = 3 The number of shells is equal to the number of periods. So, the element belongs to third period. The number of valence electrons shows the group of the element. So, the element belongs to 10 + 3 = 13 i.e., thirteenth group. (ii) Equation: NaCl + 58 g AgNO 3 AgCl + NaNO 3 143 g 143 g of AgCl is obtained from 58 g of NaCl 14.3 g of AgCl is obtained from = 58 14.3 143 = 5.8 g of NaCl Percentage of NaCl in the given sample = 5.8 30 100 = 19.33 % (iii) i. Two tests to identify acetic acid. a. When acetic acid reacts in the presence of concentrated sulphuric acid, a pleasant fruity smell of ester is produced. b. On adding neutral FeCl3, wine red colour is produced. ii. It is a fatty acid and the name acetic acid comes from the Latin word 'acetum' which means vinegar. Vinegar (or sirka) is a dilute (4-5%) solution of acetic acid. (iv)The products of given reactions are follows: Page 10 of 12 i. Ca(OH)2 + 2NaNO3 ii. Fe(OH)2 + Na2SO4 iii. Fe(OH)3 + 3NaCl iv. Cu(OH)2 + Na2SO4 v. Zn(OH)2 + Na2SO4 vi. Pb(OH)2 + 2NaNO3 7. Question 7 (i) i. ii. (ii) i. 6 1023 atoms of sulphur = 32 g 1022 atoms of sulphur = 32 23 1022 = 0.533 g 6 10 ii. Molar mass of CO2 = 12 + 2 16 = 44g 1 mole of CO2 weights = 44 g 0.1 mole of CO2 weights = 44 0.1 = 4.4 g (iii)Three different condition to be maintained during electroplating are as follows i. In electrolysis the article deposited is always made the cathode since, the metal is deposited at cathode. ii. The metal to be plated on the article is always made the anode since, metal anode continuously dissolve into the solution, it has to be replaced periodically. iii. Less amount of current is supplied for longer time. (iv) i. H O | || ii. H C C OH | H H H H H | | | | iii. H C C C C H | | | | H H OH H 8. Question 8 (i) Sodium chloride (Na+Cl-) is an ionic compound. When dissolved in water, the ions present in it can migrate towards the oppositely charged electrodes and such an aqueous solution of sodium chloride conducts electricity. (ii) 2C H + 7O 4CO + 6H O 2 6 2 2 vol 7 vol 2 2 4 vol 2 vol 300 cc 1 vol = 150 cc 300 2 i. 4 vol of CO2 4 150 600 cc of CO2 ii. 7 vol of O2 7 150 1050 cc of O2 Vol. of unused O2 = 1250 - 1050 = 200 cc of O2 (iii) i. Acid: Acid is the chemical compound which on dissolving in water, produces hydronium ions as the only positively charged particles. ii. pH Scale: The scale used for determining the acidic or alkaline character of the solution. Page 11 of 12 iii. Neutralisation: When H+ ions derived from an acid combine with hydroxyl ions of a base to form unionized water molecule is called as neutralisation. (iv) i. Use of sulphuric acid in storage batteries. ii. Use of sulphuric acid in the preparation of hydrochloric acid, nitric acid and acetic acid. iii. Use of sulphuric acid in the preparation of sulphur dioxide. Page 12 of 12

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