Chemistry Exam Questions for SS1 First Term with Answers

You’re welcome to our school exams series where we provide you with termly examination questions in different subjects. In today’s post, we will focus on Chemistry exam questions. We will cover Chemistry exam questions for SS1 First term with answers. This means that we’ll be providing you with answers to the questions at the end. Also, you will get a few success tips on how to pass Chemistry examinations with flying colors. Remember to use the comments sections if you have questions, and don’t forget to join our Free Online Tutorial Classes on YouTube. (Subscribe to the Channel)

Introduction to Chemistry as a School Subject

Before we venture into Past Chemistry Exam Questions for SS1 First term, here’s a brief introduction to the subject:

Chemistry is the branch of science that studies the composition, structure, properties, and changes of matter. It helps students understand the substances that make up everything around them — from the air we breathe to the food we eat. As a school subject, Chemistry connects theory with real-life applications in fields like medicine, agriculture, engineering, and environmental science. It develops students’ skills in observation, experimentation, and problem-solving, preparing them for further studies and scientific careers.

Chemistry Exam Questions for SS1 First Term

Chemistry Exam Questions for SS1 First Term are divided into two sections:

• Section A
• Section B

The first section, namely, Section A is the objective test, and students are expected to attempt all questions in the section. Section B is the theory part, and students are expected to follow specific instruction and answer the required number of questions.

Note that what you have below are SS1 Chemistry First Term Exam Past Questions made available to assist students in their revision for 1st term examinations and also teachers in structuring standard examinations.

SECTION A: Objective Test

Instruction: Answer all questions in this section by choosing from the options lettered A—D. Each question carries equal marks.

1. Which of the following is a covalent compound?
A. Sodium chloride
B. Magnesium sulfide
C. Hydrogen chloride
D. Potassium nitrate

2. The components of universal indicator solution can best be separated by:
A. Chromatography
B. Titration
C. Evaporation
D. Fractional distillation

3. An element has mass number 27 and atomic number 13. What is the composition of its nucleus?
A. 13 protons and 14 neutrons
B. 14 protons and 13 neutrons
C. 13 protons and 13 neutrons
D. 14 protons and 14 neutrons

4. How many unpaired electrons are in the p-orbitals of a fluorine atom?
A. 0         B. 1
C. 2         D. 3

5. Two elements X and Y combine to form a compound of formula X₂Y₃. Which pair of electronic configurations (in shells) fits X and Y?
A. X: 2,8,2 and Y: 2,8,3
B. X: 2,2 and Y: 2,3
C. X: 2,8,2 and Y: 2,8,7
D. X: 2,6 and Y: 2,5

6. Element X has electronic configuration 2,8,2 and element Y has 2,8,7. The bonding between X and Y is most likely:
A. Metallic bonding
B. Covalent bonding
C. Electrovalent (ionic) bonding
D. Dative (coordinate) bonding

7. Carbon deposits in a car exhaust pipe mainly because of:
A. Presence of carbon in petrol
B. Dehydrogenation of petrol
C. Incomplete combustion of petrol
D. Presence of additives in petrol

8. Which of the following is NOT a heavy chemical?
A. Tetraoxosulphate(VI) acid (H₂SO₄)
B. Caustic soda (NaOH)
C. Sodium trioxocarbonate(VI) (Na₂CO₃)
D. Ethane (C₂H₆)

9. Octane number is highest in petrol containing a high proportion of which hydrocarbon?
A. Heptane
B. Octane
C. 2-Methylpentane
D. 2,2,4-Trimethylpentane

10. When the kerosene fraction is heated strongly and a lower boiling liquid is obtained, the process is called:
A. Polymerization
B. Refining
C. Hydrogenation
D. Cracking (fractional distillation is not the correct name here)

11. Which statement best explains “cracking”? It is a process in which:
A. An alkene adds to itself repeatedly to form a long-chain polymer
B. Large hydrocarbon molecules are broken into smaller molecules
C. Carbon atoms arrange in zig-zag chains
D. Aromatic hydrocarbons are always produced

12. For the reaction: MnO₂(s) + x HCl(aq) → MnCl₂(aq) + y H₂O(l) + z Cl₂(g), what are the values of x, y and z?
A. x = 4, y = 2, z = 1
B. x = 1, y = 2, z = 1
C. x = 2, y = 1, z = 2
D. x = 4, y = 1, z = 2

13. Boyle’s law relates pressure (P) and volume (V) of a gas at constant temperature. Which mathematical expression correctly shows this relation?
A. V ∝ 1/P
B. V₁/T₁ = V₂/T₂
C. V ∝ T (at constant P)
D. P ∝ T (at constant V)

14. Which reason explains why sulfuric acid (H₂SO₄) is regarded as a strong acid?
A. It is dibasic
B. It is often concentrated
C. It ionizes completely in aqueous solution (first ionization)
D. It is corrosive

15. The number of replaceable hydrogen atoms in one molecule of an acid indicates its:
A. Basicity      B. Alkalinity
C. Acidity       D. Reactivity

16. Which of the following are characteristic properties of acids?
A. They have a soapy feel only.
B. They form hydronium ions in water and liberate CO₂ from carbonates.
C. They turn blue litmus red and have a soapy feel.
D. They form hydronium ions in water, turn blue litmus red, and react with carbonates to give CO₂.

17. Which of the following acids is NOT monobasic?
A. Nitric acid (HNO₃)
B. Hydrochloric acid (HCl)
C. Ethanoic acid (CH₃COOH)
D. Sulfuric acid (H₂SO₄)

18. An acid in the presence of water produces:
A. Salts
B. Oxygen
C. Effervescence
D. Hydronium (hydroxonium) ions, H₃O⁺

19. Which of the following is an acid salt?
A. (NH₄)₂CO₃
B. CH₃COONa
C. KHSO₄
D. MgSO₄

20. General methods for preparing salts include: neutralization, precipitation, double decomposition and action of an acid on a metal. Which option lists these correctly?
A. Action of an acid on a metal only
B. Neutralization and precipitation only
C. Double decomposition and action of an acid on a metal only
D. Neutralization, precipitation, double decomposition and action of an acid on a metal

21. Alums are classified as:
A. Basic salts
B. Acid salts
C. Anhydrous salts
D. Double salts

22. Which of the following salts will NOT produce a gas when reacted with dilute hydrochloric acid?
A. CuSO₄      B. CaCO₃
C. FeS           D. K₂CO₃

23. Which method is best for preparing an insoluble salt in the laboratory?
A. Action of an acid on a metal
B. Double decomposition (mixing two soluble salts)
C. Neutralization of an acid with an alkali
D. Action of an acid on an oxide

24. Which statement about a solution of pH 4 is correct?
A. It contains more OH⁻ than H₃O⁺
B. Its pOH value is 10
C. It is more acidic than a solution of pH 2
D. Its hydrogen ion concentration is 4.0 × 10⁻² mol dm⁻³

25. The Acheson process is used to produce:
A. Graphite from coke at high temperature
B. Coke from graphite at high temperature
C. Anthracite from carbon
D. Wood-charcoal from coal

26. Which of these is NOT a reaction involving charcoal (carbon)?
A. C + O₂ → CO₂
B. CO₂ + C → 2CO
C. 2CO + O₂ → 2CO₂
D. CO₂ + 2CO → 2CO

27. Kipp’s apparatus is used to prepare an intermittent supply of gases by reacting:
A. A liquid with a gas
B. A liquid with a solid
C. A solid with a gas
D. A liquid with a liquid

28. Which gas dissolves in ammoniacal copper(I) chloride but is insoluble in water?
A. NH₃        B. CO
C. N₂O        D. CO₂

29. Fine chemicals are characterised by each of the following EXCEPT:
A. They are chemically pure.
B. They are produced by batch processes.
C. They are produced in very large quantities because of widespread applicability.
D. They are produced in small quantities because of limited applicability.

30. The exceptionally large number of carbon compounds is essentially due to carbon’s ability to:
A. Catenate (form chains) readily
B. Allow various other groups to catenate
C. Allow nitrogen, hydrogen, phosphorus and halogens to catenate with themselves
D. Make hydrocarbons dominate other groups

31. Universal indicator is added to a colourless solution and the indicator turns dark blue. What does this indicate?
A. The solution is acidic
B. The solution is neutral
C. The solution is alkaline (basic)
D. The solution is oxidizing

32. Which ion is present in all acidic solutions?
A. H⁺ (hydrogen ion)
B. OH⁻ (hydroxide ion)
C. H⁻ (hydride ion)
D. O²⁻ (oxide ion)

33. What name is given to a base that dissolves in water?
A. Amphoteric substance
B. An alkali
C. A salt
D. A hydride

34. Which ionic equation takes place during neutralisation of an acid by an alkali?
A. H⁺ + OH⁻ → H₂O
B. HCl → H⁺ + Cl⁻
C. NH₃ + H₂O → NH₄⁺ + OH⁻
D. Na⁺ + Cl⁻ → NaCl

35. Which of the following could be used to neutralise acidic soil?
A. Sodium chloride (NaCl)
B. Calcium oxide (CaO)
C. Sulfuric acid (H₂SO₄)
D. Hydrochloric acid (HCl)

36. Sulfuric acid reacts with magnesium oxide to give:
A. Magnesium sulfate + carbon dioxide + water
B. Magnesium sulfate + hydrogen
C. Magnesium sulfate + water
D. Magnesium chloride + water

37. Which pair of reagents would produce potassium nitrate (KNO₃)?
A. Sodium hydroxide and sulfuric acid
B. Potassium carbonate and nitric acid
C. Potassium hydroxide and nitric acid
D. Potassium hydroxide and hydrochloric acid

38. Which acid is used to make salts whose names end in “-sulfate”?
A. Sulfamic acid
B. Nitric acid
C. Sulfuric acid
D. Hydrochloric acid

39. What ion is present in nitric acid (HNO₃)?
A. NO₃⁻ (nitrate ion)
B. NH₄⁺ (ammonium ion)
C. OH⁻ (hydroxide ion)
D. SO₄²⁻ (sulfate ion)

40. Zinc oxide reacts with nitric acid to give:
A. Zinc nitrate + water
B. Zinc chloride + hydrogen
C. Zinc nitrate + water + carbon dioxide
D. Zinc sulfate + water

41. Which two chemicals could be reacted to make ammonium chloride (NH₄Cl)?
A. Ammonium hydroxide and hydrochloric acid
B. Ammonia and sulfuric acid
C. Potassium hydroxide and nitric acid
D. Ammonium nitrate and sodium chloride

42. Calcium carbonate reacts with hydrochloric acid to give:
A. Calcium chloride + hydrogen
B. Calcium chloride + water + carbon dioxide
C. Calcium sulfate + water
D. Calcium hydroxide + carbon dioxide

43. Which of these salts is most likely to be soluble in water?
A. Potassium nitrate (KNO₃)
B. Iron(II) carbonate (FeCO₃)
C. Copper(II) oxide (CuO)
D. Lead(II) iodide (PbI₂)

44. What is the name of the white precipitate formed when silver nitrate solution reacts with sodium chloride solution?
A. Sodium nitrate
B. Silver chloride
C. Sodium chloride
D. Silver nitrate

45. When producing a soluble salt by reacting an acid and an alkali, which method is used to obtain dry solid crystals from the solution?
A. Filtration of the mixture directly
B. Chromatography
C. Evaporation of the solvent and crystallisation
D. Distillation of the acid

46. In an acid–alkali titration, which piece of apparatus is used to deliver a fixed volume of one solution into the conical flask?
A. Burette
B. Pipette
C. Beaker
D. Measuring cylinder

47. When processing titration results that are very close together, what is the correct statistical treatment?
A. Take the average (mean) of the concordant results
B. Ignore them as anomalies
C. Pick the highest only
D. Use the smallest only

48. Which of the following cannot be obtained directly from the destructive distillation of coal?
A. Ammoniacal liquor
B. Coke
C. Producer gas
D. Crude oil (petroleum)

49. The use of diamond in cutting and polishing (abrasives) is due to its:
A. High melting point
B. Durability
C. Lustre
D. Hardness

50. The liquid product often obtained from the destructive distillation of coal (coal tar fractions) includes:
A. Kerosene
B. Ethanol
C. Ammoniacal liquor
D. Paraffin oil (lamp oil)

51. Which of the following best describes an amphoteric oxide?
A. An oxide that reacts only with acids
B. An oxide that reacts only with bases
C. An oxide that reacts with both acids and bases
D. An oxide that reacts with water to form an acid

52. The empirical formula of a compound containing 40% carbon, 6.7% hydrogen and 53.3% oxygen by mass is:
A. CH₂O       B. C₂H₄O₂
C. CHO        D. C₂H₂O

53. Which test distinguishes between hydrogen gas and oxygen gas in the laboratory?
A. Pop test (a lighted splint produces a pop) for hydrogen; glowing splint rekindles for oxygen
B. Ammonia test for hydrogen; limewater for oxygen
C. Limewater test for hydrogen; pop test for oxygen
D. Brown ring test for both gases

54. Which statement is true about catalysts?
A. Catalysts are consumed in the reaction.
B. Catalysts lower the activation energy and are not consumed.
C. Catalysts increase the reaction temperature.
D. Catalysts change the equilibrium constant of the reaction.

55. In electrolysis of molten sodium chloride, the product at the cathode is:
A. Chlorine gas
B. Sodium metal
C. Hydrogen gas
D. Sodium hydroxide

56. Which of the following is an example of a hydrocarbon?
A. Ethane (C₂H₆)
B. Ethanol (C₂H₅OH)
C. Acetic acid (CH₃COOH)
D. Sodium ethoxide (C₂H₅ONa)

57. Which reagent will produce ammonia (NH₃) gas when treated with a strong base and warmed?
A. Ammonium chloride (NH₄Cl)
B. Potassium nitrate (KNO₃)
C. Sodium sulfate (Na₂SO₄)
D. Calcium carbonate (CaCO₃)

58. Which of these statements about graphite and diamond is CORRECT?
A. Both graphite and diamond are good conductors of electricity.
B. Graphite conducts electricity but diamond does not.
C. Diamond conducts electricity but graphite does not.
D. Neither graphite nor diamond conduct electricity.

59. Which of the following lab observations indicates that a gas is carbon dioxide?
A. It relights a glowing splint.
B. It turns limewater milky (cloudy).
C. It gives a pop sound with a lighted splint.
D. It dissolves in water to give an alkaline solution.

60. Which substance will react with dilute hydrochloric acid to release a gas that turns limewater milky?
A. Calcium carbonate (CaCO₃)
B. Sodium sulfate (Na₂SO₄)
C. Copper(II) sulfate (CuSO₄)
D. Magnesium sulfate (MgSO₄)

SECTION B: Essay / Theory

INSTRUCTION – Answer only five (5) questions in this section. Write your answers clearly and show working where necessary.

1. (a) Describe a simple laboratory test to prove that a given colourless liquid is an acid. Include the observations and the chemical equation(s) where applicable.
(b) Explain why sulfur dioxide (SO₂) is described as an acid anhydride. Give one chemical equation to support your explanation.

2. (a) State and explain four general methods of preparing salts in the laboratory. For each method give one balanced chemical equation as an example.
(b) Describe a chemical test (without using litmus paper or indicator) that would show sodium hydroxide is a base. Write the chemical equation(s) involved.

3. (a) The concentration of H⁺ ions in a solution is 1.0 × 10⁻³ mol dm⁻³. Calculate the pH of the solution and show your working.
(b) Explain briefly how you would prepare 250 cm³ of 0.1 mol dm⁻³ sodium chloride solution starting from solid sodium chloride. Show calculations.

4. (a) Explain, with diagrams if necessary, why graphite conducts electricity while diamond does not. Include reference to structure and bonding in each allotrope.
(b) State two properties of carbon(II) oxide (carbon monoxide) that make it poisonous.
(c) Give two properties of carbon(IV) oxide (carbon dioxide) that make it useful in fire extinguishers.

5. (a) List four products obtained from the destructive distillation of coal and briefly state one use for each product.
(b) Explain how producer gas is prepared and name two uses of producer gas.

6. (a) Define fractional distillation of crude oil and name five fractions obtained in increasing order of boiling point.
(b) Distinguish between heavy chemicals and fine chemicals. Give two examples of each.
(c) Define hydrocarbons and give two examples, stating whether each is saturated or unsaturated.

7. (a) Describe the laboratory preparation of an insoluble salt by precipitation. Include procedure and a balanced equation for the reaction used in your example.
(b) Explain what is meant by an acid salt and give one example with its formula.
(c) Briefly describe how you would carry out an acid–alkali titration to determine the concentration of a given hydrochloric acid solution. Include apparatus, procedure and how results are used to calculate concentration.

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Answers to Chemistry Exam Questions for SS1 First Term

Answers to Section A (Objective Test)

The following table gives the correct answers to the objective section of Chemistry exam questions for SS1 First term. If you are using a mobile device, hold the table and scroll to the right or left for a complete view.

So here you have the answers to the objective section of Chemistry Exam Questions for SS1 First term. Use the comments section to let me know if you have any questions you would want me to clarify or discuss further.

Answers to Section B (Theory)

Answers to Question 1.

(a) To prove that a given colourless liquid is an acid, dip a blue litmus paper into the liquid. If it turns red, the liquid is acidic. Alternatively, add a small piece of marble (CaCO₃) to the liquid; effervescence (bubbling) due to the release of carbon dioxide gas indicates that it is an acid.

Chemical equation: CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂↑

(b) Sulfur dioxide (SO₂) is described as an acid anhydride because it reacts with water to form an acid, specifically sulfurous acid (H₂SO₃).

Equation: SO₂ + H₂O → H₂SO₃

Answers to Question 2.

(a) General methods of preparing salts:

1. Neutralization: Reaction between an acid and a base to form salt and water.
   Example: HCl + NaOH → NaCl + H₂O
2. Action of acid on metal: Acid reacts with metal to produce a salt and hydrogen gas.
   Example: 2HCl + Zn → ZnCl₂ + H₂↑
3. Action of acid on carbonate: Acid reacts with a carbonate to give salt, water, and carbon dioxide.
   Example: 2HCl + CaCO₃ → CaCl₂ + H₂O + CO₂↑
4. Double decomposition (precipitation): Mixing two soluble salts to produce an insoluble salt.
   Example: AgNO₃ + NaCl → AgCl↓ + NaNO₃

(b) To test that sodium hydroxide is a base, add ammonium chloride (NH₄Cl) and warm gently. A colourless gas with a characteristic pungent smell (ammonia) will be evolved.

Equation: NH₄Cl + NaOH → NaCl + H₂O + NH₃↑

Answers to Question 3.

(a) Given [H⁺] = 1.0 × 10⁻³ mol dm⁻³

pH = –log[H⁺] = –log(1.0 × 10⁻³) = 3

Therefore, pH = 3.

(b) To prepare 250 cm³ (0.25 dm³) of 0.1 mol dm⁻³ NaCl solution:

Moles required = M × V = 0.1 × 0.25 = 0.025 mol

Molar mass of NaCl = 58.5 g/mol

Mass required = 0.025 × 58.5 = 1.46 g

Procedure: Weigh 1.46 g of pure sodium chloride, dissolve it in a small volume of distilled water, transfer into a 250 cm³ volumetric flask, and make up to the mark with distilled water. Stopper and shake to mix thoroughly.

Answers to Question 4.

(a) Graphite conducts electricity because each carbon atom is bonded to three others in hexagonal layers, leaving one free electron per atom to move and conduct electricity. Diamond does not conduct because all four valence electrons are involved in strong covalent bonds, leaving no free electrons.

(b) Carbon(II) oxide is poisonous because:

1. It binds strongly to haemoglobin, preventing oxygen transport.
2. It is colourless and odourless, making it hard to detect.

(c) Carbon(IV) oxide is useful in fire extinguishers because:

1. It does not support combustion.
2. It is denser than air, forming a blanket that cuts off oxygen supply to the fire.

Answers to Question 5.

(a) Products of destructive distillation of coal and their uses:

• Coke: Used as fuel and in the extraction of metals.
• Coal tar: Used for making dyes, drugs, and explosives.
• Ammoniacal liquor: Used as a source of ammonia for fertilizers.
• Coal gas: Used as domestic fuel and for lighting.

(b) Producer gas is prepared by passing air and steam alternately over red-hot coke, producing a mixture of carbon monoxide and nitrogen.

Equation: 2C + O₂ + 4N₂ → 2CO + 4N₂

Uses: As an industrial fuel and as a reducing agent in metallurgy.

Answers to Question 6.

(a) Fractional distillation of crude oil is the process of heating crude oil and separating it into fractions based on differences in their boiling points. Fractions in increasing order of boiling point are:

Petroleum gas → Petrol → Kerosene → Diesel oil → Lubricating oil → Bitumen.

(b) Heavy chemicals are produced in large quantities and used in industries, e.g. Sulfuric acid (H₂SO₄), Sodium hydroxide (NaOH).
Fine chemicals are pure and produced in small quantities, e.g. drugs, perfumes.

(c) Hydrocarbons are compounds that contain only carbon and hydrogen.

• Ethane (C₂H₆) — Saturated hydrocarbon.
• Ethene (C₂H₄) — Unsaturated hydrocarbon.

Answers to Question 7.

(a) To prepare an insoluble salt by precipitation, mix two soluble salt solutions whose ions will form an insoluble compound. Example: Adding sodium chloride to silver nitrate solution produces a white precipitate of silver chloride.

Equation: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)

Filter, wash, and dry the precipitate.

(b) An acid salt is a salt formed when only part of the replaceable hydrogen ions of an acid have been replaced by a metal. Example: Potassium hydrogen sulfate (KHSO₄).

(c) In an acid–alkali titration, use a pipette to measure a fixed volume of the alkali into a conical flask. Add a few drops of phenolphthalein indicator. Fill a burette with the acid and add it slowly to the alkali while swirling until the pink colour just disappears. Record the volume of acid used (titre). Repeat until concordant results are obtained and calculate concentration using:

Equation: M₁V₁ = M₂V₂ (for monoprotic acid and base reactions).

Read Also: Chemistry Exam Questions for SS1 Third Term

How to Pass Chemistry Exam Questions for SS1 First Term

Passing your Chemistry exam questions for SS1 First term requires a combination of preparation, understanding, and strategy. Here are actionable tips to help you excel:

1. Understand Basic Concepts:

Don’t just memorize definitions and formulas. Take time to understand the meanings of key terms such as elements, compounds, mixtures, acids, bases, and salts. This will help you apply them correctly in problem-solving.

2. Master the Laboratory Techniques:

Pay attention during practical classes. Learn how to identify acids, bases, and salts through simple tests, and understand how to record accurate observations and results. Many exam questions come from practical applications.

3. Study Chemical Equations:

Learn how to write and balance chemical equations correctly. Understanding the relationship between reactants and products is key to scoring high in both objective and theory questions.

4. Practice Past Questions Regularly:

Work through past SS1 Chemistry exam questions to know how topics are usually set. This helps you to become familiar with the exam pattern and identify your weak areas.

5. Learn Calculations and Units:

Topics like concentration, molarity, and pH require calculations. Learn the correct formulas and always write your workings clearly in the exam.

6. Pay Attention to Structures and Bonding:

Understand the structures of substances like graphite and diamond, and be able to explain how their bonding affects their properties. Such questions often appear in theory sections.

7. Revise Consistently:

Don’t wait until the exam period. Revise a little every day, summarizing each topic in your own words. Create flashcards for formulas, definitions, and equations.

8. Stay Calm and Manage Time:

During the exam, read each question carefully and answer the simpler ones first. Manage your time wisely to ensure that you complete the paper.

It’s a wrap!

If you need more clarification on SS1 First Term Questions on Chemistry, you can use the comments box below. We’ll be there to answer you asap. Don’t forget to join our Free Online Tutorial Classes on YouTube. (Subscribe to the Channel)

Best wishes..