Chemistry Exam Questions for SS2 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 SS2 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 SS2 First term, here’s a brief introduction to the subject:

Chemistry is one of the core science subjects taught in secondary schools. It deals with the study of the composition, structure, properties, and changes of matter. In simple terms, Chemistry helps students understand what materials are made of, how they interact, and why they behave the way they do.

As a school subject, Chemistry builds a bridge between Physics and Biology. It explains many natural and industrial processes such as respiration, combustion, rusting, fermentation, and the manufacture of everyday materials like soap, fertilizers, plastics, and drugs.

Through practical experiments and theoretical lessons, students learn important scientific skills such as observation, measurement, problem-solving, and critical thinking. The knowledge of Chemistry also prepares students for careers in Medicine, Engineering, Agriculture, Pharmacy, and Environmental Science.

In summary, Chemistry is the science of substances and their transformations — a subject that helps us understand the world around us and equips students with the foundation for technological and scientific advancement.

Chemistry Exam Questions for SS2 First Term

Chemistry Exam Questions for SS2 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 SS2 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 processes is a physical change?
A. Rusting of iron
B. Melting of ice
C. Decomposition of organic matter
D. burning of candle

2. A mixture of sodium chloride and ammonium chloride is separated by
A. Filtration            B. evaporation
C. decantation       D. sublimation

3. Air is chemically regarded as a mixture because
A. it has no constant composition
B. it cannot be separated to different components by physical separating techniques
C. it has a chemical formula
D. the various components lose their individual characteristics

4. The following are suitable criteria for testing the purity of a substance except
A. boiling point
B. chromatography
C. colour
D. melting point

5. Consider the changes in state of matter as in the sketch below:

State Y represent the process of
A. boiling                B. melting
C. sublimation        D. Freezing

6. The atomicity of nitrogen is
A. 4            B. 3
C. 2            D. 1

7. Analysis of two different samples of an oxide revealed that the percentages of an element are 80.1% and 79.65. the findings are in agreement with the law of
A. conservation of matter
B. Definite proportion
C. multiple proportion
D. Reciprocal proportion

8. The relative molecular mass of calcium hydroxide [Ca(OH)₂] is_________. [Ca = 40, O = 16, H = 1] A. 101            B. 92
C. 74              D. 57

9. What is the percentage by mass of oxygen in CaCO₃? [Ca = 40, C = 12, O = 16] A. 40%           B. 48%
C. 12%           D. 70%

10. An oxide contains 30% by mass of nitrogen what is the empirical formula of the oxide?
A. NO₂           B. N₂O₃
C. NO            D. N₂O

11. A compound has the empirical formula of CH₂O. The molecular formula is__________. [m.m of the compound = 180g/mol] A. CH₂O           B. C₂H₄O₂
C. C₄H₈O₄        D. C₆H₁₂O₆

12. Consider the equation below: XNH_3(g) + 5O_2(g) → 4NO_(g) + 6H₂O_(g). What is the value of X in the equation?
A. 4            B. 3
C. 2            D. 6

13. The quantum number which divides a shell into orbitals is
A. magnetic      B. Azimuthal
C. spin              D. principal

14. The pH of a sample of sachet water was tested to be 6.0, the molar concentration of hydronium ion of the water sample is
A. 1.0 × 10⁶ molar
B. 1.0 × 10^-6 molar
C. 1.0 × 10^-5 molar
D. 1.0 × 10⁷ molar

15. A member of atoms having the same proton number and different neutron numbers is called
A. an isobar
B. an isotope
C. an isotone
D. a nuclear isomer

16. The oxidation number of manganese is +5 in
A. MnO₂           B. K₃MnO₄
C. KMnO₄         D. MnSO₄

17. The group to which an element is placed in the modern periodic table is determined by its number of
A. shielding electrons
B. valence electrons
C. bonding electrons
D. penultimate electrons

18. If the vapour density of a volatile hydrocarbon with the empirical formula of CH₂ is 42, its molecular formula is __________. (C = 12, H = 1)
A. C₆H₁₄           B. C₆H₁₂
C. C₄H₈            D. C₄H₁₀

19. The empirical formula of an organic compound containing 72% carbon, 12% hydrogen and 16% oxygen by mass is__________ (C = 12, O = 16, H = 1)
A. C₃H₈O            B. C₆H₁₂O
C. C₆H₁₂O₂         D. C₇H₁₂O₁₆

20. The instrument used for measuring pH is
A. indicator        B. pH meter
C. litmus            D. hygrometer

21. The percentage by mass of hydrogen in hydrogen ethanoate (CH₃COOH) is __________. (C = 12, O = 16, H = 1)
A. 1.67%         B. 6.67%
C. 5%             D. 60%

22. The percentage by mass of other elements except hydrogen in hydrogen ethanoate (CH₃COOH) is ________. (C = 12, O = 16, H = 1)
A. 6.67%        B. 93.33%
C. 93%           D. 60%

23. The shape of carbon (IV) oxide is
A. pyramidal           B. linear
C. orthogonal         D. tetrahedral

24. If two atoms of an element are represented as ¹¹₅Y and ¹⁰₅X, find the R.A.M. of the element when the percentage by mass of ¹⁰₅X in a natural sample is 20%
A. 10.2           B. 10.4
C. 10.6           D. 10.8

25. The electronic configuration in terms of K, L, M, N … of an atom with 15 electrons is
A. 2, 8, 1            B. 2, 7
C. 2, 8, 5            D. 2, 8, 8, 5

26. The following are the characteristics of ionic compounds except …..
A. they have melting points
B. they consist of ions, making them highly polar
C. they are usually soluble in polar solvents [water] D. they consist of molecules

27. If a non-metal X, with the configuration of 2, 5 reacts with hydrogen gas, what is the formula of the compound formed?
A. XH          B. XH₂
C. XH₃         D. XH₄

28. In ammonium chloride particle, NH₄Cl, the bonds present are
A. covalent only
B. ionic and covalent
C. Covalent and dative
D. Ionic, covalent and dative

29. A solid compound with high melting and boiling points is likely to be
A. a metal
B. covalent
C. electrovalent
D. coordinated

30. Which of the following compound is not classified as a heavy chemical?
A. H₂SO₄             B. C₂H₄
C. CaOCl₂            D. NH₃

31. A mixture of ethanol and kerosene is best separated by
A. chromatography
B. simple distillation
C. separating funnel
D. electrophoresis

32. Which of the following processes is not easily reversible?
A. melting of ice
B. conversion of liquid water to steam
C. rusting of iron
D. magnetization of iron

33. The negatively charged particle in the atom is the
A. positron           B. neutrino
C. electron           D. meson

34. The standard separation technique that can show the different dyes in black ink is
A. ion-exchange chromatography
B. gas phase chromatography
C. paper chromatography
D. column chromatography

35. A balanced stoichiometric chemical equation obeys the law of
A. constant composition
B. multiple composition
C. conservation of mass
D. equivalent proportion

36. P₁V₁ = P₂V₂ is an expression
A. Charles’s law
B. Boyle’s law
C. Graham’s law
D. Avogadro’s law

37. If 10cm³ of hydrogen gas were sparked with 20cm³ of oxygen gas, calculate the volume of oxygen gas consumed.
A. 25cm³          B. 15cm³
C. 10cm³          D. 5cm³

38. 720cm³ of a gas, H₂ diffused through a porous pot in 2 minutes. The rate of diffusion in seconds is
A. 6.0cm³/s          B. 5.0cm³/s
C. 4.0cm³/s          D. 3.0cm³/s

39. How long in seconds will 720cm³ of oxygen gas take to diffuse under similar conditions with H₂ gas in 26 above
A. 6.0cm³/s        B. 12cm³/s
C. 24cm³/s         D. 36cm³/s

40. 2.0 moles of an ideal gas are at a temp. of -13°C and a pressure of 2 atm. What will be the volume of the gas at that temp.?
A. 25.3dm³         B. 23.3dm³
C. 21.3dm³         D. 19.3dm³

41. The acid in oranges is
A. lactic acid
B. citric acid
C. ascorbic acid
D. fatty acid

42. Strong acids are those that
A. ionize partially or slightly in aqueous solution
B. do not ionize at all when dissolved in water
C. ionize completely in water when dissolved
D. None of the above

43. The conjugate base of HNO₃ acid is
A. NO₃^–          B. N^3-
C. NO₂^–          D. NO₂

44. The equation: H⁺_(aq) + OH^–_(aq) → H₂O_(l) represents a
A. displacement reaction
B. combination reaction
C. neutralization reaction
D. precipitation reaction

45. KHSO₄ is an
A. double salt
B. acidic salt
C. basic salt
D. complex salt

46. The concentration of [H⁺] of a solution is 30×10^-3 moldm^-3. What is the P^H of the solution?
A. 1.5            B. 2.5
C. 3.5            D. 4.5

47. The most reactive element known is
A. oxygen           B. sodium
C. caesium          D. fluorine

48. The most abundant element in the universe is
A. oxygen             B. silicon
C. aluminum        D. hydrogen

49. The most abundant element in the earth crust is
A. oxygen              B. silicon
C. aluminum         D. sodium

50. The most abundant metal in the earth crust is
A. aluminum         B. iron
C. gold                  D. copper

51. The most reactive or electropositive metal is
A. caesium            B. sodium
C. potassium         D. iron

52. The number of bonds formed by an atom in a molecule is called
A. valence
B. atomicity
C. oxidation number
D. coordination number

53. The stoichiometric number of hydrogen ions that can be released by a molecule of an acid in water is called
A. basicity          B. acidity
C. molarity         D. molality

54. The valence of oxygen is
A. 2            B. 6
C. 8            D. 4

55. Which of the isotopes of oxygen would you choose to match the percentage abundance of 99.759% in the earth crust?
A. ¹⁶₈O           B. ¹⁷₈O
C. ¹⁸₈O           D. ¹⁹₈O

56. The basicity of orthoboric acid (H₃BO₃) molecule is
A. 1            B. 2
C. 3            D. 6

57. When crystals of Na₂CO₃ · 10H₂O the crystals lose almost all their water molecules to form Na₂CO₃ · H₂O. This phenomenon is called
A. hydration
B. hydrocopy
C. efflorescence
D. deliquescence

58. 3CuO + 2NH₃ → 3Cu + N₂ + 3H₂O (with heat). The oxidation product of the above reaction is
A. Cu               B. N₂
C. H₂O             D. CuO

59. In terms of electron transfer, oxidized specie is defined as
A. substance that gains electron
B. substance that loses electron
C. substance increases in oxidation number
D. substance accepts proton

60. Cu_(s) + 2AgNO_3(aq) → Cu(NO₃)_2(aq) + Ag_(s). This equation can be written in ionic form as follows:
A. Cu_(s) + 2NO_3(aq)^– → Cu(NO₃)_2(aq)
B. Cu_(s) + 2Ag⁺_(aq) → Cu²⁺_(aq) + 2Ag_(s)
C. Cu²⁺_(aq) + Ag⁺_(aq) → Cu_(s) + 2Ag_(s)
D. Cu_(s) + 2Ag_(s) → 2Ag_(s) + Cu²⁺_(aq) + 2Ag_(s)

61. In K₂Cr₂O₇, the oxidation number of Cr is
A. +3             B. +4
C. +6             D. +7

62. ClO₃^– + 6H⁺ + xe^– → Cl^– + 3H₂O. what is the value of x in this half-cell equation?
A. 6            B. 5
C. 4            D. 3

63. Consider the equation PN^3- + qNO₃^– + rH⁺ → XNO₂ + YH₂O the values of q and x are respectively
A. 5 and 6         B. 6 and 7
C. 7 and 8         D. 8 and 9

64. Consider another equation: MnO₄^– + 5Fe³⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O. the oxidation change of Mn in the above equation is
A. +4             B. -5
C. +3             D. -6

65. The specie that is reduced in the equation: 2NaBr_(aq) + Cl_2(aq) → 2NaCl_(aq) + Br_2(l) is
A. Na⁺_(aq)         B. Cl_2(aq)
C. Cl^–_(aq)            D. Br^–_(aq)

66. The equation: Pb²⁺_(aq) + K₂CO_3(aq) → 2K⁺_(aq) + PbCO_3(s) represents
A. displacement
B. double decomposition
C. combination
D. redox

67. Sugar when dissolved in water is a non-electrolyte because
A. it dissociates completely into ions
B. it does not dissociate at all
C. it does not dissolve
D. it is an organic compound

68. Metallic conductors conduct electricity by the movement of
A. ions                B. molecules
C. electrons        D. protons

69. During electrolysis, the type of reaction that takes place at the anode is
A. reduction
B. gain of electrons
C. oxidation
D. decomposition

70. Metallic bond is a very strong bond in metals because
A. repulsion between the nucleus and electrons
B. attraction between the nucleus and electron cloud
C. attraction between the protons and neutrons
D. repulsion between the neutrons and electron cloud

71. Which of the following compounds is covalent?
A. Na₂S          B. MgCl₂
C. K₂O            D. NH₃

72. Which of the following metals will not displace hydrogen ion (H⁺) from a solution of acid?
A. Zn             B. Cu
C. Mg            D. Fe

73. The reaction: Pb²⁺_(aq) + CO₃^2- → PbCO_3(s) is an example of
A. double decomposition
B. combination
C. displacement
D. redox reaction

74. Which of the following substances represents a basic salt?
A. KHSO₄         B. Zn(OH)Cl
C. HNO₃          D. MgCl₂

75. Deliquescent substances are also
A. efflorescent         B. hygroscopic
C. dehydration        D. hydrolysing

76. What is the oxidation number of phosphorus in PO₄^3-?
A. 2           B. 3
C. 4           D. 5

77. The oxidation change of nitrogen in the half cell reaction: NO₃^– + 2H⁺ + 2e^– → NO₂^– + H₂O is
A. -1           B. -2
C. +1          D. +2

78. Consider the equation: 3CuO + 2NH₃ → 3Cu + N₂ + 3H₂O. What is the oxidation product of the above reaction?
A. CuO            B. Cu
C. N₂               D. H₂O

79. ClO₃^– + 6H⁺ + Xe^– → Cl^– + 3H₂O. What is the value of X in the equation above?
A. 4              B. 5
C. 6              D. 7

80. Oxidation in terms of electron transfer is defined as
A. gain of electrons
B. loss of electrons
C. gain of hydrogen
D. loss of oxygen

81. Which of the following substances is an electrolyte?
A. kerosene
B. an aqueous solution of sugar
C. an aqueous solution of NaCl
D. an aqueous solution of ethanol

SECTION B: THEORY/ESSAY

PART A:

Question 1

(a) Copy and complete the following table:

(b) Potassium has two isotopes namely k-39 and k-41. If they relative atomic mass of k is 39.2, find the percentage proportion of each isotope in a natural sample.

(c) An organic compound containing C, H, N and O weighs 1.26g. Under elementary analysis showed 0.624g of carbon, 0.065g of hydrogen and 0.364g of Nitrogen. Find its molecular formula if the relative molecular mass is 194g/mol. [C = 12, H = 1, O = 16, N = 14]

Question 2

(a) Two elements represented by the letter X and Y have atomic number 9 and 12 respectively
i. Write the electronic configuration of X and Y, using s, p, d, f notation
ii. Name the group to which X belongs
iii. Name the period to which Y belongs
iv. Write the formula to the compound formed between X and Y

(b) If 0.50 mole of MgSO₄ · XH₂O has a mass of 123g, calculate the value of X. (H = 1, O = 16, Mg = 24, S = 32)

(c) Hydrogen reacted with oxygen to form steam.

i. Write a balanced equation for the reaction if 50cm³ of Hydrogen were mixed with 20cm³ of oxygen
ii. Calculate the volume of steam produced
iii. Which reaction is in excess and by how much?
iv. What was the total volume of the gaseous mixture at the end of the reaction.

Question 3

(a) i. What is an acid?
ii. What is meant by Basicity of an acid
iii. State three physical properties of a base

(b) State the type of salt represented by each of the following compounds
i. K₄Fe(CN)₆
ii. (NH₄)₂Fe(SO₄)₂ · 6H₂O
iii. Mg(OH)NO₃
iv. NaH₂PO₄

(c) What is meant by the term Strength of an acid?

PART B:

Question 4

(a) Define each of the following terms:
i. Combination reaction
ii. Electrolysis
iii. Thermal decomposition reaction
iv. Electrolyte

(b) Differentiate between; [Note: 3 differences for all]
i. Electrolytes and Non-Electrolytes
ii. Electrolytes and Conductors
iii. Strong Electrolytes and Weak Electrolytes

Question 5

(a) Balance the following half – cell equations:
i. N^3-_(aq) → N_2(g)
ii. MnO_4(aq)^– → MnO_2(s)

(b) Balance the following redox equation
i. Cr₂O₇^2- + H₂O₂ → Cr³⁺ + O_2(g)
ii. MnO₄^– + Fe²⁺ → Mn²⁺ + Fe³⁺

Question 6

(a) Consider the equation:
Pb(NO₃)_2(aq) + 2NaCl_(aq) → PbCl_2(s) + 2NaNO_3(aq)
Write the above equation in three ionic forms

(b) MnO₂ + 4HCl_(aq) → MnCl_2(aq) + Cl_2(g + 2H₂O
Mention the:
i. Oxidizing agent
ii. Reducing agent
iii. Oxidation product
iv. Reduction product of the above reaction

(c) Give the reason why an aqueous solution of NaCl_(aq) conducts electricity while aqueous solution of sugar does not conduct electricity.

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)

Answers to Chemistry Exam Questions for SS2 First Term

Answers to Section A (Objective Test)

The following table gives the correct answers to the objective section of Chemistry exam questions for SS2 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 SS2 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)

PART A

Question 1

(a) Completed Table

(b) Calculation of Percentage Abundance of Isotopes

Let the percentage of K-39 be x%.

Therefore, percentage of K-41 = (100 − x)%.

Average atomic mass:

39x + 41(100 − x) = 39.2 × 100

39x + 4100 − 41x = 3920

−2x = −180

x = 90

Therefore:

• K-39 = 90%
• K-41 = 10%

(c) Determination of Molecular Formula

Mass of oxygen = 1.26 − (0.624 + 0.065 + 0.364)

= 1.26 − 1.053

= 0.207g

Divide all by the smallest value (0.013):

C = 4, H = 5, N = 2, O = 1

Empirical formula = C₄H₅N₂O

Empirical formula mass:

= (4 × 12) + (5 × 1) + (2 × 14) + 16

= 48 + 5 + 28 + 16

= 97

Molecular formula mass = 194

194 ÷ 97 = 2

Molecular formula = (C₄H₅N₂O)₂

= C₈H₁₀N₄O₂

Question 2

(a)

i. Electronic configurations

X (Atomic number 9): 1s² 2s² 2p⁵

Y (Atomic number 12): 1s² 2s² 2p⁶ 3s²

ii. Group of X

X belongs to Group 17 (Halogens).

iii. Period of Y

Y belongs to Period 3.

iv. Formula of compound formed

XY₂ or MgF₂

(b) Calculation of X in MgSO₄ · XH₂O

0.50 mole has a mass of 123g

Therefore molar mass = 123 ÷ 0.50 = 246g/mol

Molar mass of MgSO₄:

= 24 + 32 + (16 × 4)

= 120g/mol

Mass of water = 246 − 120 = 126

18X = 126

X = 7

Therefore, the compound is MgSO₄·7H₂O

(c)

i. Balanced equation

2H_2(g) + O_2(g) → 2H₂O_(g)

ii. Volume of steam produced

2 volumes of H₂ produce 2 volumes of steam.

Therefore, 40cm³ of H₂ will react with 20cm³ of O₂.

Steam produced = 40cm³

iii. Excess reactant

Hydrogen is in excess.

Excess hydrogen = 50 − 40 = 10cm³

iv. Total volume at the end

Steam = 40cm³

Excess hydrogen = 10cm³

Total gaseous mixture = 50cm³

Question 3

(a)

i. Acid

An acid is a substance that produces hydrogen ions (H⁺) when dissolved in water.

ii. Basicity of an acid

Basicity of an acid is the number of replaceable hydrogen ions present in one molecule of the acid.

iii. Three physical properties of bases

• They taste bitter.
• They feel soapy or slippery.
• They turn red litmus paper blue.

(b) Types of salts

• i. K₄Fe(CN)₆ — Complex salt
• ii. (NH₄)₂Fe(SO₄)₂·6H₂O — Double salt
• iii. Mg(OH)NO₃ — Basic salt
• iv. NaH₂PO₄ — Acidic salt

(c) Strength of an acid

Strength of an acid refers to the degree of ionization of the acid in water.

A strong acid ionizes completely while a weak acid ionizes partially in water.

PART B

Question 4

(a) Definitions

i. Combination reaction

A combination reaction is a reaction in which two or more substances combine to form a single product.

ii. Electrolysis

Electrolysis is the chemical decomposition of an electrolyte by the passage of electric current through it.

iii. Thermal decomposition reaction

It is a reaction in which a compound breaks down into simpler substances when heated.

iv. Electrolyte

An electrolyte is a substance that conducts electricity in molten or aqueous state due to the presence of mobile ions.

(b) Differences

i. Electrolytes and Non-electrolytes

ii. Electrolytes and Conductors

iii. Strong and Weak Electrolytes

Question 5

(a) Balanced half-cell equations

i. 2N^3-_(aq) → N_2(g) + 6e^–

ii. MnO₄^– + 4H⁺ + 3e^– → MnO_2(s) + 2H₂O

(b) Balanced redox equations

i. Cr₂O₇^2- + 3H₂O₂ + 8H⁺ → 2Cr³⁺ + 7H₂O + 3O₂

ii. MnO₄^– + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O

Question 6

(a) Ionic equations

i. Complete ionic equation

Pb²⁺_(aq) + 2NO₃^–_(aq) + 2Na⁺_(aq) + 2Cl^–_(aq) → PbCl_2(s) + 2Na⁺_(aq) + 2NO₃^–_(aq)

ii. Spectator ions

Na⁺ and NO₃^–

iii. Net ionic equation

Pb²⁺_(aq) + 2Cl^–_(aq) → PbCl_2(s)

(b)

MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O

• i. Oxidizing agent — MnO₂
• ii. Reducing agent — HCl (Cl^–)
• iii. Oxidation product — Cl₂
• iv. Reduction product — MnCl₂

(c)

An aqueous solution of NaCl conducts electricity because it dissociates into free moving ions (Na⁺ and Cl^–) in water.

Sugar solution does not conduct electricity because sugar does not ionize in water; therefore, there are no free ions to carry electric current.

Read Also: Chemistry Exam Questions for SS1 First Term with Answers

How to Pass Chemistry Exam Questions for SS2 First Term

Passing your Chemistry exam questions for SS2 First term requires a combination of preparation, understanding, and strategy. Here are actionable tips to help you excel:

1. Know the syllabus. Check topics set for the term. Focus on them first. Don’t waste time on off-syllabus items.
2. Make a study plan. Break topics into small parts. study one part each day. Include time for revision and practice.
3. Understand ideas — don’t just memorise. Learn why reactions happen. Practice writing equations until they become natural.
4. Memorise key facts and formulas. Write important numbers, gas tests, and formulas on a single sheet. Read it daily.
5. Practice past questions. Do real exam questions under timed conditions. Mark yourself and learn from mistakes.
6. Master practical skills. Know common lab procedures, observations and safety points. Practical questions often come in theory form.
7. Answering objective questions (MCQs). Read the stem carefully. Cover the options and think of an answer first. Then confirm with the choices.
8. Answering theory questions. Start with a short definition. Use numbered points. Give equations where needed. Finish with a short conclusion.
9. Draw clear diagrams. Label parts neatly. A neat diagram can earn marks fast. Practice common diagrams: apparatus, fractionating column, electron dot structures.
10. Show your working. For calculations, write each step. Examiners give marks for method even if the final number is slightly wrong.
11. Manage your time in the exam. Answer easy questions first. Allocate time for each section. Leave 10 minutes at the end to check your paper.
12. Use correct units and significant figures. Avoid losing marks for missing units. Give answers to the required number of significant figures when asked.
13. Keep neat handwriting. Illegible answers may be misunderstood. Write clearly and use paragraphs or bullet points.
14. Stay calm and rest well. Sleep the night before. Eat a light breakfast. A calm mind thinks better.
15. After the exam. Check the paper and learn from errors. Make a note of areas to improve for next time.

Work every day. Practice with purpose. You will pass if you prepare well.

It’s a wrap!

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