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Chemistry Examination Question for SS1(Senior Secondary School 1)


  • Searching for Chemistry Examination questions for senior secondary school students in class 1? Here in this page we’ve put together over 20 Chemistry examination questions for SS1 Students.


  1. Chemistry can be applied in the following fields EXCEPT A. Agriculture Oil and gas  C. Politics  D. Metallurgy
  2. Separation of mixtures of solids with various sizes can be done A. Magnetic separation B. Coarsing C. Sublimation   D. Sieving
  3. Which of the following is an example of a chemical change? A.Dissolution of salt in water B. Rusting of iron C. Melting of ice  D.Separating of mixture by distillation
  4. These are basic particles from which matter could be made EXCEPT A. Salt B. Atoms C. Ions   D. Molecules
  5. A molecule of neon is A. Diatomic Ionic  C. Triatomic  D. Minoatomic
  6. Which of these requires crystallization most? A. Drug making Cement making  C. Paint making  D. Perfume making
  7. Which one is the odd-one out? A. Air Urine  C. Brass  D. Sand
  8. Chemical hypothesis is different from chemical law that A. Hypothesis is not reasonable explanation to observation made while law is reasonable Hypothesis is a reasonable explanation to observations while law is a statement from a scientist   C. Hypothesis is a reasonable explanation to observations while law is a statement which confirms the hypothesis after extensive tests  D. None of the above
  9. Separating funnel is used for separating a mixture of A. Liquids with different boiling points  Liquids with sediment  C. Liquids with different colour  D. Liquids that are immiscible
  10. The simplest unit of water that retains its properties is called? An atom   B. An element  C. An hydroxide   D. A molecule
  11. Of the basic particles that make up an atom, the one with the smallest mass is A. A proton A neutron   C. An     D. An electron
  12. The atomic mass of an element is mostly due to the mass of A. Electrons and protons Electrons and neutrons  C. Protons and neutrons D.Positions and neutrons
  13. One of the following is NOT a branch of chemistry Analytical chemistry   B. Medicinal chemistry  C. Organic Chemistry  D. Hybrid chemistry
  14. One of these professions has no need for chemistry A. Mining B. Engineering C. Philosophy D. Geology
  15. How many molecules are there in 1 mole of chlorine molecules? A. 35.5 molecules 6.02 x 10-23 molecules  C. 17.0 molecules  D. 6.02 x 23 molecules
  16. A heterogeneous mixture can be defined as any mixture A. Whose compositions combine to produce a uniform substance Whose compositions combine to produce a non-uniform substance  C. Formed by solids and liquids  D. Of a solute and a solvent
  17. Atomicity of Ozone is A. 1 2    C. 3   D. 4
  18. The relative molecular mass of Lead (ii) trioxonitrate (v) is? (Pb = 207,

N = 14, O = 16) A. 170  B. 222   C. 232  D. 132

19. The percentage of oxygen in sulphur(iv) oxide is (S = 32, O=16) A. 5%   50%   C. 500%   D. 25%

20. The empirical formula of CH6 is CH  B. C3H3   C. C6H6   D. 3CH

21. Which of the following techniques can be used to obtained ethanol from a mixture of ethanol and water? A. Boiling  B. Chromatography  C.Crystallization D. Distillation

22.What is the relationship between empirical formula and molecular formula? A. Empirical formula = Molecular formula Empirical formula  = n x molecular formula (n=1,2,3…)   C. Molecular formula = n x Empirical  formula (n = 1, 2,3…) D. Molecular formula x Empirical  formula = 1

23. Based on the IUPAC way of representing symbols, the symbol for Iron is A. He   Ir    C. Ion  D. Fe

24.Calculate the percentage by mass of Lead in 1 mole of Pb (NO3)2

(Pb = 207; N = 14, 0 = 16) A. 76.9%   b. 62.5%   C. 77.5%   D. 87.3%

25. How many moles of magnesium atoms are present in 0.80g of magnesium? (Mg = 24) A. 0.003mole 0.30mole  C. 0.33mole  D.0.03mole

26. Modern standard element with which chemists define relative atomic mass  is A. 12C    13C    C. 3H   D. 14C

27.Which of the following are mixtures? (i) Petroleum (ii) Rubber latx  (iii) Vulcanizers solution (iv) carbon (ii) sulphur  i, ii and iii   B. i, ii and iv   C. i  and iii only  D. i  and iv

28. Which of the following substances is NOT a homogenous mixture? A.Filtered seawater B. Soft drink c. Flood water   D. writing ink

29.Fractional crystallization is a method of separating A. Crude oil B.Liquid-liquid mixture C. coal D. solids of different solubilities in a liquid

30. There are three main states of matter; liquid, solid, and gas. All have different properties. Which statement describes the physical state of a solid but not a liquid or gas? A. It has its own shape It does not have its own shape  C. It takes the shape of its container   D. It changes shape with temperature



SECTION B – THEORY

Instruction: This section is divided into two parts. Attempt only ONE question in part I and any THREE (3) questions in Part II


PART I [40MARKS]

  1. Using a neat diagram, explain how a mixture of two immiscible liquids of your choice can be separated.

2a.     Define the terms (i) mixture  (ii)compound. Give three differences between them

  1. Classify the following substances as an element, a mixture or a compound (i) Limestone (ii) Diamond  (iii) Sand (iv) Soil (v) Urine (vi) Bronze  (vii) Sugar (viii) Gold   (ix) Clay  (x) Urea  (xi) Antimony   (xii) Soap (xiii) Milk  (xiv) Air  (xv) Neon  (xvi) Iron
  2. Why is sodium chloride solution regarded as a mixture?
  3. How would you separate the components of the following mixtures?

(i) A mixture of sodium chloride and ammonium chloride  (ii) A mixture of Iron dust and zinc dust  (iii)A mixture of water and sugar

(iv) A mixture of two solids which have widely different solubilitus in water  (v) A pure solid from a concentrated solution of its salt.

PART II  [ 60 MARKS]


  1. State Dalton’s atomic theory and its corresponding modification

4a.     How is a Homogenous mixture different from a Heterogeneous mixture?

  1. Classify each of the following changes as either a physical change or a chemical change

(i)       The addition of water to quicklime

(ii)      The melting of candle ware

(iii)     The change in colour of zinc oxide from white to yellow when

Heated

(iv)     The hardening of cement by the absorption of carbon(iv) oxide

(v)      The addition of a base to an acid to form salt and water only


5a.     Define the relative atomic mass of an element

  1. Calculate the relative molecular mass of;
  2. Slaked lime, Ca(OH)2
  3. Sodium trioxonitrate(v), NNO­3

iii.      Hydrated copper(ii) tetraoxosulphate(vi), CuSO4 – 5H2O

  1. What do you understand by the atomicity of an element?

(Ca = 40; O = 16;  H=1; Na = 23; N = 28; S = 32; Cu = 64)

  1. Find the empirical formula of a compound which on analysis yields the following as the reacting masses. Carbon = 2.0g, hydrogen = 0.34g, Oxygen = 2.67g. from your result, find the molecular formula of the compound, if its relative molecular mass is 60.

7a.     Define the following

(i) Mole   (ii) Molecule   (iii) Iron   (iv) atom

  1. How many moles are there in 20g of CaCO3?
  2. Calculate the percentage by mass of nitrogen in trioxonitrate(v) acid
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