Ss 3 Chemistry Exams 2nd Term

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SS 3 Chemistry Exams 2nd Term

SECTION A

1. ____ is an example of radiation (a) Aloha (b) Carbon (c) Uranium (d) Nucleus.
2. Alpha particle was deflected towards negative plate while Beta deflected toward (a) Neutral plate (b) Negative plate (c) Zero plate (d) positive plate
3. Examples of radioactive elements are except (a) Uranium (b) Polonium (c) Thorium (d) Oxygen
4. ²³⁵ ₉₂U + ¹n → ^{141 ­} ₅₆Ba + ⁹² ₃₆Kr + 3 ¹ ₀n

The above nuclear reaction represents (a) nuclear fission (b) nuclear fusion (c) oxidation reaction (d) esterification reaction.

1. ²³⁸ ₉₂U ²³⁴ ₉₀Th + A. In the equation, A represents (a) hydrogen (b) beryllium

(c) helium (d) oxygen

1. Chain reaction helps during the preparation of ____ (a) Solar bomb (b) atomic bomb (c) hydrogen bomb (d) nuclear fusion
2. A lone pair of electron is found in (a) ammonia (b) methane (c) water (d) carbon(iv) oxide
3. Examples of covalent molecules with linear shapes are except (a) oxygen (b) hydrogen (c) water (d) hydrogen chloride
4. Example of compound with double bonds is (a) water (b) carbon(iv) oxide (c) methane (d) ammonia
5. The following are types of crystalline solid except (a) covalent (b) ionic (c) metallic (d) methane
6. Both metallic substance and electrovalent compound are similar because (a) Both dissolve readily in water. (b) they have low melting point. (c) they can conduct electricity. (d) they have low boiling point.
7. The dotted line in an intermolecular bond stands for ____ (a) oxygen (b) hydrogen bond (c) ionic bond (d) covalent bond
8. Vander Wall force of attraction can be grouped as (a) Strongest force (b) hydrogen bond

(c) weakest force (d) ionic bond.

1. Metallic bond can easily be identified by the presence of (a) positive charge (b) negative charge (c) neutral charge (d) double bonds.
2. Which of these is not an alkali? (a) Sodium hydroxide (b) Potassium hydroxide (c) Aqueous ammonia (d) none of the above
3. Which compound is added to fused NaCl to lower its melting point? (a)CaCO₃ (b) CaCl₂

(c) Ca(OH)₂ (d) Ca(NO₃)₂

1. NaHCO₃ is also called? (a) Chalk (b) Baking powder (c) Lime (d) Slaked lime
2. What is the colour of sodium flame (a) white (b) red (c) black (d) green
3. The great affinity of aluminium for oxygen at high temperatures is employed in the

A. electrolytic process B. thermit process C. Haber process D. lead chamber process

1. Aluminium materials should not be exposed to alkalis because aluminium is A. basic B. acidic C. an oxidizing agent D. a reducing agent
2. Wrought iron is the A. purest form of iron B. most brittle form of iron C. most impure D. form of iron containing no carbon
3. Which one is the most common iron ore? A. Magnetite B. Haematite C. Carnallite D. Dolomite
4. One of the following gives ‘pop’ sound when contact with lighted splint. (a) O₂ (b) H₂ (c ) NH₃

(d) CO₂

1. Example of cations that gives gas during its confirmatory test is (a) SO₃^2- (b) SO₄^2- (c) CO₃^2-

(d) NH₄⁺

1. Deep green colour of flame indicate the presence of (a) sodium (b) calcium (c) copper (d) iron
2. The only alkaline gas that changes moist red litmus paper to blue is (a)NH₃ (b) HCl (c) NaOH (d) NH₄OH
3. Brown ring test is used to confirm (a) S^2- (b)NO^3- (c) SO₄^2- (d) SO₃^2-
4. The presence of SO₃^2- change the colour of acidified K₂Cr₂)⁷ from (a) green to red (b) purple to colourless (c) orange to green (d) green to orange
5. A greenish yellow gas that change moist iodide paper black is (a) Cl₂ (b) SO₂ (c) H₂ (d) O₂
6. Sometimes in the presence of conc HsSO₄, copper turning and heat NO^3- gives (a) brown ring reaction (b) pure brown fume (c ) reddish brown (d) effervescence
7. X which fumes in most air can be suitably stored (a) under paraffin or naphtha (b) In a white bottle (c) inside a corked conical flask (d) inside a burette.
8. The observation in bubbling SO₂ into acidified KMnO₄ solution is (a) The solution turns to green (b) the solution becomes decolourized (c) no visible reaction (d) the solution turns steam
9. The two substances that can give both H₂ and ZnSO₄ when added to H₂SO₄ are: (a) Magnesium and Zinc (b) Magnesium and CuO (c) Sodium and NaOH (d) iron and copper
10. C + water give colourless solution (a) c is a soluble salt (b) c is partially dissolve in water (c) c is a filterate (d) c is a residue

SECTION B (THEORY)

1. State what would observe on
2. mixing Zinc dust with CuSO₄ solution
3. adding concentrated HNO₃ to freshly prepared FeSO₄ solution
4. State the colour of these solutions a. KMnO₄ b. K₂Cr₂O₃ c. HOBr d. CuSO₄.5H₂O e. Ca(OH)₂
5. State the flame test for the following :

a. Calcium b. Copper c. sodium d. iron

1. (a) Write the electronic configuration of iron?

(b) Iron forms the iron(II) ion, Fe²⁺ and the iron(III) ion, Fe³⁺.

1. Write the electronic configurations of these ions.
2. Which of them is more stable?
3. Give reason for your answer.
4. Why is it necessary to concentrate the ore before extraction of any metal?
5. State four properties of the following chemical bonds:
6. Electrovalent bond
7. covalent bond
8. dative bond
9. hydrogen bond
10. metallic bond
11. Explain the following simple covalent molecules and draw their shape (a) methane (b) Water (c) carbon (iv) oxide.
12. Explain briefly the principle of the operation of a nuclear power plant
13. State the three main type of radiation with their properties each.