Chemistry 9 Full Book Test

Question ListCategory: Chemistry Class 9Chemistry 9 Full Book Test
Teacher Staff asked 1 year ago

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 Paper: Chemistry              Class: 9           Time Allowed: 30 Mins                  Marks: 12 

NOTE: You have four choices for each objective type question as a, b, c and d. The choice which you think is correct; fill that circle in front of that question number. Use marker or pen to fill the circle. Cutting or filling two or more circles will result in zero mark in that question.
Q.1 (MCQ)
1. Industrial chemistry deals with the manufacturing of compounds:
(a) in the laboratory     (b) on micro scale      (c) on commercial scale       (d) on economic
2. Which one of the following can be separated by physical methods:
(a) mixtures        (b) elements         (c) compounds         (d) radicals
3. Which one of the following results in the discovery of proton:
(a) Cathode rays        (b) Canal rays          (c) X-rays         (d) Alpha rays
4. Which one of the following is the most penetrated in the particles of matter?
(a) Protons        (b) Electrons         (c) Neutrons         (d) Alpha particles
5. The atomic radii of the elements in Periodic Table:
(a) increase from left to right in a period     (b) increase from top to bottom in a group
(c) decrease from top to bottom in a group     (d) do not change from left to right in a period
6. The amount of energy given out when an electron is added to an atom is called:
(a) lattice energy         (b) ionization energy      (c) electronegativity       (d) electron affinity
7. Atoms react with each other because:
(a) they are attracted to each other        (b) they are short of electrons
(c) they want to attain stability               (d) they want to disperse
8. An atom having six electrons in its valence shell will achieve noble gas electronic configuration by:
(a) gaining one electron              (b) losing all electrons
(c) gaining two electrons            (d) losing two electrons
9. How many times liquids are denser than gases?
(a) 100 times                (b) 1000 times              (c) 10, 000 times                 (d) 100.00
10. Gases are the lightest form of matter and their densities are expressed in terms of:
(a) mg cm -3              (b) g cm -3              (c) g dm -3               (d) kg dm -3
11. Mist is an example of solution:
(a) liquid in gas             (b) gas in liquid              (c) solid in gas                     (d) gas in solid
12. Which one of the following is a ‘liquid in solid’ solution?
(a) sugar in water              (b) butter                    (c) salt in water            (d) fog

 

 Paper: Chemistry            Class: 9         Time Allowed: 2:30 Hours                 Marks: 63 

PART- I (Short Questions)

Q.2 Write short answers to any six (6) questions: (6 × 2 = 12)
(i) How can you differentiate between organic and inorganic chemistry?
(ii) What is empirical formula of acetic acid (CH3COOH)? Find out its molecular mass.
(iii) Difference between Atom and Gram Atom?
(iv) Write two / four properties of canal rays.
(v) Describe the defects of Rutherford’s atomic model.
(vi) State Newland’s law of octaves.
(vii) What is an ionic bond? Give two examples of ionic compounds.
(viii) Differentiate between a lone pair and a bond pair of electron.
(ix) Sort out ionic and covalent compounds from the following:
HF, NaCl, H2O, NH3, O2, MgO, H2SO4, N2, CH4

Q.3 Write short answers to any Five (5) questions: (5 × 2 = 10)
(i) Define diffusion. How diffusion occurs in gases?
(ii) What is the difference between a solution and an aqueous solution?
(iii) Define solute and solvent with examples.
(iv) What is the effect of temperature on the solubility of salts like Li2SO4 and Ce2(SO4)3 in water?
(v) We desire to prepare 100 cm3 0.4 M solution of MgCl2, how much MgCl2 is needed?
(vi) What will happen if the solute-solute forces are stronger than those of solute-solvent forces?
(vii) Why is the melting point of a solid considered its ‘identification characteristic?
(viii) What is the relationship between evaporation and boiling point of a liquid?

Q.4 Write short answers to any Five (5) questions: (5 × 2 = 10)
(i) Define the term allotropy with examples.
(ii) Define oxidation in terms of addition or removal of oxygen or hydrogen. Explain with examples.
(iii) Find out the oxidation number of underlined element in Na2SO4.
(iv) Discuss, why galvanizing is considered better than that of tin plating.
(v) How can we distinguish a metal from a non-metal by simple physical methods?
(vi) How does oxygen react with group IIA alkaline earth metals?
(vii) Why the cations are smaller and anions are bigger in size than their respective neutral atoms.
(viii) Discuss, why the soften and hardness of metal depend upon the metallic bonding?

PART – II (Long Questions)

NOTE: Attempt any THREE Questions. (3 × 7 = 21)
Q.5 (a) Enlist and explain different branches of chemistry. Also describe the Scope / applications of each
branch in daily life. (4)
(b) What is a metallic bond? Explain metallic bonding with the help of a diagram. (3)
Q.6 (a) Describe some typical properties of solids. (4)
(b) A solution contains 50g of sugar dissolved in 450 g of water. What is concentration of this
solution? (3)
Q.7 (a) How we can prepare NaOH on commercial scale. Discuss its chemistry along with the
diagram. (4)
(b) Describe the reactions of halogens. (3)
Q.8 (a) Give the applications of isotopes in the field of radiotherapy and medicines. OR (4)
Describe the uses of isotopes in different field of life.
(b) Discuss the important features of modern periodic table. OR (3)
Write down some salient features of long form of periodic table.
Q.9 (a) It is desired to increase the volume of a fixed amount of gas from 87.5 to 118cm3 while holding
the pressure constant. What would be the final temperature if the initial temperature is 23oC? (4)
(b) What is the general principle of solubility? Discuss the effect of temperature on solubility. OR
What is solubility? Describe the factors that are effected on solubility. (3)

PART – III (Practical Questions)

NOTE: Attempt any TWO questions. (Practical Part) (2 × 5 = 10)
Q. 10 (a) (i) Which of the following methods will be used to separate the mixture containing common salt
and sand? (2)
(a) Sublimation (b) Filtration after shaking with water
(c) With the help of bar magnet (d) With the separating funnel
(ii) How much NaOH will be required to prepare 0.1 M of its 100cm3 solution? (3)
(b) (i) Very often salt is added to water when boiling an egg? Can you think of a reason to do so? (2)
(ii) Which materials are attracted by a magnet? (3)

Material Attracted by Magnet or Not Yes No

MaterialAttracted by Magnet or Not
 YesNo
(i)           Plastic  
(ii)          Copper  
(iii)         Brass  
(iv)         Nickel  
(v)          Iron Nails  
(vi)         Zinc  
(vii)        Gold  
(viii)         Wood  

(c) (i) Name the method which can be used to separate boiled rice from water in the kitchen. (2)
(ii) Calcium is necessary for healthy teeth and strong bones. The mineral water bottles contain (3)
approximately 55mg / dm3 Ca2 + ions. Calculate the polarity of calcium ions in the mineral
water?

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