Classification of Matter - MCQ and Fill in the blank questions with answer

Fill in the blanks

1. A substance that is made up of only one type of atom is called a(n)_______________.
2. Two or more substances physically combined form a(n)______________.
3. Two or more substances chemically combined are called a(n)_______________.
4. Sand is a good example of a(n) ______________ mixture.
5. _______________ elements, such as oxygen (O2), are found in nature in their elemental form as two-atom molecules.

MCQ

6. Which of the following substances cannot be broken down by ordinary chemical reactions?
a) water c) carbon dioxide b) gold d) glucose

7. Which of the following substances does not possess uniform composition?
a) pure water b) salt water c) helium gas d) salad

8. Which of the following is made up of only one type of atom?
a) NO b) He c) CO d) MgS

9. Which of the following represents a mixture?
a) NaCl(s) b) NaCl(l) c) NaCl(g) d) NaCl(aq)

10. Which of the following shows a ternary compound?
a) CO b) NaCl c) NH3 d) NaNO2

Answer Key
The actual answers will be shown in brackets, followed by the explanation.


1. [element]

2. [mixture]—You might have said “solution, “homogeneous mixture,” or
“heterogeneous mixture,” which are also true answers. “Mixture” is the
most general of the possible correct answers.

3. [compound]—Remember: The key is that the elements in a compound are
chemically combined. If the question asked about things that are physically
combined, the answer would have been a “mixture.”

4. [heterogeneous]—Sand is composed of particles of different substances,
mixed together in a non-uniform distribution.

5. [diatomic]—“Diatomic” means “two-atom,” so think of O2 or H2 when you
see it.

6. [B. gold]—Gold is an element, and elements can’t be broken down into
simpler substances by ordinary chemical means.

7. [D. salad]—We toss a salad to try to make its composition more uniform,
but it never becomes truly uniform.

8. [B. He]—NO, CO, and MgS all represent compounds. We can tell because
they all contain more than one capital letter and, therefore, more than one
elemental symbol.

9. [D. NaCl(aq)]—The “(aq)” indicates that the salt has been dissolved in water,
making it a mixture of two or more substances physically combined.

10. [D. NaNO2]—A ternary compound contains three different elements.
Sodium nitrite (NaNO2) contains the elements sodium, nitrogen, and
oxygen, so it fits the definition.

Phases of Matter: Fill in the blanks with answer

1. _______________ is the process by which a gas becomes a liquid.
2. _______________ is the process by which a liquid becomes a gas.
3. The normal boiling point of water is __________.
4. The _______________ of a liquid is its resistance to flow.
5. _______________ is the process by which a solid turns directly to a
gas.
6. _______________ have definite shape and definite volume.
7. _______________ is the process by which a solid turns to a liquid.
8. _______________ is the process by which a gas turns directly to a
solid.
9. _______________ is the process by which a liquid becomes a solid.
10. True solids are said to possess ______________ structure.

Answer

1. [condensation]—If you go outside on a cool morning, you may find
condensation on many cool surfaces.
2. [vaporization]—The steam that you see coming from a teapot is the result
of vaporization.
3. [100 oC or 373 K]—You will learn more about the Kelvin scale in Chapter 2.
4. [viscosity]—Liquids with a great deal of viscosity are very resistant to flow.
5. [sublimation]
6. [solids]—Solids don’t take the shape and size of their containers.
7. [fusion]—The term fusion is also used for a nuclear process that we will
discuss in Chapter 6.
8. [deposition]—When water vapor “freezes” onto a cold surface, deposition
is taking place.
9. [solidification]—This is the process that we normally call “freezing.” Many
people associate the term “freezing” with “cold,” but the process of
solidification can happen at relatively high temperatures for some substances.
10. [crystalline]

Chemical Kinetics : Fill in the blanks exam chemistry questions part 2

16. By __________ the surface area of the reactants, the rate of reaction is increased.

17. Rate of reaction generally __________ with the rise of temperature.

18. A __________ is a substance, which either accelerates or retards the rate of reaction without taking part in the reaction.

19. In the preparation of Oxygen from Potassium Chlorate, __________ is used as catalyst.

20. In the oxidation of SO2 to SO3 by the contact process for the manufacture of H2SO4 __________ is used as catalyst.

21. An unstable intermediate compound formed during a chemical reaction is called __________.

22. When a catalyst and the reactants are in the same phases, it is known as __________ catalyst.

23. When a catalyst and the reactants are in different phases, it is called __________.

24. When a catalyst increases the rate of reaction, it is called __________ catalyst.

25. When a catalyst retards the rate of reaction, it is called __________ catalyst.

26. A negative catalyst __________ the energy of activation, hence the rate of reaction is decreased.

27. The ratio between the rate of reaction and concentration of reactants is known as __________.

28. Velocity constant is independent of concentration but depends on __________.

29. Ionic reactions are __________ than molecular reactions.

30. The value of specific rates constant for a reaction __________ with time.

31. The sum of all exponents of concentration terms in the equation is called __________.

32. The sum of moles taking part in a chemical reaction is called __________ of the reactions.

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Solutions and Electrolytes: Fill in the blanks type chemsitry questions Part -1

1. A mixture of two or more substances, which are homogeneously mixed, is called a __________.

2. __________ is defined as the amount of solute dissolved in a given amount of solvent.

3. A solution is composed of two components __________ and __________.

4. A solution containing one mole of solute per dm3 of solution is called one __________ solution.

5. Molarity is denoted by __________.

6. 1M solution of NaOH contains __________ gms of it dissolved per dm3 of solution.

7. A solution containing one mole of solute dissolved by per kg of solvent is called __________ solution.

8. Molality is denoted by __________.

9. 1M solution of H2SO4 contains __________ gms of it per kg of solvent.

10. The process in which ions are surrounded by water molecules is called __________.

11. The water molecules attached with the hydrated substance are called __________.

12. Hydrated copper sulphate evolves __________ water molecules on heating.

13. The interaction between salt and water to produce acids and bases is called __________.

14. The products of ionic concentration in a saturated solution at a certain temperature are called the __________.

15. Solubility product constant expressed as __________.

16. The suppression of ionization by adding a common ion is called __________.

17. The process of dissociation of an electrolyte into ions is known as __________.

18. The chemical decomposition of a compound in a solution or in fused state brought about by a flow of electric current is known as __________.

19. Electrolysis is performed in an electrolytic cell, which is known as __________.

20. The positive electrode of a voltmeter is called __________ and negative as __________.

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Chemical Equilibrium-Fill in the blank type exam question Part 2

21. __________ is purified in industries by Common Ion Effect.

22. A reaction moves to the left when the concentrations of the products are __________.

23. A reaction moves to the right when the concentrations of the products are __________.

24. Increase in pressure will move the reaction in the direction of __________ volume.

25. Decrease in pressure will move the reaction in the direction of __________ volume.

26. An increase of temperature favours the formation of products in case of __________ reaction.

27. A decrease of temperature fovours the formation of products in case of __________ reaction.

28. Heating moves an endothermic reaction to the __________.

29. Cooling move an exothermic reaction to the __________.

30. The product of ionic concentration in a saturated solution is called __________ constant.

31. When HCl is added to NaCl, the concentration of __________ ion is increased.

32. Chemical reaction involving the substances in more than one phases are called __________.

33. The formation of NH3 is exothermic process hence __________ temperature will favour the formation of NH3.

34. The formation of NO from N2 and O2 is endothermic process hence __________ temperature will favour the formation of NO.

35. Chemical Equilibrium is __________ equilibrium.

36. Molar concentration is also called __________.

37. The rate at which a substance takes part in a chemical reaction depends upon its __________.

38. __________ principle is applied to all reversible reaction.

39. A common ion __________ the solubility of the salt.

40. Number of moles present per dm3 of a substance is called __________.

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Chemical Equilibrium-Fill in the blank type exam question Part 1

1. The reactions, which proceed in both the directions, are called __________ reactions.

2. The reactions, which proceed to one direction only, are called __________ reactions.

3. Reversible reactions are __________ completed.

4. Irreversible reactions are __________ after some time.

5. A reversible reaction is said to be in __________ when the rate of forward reaction becomes equal to the rate of backward reaction.

6. The concentrations of reactants and products are __________ at equilibrium point.

7. The value of Kc depends upon the __________ of the reactants.

8. A increase of the value of Kc tends to move the reaction to the __________ direction.

9. A decrease of the value of Kc tends to move the reaction to the __________ direction.

10. An increase in the concentration of the reactants will move the reaction to the __________ direction.

11. A decrease in the concentration of the reactants will move the reaction to the __________ direction.

12. Equilibrium constant is denoted by __________.

13. When the equilibrium constant value is very __________, we can conclude that the forward reaction is almost completed.

14. When equilibrium constant value is very __________ we can conclude that forward reaction will occur to very little extent.

15. According to __________ principle, if system in equilibrium is subjected to a stress, the equilibrium shifts in a direction to minimize or undo the effect of the stress.

16. In exothermic reaction, the __________ of temperature favour the forward rate of reaction.

17. In endothermic reactions, the __________ of temperature favour the forward rate of reaction.

18. A __________ is a substance which effects the rate of reaction but remains unaltered at the end of the reaction.

19. A catalyst increases the velocity of the reaction by decreasing the __________.

20. The suppression of degree of ionization of a sparingly soluble weak electrolyte by the addition of a strong electrolyte containing an ion in common is called __________.

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