Five Year Papers

1.         The process in which a solid directly changes to vapours without melting is called __________.

(Evaporation, Condensation, Sublimation)

2.         The oxidation number of P in PO^3-₄ is __________.

(3+, 5+, 3-)

3.       The pH of 0.001 M HCl is __________.

(2, 4, 3)

4.         K ( rate constant) is dependent on __________.

(temperature, concentration, volume)

5.         The universal indicator in water shows the colour __________.

(red, green, blue)

6.         The pH of blood is __________.

(7.3, 8.4, 5.6)

7.         The oxidation potential of hydrogen electrode is __________.

(0.0           volt, +0.76volt, -0.36volt)

8.         __________ quantum number describes the shape of a molecule.

(Pricipal, Azimuthal, Spin)

9.         An orbital can have the maximum number of two electrons but with opposite spin, it is called __________.

(Pauli’s Exclusion Principle, Hund’s Rule, Aufbau Principle)

10.     When a-particle is emitted from the nucleus of radioactive element, the mass number of the atom __________.

(Increases, Decreases, Does not change)

11.     Dissociation of KclO3 is a __________ process.

(Reversible, Irreversible)

12.     The e/m ratio of cathode rays is the __________ when Hydrogen is taken in the discharge tube.

(Lowest, Highest)

13.     The negative ion tends to expand with the __________ of negative change on it.

(Decreases, Increases)

14.     Ionic compounds have __________ melting points.

(Low, High)

15.     The allotropic forms of an element are called __________.

(Polymorphs, Isomorphs)

16.     Absolute Zero is equal to __________.

(273.16°C, -273.16°C)

17.     The compounds having hydrogen bond generally have __________ boiling points.

(High, Low)

18.     Surface tension __________ with the rise of temperature.

(Increases, Decreases)

19.     Mercury forms __________ meniscus in a glass tube.

(concave, convex)

20.     The reactions with the high value of energy of activation are __________.

(slow, fast)

21.     2.000 has/have __________ significant figure(s).

(1, 4)

22.     E + PV is called __________.

(Entropy, Enthalpy)

23.     The shorter the bond length in a molecule, the __________ will be bond energy.

(Lesser, Greater)

24.     Positive rays are produced from __________.

(anode, Cathode, Ionization of gas in a discharge tube)

25.     __________ of the following contains the fewer number of molecules.

(1 gm of hydrogen, 4 gm of oxygen, 2 gm of nitrogen)

26.     the true statement about the average speed of the molecules of hydrogen, oxygen and nitrogen confined in a container is __________.

(Hydrogen is quicker, Oxygen is quicker, The molecules of all the gases have the same average speed)

27.     The correct statement about the glass is __________.

(It is crystalline solid, Its atoms are arranged in an orderly fashion, It is a super cooled liquid)

28.     When a substance that has absorbed energy emits it in the form of radiation the spectrum obtained is __________.

(Continuous Spectrum, Line Spectrum, Emission Spectrum)

29.     __________ of the overlap forms strong bond.

(S-S, P-S, P-P)

30.     __________ compound has a greater angle between a covalent bond.

(H₂O, NH₃, CO₂)

31.     When sodium chloride is mixed in water then __________.

(pH is changed, NaOH and HCl are formed, Sodium and chloride ions become hydrated)

32.     The boiling point of a liquid __________ with an increase in pressure.

(Decreases, Increases, remains constant)

33.     An Azimuthal Quantum Number describes the __________.

(size of an atom, shape of an orbital, spin of orbital)

34.     The rate of the backward reaction is directly proportional to the product of the molar concentration of __________.

(Reactants, Products, None of them)

Chapter 1

Introduction To Fundamental Concepts

 

1.       The formula, which gives the simple ratio of each kind of atoms present in the molecule of compound, is called __________.

(Molecular Formula, Empirical Formula, Structural Formula)

2.      The formula, which expresses the actual number of each kind of atom present in the molecule of a compound, is called __________.

(Empirical Formula, Molecular Formula, Structural Formula)

3.      Mole is a quantity, which has __________ particles of the substance.

(One billion, 6.02 x 10²³, 1.013 x 10⁵)

4.      The simplest formula of a compound that contain 81.8% carbon and 18.2% hydrogen is __________.

(CH₃, CH, C₂H₆)

5.      The empirical Formula of a compound __________.

(is always the same as the molecular formula, Indicates the exact composition, Indicates the simplest ratio of the atoms)

6.      Very small and very large quantities are expressed in terms of __________.

(significant figures, Exponential Notation, Logarithm)

7.      Two moles of water contains __________ molecules.

(6.02 x 10²³, 1.204 x 10²⁴, 3.01 x 10²³)

8.      One mole of Cl^- ions contains __________ ions.

(6.02 x 10²³, 1.204 x 10²⁴, 3.01 x 10²³)

9.      220 gms of CO₂ contains __________ moles of CO₂.

(One, Five, Ten)

10.  In rounding off __________ figure is dropped.

(First, Last, No)

11.  Precision is linked with __________.

(Individual measurements, Actual results, Accepted Value)

12.  Accuracy refers to how closely a measured value agrees with __________.

(Individual result, Actual result, Average value)

13.  6600 contains __________ significant figures.

(2, 3, 4)

14.  3.7 x 10⁴ contains __________ significant figures.

(2, 3, 5)

15.  9.40 x 10^-19 contains __________ significant figures.

(2, 3, 5)

16.  The figure 39.45 will be rounded off to __________.

(39.4, 39.5, 39)

17.  __________ means that the result obtained in different experiments are very close to the accepted values.

(Accuracy, Precision, Significant Figure)

18.  The average weight of atoms of an element as compared to the weight of one atom of carbon taken as __________ is called the atomic weight.

(12, 13, 14)

19.  58.5 is __________ of NaCl.

(Atomic weight, Formula Weight, Molecular Weight)

20.  18.0 a.m.u is the __________ weight of water.

(Atomic, Formula, Molecular)

21.  28 gms of nitrogen will have __________ molecules.

(6.02 x 10²³, 12.04 x 10²³, 3.01 x 10²³)

22.  22.4 dm³ of CO₂ is __________ 22.4 dm³ of SO₂.

(Heavier than, Lighter than, Equal to)

23.  100 gms of water is equal to __________ moles.

(5.56, 27.78, 6.25)

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

(Reversible, Irreversible, Neutrilization)

25.  The reactions, which proceed in forward direction only are called __________ reactions.

(Reversible, Irreversible, Ionic)

26.  Molecular weight is used for __________ substances.

(Ionic, Non ionic, Neutral)

27.  Formula weight is used for __________ substances.

(Ionic, Non ionic, Neutral)

28.  The modern system of measurement is called __________ system.

(SI, Metric, F.P.S)

29.  The S.I unit of mass is __________.

(kilogram, gram, pound)

30.  One mole of glucose contains __________ gms.

(100, 180, 342)

Chapter 2

The Three States of Matter

1.      __________ was the first scientist who expressed a relation between pressure and the volume of a gas.

(Charles, Boyle, Avogadro)

2.      If the pressure upon a gas confined in a vessel varies, the temperature remaining same, the volume will __________.

(Vary directly as the pressure, Vary inversely as the temperature, Vary inversely as the pressure)

3.      The statement concerning the relation of temperature to the volume of a gas under fixed pressure was first synthesized by __________.

(Boyle, Charles, Avogadro)

4.      Absolute Zero is                                                                                                                                                                                                                                                                                                                       __________.

(273°C, -273°C, -273°K)

5.      Gases intermix to form __________.

(Homoge\=                                                                                         ous mixture, Heterogenous mixture, compound)

6.      Water can exists in __________ physical states at a certain condition of temperature pressure.

(One, Two, three)

7.    The temperature at which the volume of a gas theoretically becomes zero is called __________.

(Transition temperature, Critical Temperature, Absolute Zero)

8.      Gases deviate from ideal behaviour at __________ pressure and __________ temperature.

(Low, High, Normal)

9.      Very low temperature can by produced by the __________ of gases.

(Expansionn, Contraction, Compression)

10.  Boiling point of a liquid __________ with increase in pressure.

(increases, decreases, remains same)

11.  273°K = __________

(100°C, 273°C, 0°C)

12.  -273°C is equal to __________.

(0°K, 273°K, 100°K)

13.  Evaporation takes place at __________.

(All temperatures, At constant temperature, at 100°C)

14.  __________ is the temperature at which the vapour pressure of a liquid becomes equal to atmospheric pressure.

15.  The freezing point of water in Fahrenheit scale is __________.

(0°F, 32°F, 212°F)

16.  All gases change to solid before reaching to __________.

(-100°C, 0°C, -273°C)

17.  Pressure of the gas is due __________ of the molecules on the wall of the vessel.

(Collisionns, Attraction, Repulsion)

18.  Boiling point of water in absolute scale is __________.

(212°K, 100°K, 373°K)