CHAPTER 3 MULTIPLE CHOICE QUESTIONS

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MULTIPLE CHOICE QUESTIONS

 

1. Which of the experiments convinces about the divisibility of atoms?

(i) Radioactivity

(ii) X-rays

(iii) Spectroscopic studies

(iv) All of the above

 

2. Which light is emitted by a fluorescent material?

(i) UV

(ii) Visible

(iii) IR

(iv) X- Rays

 

3. Cathode rays emitted from cathode are

(i) Cananl rays

(ii) Protons

(iii) Electrons

(iv) Positrons

 

4. Charge to muss ratio (el m) of the electron is determined by

(i) R .A. Millikan

(ii) J.J Thompson

(iii) G.J. Stoney

(iv) None of these

 

7. Alpha particles are

(i) Neutrons

(ii) Protons

(iii) Electrons

(iv) Helium nuclei

 

8. The beam attracted towards the negatively charged plate are

(i) Alpha particles

(ii) Neutrons

(iii) Beta particles

(iv) Gamma particles

 

9. Which rays are not deflected by electric and magnetic field?

(i) Alpha

(ii) Beta

(iii) Gamma

(iv) None of these

 

10. Which rays carry no charged and non- material in nature?

(i) Alpha

(ii) Beta

(iii) Gamma

(iv) None of these

 

11. Neutron was discovered by

(i) Moseley

(ii) Milliken

(iii) Chadwick

(iv)Rutherford

 

12. The phenomena of the emission of radiation from nuclei of lighter atoms due to bombardment of moving particles is known as

(i) Fission

(ii) Fusion

(iii) Artificial radioactivity

(iv) None of these

13. When high energy electrons collide with the anode, a very penetrating kind of radiation is produced roentgen called them

(i) Alpha – rays

(ii) Beta – rays

(iii) Gamma- rays

(iv) X- rays

 

14. Neutron possesses

(i) Positive charge

(ii) Negative charge

(iii) No charge

(iv) None of these

 

15. Rutherford bombarded by a number of electrons equal to the number of

(i) Beta particles

(ii) Neutron

(iii) Alpha particles

(iv) Electron

 

16 The nucleus is surrounded by a number of electrons equal to the number of

(i) Neutron

(ii) Proton

(iii) Negatron

(iv) Positron

 

17. According to rutherford’s model, the nucleus is surrounded by

(i) Proton

(ii) Neutron

(iii) Positron

(iv) Electron

 

18. Nucleus was discovered by

(i) Schrodinger

(ii) Chadwick

(iii) Bohr

(iv)Rutherford

 

19. The spectrum of incandescent gas is

(i) Absorption

(ii) Emission

(iii) Line

(iv) Continuous

 

20. The number of waves passing through a point in one second is called

(i) Wave number

(ii) Velocity

(iii) Frequency

(v) Wavelength

 

21. The distance between two successive crests in one or through is called

(i) Velocity

(ii) Frequency

(iii) Wavelength

(iv) Intensity

 

22. When a substance that has absorbed energy emits it in the form of radiation. The spectrum is

(i) Absorption spectrum

(ii) Emission spectrum

(iii) Line spectrum

(iv) Continuous spectrum

 

23. The quantum number which describes the shape of the orbital is

(i) Principle quantum number

(ii) Spin quantum number

(iii) Azimuthal quantum number

(iv) Magnetic quantum number

 

24. The quantum number which describe the orientation of the orbital is

(i) Spin quantum number

(ii) Principle quantum number

(iii) Azimuthal quantum number

(iv) Magnetic quantum number

 

25. In a spectrum of light shortest and longest wave length respectively are:

(i) Violet and red

(ii) Blue and red

(iii) Red and blue

(iv) Violet and indigo

 

25. Hydrogen atomic spectra are obtained by:

(i) De- excitation of a higher energy state

(ii) Emission of a gamma ray from the nucleus

(iii) Absorption of energy by ground state

(iv) Absorption of a an electron by the nucleus

 

26. Radioactivity Is due to:

(i) Stable electronic configuration

(ii) Stable nucleus

(iii) Unstable electronic configuration

(iv) Unstable nucleus

 

27. Emission of B particles from an element shows its:

(i) Atomic mass increase by 1

(ii) Atomic mass decrease by 1

(iii) Atomic charge increase by 1

(iv) Atomic charge decrease by 1

 

28. The orbital which has spherical shape is called

(i) s – orbital

(ii) p – orbital

(iii) d – orbital

(iv) f – orbital

 

29. When the electron jumps from third, fourth, fifth, orbits to the second orbit, the transitions are known as

(i) Paschen

(ii) P fund

(iii) Balmer

(iv) Brackett series

 

30. When the electron jumps from second ,third , fourth, orbits to the first orbit, the transitions are known as

(i) Balmer series

(ii) Lyman series

(iii) P fund series

(iv) Brackett series

31. Paschen, p fund and bracket series are found in

(i) UV region

(ii) Visible region

(iii) IR region

(iv) None of these

 

32. Bohr’s theory satisfactorily explains

(i) Stability of atom

(ii) Ionization energy

(iii) Spectra of hydrogen

(iv) All of the above

 

33. The first important discovery about the nature of cathode rays made by

(i) J. Perrin

(ii) De- Broglic

(iii) Crooks

(iv) Hittorf

 

34. Cathode rays possess

(i) Negative charge

(ii) Positive charge

(iii) Neutral

(iv) None of these

 

35. Canal rays are

(i) Negative rays

(ii) Positive rays

(iii) Neutral

(iv) None of these

 

36 The wavelength of green light in the range of

(i) 510-580 nm

(ii) 400-450 nm

(iii) 300-400 nm

(iv) 600-700 nm

 

37 .When spectrum of hydrogen is taken in the magnetic field, some new lines are created.

(i) n = 2

(ii) n = 4

(iii) n = 8

(iv) None of these

 

38. Quantum mechanical model of atom develop on the basis of Schrodinger equation helps to calculate

(i) Bond energy

(ii) Bond length

(iii) Shapes of molecules

(iv) All of the above

 

39 if the value of 1 = 0 me orbital is

(i) s

(ii) p

(iii) d

(iv) 2

 

40 The maximum number of electrons in d-orbital is

(i) 6

(ii) 8

(iii) 12

(iv) 10

 

41 The electrons are put in energy sub- levels in the order of increasing energy values. This is a statement of

(i) Hund’s rule

(ii) Aufbau principle

(iii) Pauli exclusion principle

(iv) Phase rule

 

42 Which of the following has highest electro-negativity?

(i) Cl

(ii) N

(iii) F

(iv) O

 

43. The measure of the ability of an atom to attract an electron pair to it self in a chemical bond is called

(i) Ionization energy

(ii) Electron affinity

(iii) Electro negativity

(iv) None of these

 

44. When the orbital of same energy are available to electrons, they will live in the separate orbital. This is a statement of

(i) Hund‘s rule

(ii) Aufbau principle

(iii) Pauli exclusion principle

(iv) Phase rule

 

45 The maximum number of electrons in orbital is

(i) 2

(ii) 4

(iii) 6

(iv) 8

 

46. The value of spin quantum number is

(i) +1/2

(ii) – 1/2

(iii) +1/2 or -12

(iv) +2

 

47. Electron behave like

(i) Waves

(ii) Particle

(iii) Wave and particle

(iv) None of these

 

48. f-orbital has maximum number of electrons

(i) 10

(ii) 6

(iii) 2

(iv) 14

 

49. Natural radioactivity is shown by elements which have atomic number

(i) 70

(ii) More than 80

(iii) X- rays

(iv) None of these

 

50. Which orbital has the lowest energy?

(i) 3d

(ii) 4s

(iii) Sp

(iv) 4f

 

51. Which ion has greater size?

(i) Cl-

(ii) l

(iii) F-

(iv) Br-

 

52. Sl unit of wave length is V

(i) Meter cube

(ii) Meter

(iii) Meter square

(iv) Per metre

 

53. lf the electro negativity difference between atoms is more than 1.7, the bond is

(i) Ionic

(ii) Covalent

(iii) Coordinate

(iv) Metallic

54 The maximum number of electrons in d- orbital is

(i) 4

(ii) 10

(iii) 4

(iv) C

 

55. Electro negativity depends on

(i) Atomic size

(ii) Atomic numbers

(iii) Atomic volume

(iv) All of the above

 

56. A covalent bond is formed when E.N values difference is

(i) Greater than 1.7

(ii) Equal to 1.7

(iii) Less than 1.7

(iv) None of these

 

57 Which element has higher electron affinity value?

(i) He

(ii) Ne

(iii) Ar

(iv ) Kr

 

58. Ionization energy depends on

(i) Magnitude of nuclear charge

(ii) Atomic radius

(iii) Shielding effect

(iv) All of the above

 

59. Which elements has high first ionization energy value?

(i) Li

(ii) Be

(iii) B

(iv) C

 

60. Which element has low ionization value?

(i) He

(ii) Li

(iii) Na

(iv) K

 

61. Which of the following is correct one?

(i) C = h / v

(ii) h = m/v

 

62. Balmer series lie in:

(i) infra red region

(ii) Visible region

(iii) Ultra – violet region

(iv) Invisible

 

63. The electron losses energy when:

(i) It jump from higher to lower orbit

(ii) It jumps from lower to higher orbit

(iii) Electron is in constant motion

(iv) All of these

 

64. In 1913. Mosely used the X- rays to determine the

(i) Mass number

(ii) Atomic number

(iii) Relative atomic mass

(iv) Avogadro’s Number

 

65. No two electrons in an atom can have a set of some four quantum number ” is

called:

(i)Newton’ first law

(ii) Pauli’s exclusion principles

(iii) Hund’s rule

(iv) None of these

 

67. Two electrons in the helium atom:

(i) Have different spin quantum No.

(ii) Have same spin quantum No

(iii) Occupy different shells

(iv) None of these

 

68. T.V picture tube is a type of:

(i) X- rays tube

(ii) Discharge tube

(iii) Milliken tube

(iv) Positive rays tube

 

69. The presence of three unpaired electrons in nitrogen atom can be explained by:

(i) Pauliexclusion principle

(ii) Hund‘s rule

(iii) Aufbau principle

(iv) Heisenberg’s uncertainly principle

 

70. Velocity of:

(i) Alpha particles greater than beta particles

(ii) Beta particles greater than alpha particles

(iii) Alpha particles is same as beta particles

(iv) Alpha particles is same of velocity of lights

 

71. An electron is said to be excited inside an atoms is:

(i) It losses energy

(ii) More than zero

(iii) Less than Zero

(iv) Constant

 

72. The statement is not true:

(1) No two electrons can have the same set of tour quantum number

(ii) The energy level K contains only one orbital and two or less electrons

(iii) The energy level L has four orbital s and can have maximum of eight electrons

(iv) The N energy level contains six sub levels and maximum of 32 electrons

 

73. An orbital can have maximum of:

(i) 2 electrons

(ii) G electrons

(iii) 8 electrons

(iv) 32 electrons

 

74. In ground state carbon atoms has:

(i) Three unaired electrons

(ii) Two lone pair electrons

(iii) Two unpaired electrons

(iv) One unpaired electron

 

75. If t = 2 the orbital is called as Z

(i) s

(ii) d

(iii) f

(iv) p

 

78. The lowest energy level which can have electron can have is:

(i) L

(ii) K

(iii) M

(iv) N

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