For a Bohr atom, angular momentum of an electron is
(n = 1, 2, 3……)

According to Mosley the relationship between the
frequency (  ) of lines in X- rays spectra and atomic
number (Z) of an element is given by the expression

The element with A and Z values are same in

The ratio between the number of neutrons present
in C12 and Si30 atoms is

The nitride ion in lithium nitride is composed of

The molecule having maximum number of electrons is

In which of the following cation and anion have same number of electrons

In Manganese atom in ground state, the total number
of orbitals populated with one or more electrons are

The Z and A values of an element are 25 and 55. The
number of electrons, protons and neutrons in its most
stable ion respectively are

Nucleus was discovered in

Nucleons are

The presence of nucleus in the atom was predicted by

Of the following fundamental particles, the one with
least mass is

Magnitude of deflection of cathode rays in discharge
tube is more when

One of the fundamental particles is missing in one of the isotopes. The particle and isotope are respectively

Tritium atom contains

The  (alpha) –particles are

Which is not deflected by magnetic field

Which of the following species contains 10 electrons, 11 protons, 12 neutrons

The charge on the atom containing 17 protons, 18 neutrons and 18 electrons is

The e/m value of electron is

The total number of neutrons in dipositive zinc ion
with mass number 70

The radiation having maximum wavelength is

31. The radiation having highest energy is

32. Which one of the following has more wave number

33. The product of which of the following is equal to the
velocity of light

34. All types of electromagnetic radiation possess same

The ratio of energy to frequency of electromagnetic
radiation is called
1) Bohr’s constant 2) Rydber’s constant
3) Planck’s constant 4) Ritz constant

36. The radiation of least energy amongst the following
1) x – rays 2) I.R 3) Visible 4) U.V

37. Out of the following, the radiation with lowest frequency is

38. Which of the following statements about electromagnetic
spectrum is not correct
1) Infra red rays have larger wavelength than cosmic
rays
2) The frequency of microwaves is less than that of
UV rays
3) X – rays have larger wave number than micro waves
4) The velocity of x – rays is more than that of
microwaves

39. A photon in X region is more energetic than in the
visible region X is
1) IR               2) UV                 3) Microwaves              4) Radio waves

Line spectrum is characteristic of

Molecules give a band of spectral lines during
emission. This is because

The band spectrum is caused by
1) molecules 2) atoms
3) any substance in solid state
4) any substance in liquid state

43 . When an electron jumps from higher orbit to lower
orbit, then the spectrum contain ____lines on__
backgound.
1) dark; bright 2) bright, dark
3) bright, bright 4) dark, dark

44. Colour of the lines found in the emission spectrum
of Sodium
1) Black 2) Yellow 3) Red 4) Grey

45. The spectrum with all wavelengths may be
1) absorption spectrum 2) emission spectrum
3) continuous spectrum 4) discontinuous spectrum

Normal hydrogen atoms can not give

47. Paschen series is due to the electronic transition from
all higher levels to

48. In hydrogen spectrum the following series of lines
belongs to U.V region

49. The spectral series observed in Far infra-red region
of hydrogen spectrum is

50. Transition of electron from M-shell to K-shell results
in the emission of
1) Cosmic rays 2) infrared rays
3) ultraviolet rays 4) X- rays

53. Energy difference between two adjacent orbits is
minimum if they are
1) K,L – shells                   2) L,M shells
3) M,N – shells                 4) N,O – shells

Hydrogen electron is present in the N shell. If it loses
energy, a spectral line may be observed in the region
1) infra red                       2) visible                  3) ultra violet                   4) any of these

Rydberg constant is
1) Same for all elements
2) Different for different elements
3) A universal constant
4) Is different for lighter elements but same for heavier
elements

57. If the mass of electron is reduced to half, the Rydberg’s
constant
1) Remains unchanged 2) Becomes half
3) Becomes double 4) Becomes one – fourth

58. Which of the following transition is associated with coloured spectral line
1) n = 5 to n = 3 2) n = 4 to n = 2
3) n = 2 to n = 1 4) n = 3 to n = 1

The electron level which allows the hydrogen to
absorbs photons but not to emit is
1) 1s                         2) 2s                     3) 2p                   4) 3d

61. As the electron moves away from the nucleus, its
kinetic energy and potential energy are respectively
1) decrease, decrease                         2) increase, increase
3) increase, decrease                          4) decrease, increase

62. With the increase in orbit number (n), the difference
between energy of adjacent energy levels
1) increases                          2) decreases
3) remains constant              4) cannot be predicted

63. When the atomic electron is at infinite distance from
the nucleus, its energy is
1) infinity                       2) zero                     3) negative                    4) positive

64. The total energy of the electron revolving round the
nucleus is
1) zero

2) less than zero

3) more than zero
4) in some atoms less than zero and in certain atoms
more than zero

65. The change in velocity when hydrogen electron jumps
from K shell to L shell is
1) one-half of its original velocity
2) twice to its original velocity
3) one-quarter of its original velocity
4) equal to its original velocity

66. In which orbit of He+ angular momentum of the
electron is h/2 π
1) first orbit                    2) second orbit
3) third orbit                   4) fourth orbit

67. The angular momentum of an electron in an atom depends on

Properties of electrons that are quantized in Bohr’s
atomic model are
1) mass and energy
2) energy and angular momentum
3) angular momentum and mass
4) mass and charge

69. Bohr’s model violates the rules of classical physics
because it assumes that
1) all electrons have same charge
2) the nucleus have same charge
3) electrons can revolve around the nucleus
4) a charged particle can accelerate without emitting
radiant energy

70. Bohr’s model of atom explains
1) zeeman effect 2) photo electric effect
3) stark effect 4) none of the above

71. Bohr’s model of atom can explain the spectrum of all
except
1) H 2) He+ 3) Li++ 4) He

72. The metal that emits photo electrons very easily is
1) Iron 2) Lithium 3) Potassium 4) Copper

73. The minimum energy required to eject an electron
from an atom is called
1 ) Kinetic energy 2) Electrical energy
3) Chemical ellergy 4) Work function

74. The photoelectric emission from a surface starts only
when the light incident upon the surface has certain
minimum
1) Intensity 2) Wave length
3) Frequency 4) Velocity

76. Einstein photo electric effect is represented in the form of equation is

78. In order to designate an orbital in an atom the no. of
quantum no. required
1) One 2) Two 3) Three 4) Four

79. The quantum number which determines the size of
the orbit is
1) n 2) l 3) m 4) s

80. For 24th electron the principal quantum number
value is
1) 24 2) 4 3) 3 4) 5

81. The quantum number which determines the number
of sub-energy levels in any main energy level is
1) n 2) l 3) m 4) s

82. An orbital is made of four lobes. Its azimuthal quantum
number value is
1)0 2) 4 3) 2 4)1

83. The quantum number which determines the shape of
the orbital is

84. Azimuthal quantum number was proposed to explain

85. The quantum number that was proposed to explain the Zeeman effect is

86. The magnetic quantum number for the outermost
electron in sodium atom is

87. The quantum number which determines the
orientation of orbitals is

88. The m value not possible of a 4f-electron is

89. The magnetic quantum number of electrons of Be

90. The direction of spin of an electron is represented by

91. The quantum no. not obtained from Schrodinger’s
wave equation is

92. 14 electrons cannot be accommodated in following sub-energy level

93. The quantum number which determines the energy of a sublevel is

94. The (n+l) value of 5p-sub level is

95. The sub-energy level having minimum energy is

96. Among the various quantum numbers. (n, I, m, s) describing an electron which can have the largest value

97. Maximum number of electrons can be accomodated in the following subshell

98. The sub-energy level which can accomodate maximum number of electrons with parallel spin values is

99. The quantum number which cannot say any thing about an orbital is

100. The electrons occupying the same orbital have the same values for all the quantum number except for