JEE Questions for Chemistry Structure Of Atom Quiz 13 - MCQExams.com

The kinetic energy of an electron in the second Bohr orbit of a hydrogen atom is [a0 is Bohr radius]

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  • 2)
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If the radius of H is 0.54 Å, then what will be the radius of 3Li2+ ?
  • 0.17 Å
  • 0.36 Å
  • 0.53 Å
  • 1.59 Å
The work function (ϕ)of some metals are listed below. The number of metals which will show photoelectric effect when light of 300 nm wavelength falls on the metal is
Chemistry-Structure of Atom-8142.png
  • 2
  • 4
  • 6
  • 8
A gas absorbs photon of 355 nm and emits at two wavelengths. If one of the emission is at 680 nm, the other is at
  • 1035 nm
  • 325 nm
  • 743 nm
  • 518 nm
The frequency of light emitted for the transition n = 4 to n = 2 of He+ is equal to the transition in H atom corresponding to which of the following?
  • n = 3 to n = 1
  • n = 2 to n = 1
  • n = 3 to n = 2
  • n = 4 to n = 3
Which transition in the hydrogen atomic spectrum will have the same wavelength as the transition, n = 4 to n = 2 of He+ spectrum ?
  • n = 4 to n = 3
  • n = 3 to n = 2
  • n = 4 to n = 2
  • n = 3 to n = 1
  • n = 2 to n = 1
The energy of an electron in first Bohr orbit of H-atom is -13.6 eV. The possible energy value of electron in the excited state of Li2+ is
  • -122.4 eV
  • 30.6 eV
  • -30.6 eV
  • 13.6 eV
The electronic transitions from n = 2 to n = 1 will produce shortest wavelength in (where, n = principal quantum state)
  • Li2+
  • He+
  • H
  • H+
The energy required to break one mole of Cl — Cl bonds in Cl2 is 242 kJ mol-1. The longest wavelength of light capable of breaking a single Cl — Cl bond is
  • 594 nm
  • 640 nm
  • 700 nm
  • 494 nm
Ionisation energy of He+ is 19.6 × 10-18 J atom-1. The energy of the first stationary state (n =of Li2+ is
  • 4.41 × 10-16 J atom-1
  • -4.41 × 10-17 J atom-1
  • -2.2 × 10-15 J atom-1
  • 8.82 × 10-17 J atom-1
The radius of the first Bohr orbit of hydrogen atom is 0.529 Å. The radius of the third orbit of H+ will be
  • 8.46 Å
  • 0.705 Å
  • 1.59 Å
  • 4.76 Å
The wave number of the spectral line in the emission spectrum of hydrogen will be equal to 8/9 times the Rydberg's constant, if the electron jumps from
  • n = 3 to n = 1
  • n = 10 to n = 1
  • n = 9 to n = 1
  • n = 2 to n = 1
The ratio of the difference in energy between the first and the second Bohr orbit to that between the second and the third Bohr orbit is
  • 1/2
  • 1/3
  • 4/9
  • 27/5
The wave number of the first line in the Lyman series in hydrogen spectrum is
  • 72755.5 cm-1
  • 109678 cm-1
  • 82258.5 cm-1
  • 65473.6 cm-1
The number of photons emitted per second by a 60 W source of monochromatic light of wavelength 663 nm is (h = 6.63 × 10-34 Js)
  • 4 × 10-20
  • 1.54 × 1020
  • 3 × 10-20
  • 2 × 1020
  • 1 × 10-20
Bohr's radius of 2nd orbit of Be3+ is equal to that of
  • 4th orbit of hydrogen
  • 2nd orbit of He+
  • 3rd orbit of Li2+
  • 1st orbit of hydrogen
The ionisation enthalpy of hydrogen atom is 1.312 × 106 J mol-1. The energy required to excite the electron in the atom from n1 = 1 to n2 = 2 is
  • 8.51 × 105 J mol-1
  • 6.56 × 105 J mol-1
  • 7.56 × 105 J mol-1
  • 9.84 × 105 J mol-1
An electronic transition in hydrogen atom results in the formation of Hα line of hydrogen in Lyman series, the energies associated with the electron in each of the orbits involved in the transition (in kcal mol-1) are
  • -313.6, -34.84
  • -313.6, -78.4
  • -78.4, -34.84
  • -78.4, -19.6
Deflection back of a few particles on hitting thin foil of gold shows that
  • nucleus is heavy
  • nucleus is small
  • Both (and (2)
  • elctrons create hinderance in the movement of α-particles
Time period of a wave is 5 × 10-3s, what is the frequency ?
  • 5 × 10-3 s-1
  • 2 × 102 s-1
  • 23 × 103 s-1
  • 5 × 102 s-1
An electron from one Bohr stationary orbit can go to next higher orbit
  • by emission of electromagnetic radiation
  • by absorption of any electromagnetic radiation
  • by absorption of electromagnetic radiation of particular frequency
  • without emission or absorption of electromagnetic radiation
Splitting of spectrum lines in magnetic field is
  • Stark effect
  • Raman effect
  • Zeeman effect
  • Rutherford effect
The scientist who proposed the atomic model based on the quantisation of energy for the first time is
  • Max Planck
  • Niels Bohr
  • de-Broglie
  • Heisenberg
What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman series?
(h = Planck's constant, c = velocity of light, R = Rydberg's constant).

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    Chemistry-Structure of Atom-8162.png

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The frequency of radiation emitted when the electron falls from n = 4 to n = 1 in a hydrogen atom will be (given, ionisation energy of H = 2.18 × 10-18 J atom-1 and h = 6.625 × 10-34 Js)
  • 1.54 × 1015 s-1
  • 1.03 × 1015 s-1
  • 3.08 × 1015 s-1
  • 2.00 × 1015 s-1
Stark effect refers to the
  • splitting up of the lines in an emission spectrum in the presence of an extemal electrostatic field
  • random scattering of light by colloidal particles
  • splitting up of the lines in an emission spectrum in a magnetic field
  • emission of electrons from metals when light falls upon them
The relationship between the energy E1 of the radiation with a wavelength 8000 Å and the energy E2 of the radiation with a wavelength 16000 Å is
  • E1 = 6E2
  • E1 = 2E2
  • E1 = 4E2
  • E1 = 1/2E2
  • E1 = E2
Rutherford's experiment on the scattering of α-particles showed for the first time that the atom has
  • electrons
  • protons
  • nucleus
  • neutrons
The energy of the electron in first Bohr's orbit is -13.6 eV. The energy of the electron in its first excited state is
  • -3.4 eV
  • -27.8 eV
  • -6.8 eV
  • -10.2 eV
Angular momentum of an electron in the n th orbit of hydrogen atom is given by

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  • nh

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0:0:1


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