The fact that electric charges are integral multiples of the fundamental electronic charge was proved experimentally by 
(1) Planck                   

(2) J.J. Thomson

(3) Einstein                 

(4) Millikan

Subtopic:  Various Atomic Models |
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The specific charge of an electron is 

(a) 1.6×10-19 coulomb

(b) 4.8×10-10 stat coulomb

(c) 1.76×1011 coulomb/kg

(d) 1.76×10-11  coulomb/kg

Subtopic:  Various Atomic Models |
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The ratio of specific charge of an α-particle to that of a proton is 
(1) 2 : 1                     

(2) 1 : 1

(3) 1 : 2                     

(4) 1 : 3

Subtopic:  Various Atomic Models |
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Which of the following have the highest specific charge

(1) Positron                   

(2) Proton

(3) He++                          

(4) None of these

Subtopic:  Various Atomic Models |
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For the Bohr's first orbit of circumference 2πr, the de-Broglie wavelength of revolving electron will be

(a) 2πr                       (b) πr
(c) 12πr                      (d) 14πr

Subtopic:  Bohr's Model of Atom |
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According to de-Broglie, the de-Broglie wavelength for electron in an orbit of hydrogen atom is 10-10 m. The principle quantum number for this electron is r=5.13×10-11m
(a) 1           (b) 2
(c) 3           (d) 4

Subtopic:  Bohr's Model of Atom |
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The energy of a photon of light with wavelength 5000 Å is approximately 2.5 eV. This way the energy of an X-ray photon with wavelength 1Å would be 
(1) 2.5/5000 eV             

(2) 2.5/50002 eV

(3) 2.5×5000 eV           

(4)  2.5×50002 eV

Subtopic:  X-Ray (OLD NCERT) |
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The graph that correctly represents the relation of frequency v of a particular characteristic X-ray with the atomic number Z of the material is

Subtopic:  X-Ray (OLD NCERT) |
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If in nature there may not be an element for which the principal quantum number n > 4, then the total possible number of elements will be

(1) 60                   

(2) 32

(3) 4                     

(4) 64

Subtopic:  Various Atomic Models |
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In the \(n^{th}\) orbit, the energy of an electron is \(E_{n}=-\frac{13.6}{n^2} ~\text{eV}\) for the hydrogen atom. What will be the energy required to take the electron from the first orbit to the second orbit?
1. \(10.2~\text{eV}\)
2. \(12.1~\text{eV}\)
3. \(13.6~\text{eV}\)
4. \(3.4~\text{eV}\)

Subtopic:  Bohr's Model of Atom |
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