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REVISION SHEET
CLASS -XII
Chapter -12
Atoms
2015
Short answer Type Questions [I] [2 Marks]
1.
Show that the radius of the orbit in hydrogen atom varies as n 2 , where n is the principal quantum number of the
atom. Ans. r  n2
2.
State Bohr’s postulate of hydrogen atom which successfully explains the emission lines in the spectrum of
hydrogen atom. Use Rydberg formula to determine the wavelength of Hα line.
Ans. 6990 Å
Short Answer Type Question [II] [3 Marks]
3.
Using Rydberg’s formula, calculate the longest wavelengths belonging to lyman and balmer series. In which
region of hydrogen spectrum do these transitions lie? Ans. =6545Å
2014
Short Answer Type Questions [I] [2 Marks]
4.
Using Rutherford model of the atom, derive the expression for the total energy of the electron in hydrogen
atom. What is the significance of total negative energy possessed by the electron?
5.
Using Bohr’s postulates of the atomic model, derive the expression for radius of nth electron orbit. Hence, obtain
the expression for Bohr’s radius.
Short Answer Type Questions [II] [3 Marks]
6.
A 12.5 eV electron beam is used to bombard gaseous hydrogen at room temperature. Upto which energy level
the hydrogen atoms would be excited ? Calculate the wavelengths of the first member of Lyman and the first
member of Balmer series.
Ans. E4  
7.
o
13.6
 0.85 eV , 6.563 10 7m  6563A
16
A 12.9 eV beam of electrons is used to bombard gaseous hydrogen at room temperature. Up to which energy
level the hydrogen atoms would be excited? Calculate the first member of paschen series and first membe r of
Balmer series. Ans. 1  18752Å
8.
A 12.3 eV electron beam is used to bombard gaseous hydrogen at room temperature. Up to which energy level
the hydrogen atoms would be excited? Calculate the wavelengths of the second member of Lyman series and
second member of balmer series.
Ans. 4860 Å
Page 1
Long Answer Type Questions [5 Marks]
9.
(a)
Using Bohr’s postulates, derive the expression for the total energy of the electron in the stationary states
of the electron in the stationary states of the hydrogen atom. Ans. 1215Å
(b)
Using Rydberg formula, calculate the wavelength of the spectral lines of the first member of the lyman
series and of the Balamer series.
Ans. 6563Å
2013
Short Answer Type Questions [II] [3 Marks]
10.
Using Bohr’s postulates, obtain the expression for the total energy, of the electron in the stationary states of the
hydrogen atom. Hence, draw the energy level diagram showing how the line spectra corresponding to balmer
series occur due to transition between energy levels.
11.
[Delhi]
Using Bohr’s postulates, obtain the expression for (i) kinetic energy and (ii) potential energy of the electron in
stationary state of hydrogen atom. Draw the energy level diagram showing how the transitions between energy
levels result in the appearance of Lyman series.
12.
(a)
The energy levels of a hypothetical hydrogen-like atom are shown in the figure. Find out the transition,
from the ones shown in the figure, which will result in the emission of a photon of wavelength 275 nm.
(b)
Which of these transitions corresponds to the emission of radiation of (i) maximum and (ii) minimum
wavelength? Ans. 4.5 eV. 10 eV.
Long Answer Type Questions [5 Marks]
13.
Using Bohr’s postulates, derive the expression for the frequency of radiation emitted when electron in hydrogen
atom undergoes transition from higher energy state (quantum number n1 ) to the lower state
n  .
ƒ
when electron in hydrogen atom jumps from energy state ni  4 to nƒ  3,2,1, identify the spectral series to
which the emission lines belong.
2012
Short Answer Type Questions [II] [3 Marks]
14.
(a)
Using Bohr’s second postulate of quantization of orbital angular momentum show that the circumference
of the electrons in the nth orbital state in hydrogen atom is n times the de Broglie wavelength associated
with it.
(b)
The electron in hydrogen atom is initially in the third excited state. What is the maximum number of
spectral lines which can be emitted when it finally moves to the ground state?
Page 2
15.
The ground state energy of hydrogen atom is -13.6 eV. If an electron makes a transition from an energy level 0.85 eV to -3.4 eV, calculate the wavelength of the spectral line emitted. To which series of hydrogen spectrum
does this wavelength belong?
16.
Ans. 4870 Å
Using Bohr’s postulates for hydrogen atom, show that the total energy (E) of the electron in the stationary states
can be expressed as the sum of kinetic energy (K) and potential energy (U), where K = -2U. Hence, deduce the
expression for the total energy in the nth energy level of hydrogen atom.
2011
Short Answer Type Questions [II] [3 Marks]
17.
The energy of a hypothetical atom are shown below. Which of the shown transitions will results in the emission
of a photon of wavelength 275 nm? Which of these transitions corresponds to emission of radiation of (i)
maximum and (ii) minimum wavelength ?
18.
(a)
Using postulates of Boht’s theory of hydrogen atom, show that
(i)
the radii of orbits increase as n 2 , and
(ii)
the total energy of the electron increase as 1/ n 2 , where n is the principal quantum number of the atom.
(b)
calculate the wavelength of H α line in Balmer series of hydrogen atom, given Rydbeg constant R =
1.0947 × 107 m-1 . Ans.  6563.4 Å
19.
Using the polstulates of Bohr’s model of hydrogen atom. Obtain an expression for the frequency of radiation
emitted when the atom makes a transition from the higher energy state with quantum number n i to the lower
energy state with quantum number nƒ (nƒ  ni ).
2010
Very short Answer Type Questions [1 Mark]
20.
What is the ratio of radii of the orbits corresponding to first excited state and ground state in a hydrogen atom?
21.
The radius of innermost electron orbit of a hydrogen atom is 5.31011 m. what is the radius of orbit in the
second excited state?
22.
Write the expression for Bohr’s radius in hydrogen atom.
23.
Define ionisation energy. What is its value for a hydrogen atom?
24.
Find the ratio of energies of photons produced due to transition of an electron of hydrogen atom from its
(i)
second permitted energy level to the first level, and
(ii)
the highest permitted energy level to the first permitted level
Page 3
25.
The ground state energy of hydrogen atom is -13.6 eV. What are the kinetic and potential energies of electron in
this state?
26.
State Bohr’s quantization condition for defining stationary orbits.
2009
Very Short Answer Type questions [1 Marks]
27.
In the Rutherford scattering experiment the distance of closest approach for a α- particle is d0 . If α-particle
is replaced by a proton, how much kinetic energy in comparison to α-particle will it require to have the same
distance of closed approach d0 ?
Short Answer Type Questions [I] [2 Marks]
28.
The energy of the electron in the ground state of hydrogen atom is -13.6 eV.
(i)
What does the negative sign signify?
(ii)
How much energy is required to take an electron in this atom from the ground state to the first excited
state?
Short Answer Type Question [II] [3 Marks]
29.
(a)
The energy levels of an atom are as shown below. Which of them will result in the transition of a photon
of wavelength 275 nm?
(b)
Which transition corresponds to emission of radiation of maximum wavelength?
Page 4