What is the angular momentum of an electron in the third orbit of an atom?

(a) $3.15 \times 10^{-34}$ Js

(b) $3.15 \times 10^{-30}$ Js

(c) $3.15 \times 10^{-31}$ Js

(d) $3.15 \times 10^{-33}$ Js

Solution

Which series of the hydrogen spectrum has wavelength in the visible range

(a) Lyman.

(b) Balmer.

(c) Paschen.

(d) Bracket.

Solution

The value of fine structure constant is ?

(a) $\frac {1}{136}$

(b) $\frac {1}{130}$

(c) $\frac {1}{138}$

(d) $\frac {1}{137}$

Solution

If the electron in the hydrogen atom jumps from third orbit to second orbit, the wavelength of the emitted radiation is ?

(a) 5R/36

(b) 36/5R

(c) R/6

(d) 5/R

Solution

if an atom moves from 2E energy level to E energy level,the wavelength $\lambda$ is emitted. If the transition takes place from 4E/3 energy level to E energy level, the wavelength emitted will be

(A) $\frac {\lambda}{3}$

(B) $3 \lambda$

(C) $\frac {3\lambda}{4}$

(D) $\frac {4\lambda}{3}$

Solution

Maximum frequency of the emission is obtained for the transition

(a) n=2 to n=1

(b) n=6 to n=2

(c) n=1 to n=2

(d) n=2 to n=6

Solution

The radius of an electron orbit in a hydrogen atom is of the order of

(a) $10^{-8}$ m.

(b) $10^{-9}$ m.

(c) $10^{-11}$ m.

(d) $10^{-13}$ m.

Solution

If an electron jumps from Ist orbit to 4th Orbit then it will

(a) not lose energy.

(b) absorb energy.

(c) release energy.

(d) increases and decreases periodically

Solution

The energy of a hydrogen atom in the ground state is -13.6 eV. The energy of a He

(a)-13.6 eV

(b)-6.8 eV

(c)-54.4.6 eV

(d)-27.2 eV

Solution

Energy of an electron in the second orbit of hydrogen atom is E and energy of electron in 3rd orbit($E_3$) of He

(a) $E_3 = \frac {16E}{3}$

(b) $E_3 = \frac {16E}{9}$

(c) $E_3 = \frac {4E}{9}$

(d) $E_3 = \frac {4E}{3}$

Solution

The ratio of minimum to maximum wavelength in balmer series is

(a) 1 :4.

(b) 5 : 9

(c) 3 :4

(d) 5 : 36

Solution

The short wavelength limits of the lyman, Paschen and Balmer series in the hydrogen spectrum are a , b and c respectively . Arrange these wavelength in the increasing order?

(a)a < b < c

(b)c < b < a

(c)a < c < b

(d)b < c < a

Solution

With increasing quantum number, the energy difference between adjacent level

(a) increases

(b) decreases

(c) same

(d) increase and then decreases

Solution

Bohr's Radius ($r_0$) is given by?

(a) $r_0 = \frac {h^2}{8 \pi ^2 mke^2}$

(b) $r_0 = \frac {h^2}{9 \pi ^2 mke^2}$

(c) $r_0 = \frac {h^2}{2 \pi ^2 mke^2}$

(d) $r_0 = \frac {h^2}{4 \pi ^2 mke^2}$

Solution

(a) a -> p, b -> q , c -> r.

(b) a -> r, b -> q , c -> p.

(c) a -> r, b -> p , c -> q.

(d) a -> p, b -> r , c -> q.

Solution

The ground state energy of the hydrogen atom is $E_0$. The kinetic energy of the electron in the 3rd excitel level

(a) $-\frac {E_0}{16}$

(b) $-\frac {E_0}{9}$

(c) $\frac {E_0}{16}$

(d) $\frac {E_0}{9}$

Solution

The ground state energy of the hydrogen atom is $E_0$. The Potential energy of the electron in the 2nd excitel level

(a) $\frac {E_0}{8}$

(b) $\frac {E_0}{9}$

(c) $\frac {E_0}{16}$

(d) $\frac {2E_0}{9}$

Solution

The electron in hydrogen atom is initially in the third excited state.What is the maximum number of lines of spectrum lines which can be emitted whne it finally moves to the ground state

(a) 3

(b) 4

(c) 5

(d)6

Solution

A set of atoms in an excited state decays.

(a) in general to any of the states with lower energy.

(b) into a lower state only when excited by an external electric field.

(c) all together simultaneously into a lower state.

(d) to emit photons only when they collide

Solution

A hydrogen atom and a Li

(a) $I_H=I_{Li}$ , $|E_{Li}| > |E_H|$

(b) $I_H < I_{Li}$ , $|E_{Li}| < |E_H|$

(c) $I_H > I_{Li}$ , $|E_{Li}| > |E_H|$

(d) $I_H=I_{Li}$ , $|E_{Li}| < |E_H|$

Solution

Define the distance of closest approach. An alpha-particle of kinetic energy 'K' is bombarded on a thin gold foil. The distance of the closest approach is 'r'. What will be the distance of closest approach for an alpha-particle of double the kinetic energy?

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 Ballmer series occur due to transition between energy levels.

(i)State Bohr's postulates to define stable orbits in hydrogen atom. How does de -broglie hypothesis explain the stability of these orbits?

(ii) A hydrogen atom initially in the ground state absorbs a photon which excites it to the n=4 level . Estimate the frequency of the photon

Solution

Derive the Bohr's Quantisation condition for angular momentum of the orbitting of electron in hydrogen atom using de Broglie hypothesis.

Using Bohr's postulates of the atomic model, derive the expression for the radius of the nth electron orbit.Also obtain the expression for Bohr's Radius. Show graphically the variation of the radius of the orbit with the principle quantum number

Calculate the ratio of the frequencies of the radiation emitted due to transition of the electron in a hydrogen atom from its (i) second permitted energy level to the first level and (ii) highest permitted energy level to the second permitted level

Solution

Calculate the shortest wavelength of light emitted in the Paschen series of hydrogen spectrum. Which part of the electromagnetic spectrum , does it belong?br> Explain the above observations on the basis of Einstein's photoelectric equation.?

Solution

A 12.5 eV electron beam is used to excite a gaseous hydrogen atom at room temperature. Determine the wavelength and the corresponding series of the lines emmitted

Solution

Find the relation between the three wavelength $\lambda _1$,$\lambda _2$ and $\lambda _3$ from energy level diagram shown below?

Solution

Find out the wavelength of the electron orbiting in the ground state of the hydrogen atom?

Solution

Draw the energy-level diagram of hydrogen atom. This atom in its ground state is excited by absorption of radiation of wavelength 970 $A^o$. How many different kinds of lines are possible in the emitting spectrum?. calculate the longest wavelength among them.Take ionization energy of hydrogen atom as 13.6 eV, h=$6.6 \times 10^{-34}$ Js. c = $3 \times 10^8$ m/s ,1 eV = $1.6 \times 10^{-19}$ J

Solution

(i)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?

Solution

In a Geiger Marsden experiment, calculate the distance of closest approach to the nucleus of Z=80, when an alpha-particle of 8MeV energy impings on it before it comes momentarily to rest and reverses its direction.

How will the distance of closest approach be affected when the kinetic energy of the a- particle is doubled ?

Solution

The energy of the electron, the hydrogen atom, is known to be expressible in the form

$E_{nth}=- \frac {13.6}{n^2}$ eV n=1,2,3...

Use this expression to show that the

(i) electron in the hydrogen atom can not have an energy of -6.8 eV.

(ii) spacing between the lines (consecutive energy levels) within the given set of the observed hydrogen atom spectrum decreases as n increases.

Solution

Photons, with a continuous range of frequencies, are made to pass through a simple of rarefied hydrogen. The transitions, shown in Fig. indicate three of the spectral absorption lines in the continuous spectrum.

(i) Identify the spectral series, of the hydrogen emission spectrum, to which each of these three lines correspond.

(ii) Which of these lines corresponds to the absorption of radiation of maximum wavelength?

Solution

Using the Rydberg formula, calculate the wavelengths of the first four spectral lines in the Lyman series of the hydrogen spectrum.

Given $h=6.6 \times 10^{-34} $ Js,$c=3 \times 10^{8} $ m/s,$e=1.6 \times 10^{-19}$ C

Solution

Class 12 Maths Class 12 Physics

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