Advertisements
Advertisements
प्रश्न
The earth revolves round the sun due to gravitational attraction. Suppose that the sun and the earth are point particles with their existing masses and that Bohr's quantization rule for angular momentum is valid in the case of gravitation. (a) Calculate the minimum radius the earth can have for its orbit. (b) What is the value of the principal quantum number n for the present radius? Mass of the earth = 6.0 × 10−24 kg. Mass of the sun = 2.0 × 1030 kg, earth-sun distance = 1.5 × 1011 m.
Advertisements
उत्तर १
Given:
Mass of the earth, me = 6.0 × 1024 kg
Mass of the sun, ms = 2.0 × 1030 kg
Distance between the earth and the sun, d = 1.5 × 1111 m
According to the Bohr's quantization rule,
Angular momentum, L =`(nh)/(2pi)`
⇒`mvr=(nh)/(2pi) ....(1)`
Here,
n = Quantum number
h = Planck's constant
m = Mass of electron
r = Radius of the circular orbit
v = Velocity of the electron
Squaring both the sides, we get
`m_e^2v^2r^2 = (n^2h^2)/(4pi^2)` ....(2)
Gravitational force of attraction between the earth and the sun acts as the centripetal force.
`F = (Gm_em_s)/r^2 = (m_ev^2)/r`
`rArr v^2 = (Gm_s)/r` ......(3)
Dividing (2) by (3), we get
`m_e^2 r = (n^2h2)/(4pi^2Gm_s)`
(a) For n = 1,
`r = sqrt((h^2)/(4pi^2Gm_sm_e^2))`
`r = sqrt((6.63xx10^-34)^2/(4xx(3.14)^2xx(6.67xx10^-11)xx(6xx10^24)^2xx(2xx10^30))`
`r = 2.29xx10^-138 m`
`r =2.3xx10^-138 m`
(b)
From (2), the value of the principal quantum number (n) is given by
`n^2 = (m_e^2xxrxx4xxpixxGxxm_s)/h^2`
`rArr n = sqrt(m_e^2xxrxx4xxpixxGxxm_s)/h^2`
`n=sqrt(((6xx10^24)^2xx(1.5xx10^11)xx4xx(3.14)^2xx(6.67xx10^-11)xx(2xx10^30))/(6.6xx10^-34))`
n = 2.5 ×1074
उत्तर २
Given:
Mass of the earth, me = 6.0 × 1024 kg
Mass of the sun, ms = 2.0 × 1030 kg
Distance between the earth and the sun, d = 1.5 × 1111 m
According to the Bohr's quantization rule,
Angular momentum, L =`(nh)/(2pi)`
⇒`mvr=(nh)/(2pi)`
....(1)
Here,
n = Quantum number
h = Planck's constant
m = Mass of electron
r = Radius of the circular orbit
v = Velocity of the electron
Squaring both the sides, we get
`m_e^2v^2r^2 = (n^2h^2)/(4pi^2)` ....(2)
Gravitational force of attraction between the earth and the sun acts as the centripetal force.
`F = (Gm_em_s)/r^2 = (m_ev^2)/r`
`rArr v^2 = (Gm_s)/r` ......(3)
Dividing (2) by (3), we get
`m_e^2 r = (n^2h2)/(4pi^2Gm_s)`
(a) For n = 1,
`r = sqrt((h^2)/(4pi^2Gm_s_e^2))`
`r = sqrt((6.63xx10^-34)^2/(4xx(3.14)^2xx(6.67xx10^-11)xx(6xx10^24)^2xx(2xx10^30))`
`r = 2.29xx10^-138 m`
`r =2.3xx10^-138 m`
(b)
`n^2 = (m_e^2xxrxx4xxpixxGxxm_s)/h^2`
`rArr n = sqrt(m_e^2xxrxx4xxpixxGxxm_s)/(6.6xx10^-34)^2`
n = 2.5 ×1074
APPEARS IN
संबंधित प्रश्न
What is the energy in joules, required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state? The ground state electron energy is –2.18 × 10–11 ergs.
Explain, giving reasons, which of the following sets of quantum numbers are not possible.
- n = 0, l = 0, ml = 0, ms = + ½
- n = 1, l = 0, ml = 0, ms = – ½
- n = 1, l = 1, ml = 0, ms = + ½
- n = 2, l = 1, ml = 0, ms = – ½
- n = 3, l = 3, ml = –3, ms = + ½
- n = 3, l = 1, ml = 0, ms = + ½
In Bohr’s model of the hydrogen atom, the radius of the first orbit of an electron is r0 . Then, the radius of the third orbit is:
a) `r_0/9`
b) `r_0`
c) `3r_0`
d) `9r_0`
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 ni) to the lower state, (nf).
When electron in hydrogen atom jumps from energy state ni = 4 to nf = 3, 2, 1, identify the spectral series to which the emission lines belong.
Write the expression for Bohr’s radius in hydrogen atom ?
The numerical value of ionization energy in eV equals the ionization potential in volts. Does the equality hold if these quantities are measured in some other units?
Which of the following parameters are the same for all hydrogen-like atoms and ions in their ground states?
Find the wavelength of the radiation emitted by hydrogen in the transitions (a) n = 3 to n= 2, (b) n = 5 to n = 4 and (c) n = 10 to n = 9.
In form of Rydberg's constant R, the wave no of this first Ballmer line is
A set of atoms in an excited state decays ______.
An ionised H-molecule consists of an electron and two protons. The protons are separated by a small distance of the order of angstrom. In the ground state ______.
- the electron would not move in circular orbits.
- the energy would be (2)4 times that of a H-atom.
- the electrons, orbit would go around the protons.
- the molecule will soon decay in a proton and a H-atom.
The ground state energy of hydrogen atoms is -13.6 eV. The photon emitted during the transition of electron from n = 3 to n = 1 unknown work function. The photoelectrons are emitted from the material with a maximum kinetic energy of 9 eV. Calculate the threshold wavelength of the material used.
State Bohr's postulate to explain stable orbits in a hydrogen atom. Prove that the speed with which the electron revolves in nth orbit is proportional to `(1/"n")`.
The value of angular momentum for He+ ion in the first Bohr orbit is ______.
Find the ratio of energies of photons produced due to transition of an election 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.
What is the energy of an electron in stationary state corresponding to n = 2?
Find the angular momentum of an electron revolving in the second orbit in Bohr's hydrogen atom.
The wavelength of the second line of the Balmer series in the hydrogen spectrum is 4861 Å. Calculate the wavelength of the first line of the same series.
Calculate the radius of the second orbit of He+.
