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.
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
State Bohr’s third postulate for hydrogen (H2) atom. Derive Bohr’s formula for the wave number. Obtain expressions for longest and shortest wavelength of spectral lines in ultraviolet region for hydrogen atom
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.
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.
If the velocity of the electron in Bohr’s first orbit is 2.19 × 106 ms-1, calculate the de Broglie wavelength associated with it.
State Bohr postulate of hydrogen atom that gives the relationship for the frequency of emitted photon in a transition.
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.
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?
Obtain Bohr’s quantisation condition for angular momentum of electron orbiting in nth orbit in hydrogen atom on the basis of the wave picture of an electron using de Broglie hypothesis.
Which of these statements correctly describe the atomic model according to classical electromagnetic theory?
Using Bohr's postulates derive the expression for the radius of nth orbit of the electron.
Consider two different hydrogen atoms. The electron in each atom is in an excited state. Is it possible for the electrons to have different energies but same orbital angular momentum according to the Bohr model? Justify your answer.
In form of Rydberg's constant R, the wave no of this first Ballmer line is
For the ground state, the electron in the H-atom has an angular momentum = h, according to the simple Bohr model. Angular momentum is a vector and hence there will be infinitely many orbits with the vector pointing in all possible directions. In actuality, this is not true ______.
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 value of angular momentum for He+ ion in the first Bohr orbit is ______.
The electron in a hydrogen atom first jumps from the third excited state to the second excited state and subsequently to the first excited state. The ratio of the respective wavelengths, λ1/λ2, of the photons emitted in this process is ______.
A 20% efficient bulb emits light of wavelength 4000 Å. If the power of the bulb is 1 W, the number of photons emitted per second is ______.
[Take, h = 6.6 × 10-34 J-s]
State three postulates of Bohr's theory of hydrogen atom.
On the basis of Bohr's theory, derive an expression for the radius of the nth orbit of an electron of hydrogen atom.