Advertisements
Advertisements
प्रश्न
The longest wavelength doublet absorption transition is observed at 589 and 589.6 nm. Calculate the frequency of each transition and energy difference between two excited states.
Advertisements
उत्तर
For λ1 = 589 nm
Frequency of transition `("v"_1) = "c"/lambda_1`
`= (3.0xx10^(8) " ms"^(-1))/(589xx10^(-9) " m")`
Frequency of transition (ν1) = 5.093 × 1014 s–1
Similarly, for λ2 = 589.6 nm
Frequency of transition `("v"_2) = "c"/lambda_2`
`= (3.0 xx 10^8 " ms"^(-1))/(589.6xx10^(-9) " m")`
Frequency of transition (ν2) = 5.088 × 1014 s–1
Energy difference (ΔE) between excited states = E1 – E2
Where,
E2 = energy associated with λ2
E1 = energy associated with λ1
ΔE = hν1 – hν2
= h(ν1 – ν2)
= (6.626 × 10-34 Js) (5.093 × 1014 – 5.088 × 1014)s-1
= (6.626 × 10-34 J) (5.0 × 10-3 × 1014)
ΔE = 3.31 × 10-22 J
संबंधित प्रश्न
- Using the Bohr’s model, calculate the speed of the electron in a hydrogen atom in the n = 1, 2 and 3 levels.
- Calculate the orbital period in each of these levels.
In accordance with the Bohr’s model, find the quantum number that characterises the earth’s revolution around the sun in an orbit of radius 1.5 × 1011 m with orbital speed 3 × 104 m/s. (Mass of earth = 6.0 × 1024 kg)
Using Bohr’s postulates, obtain the expressions 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 Lymann Series.
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?
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?
In a laser tube, all the photons
The dissociation constant of a weak base (BOH) is 1.8 × 10−5. Its degree of dissociation in 0.001 M solution is ____________.
The energy of an electron in an excited hydrogen atom is - 3.4 eV. Calculate the angular momentum of the electron according to Bohr's theory. (h = 6.626 × 10-34 Js)
In form of Rydberg's constant R, the wave no of this first Ballmer line is
The wavelength of the first time line of Ballmer series is 6563 A°. The Rydberg constant for hydrogen is about:-
The energy of an electron in hth orbit of hydrogen atom is –13.6/n2ev energy required to excite the electron from the first orbit to the third orbit is
In Bohr's atomic model of hydrogen, let K. P and E are the kinetic energy, potential energy and total energy of the electron respectively. Choose the correct option when the electron undergoes transitions to a higher level:
What is the energy of an electron in stationary state corresponding to n = 2?
State three postulates of Bohr's theory of 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.
State the Bohr's postulate of angular momentum of an electron.
What is the velocity of an electron in the 3rd orbit of hydrogen atom if its velocity in the 1st orbit is v0?
