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
APPEARS IN
संबंधित प्रश्न
Obtain an expression for the radius of Bohr orbit for H-atom.
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
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 photon of the wavelength 150 pm strikes an atom and one of its inner bound electrons is ejected out with a velocity of 1.5 × 107 ms–1, calculate the energy with which it is bound to the nucleus.
Using Bohr's postulates, derive the expression for the orbital period of the electron moving in the nth orbit of hydrogen atom ?
Using Bohr's postulates, derive the expression for the total energy of the electron in the stationary states of the hydrogen atom ?
Using Bohr’s postulates for hydrogen atom, show that the total energy (E) of the electron in the stationary states tan 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.
Which of the following parameters are the same for all hydrogen-like atoms and ions in their ground states?
When a photon stimulates the emission of another photon, the two photons have
(a) same energy
(b) same direction
(c) same phase
(d) same wavelength
The Bohr radius is given by `a_0 = (∈_0h^2)/{pime^2}`. Verify that the RHS has dimensions of length.
Radiation coming from transition n = 2 to n = 1 of hydrogen atoms falls on helium ions in n = 1 and n = 2 states. What are the possible transitions of helium ions as they absorbs energy from the radiation?
In which of the following systems will the wavelength corresponding to n = 2 to n = 1 be minimum?
Calculate angular momentum of an electron in the third Bohr orbit of a hydrogen atom.
According to Bohr's theory, an electron can move only in those orbits for which its angular momentum is integral multiple of ____________.
What is the energy in joules released when an electron moves from n = 2 to n = 1 level in a hydrogen atom?
On the basis of Bohr's model, the approximate radius of Li++ ion in its ground state ifthe Bohr radius is a0 = 53 pm :
The ratio of the ionization energy of H and Be+3 is ______.
When an electron falls from a higher energy to a lower energy level, the difference in the energies appears in the form of electromagnetic radiation. Why cannot it be emitted as other forms of energy?
A hydrogen atom in is ground state absorbs 10.2 eV of energy. The angular momentum of electron of the hydrogen atom will increase by the value of ______.
(Given, Planck's constant = 6.6 × 10-34 Js)
For the reaction \[\ce{2NO2 (g) ⇌ N2O4(g)}\], when ΔS = −176.0 JK−1 and ΔH = −57.8 kj mol−1, the magnitude of ΔG at 298 K for the reaction is ______ kJ mol−1. (Nearest integer)
