English

How will the energy of a hydrogen atom change if n increases from 1 to ∞?

Advertisements
Advertisements

Question

How will the energy of a hydrogen atom change if n increases from 1 to ∞?

Short/Brief Note
Advertisements

Solution

`"E"_"n" ∝ (-1)/"n"^2`

Energy is minimum at n = 1

As n increases, the energy becomes less negative, which means energy increases.

shaalaa.com
  Is there an error in this question or solution?
2021-2022 (March) Term 2 - Delhi Set 2

RELATED QUESTIONS

What is the maximum number of emission lines when the excited electron of an H atom in n = 6 drops to the ground state?


  1. Using the Bohr’s model, calculate the speed of the electron in a hydrogen atom in the n = 1, 2 and 3 levels.
  2. Calculate the orbital period in each of these levels.

When the electron orbiting in hydrogen atom in its ground state moves to the third excited state, show how the de Broglie wavelength associated with it would be affected.


The spectral line obtained when an electron jumps from n = 5 to n = 2 level in hydrogen atom belongs to the ____________ series.


Hydrogen atom has only one electron, so mutual repulsion between electrons is absent. However, in multielectron atoms mutual repulsion between the electrons is significant. How does this affect the energy of an electron in the orbitals of the same principal quantum number in multielectron atoms?


The inverse square law in electrostatics is |F| = `e^2/((4πε_0).r^2)` for the force between an electron and a proton. The `(1/r)` dependence of |F| can be understood in quantum theory as being due to the fact that the ‘particle’ of light (photon) is massless. If photons had a mass mp, force would be modified to |F| = `e^2/((4πε_0)r^2) [1/r^2 + λ/r]`, exp (– λr) where λ = mpc/h and h = `h/(2π)`. Estimate the change in the ground state energy of a H-atom if mp were 10-6 times the mass of an electron.


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:


The line at 434 nm in the Balmer series of the hydrogen spectrum corresponds to a transition of an electron from the nth to second Bohr orbit. The value of n is ______.


An electron in a hydrogen atom has an energy of -3.4 eV. The difference between its kinetic and potential energy is ______.


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)


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×