List of top Chemistry Questions on Developments Leading to the Bohr’s Model of Atom

Using s, p, d notations, describe the orbital with the following quantum numbers.
  1. n=1, l=0
  2. n = 3, l=1
  3. n = 4, l =2
  4. n=4, l=3
What is the maximum number of emission lines when the excited electron of a H atom in n = 6 drops to the ground state?
Yellow light emitted from a sodium lamp has a wavelength (λ) of 580 nm. Calculate the frequency (ν) and wavenumber (v) of the yellow light
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.
Calculate the wavenumber for the longest wavelength transition in the Balmer series of atomic hydrogen.
  1. The energy associated with the first orbit in the hydrogen atom is –2.18×10–18 J atom–1. What is the energy associated with the fifth orbit ?
  2. Calculate the radius of Bohr’s fifth orbit for hydrogen atom.
What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?
Electromagnetic radiation of wavelength 242 nm is just sufficient to ionize the sodium atom. Calculate the ionization energy of sodium in kJ mol–1.
A photon of wavelength \(4×10^{–7} m\) strikes on metal surface, the work function of the metal being \(2.13\ eV\). Calculate:
  1. the energy of the photon (eV)
  2. the kinetic energy of the emission, and
  3. the velocity of the photo electron (\(1\ eV= 1.6020×10^{–19} J\)).
Calculate the wavelength, frequency and wave number of a light wave whose period is \(2.0×10^{–10}\ s\).
What is the number of photons of light with a wavelength of 4000 pm that provide 1J of energy?