Bohr’s Theory of Hydrogen Atom
Physics ⇒ Modern Physics
Bohr’s Theory of Hydrogen Atom starts at 11 and continues till grade 12.
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Calculate the energy of the electron in the second Bohr orbit (n=2) of hydrogen atom. (Given: En = -13.6 eV/n2)
Calculate the ratio of the radii of the third and first Bohr orbits in hydrogen atom.
Describe the main limitation of Bohr’s model.
Explain the term ‘stationary orbits’ as used in Bohr’s model.
Explain why the electron does not spiral into the nucleus according to Bohr’s model.
Explain why the energy levels in hydrogen atom are negative according to Bohr’s theory.
If an electron in a hydrogen atom jumps from n=4 to n=2, what is the energy of the emitted photon? (En = -13.6 eV/n2)
If the energy of an electron in the nth orbit is En, what is the total energy of the electron in the second orbit?
If the energy of the ground state of hydrogen atom is -13.6 eV, what is the energy required to excite the electron to the third orbit?
State Bohr’s quantization condition for angular momentum.
State one experimental observation that could not be explained by Rutherford’s model but is explained by Bohr’s model.
State the formula for the energy of the nth orbit in hydrogen atom according to Bohr’s theory.
State the relationship between the energy difference of two orbits and the frequency of emitted photon in Bohr’s model.
The energy difference between two Bohr orbits in hydrogen atom is 10.2 eV. What is the wavelength of the emitted photon? (h = 6.63 × 10-34 J s, c = 3 × 108 m/s, 1 eV = 1.6 × 10-19 J)
What is the significance of the principal quantum number n in Bohr’s theory?
What is the value of the Bohr radius?
Which postulate of Bohr’s theory explains the emission of spectral lines?
Who proposed the first quantum model of the hydrogen atom?
Write the formula for the radius of the nth Bohr orbit for hydrogen atom.
