Time taken for an electron to complete one revolution in the Bohr orbit of hydrogen atom is
- A$\frac{4\pi^2 m r^2}{nh}$
- B$\frac{nh}{4\pi^2 mr}$
- C$\frac{nh}{4\pi^2 m r^2}$
- D$\frac{h}{2\pi mr}$
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When electromagnetic radiation of wavelength $300 \, nm$ falls on the surface of sodium,electrons are emitted with a kinetic energy of $1.68 \times 10^{5} \, J \, mol^{-1}$. What is the minimum energy needed to remove an electron from sodium? What is the maximum wavelength that will cause a photoelectron to be emitted?
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View SolutionWrite down the postulates of Bohr's model for the hydrogen atom.
Observe the following statements:
Statement-$I$: Rutherford model of an atom cannot explain the stability of an atom.
Statement-$II$: The wavelength of $X$-rays is higher than the wavelength of microwaves.
The correct answer is:
Statement-$I$: Rutherford model of an atom cannot explain the stability of an atom.
Statement-$II$: The wavelength of $X$-rays is higher than the wavelength of microwaves.
The correct answer is:
Which of the following electronic transitions in a hydrogen atom will require the highest energy?
Find the wave number of the shortest wavelength in the Balmer series.
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