Consider a hypothetical hydrogen-like atom. The wavelength in A ∘ for the spectral lines for the transition from n = p to n = 1 are given by, λ = 1500 p 2 p 2 - 1 , where p = 2 , 3 , 4 , . . . (given h c = 12400 eV A ∘ - 1 )

The ionisation potential of this element is 8 . 27 V .

Energy of second orbit is 6 . 2 eV

A sample of hydrogen atom gas contains 100 atoms. All the atoms are excited to the same n th excited state. The total energy released by all the atoms is 4800 49 R c h ( where R c h = 13 . 6 eV ),as they come to the ground state through various types of transitions. Find

total number of photons that can be emitted by this sample may be less than 600

Maximum energy of the emitted photon will be less than 48 49 R c h .

Maximum energy of the emitted photon may be greater than 48 49 R c h .

One hydrogen atom in its ground state is excited by means of monochromatic radiation of wavelength 975 A ∘ . You may assume the ionization energy for the hydrogen atom is 13 . 6 eV .

smallest wavelength in emission spectrum would be 975 A ∘ .

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Alpha Question Bank for Engineering: Physics>Chapter 33 - Atomic Physics>Exercise - 2>Q 24

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The ionization energy of a hydrogen-like Bohr atom is $4 Rydberg$ . If the wavelength of radiation emitted when the electron jumps from the first excited state to the ground state is $N - m$ and if the radius of the first orbit of this atom is $r - m$ then the value of $N / r = P \times 10^{2}$ then, value of $P$ . (Bohr radius of hydrogen $= 5 \times 10^{- 11} m; 1 Rydberg = 2.2 \times 10^{- 18} J$ )

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Important Questions on Atomic Physics

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Alpha Question Bank for Engineering: Physics>Chapter 33 - Atomic Physics>Exercise - 2>Q 25

Consider a hypothetical hydrogen-like atom. The wavelength in $\overset{\circ}{A}$ for the spectral lines for the transition from $n = p$ to $n = 1$ are given by, $λ = \frac{1500 p^{2}}{p^{2} - 1}$ , where $p = 2, 3, 4, . . .$ (given $h c = 12400 eV {\overset{\circ}{A}}^{- 1}$ )