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In Bohr series of lines of hydrogen spectrum, the third line from the red end corresponds to which one of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen ?
The orbital angular momentum for an electron revolving in an orbit is given by $ \sqrt { l ( l+1 )} . { h \over 2 \pi } $ This momentum for an s-electron will be given by
The orbital angular momentum for an electron is given by √[l(l+1)] ħ/2π, where l is the orbital angular momentum quantum number. For an s-electron, l=0, so √[l(l+1)] becomes 0, and the orbital angular momentum is zero.
The emission spectrum of hydrogen is found to satisfy the expression for the energy change “E (in Joules) such that $ “E = 2·18 \times 10^{–18} J where n_1 = 1,2, 3 ..........and n_2 = 2,3 ,4 $ The spectral lines correspond to Paschen series it
Among the following series of transition metal ions, the one where all metal ions have same 3d electronic configuration is
For d-electron, the orbital angular momentum is
Where the value of l for d orbital is 2
Time taken for an electron to complete one revolution in the Bohr orbit of hydrogen atom is
Which of the following sets of quantum numbers is correct for an electron in 4f – orbital ?
The correct set of quantum numbers for an electron in the 4f orbital is n = 4, l = 3 (for f orbital), m = +1, s = +1/2. The principal quantum number (n) determines the shell, l determines the subshell, m determines the orientation, and s represents the spin of the electron.
The wavelength of radiation emitted when in a hydrogen atom electron falls from infinity to stationary state 1, would be (Rydberg constant  1·09 × 107m–1)
The relationship between energy E, of the radiation with a wavelength 8000 Ã… and the energy of the radiation with a wavelength 16000 Ã… is
The energy of second Bohr orbit of the hydrogen atom is $ –328 kJ mol^{–1} $ , hence the energy of fourth Bohr orbit would be
The energy of an electron in the Bohr model of the hydrogen atom is given by E = -13.6/n^2 eV, where n is the principal quantum number. For n = 2, E = -13.6/2^2 = -3.4 eV or -328 kJ/mol. For n = 4, E = -13.6/4^2 = -0.85 eV or -82 kJ/mol.
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