307582 Balmer gave an equation for wavelength of visible region of H-spectrum as \({\rm{\lambda = }}\frac{{{\rm{K}}{{\rm{n}}^{\rm{2}}}}}{{{{\rm{n}}^{\rm{2}}}{\rm{ - 4}}}}\). Where \({\rm{n = }}\) principal quantum number of energy level, \({\rm{K = }}\) constant in terms of R (Rudberg constant). The value of K in terms of R is:

307583 Which transition of the hydrogen spectrum would have the same wavelength as the Balmer transition, \({\rm{n = 4}}\) to \({\rm{n = 2}}\) of \({\rm{H}}{{\rm{e}}^{\rm{ + }}}\) spectrum?

307584 Wave number of a spectral line for a given transition is x \({\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\) for \({\rm{H}}{{\rm{e}}^{\rm{ + }}}{\rm{,}}\) then its value for \({\rm{B}}{{\rm{e}}^{{\rm{3 + }}}}\) for the same transition is

307585 What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman series?

307586 In hydrogen atomic spectrum, a series limit is found at \({\rm{12186}}{\rm{.3}}\,{\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\). Then it belong to:

307582 Balmer gave an equation for wavelength of visible region of H-spectrum as \({\rm{\lambda = }}\frac{{{\rm{K}}{{\rm{n}}^{\rm{2}}}}}{{{{\rm{n}}^{\rm{2}}}{\rm{ - 4}}}}\). Where \({\rm{n = }}\) principal quantum number of energy level, \({\rm{K = }}\) constant in terms of R (Rudberg constant). The value of K in terms of R is:

307583 Which transition of the hydrogen spectrum would have the same wavelength as the Balmer transition, \({\rm{n = 4}}\) to \({\rm{n = 2}}\) of \({\rm{H}}{{\rm{e}}^{\rm{ + }}}\) spectrum?

307584 Wave number of a spectral line for a given transition is x \({\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\) for \({\rm{H}}{{\rm{e}}^{\rm{ + }}}{\rm{,}}\) then its value for \({\rm{B}}{{\rm{e}}^{{\rm{3 + }}}}\) for the same transition is

307585 What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman series?

307586 In hydrogen atomic spectrum, a series limit is found at \({\rm{12186}}{\rm{.3}}\,{\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\). Then it belong to:

307582 Balmer gave an equation for wavelength of visible region of H-spectrum as \({\rm{\lambda = }}\frac{{{\rm{K}}{{\rm{n}}^{\rm{2}}}}}{{{{\rm{n}}^{\rm{2}}}{\rm{ - 4}}}}\). Where \({\rm{n = }}\) principal quantum number of energy level, \({\rm{K = }}\) constant in terms of R (Rudberg constant). The value of K in terms of R is:

307583 Which transition of the hydrogen spectrum would have the same wavelength as the Balmer transition, \({\rm{n = 4}}\) to \({\rm{n = 2}}\) of \({\rm{H}}{{\rm{e}}^{\rm{ + }}}\) spectrum?

307584 Wave number of a spectral line for a given transition is x \({\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\) for \({\rm{H}}{{\rm{e}}^{\rm{ + }}}{\rm{,}}\) then its value for \({\rm{B}}{{\rm{e}}^{{\rm{3 + }}}}\) for the same transition is

307585 What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman series?

307586 In hydrogen atomic spectrum, a series limit is found at \({\rm{12186}}{\rm{.3}}\,{\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\). Then it belong to:

307582 Balmer gave an equation for wavelength of visible region of H-spectrum as \({\rm{\lambda = }}\frac{{{\rm{K}}{{\rm{n}}^{\rm{2}}}}}{{{{\rm{n}}^{\rm{2}}}{\rm{ - 4}}}}\). Where \({\rm{n = }}\) principal quantum number of energy level, \({\rm{K = }}\) constant in terms of R (Rudberg constant). The value of K in terms of R is:

307583 Which transition of the hydrogen spectrum would have the same wavelength as the Balmer transition, \({\rm{n = 4}}\) to \({\rm{n = 2}}\) of \({\rm{H}}{{\rm{e}}^{\rm{ + }}}\) spectrum?

307584 Wave number of a spectral line for a given transition is x \({\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\) for \({\rm{H}}{{\rm{e}}^{\rm{ + }}}{\rm{,}}\) then its value for \({\rm{B}}{{\rm{e}}^{{\rm{3 + }}}}\) for the same transition is

307585 What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman series?

307586 In hydrogen atomic spectrum, a series limit is found at \({\rm{12186}}{\rm{.3}}\,{\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\). Then it belong to:

307582 Balmer gave an equation for wavelength of visible region of H-spectrum as \({\rm{\lambda = }}\frac{{{\rm{K}}{{\rm{n}}^{\rm{2}}}}}{{{{\rm{n}}^{\rm{2}}}{\rm{ - 4}}}}\). Where \({\rm{n = }}\) principal quantum number of energy level, \({\rm{K = }}\) constant in terms of R (Rudberg constant). The value of K in terms of R is:

307583 Which transition of the hydrogen spectrum would have the same wavelength as the Balmer transition, \({\rm{n = 4}}\) to \({\rm{n = 2}}\) of \({\rm{H}}{{\rm{e}}^{\rm{ + }}}\) spectrum?

307584 Wave number of a spectral line for a given transition is x \({\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\) for \({\rm{H}}{{\rm{e}}^{\rm{ + }}}{\rm{,}}\) then its value for \({\rm{B}}{{\rm{e}}^{{\rm{3 + }}}}\) for the same transition is

307585 What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman series?

307586 In hydrogen atomic spectrum, a series limit is found at \({\rm{12186}}{\rm{.3}}\,{\rm{c}}{{\rm{m}}^{{\rm{ - 1}}}}\). Then it belong to: