A hydrogen - like atom (described by the Bohr model) is observed to emit six wavelength , originating from all possible transitions between `- 0.85 eV and -0.544 eV` (inclading bohr these values )
(a) Find the atomic number of the atom
(b) Calculate the smallest wavelength emitted in these transitions .
(Take `hc = 1240) eV - nm`, ground state energy of hydrogen atom `= 13.6 eV)`

A hydrogen - like atom (described by the Bohr model) is observed to emit six wavelength , originating from all possible transitions between - 0.85 eV and -0.544 eV (including both these values ) (a) Find the atomic number of the atom (b) Calculate the smallest wavelength emitted in these transitions . (Take hc = 1240 eV - nm , ground state energy of hydrogen atom = 13.6 eV)

A hydrogen like atom (described by the Borh model) is observed to emit six wavelength, originating from all possible transitions between a group of levels. These levels have energies between - 0.85 eV and 0.544 eV (including both these values). (a)Find the atomic number of the atom. (b) Calculate the smallest wavelength emitted in these transitions. ( Take, hc = 1240 eV - nm, ground state energy of hydrogen atom =-13.6 eV)

A hydrogen like atom (described by the Borh model) is observed to emit six wavelength, originating from all possible transitions between a group of levels. These levels have energies between - 0.85 eV and 0.544 eV (including both these values). (a)Find the atomic number of the atom. (b) Calculate the smallest wavelength emitted in these transitions. ( Take, hc = 1240 eV - nm, ground state energy of hydrogen atom =-13.6 eV)

A hydrogen like atom (described by the Bohr model) is observed ot emit ten wavelengths, originating from all possible transition between a group of levels. These levels have energies between - 0.85 eV and -0.544 eV (including both these values). (a) Find the atomic number of the atom. (b) Calculate the smallest wavelength emitted in these transitions. (Take ground state energy of hydrogen atom =- 13.6 eV)

A hydrogen like atom (described by the Bohr model) is observed ot emit ten wavelengths, originating from all possible transition between a group of levels. These levels have energies between - 0.85 eV and -0.544 eV (including both these values). (a) Find the atomic number of the atom. (b) Calculate the smallest wavelength emitted in these transitions. (Take ground state energy of hydrogen atom =- 13.6 eV)

A H-like ion is observed to emit six different wavelength originating from all possible transitions between a group of levels. These levels have energies between -0.85 eV (Min) and -0.544 eV (Max) (a) Find atmoic number (z) of element (b) Find quantum number of levels between which transitions occur. (c) Calculate largest wavelength emitted in transitions between the levels.

Calculate the de Broglies wavelength associated with the electron revolving in the first excited state of hydrogen atom. The ground state energy of the hydrogen atom is -13.6 eV.