Example 1


State the difference between the ground state and excited state of an electron in an atom. An electron of a hydrogen atom is excited to n = 6 and falls to a lower energy level forming the Paschen series. Calculate, in kJ mol–1 , the energy of the electron at the excited level and the energy emitted as the result of the transition. Determine the shortest wavelength in nanometers (nm) in the Paschen series for the hydrogen atom.

   


 Question 2

Describe the formation of emission spectrum for hydrogen atom. Show and label the first three series of electron transitions between energy levels. An electron is a hydrogen atom is transferred from n = 5 to n = 3. Calculate the energy of the photon emitted and the wavelength of the spectral line produced.

 

Question 3 

 Describe the formation of the line emission spectrum of hydrogen atom in the Lyman series. Calculate the ionisation energy (kJ mol-1 ) of the hydrogen atom using FIGURE 1. (refer video) Name two species that exhibit similar line spectrum as that of hydrogen atom.

 

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