i.          Explain why each successive line becomes closer to the previous one until the lines form a continuum

                           ii.          Calculate the frequency of the light that produces line Q.

                           i.          Write the electronic configuration of M 3- .

                           ii.          Give a set of quantum numbers for an electron in the 3s orbital. State two differences between 2s and 3s orbitals. 

Calculate the frequency of line A.

                           i.          Write the expected and the observed valence electronic configuration of the copper in the form of orbital diagram.

                           ii.          Explain the deviation between the expected and the observed valence electronic configuration of copper.

                           iii.          Give the set of quantum number in the for the valence electron that occupy the s orbital of copper.

                           i.          State the region of the electromagnetic spectrum for the above wavelength 

                           ii.          Determine the energy level of the excited state for this transition. State the transition involved to form the emission spectrum

                           i.          Write the electronic configuration of the valence electrons for arsenic, As.

                           ii.         Give a set of quantum numbers of one valence electron in the s orbital in b(i). 

(c) Draw and label one of the three-dimensional shapes of d orbitals where electron occupied the space that lies on the axes.

(a) Calculate the ionisation energy of hydrogen atom in kJ mol-1.    

(b) (i) State Heisenberg’s uncertainty principle.    

          (ii) Give one Bohr’s postulate that is contradictory to the above principle.    

                           i.