According to the Bohr theory for the atomic spectrum of hydrogen the energy levels of the proton -electron system depends, on the quantum number n. In an electron transition from a higher quantum level , `n_(2)` to the lower level `n_(1)`, radiation is emitted. The frequency, `v` of the radiation is given by `h v = (E_(n_(2)) - E_(n_(1)))` where, h is Planck.s constant and `E_(n_(2)), E_(n_(1))` are the energy level values for the quantum number `n_(2)` and `n_(1)`. A useful formula for the wavelength, `lambda = c//v` is given by `= lambda(Å) = (912)/(Z^(2)) xx ((n_(2)^(2)n_(1)^(2))/(n_(2)^(2)-n_(1)^(2)))` where, Z = atomic number of any one electron species viz H, `He^(+), Li^(2+), Be^(3+)`,..... For hydrogen Z=1
In the above formula, when `n_(2) rarr oo`, we have `lambda = (912)/(1^(2)) xx n_(1)^(2)`. This values of `lambda` is known as the series limit for the given value of `n_(1)`. Calculate the value of `n_(1)` for the series limit `lambda = 8208 Å`

Options

A. 5
B. 2
C. 3
D. 4

Answer

C