Question

1: Calculate the wavelength of the fifth line in the hydrogen atom Paschen series?

2: Calculate the energy released in the transition described in the question above?

3: For the hydrogen atom, calculate the wavelength of the light needed to excite the electron from the fifth energy level to the ninth energy level.

Answer 1

DE = (911x10 31 ) x (1.6028101934 8 +(885*10-12 ): (6626410-24; 2* GG282) 2.18 810 18 x 55 J lor, 13.6* 51 16 eu 576 = 2.08*10 - 298 eV ,: The Energy released in above question is in the trang, tion 2.08x10 19 J on described 1.298 ev. for, hydrogen atom, the wavelength of the light needed to excite the electron from fifth energy level to the Euch ninth energy lever is to Pu Cha tez) - 109677x107 ( 2) = 303304.29 = 3.297 210-6 m = 3297x109 m - 3297 nm.

0.17 DE 1 The wavelength : of the line in the spectrum of atomic hydrogen may be described by the Simple relation. * = RH(2 h) [mayn] Where RH = Rydberg Constant for hydrogen = 1.09677 2107 m For particular series, n, nemains content; Successive vorriation in an for paschen series, n, = 3 for fifth line, h = 8 now, $ = 1.09677X10* (12- 2) e = 1047263.02 The a in 3. FE ne leve 9 9.548 x107 m = 954.86 410 m - 954.86 um . The wavelength yorogen atom fifth of the Paachen line in the series is 954.86 nm. The Energy released in the trangition: above ri m2 e DE = En-En, a Fon hydrogen atom, Z=1 m= 9.1 x 10-3kg E. = 8.85 x 10-12 2²0m 2 e = 1.602x104c h = 6.626x10 SJS.