Question

4

Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission spectrum Atoms give off light when heated or otherwise excited! The light emitted by excited atoms consists of only a few wavelengths, rather than a full rainbow of colors. When this light is passed through a prism, the result is a series of discrete lines separated by blank areas. The visible lines in the series of the hydrogen spectrum are caused by emission of energy accompanying the fall of an electron from the outer shells to the second shell. The wavelength (X) of the lines can be calculated using the Balmer-Rydberg equation Figure 1 of 1 TTTTTTT 650 700 nm

Answer 1

U bene voor I m R = 100 97 X102 nm =2] for Balmer series n=3 &m=2 = 1,097 x162 -1) A = 6560m) B). • n=4 &m=2 I=1.097X102 nm- = 48 6nm l a n=5 &m=2 1 =1.097 xlo ²1-116=ualul on=6 &m=2 t = 1.097 xlo2 (1-1) 7=ulonm | 7 nmi

را الماس الا ا و الد c) for 5th line; m=2, n = 7 T= 1.097 xlo? (4-) = =3979m| Thus, wandength for 5th line is 3970m o nome tu ya) 314