Using equation 3.0, the energies of the final and initial states can be written as

En - - Ru(1/n7)

(4)

Ery = - RH(1/ n/)

(5)

AE - Eny - En, = - Ru(1/no) + Ru(1/n/) - RH(1/np - 1/n/) (6)

AE = hv

(7)

Setting the results of equations 6.0 and 7.0 equal to one another

v = (RH/h)[1/n2 - 1/nr)

(8)

where Ru is Rydberg's constant, h is Planck's constant, n is the principal

quantum number of the initial state and my is the principal quantum number of

the final state:

EXPERIMENTAL PROCEDURE

1. From a literature source, obtain the known wavelengths for the four emission

lines in the visible wavelength range for hydrogen and record them in the

table below.

Data Table

Line Color and Wavelengths

Line Color

Line Wavelength(nm)

(Literature)

Thed

yellow

monm

2. Using the literature values for the wavelengths, convert these wavelength

values to frequencies using the relationship

V -c/ 2

191

where v is the frequency in sec ', c is the speed of light ( x 105 m/sec) and ) Is

the wavelength in nanometers. Record these frequencies in the following table.

Violet = ( 3x 10") /(4x10 ) 7.5x 10" he

green : ( 3x 100) ) (5x 10 7)= GRIM hz

yellow = ( 34 10 )/(5. 25 x 10-1):5.129 x1014 hz

Red = ( 3x 10# ) / (6.5 x 10-7)= 4.415 x 101 h2 32