n

1
CH123 Gen. Chem 10/15/03 Dr J H atom energy
levels
J/atom
kJ/mol
n
Balmer (visible)
Paschen (infrared)
Lyman (ultraviolet)
6
-6.06 x 10-20
-8.72 x 10-20
- 52.5
5
infrared
- 82.0
-1.36 x 10-19
4
-146
-2.42 x 10-19
3
-328
-5.45 x 10-19
2
656.3 nm
-1312
-2.18 x 10-18
1
486.1 nm
434.1 nm
410.2 nm
Balmer/Rydberg Equation (empirical)
1
1

R
-
where R 1.097 x 10-2 nm-1
nup2
ultraviolet
nlow2
Bohr Equation (theoretical)
E -2.18 x 10-18 J/e
Or E - 1312 kJ/mol
n2
n2
Using the Rydberg Equation and the Bohr equation,
calculate the wavelength of a photon emitted when
an electron falls from n 6 to n 2. h 6.626
x 10-34 J.s c 2.998 x 108 m/s
Hydrogennrglevels.ppt