Physics: bohr's atomic model

code PLUS

2013-11-02 6:39 pm

Which of the following is a possible energy value for a hydrogen atom?
A -0.243 eV
B -0.378 eV
C -6.80 eV
D -15.6 eV

In a hydrogen emission spectrum, the shortest wavelength of the Lyman series is about 91.4 nm. What is the initial energy level of the transition that produces this spectral line?

A n=0
B n=infinity
C n=1
D cannot be determined

An atom transits from energy level -0.5 eV to -1.5 eV. What is the wavelength of photon emitted?

Please include steps and explanation.

回答 (1)

天同

2013-11-03 3:36 am

✔ 最佳答案

1. Option B
Energy level = -13.6/n^2 eV
where n = 1, 2, 3...
-0.378 eV corresponds to n = 6

2. Option B
The shortest wavelength corresponds to the highest transition energy. Hence, n = infinity to n = 1

3. Energy of photon
= (-0.5 - (-1.5)) eV = 1 eV = 1.6 x 10^-19 J
Use: E = hc/入
where E is the photon energy
h is Planck's Constant (=6.62 x10^-32 kg.m^2/s)
c is the speed of light
入 is 1hte wavelength
hence, 入 = hc/E = (6.62x10^-34) x (3x10&8)/1.6x10^-19 m = 1.24 x 10^-6 m

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