audjwood67
06.12.2019 •
Chemistry
Calculate the energy required to excite the hydrogen electron from n = 1 to level n = 2. also calculate the wavelength of light that must be absorbed by a hydrogen atom in its ground state to reach this excited state. what kind of electromagnetic radiation is used?
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Ответ:
The energy required is 1.634×J, the wavelength is 1.215×m, and the kind of electromagnetic radiation is the ultraviolet radiation.
Explanation:
In the question above, the initial level = 1, and = 2. Then, we use Rydberg's equation to calculate the wavelength of the light absorbed by the atom during the transition.
1/wavelength = R()
where:
R is the Rydberg's constant which is equal to 1.0974×
Therefore,
1/wavelength = 1.0974××() = 1.0974×× = (-) 0.8228*10^{7}
Thus,
wavelength = = 1.215*
The energy required (E) can be calculated using:
E = h*c/wavelength
where:
h is the Planck's constant = 6.626*
c is the speed of light = 299,792,458 m/s
Therefore,
E = 6.626**299,792,458 m/s÷ 1.215* = 1.634*
The kind of electromagnetic radiation used is is the ultraviolet radiation. This is the type of electromagnetic radiation with wavelength between 10 nm and 400 nm
Ответ:
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Explanation: