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Strike441 [17]
3 years ago
15

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?
Chemistry
1 answer:
bekas [8.4K]3 years ago
5 0

Answer:

The energy required is 1.634×10^{-18}J, the wavelength is 1.215×10^{-7}m, and the kind of electromagnetic radiation is the ultraviolet radiation.

Explanation:

In the question above, the initial level n_{initial} = 1, and n_{final} = 2. Then, we use Rydberg's equation to calculate the wavelength of the   light absorbed by the atom during the transition.

1/wavelength = R(\frac{1}{n_{initial} ^{2} } -\frac{1}{n_{final} ^{2} })

where:

R is the Rydberg's constant which is equal to 1.0974×10^{7} m^{-1}

Therefore,

1/wavelength = 1.0974×10^{7} m^{-1}×(\frac{1}{1 ^{2} } -\frac{1}{2^{2} }) = 1.0974×10^{7} m^{-1}×(\frac{1}{4}-\frac{1}{1} ) = (-) 0.8228*10^{7}

Thus,

wavelength = \frac{1}{0.8228*10^{7}} = 1.215*10^{-7} \frac{1}{m}

The energy required (E) can be calculated using:

E = h*c/wavelength

where:

h is the Planck's constant = 6.626*10^{-34} J.s

c is the speed of light = 299,792,458 m/s

Therefore,

E = 6.626*10^{-34} J.s*299,792,458 m/s÷ 1.215*10^{-7} \frac{1}{m} = 1.634*10^{-18} J

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

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