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?

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

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