Answer:
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