Given that rh= 2.18 x 10⁻¹⁸j, 1 nm = 1 x 10⁻⁹m, h = 6.63 x 10⁻³⁴j·s, and c = 3.00 x 10⁸m/s:
calculate the wavelength, innanometers, of the light emitted by a hydrogen atom during a transition of its electron from the n = 7 to the n = 3 principal energy level.

The wavelength the light emitted by a hydrogen atom during a transition is 1006 nm.

Explanation:

By using Rydberg's Equation we cab determine the wavelength of the light:

Where,

= Energy difference

= Rydberg's Constant

= Final energy level

= Initial energy level

We have : , Z = 1

Now by using Plank's equation we can determine the wavelength of the light emitted.

E = Energy of the emitted light

h = Planck's constant =

c = speed of light =

For the given transition the energy of the light = E

The wavelength the light emitted by a hydrogen atom during a transition is 1006 nm.

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chemistry sucks a**

explanation: