An electron in the n=7 level of the hydrogen atom relaxes to a lower energy level, emitting light of 1005 nm. part a what is the value of n for the level to which the electron relaxed?

rom level n = 7 to level n = 3

Explanation:

Bohr's model describes the energy levels for the hydrogen atom

         En = -13.606 / n²

Where n is an integer with values of 1, 2, 3

An electronic transition occurs between two permitted levels of energy

        ΔE = -

Let's apply these relationships our problem.

Let's start by knowing the energy of level n = 7

       E₇ = - 13.606 / 7²

       E₇ = - 0.27767 eV

Now let's see what the energy of the emitted photon

       E = h f

       c = λ f

       f = c / λ

       E = h c / λ

       E = 6.63 10⁻³⁴ 3 10⁸/1005 10⁻⁹

       E = 19,791 10⁻²⁰ J

Let's reduce to eV

       E = 19,791 10⁻²⁰ (1 eV / 1.6 10⁻¹⁹)

       E = 1,237 eV

The possible transitions from this level are towards n = 6, 5, 4,3,2, 1

We must test the different values until we find the right one

Energy of the states

n        

6       -0.378

5       -0.544

4       -0.850

3       -1,512

2       -3,402

1      -13,606

Let's examine the transition n = 7 to n = 6

      ΔE = - 0.27767 - (-0.3779)

     ΔE = 0.10023 eV

n = 7 to n = 5

     ΔE = -0.27767 - (-0.5442)

     ΔE = 0.267 eV

n = 7 a n = 4

     ΔE = -0.27767- (-0.8504)

     ΔE = 0.573 eV

n = 7 a n = 3

     ΔE = -0.27767 - (- 1.5118)

     ΔE = 1.234 Ev

This is the transition sought, so that the electron goes from level n = 7 to level n = 3

c)as speed changes, wavelength and frequency change.

everything changes!

less than one you can't create energy