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An excited hydrogen atom emits light with a wavelength of 486.4 nm to reach the energy level for which n = 2. In which principal quantum level did the electron begin?

Respuesta :

hamzaahmeds

Answer:

The electron began in the quantum level of 4

Explanation:

Using the formula of wave number:

Wave Number = 1/λ = Rh(1/n1² - 1/n2²)

where,

Rh = Rhydberg's Constant = 1.09677 x 10^7 /m

λ = wavelength of light emitted = 486.4 nm = 486.4 x 10^-9 m

n1 = final shell = 2

n2 = initial shell = ?

Therefore,

1/486.4 x 10^-9 m = (1.09677 x 10^7 /m)(1/2² - 1/n2²)

1/4 - 1/(486.4 x 10^-9 m)(1.09677 x 10^7 /m) = 1/n2²

1/n2² = 0.06082

n2² = 16.44

n2 = 4

Lanuel

The principal quantum level in which the electron began is 5.

Given the following data:

  • Final transition = 2
  • Wavelength = 486.4 nm = [tex]486.4 \times 10^{-9}\;m[/tex]

Rydberg constant = [tex]1.09 \times 10^7\; m^{-1}[/tex]

To determine the principal quantum level in which the electron began, we would use the Rydberg equation:

Mathematically, the Rydberg equation is given by the formula:

[tex]\frac{1}{\lambda} = R(\frac{1}{n_f^2} -\frac{1}{n_i^2})[/tex]

Where:

  • [tex]\lambda[/tex] is the wavelength.
  • R is the Rydberg constant.
  • [tex]n_f[/tex] is the final transition.
  • [tex]n_i[/tex] is the initial transition.

Substituting the parameters into the formula, we have;

[tex]\frac{1}{486.4 \times 10^{-9}} = 1.09 \times 10^7(\frac{1}{2^2} -\frac{1}{n_i^2})\\\\\frac{1}{486.4 \times 10^{-9} \times 1.09 \times 10^7}=\frac{1}{4} -\frac{1}{n_i^2}\\\\\frac{1}{5.3018} =\frac{1}{4} -\frac{1}{n_i^2}\\\\\frac{1}{n_i^2}=\frac{1}{4}-\frac{1}{5.3018}\\\\\frac{1}{n_i^2}=0.25-0.1886\\\\\frac{1}{n_i^2}=0.0614\\\\n_i^2=\frac{1}{0.0614} \\\\n_i=\sqrt{16.29} \\\\n_i=4.0[/tex]

Initial transition = 4.0

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