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In Bohr's model of the hydrogen atom, which is no longer the standard for understanding the atom, the electron revolves around the nucleus in one of an array of available orbits. Each orbit is assigned a quantum number, n, starting with n = 1 for the orbit closest to the nucleus. The energy of an electron is inversely proportional to n squared, n2. Calculate the energy of an electron in the n =3 orbit.

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The energy of an electron in n=3 orbit will be "-1.52 eV". A complete solution is provided below.

The given values are:

  • n = 3 orbit

As we know,

The energy of orbital in [tex]n^{th}[/tex] shell will be:

→ [tex]E_n = \frac{-13.6}{n^2 \ eV}[/tex]

By substituting the values, we get

→       [tex]= -\frac{13.6}{3^2 \ eV}[/tex]

→       [tex]= -\frac{13.6}{9 \ eV}[/tex]

→       [tex]= -1.52 \ eV[/tex]

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https://brainly.com/question/13632935

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