In the course of developing his model, Bohr arrived at the following formula for the radius of the electron’s orbit: rₙ = n²h²€₀/πmee², where m_{\mathrm{e}} is the electron mass, e is its charge, and ε₀ is a constant related to charge attraction in a vacuum. Given that me = 9.109×10⁻³¹ kg, e = 1.602×10⁻¹⁹C, €₀ = 80854×10⁻¹² C²/J . m , calculate the following:
(b) The radius of the tenth (n = 10) orbit in the H atom

The three-dimensional area covering the nucleus of an atom is called electron orbital. Electrons sometimes fill low-energy orbitals which are closer to the nucleus before filling the higher ones. They mostly fill the orbitals as singly as they can and that filling is known as Hund’s rule. In the wave-like property, electrons don’t orbit a nucleus in the way a planet orbits the sun but however, but they exist as standing waves. The lowest energy possible an electron can take is the same as the fundamental frequency of a wave on a string.

the radius of the first orbit =0.0529nm

radius ∝ n²/z

radius of 10th orbit =(0.0529×100)nm=52.9A°

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