What is the energy in joules required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of light emitted when the electron returns to the ground state? The ground state electronic energy is – 2.18 * 11^-11 ergs.

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Payal Gupta | Contributor-Level 10

9 months ago

Step I: calculation of energy required

Energy of electron (E_n) = (- 2.18 x 10^-11ergs) / n²= (- 2.18 x 10^-18J) / n²

Energy in Bohr's 1^st orbit (E₁) = (- 2.18 x 10^-18J) / 1²

Energy in Bohr's 5^th orbit (E₁) = (- 2.18 x 10^-18J) / 5²

Therefore, energy required (ΔE) = E₅ – E₁ = [ (- 2.18 x 10^-18J) / 25] –

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What is the energy in joules required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of light emitted when the electron returns to the ground state? The ground state electronic energy is – 2.18 * 11-11 ergs.