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Question
According to Bohr's theory, the electronic energy of hydrogen atom in the Bohr's orbit is given by
En = 21.76×10−19n2 J
Calculate the longest wavelength of light will be needed to remove an electron from the third orbit of the He+
En = 21.76×10−19n2 J
Calculate the longest wavelength of light will be needed to remove an electron from the third orbit of the He+
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Solution
En = -21.76×10−19n2 J
For He⊕, En = -21.76×10−19×z2n2 J
E3(for He⊕ = -21.76×10−19×2232 J = -9.68 × 10−19 J
Energy required to remove an e− form the third Bohr orbit of He⊕
ΔE = 0 - E3 = 0 -(-9.68 × 10−19 J)
=9.68 × 10−19 J (Since IE is +ve)
Since Δ E = -hcλ J = 9.68 × 10−19 J
λ = -hcΔE = -6.266×10−34Js×3×108m9.68×10−19J
=2.05× 106−7 m = 2050 × 10−10 m = 2050A0
For He⊕, En = -21.76×10−19×z2n2 J
E3(for He⊕ = -21.76×10−19×2232 J = -9.68 × 10−19 J
Energy required to remove an e− form the third Bohr orbit of He⊕
ΔE = 0 - E3 = 0 -(-9.68 × 10−19 J)
=9.68 × 10−19 J (Since IE is +ve)
Since Δ E = -hcλ J = 9.68 × 10−19 J
λ = -hcΔE = -6.266×10−34Js×3×108m9.68×10−19J
=2.05× 106−7 m = 2050 × 10−10 m = 2050A0
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