Lecture 18

# Lecture 18 - Calculate the wavelength of light emitted when...

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( 29 ( 29 ( 29 m 10 21 . 1 10 64 . 1 10 00 . 3 10 626 . 6 E hc 7 J 18 - s m 8 s J 34 - - × = × × × = = λ Solve: Calculate the wavelength of light emitted when the hydrogen electron transitions from n = 2 to n = 1 E=hc/ λ, E n = -2.18 x 10 -18 J (1/ n 2 ) Concept Plan: Relationships: n i = 2, n f = 1 λ, m Given: Find: - = 2 H 1 R E n n i , n f E atom E photon λ E c h = E atom = -E photon J 10 64 . 1 2 1 1 1 J 10 18 . 2 E 18 2 2 18 atom - - × - = - × - = E photon = -(-1.64 x 10 -18 J) = 1.64 x 10 -18 J the unit is correct, the wavelength is in the UV, which is appropriate because more energy than 3→2 (in the visible) Check:

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Probability & Radial Distribution Functions ψ 2 is the probability density the probability of finding an electron at a particular point in space for s orbital maximum at the nucleus? decreases as you move away from the nucleus the Radial Distribution function represents the total probability at a certain distance from the nucleus
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## This note was uploaded on 05/20/2008 for the course CHEM 115 taught by Professor Larkin during the Spring '08 term at Bloomsburg.

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Lecture 18 - Calculate the wavelength of light emitted when...

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