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Lecture 2110/24/05

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Light Emission vs. Absorption Black body

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Dual Nature of Light Wave Refraction Diffraction Particle Photoelectric effect

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Line Emission Spectrum “Excited” atoms emit light

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Line Emission Spectrum

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Balmer series Rydberg equation Balmer Series

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Atomic Spectra and Bohr 1. 1.Any orbit should be possible and so is any energy. 2.But a charged particle moving in an electric field should emit energy. Electron would eventually run out of energy

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Bohr New theory : Quantum or Wave Mechanics e- can only exist in certain discrete orbits Stationary states e- is restricted to QUANTIZED energy states.

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n= principal quantum number n is an integer n with the lowest possible energy is said to be in the ground state Electrons with higher energy than ground state are said to be in an excited state

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Calculate the energies of n=1, n=2, and n=3 states of the hydrogen atom in J/atom. R = 1.097 x 10 7 m -1 h = 6.626 x 10 -34 J-s c = 2.998 x 10 8 m/s

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