Lecture 2 Intro to atoms

Lecture 2 Intro to atoms

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Unformatted text preview: t = 6.626 x 10- 34 Js c = speed of light = 3.00 x 108 m/s λ = wavelength; ν = frequency The Bohr atom (1913) •  Electrons move around the nucleus in fixed paths or orbits much like the planets move around the sun •  Orbit posiAons, labeled with the integer n, have specific potenAal energy •  The lowest energy state of an atom is called the ground state (an electron with n = 1 for a hydrogen atom) 2π 2 me 4 b E = − 2 2 = − n2 nh b = 2.18 × 10−18 J Niels Bohr (Nobel 1922) The Bohr atom ΔE = E h − E l = ( − b − − b ) n2 n2 h ( =b 1 n l2 − n12 = hc ( 1 ) λ h ) l with n h > n l or 1 λ = b hc ( 1 n l2 − n12 h ) Theory (Bohr) = experiment (Balmer)* • The predicted and observed spectra of hydrogen are in excellent agreement • RH (empirical)...
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This document was uploaded on 03/26/2014.

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