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Electron Structure in Atoms

Explore the wave nature of light, Quantum Numbers, Bohr's Model, and more in the study of electron structure within atoms. Learn how to calculate photon energy and electron transitions.

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Electron Structure in Atoms

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  1. Electron Structure in Atoms AP Chemistry Jeremy Wolf

  2. Wave Nature of Light • Where v (nu) is the frequency of the radiation in reciprocal seconds (s–1), l (lambda) is the wavelength in meters, c is the speed of light (3.00 x 108 m/s), and h is Plank’s constant (6.626 x 10-34 J*s). • E = h v • c = λv

  3. Sample Problem • What is the energy of a photon with the wavelength of 500 nm? • c = λv • 3.00 x 108 m/s = 500 x 10-9 m * (v) • v = 5.98 x 1014 1/s • E = h v • E = (6.626 x 10-34 J*s)(5.98 x 1014 1/s) • E = 3.96 x 10-19 Joules

  4. Photoelectric Effect

  5. Bohr’s Model • RH is the Rydberg constant (2.18 x 10–18J). The energy of an electron is, by convention, a negative number. When an electron resides in the orbit designated by n = 1, it is said to be in the ground state.

  6. Electron Transitions

  7. Wave Behavior of Matter • De Broglie’s Equation to calculate the wave nature of any particle:

  8. Quantum Numbers for Atomic Orbitals • 1. The principal QN, n, can have positive integer values. (1, 2, 3, . . . ). The principal quantum number determines the size of the orbital. The larger the value of n, the larger the orbital. • 2. The second or azimuthal QN, l, can have integer values from 0 to n–1. The value of l determines the shape of the orbital. Each value of l has a letter associated with it to designate orbital shape. • 3. The magnetic quantum number, ml, can have integer values from –l through +l. The magnetic quantum number determines the orbital's orientation in space. • The Spin QN, ms, can be either +1/2 or -1/2 and it describes the electron’s rotation about its axis as either clockwise or counter-clockwise

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