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15.1: The Bohr Model

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In 1913 Niels Bohr proposed a model for the hydrogen atom where the electron only exists in certain regions of space as it circulates around the nucleus (a single proton) as cartoonishly depicted in Figure 15.1B. He partially incorporated quantum theory by assumed that the orbiting electron can only have discrete values for the angular momentum. To model this behavior the angular momentum (mvr) was assumed to take integer values of , which is the reduced Planck constant (h/2π):

mvr=n

where n=1, 2, 3, etc. This means that velocity must be quantized: v=nmr. Next, Bohr conjectured that the “outward” centripetal force: mv2r matches the “inward” Coulomb attraction force:

mv2r=e24πε0r2

According to the above v=e24πε0mr, which must be equal to our previous expression velocity:

nmr=e24πε0mr

This allows us to solve for the electron’s radius: r=4πε0n22me2, which is a function of the integer n. If n = 1 the radius is: r=4πε02me2, which is the famous Bohr unit of length a0 = 0.053×109 m.

The energy can be calculated by adding the kinetic and potential from the electrostatic attraction: 12mv2e24πε0r, where the Coulomb energy is negative since the electron and proton have opposite charges. Since both velocity and radius are quantized, Bohr was able to show that the same is true for the energy levels:

E=e4m32π2ε2021n2

Inserting n = 1 gives the ground state energy: me432π2ε202=13.6 eV, which reveals how much energy has to be injected into the atom to fully remove the electron from the proton. And while this is the same value as measured experimentally, there are two problems with the model. For one, it doesn’t explain the experimental observations that the spectra change under an applied magnetic field. Also, the model only works for atoms with one electron. More importantly, if an electron is circulating about a fixed point then it should emit electromagnetic waves; this is how a microwave oven heats your leftovers. If so, the electron eventually loses all its energy and crashes into the nucleus, and poof no more atom! Obviously, this doesn’t happen. Consequently, the Bohr model was rejected which brings us to 1926 when Schrödinger formulated the hydrogen atom’s Hamiltonian and used an eigenvalue equation approach to solve it.


This page titled 15.1: The Bohr Model is shared under a CC BY-NC 4.0 license and was authored, remixed, and/or curated by Preston Snee.

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