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Bully Metric Bohr Model

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The following text was copied from the Wikipedia article about the Bohr model and was adapted to use Bully Metric Units:

The Bohr model of the hydrogen atom (Z = 1) or a hydrogen-like ion (Z > 1), where the negatively charged electron confined to an atomic shell encircles a small, positively charged atomic nucleus and where an electron jumps between orbits, is accompanied by an emitted or absorbed amount of electromagnetic energy ().[1] The orbits in which the electron may travel are shown as grey circles; their radius increases as n2, where n is the principal quantum number. The 3 → 2 transition depicted here produces the first line of the Balmer series, and for hydrogen (Z = 1) it results in a photon of wavelength 71 millapan (656 nanometer red light).

In atomic physics, the Bohr model or Rutherford–Bohr model was the first successful model of the atom. Developed from 1911 to 1918 by Niels Bohr and building on Ernest Rutherford's nuclear model. It supplanted the plum pudding model of J J Thomson only to be replaced by the quantum atomic model in the 1920s. It consists of a small, dense nucleus surrounded by orbiting electrons. It is analogous to the structure of the Solar System, but with attraction provided by electrostatic force rather than gravity, and with the electron energies quantized (assuming only discrete values).

Development

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In 1913 Niels Bohr put forth three postulates to provide an electron model consistent with Rutherford's nuclear model:

  1. The electron is able to revolve in certain stable orbits around the nucleus without radiating any energy, contrary to what classical electromagnetism suggests. These stable orbits are called stationary orbits and are attained at certain discrete distances from the nucleus. The electron cannot have any other orbit in between the discrete ones.
  2. The stationary orbits are attained at distances for which the angular momentum of the revolving electron is an integer multiple of the reduced Planck constant: , where is called the principal quantum number, and . The lowest value of is 1; this gives the smallest possible orbital radius, known as the Bohr radius, of 5.777 889 micropan (52.917 721 picometers) for hydrogen. Once an electron is in this lowest orbit, it can get no closer to the nucleus.
  3. Electrons can only gain and lose energy by jumping from one allowed orbit to another, absorbing or emitting electromagnetic radiation with a frequency determined by the energy difference of the levels according to the Planck relation: , where is the Planck constant.

Calculation of the orbits

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The Bohr model gives almost exact results only for a system where two charged points orbit each other at speeds much less than that of light. Calculation of the orbits requires two assumptions, a quantum rule and classical electromagnetism.

  • A quantum rule
The magnitude of angular momentum L = mevr is an integer multiple of ħ:
This quantum rule determines the electron's momentum (p) at any radius (r), for each integer n:
  • classical electromagnetism
The electron is held in a circular orbit by electrostatic attraction. The centripetal force is therefore equal to the Coulomb force.
where me is the electron's mass, e is the elementary charge, ke is the Coulomb constant and Z is the atom's atomic number. It is assumed here that the mass of the nucleus is much larger than the electron mass (which is a good assumption). This classical equation determines the square of the electron's momentum (p) at any radius (r), for each integer n:

Calculation of energy levels

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Classical energy is the sum of kinetic and potential energy. Classical kinetic energy is equal to one half of the mass multiplied by the velocity squared. And from the previous section, the momentum squared turns out to be equal to the Coulomb potential multiplied by the electron mass.

The total energy here is negative and inversely proportional to r. This means that it takes energy to pull the orbiting electron away from the atom. For infinite values of r, the energy is zero, corresponding to a motionless electron infinitely far from the proton. It will be advantageous to represent the Coulomb constant ke in terms of the Reduced Planck constant ħ, the speed of light c, the elementary charge e, and the fine-structure constant α.
From whence Bohr's three equations become:

Conversion to Bully Metric Units

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The Quantization Rule

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Quantization of angular momentum demands an integer value for the product of orbital radius with the momentum perpendicular to the radius. This appears as a series of parallel straight lines on a log-log plot. The above graphic includes plots for principle quantum numbers one through ten (n = 1 .. 10), and for various powers of ten (n = 100, 1000, 10000, and 100000).

Bohr's quantization rule:

Can be written in Bully units as:

This rule is not a special property of the Bohr atom, but rather, is a universal property of quantum mechanics called quantization of angular momentum. This rule has an extremely simple form when momentum and radius are plotted on a log-log graph using Bully units. The quantization of angular momentum appears as a series of parallel straight lines with a slope of negative one, each line representing an integer value of the principle quantum number n. The lowest energy level (n = 1) has the property that the momentum is always equal to the numerical inverse of the radius. For example, if an electron were to orbit a nucleus at 1 micropan (0.000001 la), then the quantization of angular momentum would require the electron's perpendicular momentum to be 1 actionat per micropan, or in other words a million actionats per length apan (1000000 An / la). The slope of negative one indicates that momentum is proportional to the inverse of the radius.

Bully Classical Electromagnetism

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In Bully Metric units, the speed of light (c = 1.0 la / ta), the reduced Planck constant (ħ = 1.0 An), and the elementary charge (1.0 e) are all normalized, which means that many of the electron's properties carry the same numeric value but with differing units as shown in Table 1.

Table 1: Electron Properties
Electron Mass (m) Rest Energy (mc2) (mcħ)
23717311.411 An ta la-2 23717311.411 An ta-1 23717311.411 An^2 la-1
Bohr's model of the hydrogen atom on a log-log plot in the Bully Metric units. The black line represents allowed radius-momentum value combinations according to Bohr's classical electromagnetism equations. The other lines represents allowed radius-momentum value combinations according to quantization of angular momentum.

Bohr's classical electromagnetism equations:

Can be written in Bully units as shown below (note that 137.035999177 is the inverse fine-structure constant):

For a hydrogen atom with one proton (Z = 1), this becomes:


When momentum and radius are plotted on a log-log graph using Bully units, Bohr's classical electromagnetism momentum equation appears as a straight line with a slope of negative two (negative two indicating that momentum squared is proportional to the inverse of the radius).

Bully Metric Solutions for Bohr's Hydrogen Atom

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  • The solution
The above two equations are sufficient to find exact r and p values (two equations in two unknowns) for each given integer n. Dividing momentum squared by momentum, the radius dependence drops out:

See Table 2 for the list of Bohr hydrogen atom energy level solutions in Bully Metric units. Table 3 provides a list of photons that are emitted or absorbed when an electron transitions to a different energy level within the Bohr hydrogen atom.

Table 2: Bohr Model Hydrogen Energy Levels
n Velocity Energy Momentum Radius
0.000000 0.000 0.000
1000 0.000007 -0.001 173.074 5.777889273
100 0.000073 -0.063 1730.736 0.057778893
10 0.000730 -6.315 17307.358 0.000577789
9 0.000811 -7.796 19230.398 0.000468009
8 0.000912 -9.867 21634.198 0.000369785
7 0.001042 -12.888 24724.798 0.000283117
6 0.001216 -17.541 28845.597 0.000208004
5 0.001459 -25.260 34614.717 0.000144447
4 0.001824 -39.468 43268.396 0.000092446
3 0.002432 -70.165 57691.194 0.000052001
2 0.003649 -157.872 86536.792 0.000023112
1 0.007297 -631.489 173073.583 0.000005778

Table

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Table 3: Photon
Transition Lyman series
(n=1)
Balmer series
(n=2)
Paschen series
(n=3)
Brackett series
(n=4)
n→∞ 631.152904
631.489478
0.336574
157.875323
157.872370
-0.002954
70.143290
70.165498
0.022207
39.468831
39.468092
-0.000738
n→9 623.360648
623.693312
0.332664
150.038067
150.076203
0.038136
62.346214
62.369331
0.023117
31.670641
31.671926
0.001285
n→8 621.290915
621.622455
0.331540
147.967622
148.005346
0.037724
60.282375
60.298474
0.016099
29.601623
29.601069
-0.000554
n→7 618.272041
618.601938
0.329896
144.948283
144.984829
0.036546
57.259259
57.277957
0.018698
26.567662
26.580552
0.012890
n→6 613.620732
613.948104
0.327372
140.295678
140.330995
0.035317
52.601056
52.624123
0.023067
21.922116
21.926718
0.004602
n→5 605.906685
606.229899
0.323214
132.579027
132.612790
0.033764
44.887329
44.905918
0.018590
14.205272
14.208513
0.003242
n→4 591.705868
592.021386
0.315518
118.373611
118.404277
0.030666
30.690963
30.697405
0.006442
n→3 561.024872
561.323981
0.299109
87.684591
87.706872
0.022281
n→2 473.364899
473.617109
0.252210

Electron shell transitions of Hydrogen atom with energies listed in Bully Metric values

  1. Lakhtakia, Akhlesh; Salpeter, Edwin E. (1996). "Models and Modelers of Hydrogen". American Journal of Physics 65 (9): 933. doi:10.1119/1.18691.