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of Electrons in the First Shell 
The Bohr model of a hydrogenlike ion predicts that the total energy E of an electron is given by
where Z is the net charge experienced by the electron, n is the principal quantum number and R is a constant equal to approximately 13.6 electron volts (eV). This formula is the result of the total energy being equal to
where e is the charge of the electron and r_{n} is the orbit radius when the principal quantum number is n. The orbit radius is given by
where h is Planck's constant divided by 2π and m_{e} is the mass of the electron.
Electrons in atoms are organized in shells whose capacities are equal to 2m², where m is an integer. Thus there can be at most 2 electrons in the first shell, 8 in the second shell and 18 in the third shell. Here only the first shell is being considered. For elements above helium all of the electrons have been removed except two.
Here are all the ionization potentials for such ions.
The Ionization Potentials for the Electrons in the First Shell for the Elements Helium through Copper 


Proton Number  Ionization Potential First Electron  Ionization Potential Second Electron 
2  54.41778  24.58741 
3  122.45429  75.64018 
4  217.71865  153.89661 
5  340.2258  259.37521 
6  489.99334  392.087 
7  667.046  552.0718 
8  871.4101  739.29 
9  1103.1176  953.9112 
10  1362.1995  1195.8286 
11  1648.702  1465.121 
12  1962.665  1761.805 
13  2304.141  2085.98 
14  2673.182  2437.63 
15  3069.842  2816.91 
16  3494.1892  3223.78 
17  3946.296  3658.521 
18  4426.2296  4120.8857 
19  4934.046  4610.8 
20  5469.864  5128.8 
21  6033.712  5674.8 
22  6625.82  6249 
23  7246.12  6851.3 
24  7894.81  7481.7 
25  8571.94  8140.6 
26  9277.69  8828 
27  10012.12  9544.1 
28  10775.4  10288.8 
29  11567.617  11062.38 
An ion with only one electron is equivalent to the hydrogen atom but having a positive charge of Z instead of one. The Bohr theory applies to such system. According to the Bohr theory the ionization potential should be
R is constant and n, the quantum number, is equal to 1. Thus the ionization potential should be proportional to the proton number squared. Here is the plot of the relationship.
It certainly looks like a quadratic relationship. To test this proposition more precisely the logarithms of the ionization potential and the proton numbers are computed. The plot of these quantitites is shown below.
The regression equation of the logartithm of ionization potential on the logarithm of the proton number is
The numbers in the square brackets are the tratios for the regression coefficients. For a regression coefficient to be statistically significantly different its magnitude must be greater than 2.0. As can be seen the regression coefficient for ln(#p) is highly significant. And the value appears to be essentially 2, as the Bohr theory predicts. However this proposition is tested by comparing the difference between the regression coefficient and 2 with the standard deviation of the regression coefficient. Although the difference is small, 0.004056, the standard deviation of the regression coefficient is even smaller, 0.000486039, the ratio is 8.3. Common sense however says that the Bohr theory is verified for the first electron in the the first shell.
The Z in the formula is the net charge experienced by the electron, the number of protons #p in the nucleus less any shielding ε. The Bohr theory equation is then
where R is the Rydberg constant, 13.6 eV.
Thus the appropriate regression equation would be
Since in this case there seems to be no reason for there to be any shielding for the first electron the value of ε should be essentially zero.
The results of the regression are:
The coefficient of #p is negative but statistically different from zero. The coefficient of (#p)² is notably close to 13.6. The value of ε can be found as
Somehow some small portion of the charge of the nucleus is being shielded.
The Bohr theory works marvelously well for an atom or ion with one electron but not nearly so well for multiple electrons. One line of approach is to treat the atom or ion with two electrons as a manybody problem. This approach does not come up with much in the way of definite results. An alternate line of approach is to say that electrons in the same shell shield some fraction of a positive charge in the nucleus. This shielding ratio would be based upon the proportion of the charge of an electron which is closer to the nucleus than the center of an electron. The value of one half would be plausible. However the shielding ratio could be affected by any deviation from spherical symmetry.
The shielding ratio ρ for the electrons in the first shell can be computed as
where E_{1} and E_{2} are the ionization potentials for the first and second electrons, respectively.
The values for the elements for which the data is available in the CRC Handbook of Physics and Chemistry 82nd Edition (20012002) are given below.
The Shielding Ratio of the Electrons in the First Shell for the Elements Helium through Copper 


Proton Number  Shielding Ratio 
2  0.548173226 
3  0.382298652 
4  0.293139977 
5  0.237638033 
6  0.199811573 
7  0.172363225 
8  0.151616443 
9  0.135258834 
10  0.122134019 
11  0.111348807 
12  0.10234044 
13  0.09468214 
14  0.088116709 
15  0.082392514 
16  0.077388254 
17  0.072922812 
18  0.068985102 
19  0.065513374 
20  0.062353287 
21  0.059484443 
22  0.056871451 
23  0.054487091 
24  0.052326782 
25  0.050319998 
26  0.048470039 
27  0.046745345 
28  0.045158416 
29  0.043676844 
The graph of these data displays a very regular pattern.
This appears to be a relationship of the form
The value of the parameters α and β can be found by plotting the logarithms of ρ and #p, as below.
A regression of ln(ρ) on ln(#p) gives:
The results indicate that the shielding ratio is predictable on the basis of the proton number, but the shielding of positive charge in the nucleus by the electrons in the first shell is primarily important for small nuclides.
Previously a regression equation of the form
was applied to the data for the first electron and it was found that there was a shielding of 0.179758072 units of charge. When the data for the ionization potentials of the second electron is used the regression results are
Again the coefficient of #p is negative and the coefficient of (#p)² is notably close to the Rydberg constant of 13.6. The value of the shielding that is found from the coefficients is 0.777385892. The difference between this value and the value for the first electron is 0.59762782, indicating that the second electron shields about 0.6 of a unit charge of the nucleus. This is notably close to the value of 0.5 suggested by the simplest formulation of the notion of shielding by electrons in the same shell.
(To be continued.)
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