I’m sure you have heard that the International Union of Pure and Applied Chemistry (IUPAC) recently announced the verification of four new elements on the periodic table: ununtrium (atomic number, *Z* = 113, discovered in 2003), ununpentium (*Z* = 115, discovered in 2004), ununseptium (*Z* = 117, discovered in 2010) and ununoctium (*Z* = 118, discovered in 2006).

Now that these four elements have been officially recognized, the period table is complete all the way through the 7^{th} row. This achievement brings to mind a natural question: Just how high in atomic number can the periodic table go? Is there a limit to how large elements may become?

Perhaps you have heard the claim that elements with *Z* > 137 cannot exist. This argument can be justified in a fairly simple way using the Bohr model of the atom, a bit of physics, and some algebra (see Appendix). Upon doing so, it can be shown that the velocity, *v*, of an electron in quantum state, *n*, of an atom is:

Equation 1

Where *c* is the speed of light and

is the fine structure constant (*e* is the elementary charge, *h* is Planck’s constant, and e_{0} is the permittivity of free space).

Using Equation 1, we see that atoms with *Z* > 137 require electrons in the first shell (*n* = 1) to exceed the speed of light^{1}. Because electrons have non zero rest mass, they cannot exceed the vacuum speed of light according to Einstein’s theory of relativity. Thus, atoms with *Z* > 137 cannot exist. Legend has it that the great physicist, Richard Feynman, first argued that element 137 was the largest possible element^{2}. It is either this folktale or Feynman’s fascination with the fine structure constant that have led to the unofficial naming of the yet to be discovered element 137 as “Feynmanium”^{2}. Martyn Poliakoff at the Periodic Table of Videos happens to think that the newly recognized element 117 should be named Feynmanium^{3}, but I’m hopeful they will save this designation for element 137 – if it is ever discovered.

Of course we know that quantum theory has improved upon the Bohr model, so it might not come as a surprise that current theoretical investigations have placed a limit on atomic size at *Z* < 173 or thereabouts^{2,4}. Nevertheless, I plan on sharing these ideas with my students in the near future. I am hopeful that my students will find this supplemental discussion to be as interesting and imaginative as I have. As a final note, the Periodic Table of Videos has posted a video on undiscovered large elements with Z > 118 for those wishing to explore this concept further^{5}.

*References and notes*

1. Another interesting result of Equation 1 is that electron speed increases with *Z*. In fact, 1s electrons in 6^{th} and 7^{th} period elements reach speeds that are significant fractions of light speed. The relativistic speeds achieved by electrons in heavy elements results in substantial chemical effects. Two notable examples are the yellow color of gold and liquidity of mercury at room temperature. For more information on these fascinating relativistic effects in chemistry, see

1. Relativistic Effects and the Chemistry of the Heaviest Main-Group Elements by John S. Thayer.

2. Would element 137 really spell the end of the periodic table? Philip Ball examines the evidence.

4. Feynmanium (?),Periodic Table of Videos.

5. Bigger Periodic Table, Periodic Table of Videos. It is interesting to note that the paper cited in reference 3 above is shown in this video!

*Appendix*

In the Bohr model, electrons are assumed to exist in fixed orbits around the nucleus of the atom. In other words, electrons are fixed at a distance, *r*, from the nucleus. In this case, an electron orbiting the nucleus would have a centripetal force, *F*, equal to:

Equation 1

Where *m* and *v* are the electron mass and velocity, respectively. This force must be equal to the coulombic (electrostatic) force between the electron and the nucleus:

Equation 2

Where *Z* is the nuclear charge, *e* is the elementary charge, and e* _{0}* is the permittivity of free space. Setting the centripetal and electrostatic forces equal to one another:

Equation 3

Using Equation 3 to solve for the velocity of the electron squared, we find:

Equation 4

A central assumption of the Bohr model of the atom is that the angular momentum of the electron, *L*, is quantized:

Equation 5

Where *h* is Planck’s constant and *n* is an integer. Solving Equation 5 for *r*:

Equation 6

If we substitute the right hand side of Equation 6 into Equation 4, we find:

Equation 7

Dividing both sides of Equation 7 by *v* yields:

Equation 8

We now multiply the top of bottom of Equation 8 by the speed of light, *c*:

Equation 9

We notice that Equation 9 contains the fine structure constant:

Equation 10

Thus, substitution of the fine structure constant into Equation 9 yields the equation we seek:

Equation 11

## NGSS

Students who demonstrate understanding can use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.

*More information about all DCI for HS-PS1 can be found at https://www.nextgenscience.org/dci-arrangement/hs-ps1-matter-and-its-interactions and further resources at https://www.nextgenscience.org.

Students who demonstrate understanding can use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.

Assessment is limited to main group elements. Assessment does not include quantitative understanding of ionization energy beyond relative trends.

Examples of properties that could be predicted from patterns could include reactivity of metals, types of bonds formed, numbers of bonds formed, and reactions with oxygen.