I'm totally confused by the different conventions and when to use what. In the Periodic Table I see


However, in books when talking about isotopes I see


I don't understand the difference between the two. I know what the numbers mean but I don't understand when to use which convention. Are there names for these two conventions?

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    $\begingroup$ Could you show the table or link to it? $\endgroup$
    – Karsten
    Apr 28, 2019 at 15:59

3 Answers 3


Periodic tables of elements (PTEs) are often abused by designers. Books are more trustworthy as long as they are written by scientists. Long story short, the second notation $(\ce{^{12}_{6}C})$ is the correct one. There is an easy to remember AZE notation: $^A_Z\ce{E}$.

I suspect the PTE you were looking at lists standard (averaged) atomic weights of the elements $A_\mathrm{r}$ rounded to the nearest whole number so it may appear as if those were the mass numbers $A$, probably something like this:

Basic PTE:carbon

Basic PTE:legend

* The atomic weights listed on this Table of Elements have been rounded to the nearest whole number. As a result, this chart actually displays the mass number of a specific isotope for each element. An element's complete, unrounded atomic weight can be found on the It's Elemental website: http://education.jlaborgfitselemental/

Note that a good periodic table usually includes a legend which deciphers and justifies designer's choice. Even better example is the Periodic Table of the Elements by NIST. Despite atomic number $Z$ also located in the upper left corner of the cell, its location is typographically literate as both $Z$ and $A_\mathrm{r}$ have distinct place, different typeface and the legend unambiguously denotes which is which:

NIST PTE:carbon

NIST PTE:legend

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    $\begingroup$ @BenCrowell I didn't expect the question to go beyond Chemistry.SE, so I addressed the answer to this community in the first place. But you are right, so I changed "written by chemists" to a more neutral "written by scientists" (I hope it won't hurt feelings of the engineers' community). $\endgroup$
    – andselisk
    Apr 28, 2019 at 23:00
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    $\begingroup$ I would suggest you include the explanation of that asterisk in your first graphic. Without it, the legend Atomic weight = number of protons + number of neutrons isn't quite true. $\endgroup$ Apr 29, 2019 at 5:48
  • $\begingroup$ @DawoodibnKareem I thought I covered this in the second paragraph, but since you think it should be explicitly quoted, I added the info from that PDF. $\endgroup$
    – andselisk
    Apr 29, 2019 at 5:54
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    $\begingroup$ Thanks, yes, that's better. The second paragraph did kind of cover it, but I felt that a newbie might find the distinction unclear. $\endgroup$ Apr 29, 2019 at 6:03

According to the international standard ISO 80000 Quantities and units – Part 9: Physical chemistry and molecular physics (corrected in Amendment 1, 2011-06-01), the attached subscripts and superscripts have the following meanings.


The nucleon number (mass number) of a nuclide is shown in the left superscript position, as in the following example: $$\mathrm{^{14}N}$$


The atomic number (proton number) is shown in the left subscript position, as in the following example. $$\mathrm{_{64}Gd}$$


The same meanings are described in the German standard DIN 1338 (2011).

$$^A_Z\mathrm E_\nu^z$$

This notation is also used in Nomenclature of Inorganic Chemistry – IUPAC Recommendations 2005 (Red Book). Note, however, that this document unfortunately introduced the terrible typographic disaster of the staggered notation for ions (see this question).

The mass, charge and atomic number of a nuclide are indicated by means of three indexes (subscripts and superscripts) placed around the symbol. The positions are occupied as follows:

left upper index    mass number
left lower index    atomic number
right upper index    charge

The same notation can also be found in the IUPAC Green Book Quantities, Units and Symbols in Physical Chemistry (2007).

It is also recommended in the ACS Style Guide:

Use the left superscript for mass number

Use the left subscript for atomic number


Different periodic tables show the atomic number above, below, or next to the element. They don’t show the mass number, usually, but the atomic weight (not an integer). There is a type of table, for example the Karlsruher Nuklidkarte, that shows all observed isotopes, and this type of chart does show mass numbers as well.

In the picture, the isotope chart is on the right (https://www.nucleonica.com/wiki/index.php?title=Historical) enter image description here


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