Common symbols
NA, L
SI unitmol−1
Exact value
reciprocal mole6.02214076×1023

The Avogadro constant, commonly denoted NA[1] or L,[2] is an SI defining constant with an exact value of 6.02214076×1023 mol-1 (unit of reciprocal moles).[3][4] It is used as a normalization factor in the amount of substance in a sample (in SI units of moles), defined as the number of constituent particles (usually molecules, atoms, or ions) divided by NA. In practice, its value is often approximated as 6.02×1023 mol-1 or 6.022×1023 mol-1.[5] The constant is named after the physicist and chemist Amedeo Avogadro (1776–1856).

In the SI dimensional analysis of measurement units, the dimension of the Avogadro constant is the reciprocal of amount of substance, ${\displaystyle {\mathsf {N}}^{-1}}$. The Avogadro number, sometimes denoted N0,[6][7] is the numeric value of the Avogadro constant (i.e., without units), namely the dimensionless number 6.02214076×1023.[1][8]

The Avogadro constant NA is also the factor that converts the average mass of one particle, in grams, to the molar mass of the substance, in grams per mole (g/mol).[9]

The constant NA also relates the molar volume (the volume per mole) of a substance to the average volume nominally occupied by one of its particles, when both are expressed in the same units of volume. For example, since the molar volume of water in ordinary conditions is about 18 mL/mol, the volume occupied by one molecule of water is about 18/6.022×10−23 mL, or about 0.030 nm3 (cubic nanometres). For a crystalline substance, N0 relates the volume of a crystal with one mole worth of repeating unit cells, to the volume of a single cell (both in the same units).

The Avogadro constant was historically derived from the old definition of the mole as the amount of substance in 12 grams of carbon-12 (12C); or, equivalently, the number of daltons in a gram, where the dalton is defined as 112 of the mass of a 12C atom.[10] By this old definition, the numerical value of the Avogadro constant in mol-1 (the Avogadro number) was a physical constant that had to be determined experimentally.

The redefinition of the mole in 2019, as being the amount of substance containing exactly 6.02214076×1023 particles,[8] meant that the mass of 1 mole of a substance is now exactly the product of the Avogadro number and the average mass of its particles. The dalton however is still defined as 112 of the mass of a 12C atom, which must be determined experimentally and is known only with finite accuracy. The prior experiments that aimed to determine the Avogadro constant are now re-interpreted as measurements of the value in grams of the dalton.

By the old definition of mole, the numerical value of the mass of one mole of a substance, expressed in grams, was exactly equal to the average mass of one molecule (or atom) of the substance in daltons. With the new definition, this numerical equivalence is no longer exact, and is affected by the uncertainty of the value of the dalton; but it still holds for all practical purposes. For example, the average mass of one molecule of water is about 18.0153 daltons, and of one mole of water is about 18.0153 grams. Also, the Avogadro number is the approximate number of nucleons (protons and neutrons) in one gram of ordinary matter.

In older literature, the Avogadro number was also denoted N,[11][12] although that conflicts with the symbol for number of particles in statistical mechanics.

## History

### Origin of the concept

The Avogadro constant is named after the Italian scientist Amedeo Avogadro (1776–1856), who, in 1811, first proposed that the volume of a gas (at a given pressure and temperature) is proportional to the number of atoms or molecules regardless of the nature of the gas.[13]

The name Avogadro's number was coined in 1909 by the physicist Jean Perrin, who defined it as the number of molecules in exactly 16 grams of oxygen.[14] The goal of this definition was to make the mass of a mole of a substance, in grams, be numerically equal to the mass of one molecule relative to the mass of the hydrogen atom; which, because of the law of definite proportions, was the natural unit of atomic mass, and was assumed to be 1/16 of the atomic mass of oxygen.

The name was popularized by Stanislao Cannizzaro, who advocated Avogadro's work at the Karlsruhe Congress in 1860, four years after his death.[15]

### First measurements

The value of Avogadro's number (not yet known by that name) was first obtained indirectly by Josef Loschmidt in 1865, by estimating the number of particles in a given volume of gas.[16] This value, the number density n0 of particles in an ideal gas, is now called the Loschmidt constant in his honor, and is related to the Avogadro constant, NA, by

${\displaystyle n_{0}={\frac {p_{0}N_{\rm {A}}}{R\,T_{0}}},}$

where p0 is the pressure, R is the gas constant, and T0 is the absolute temperature. Because of this work, the symbol L is sometimes used for the Avogadro constant,[17] and, in German literature, that name may be used for both constants, distinguished only by the units of measurement.[18] (However, NA should not be confused with the entirely different Loschmidt constant in English-language literature.)

Perrin himself determined the Avogadro number by several different experimental methods. He was awarded the 1926 Nobel Prize in Physics, largely for this work.[19]

The electric charge per mole of electrons is a constant called the Faraday constant and has been known since 1834, when Michael Faraday published his works on electrolysis. In 1910, Robert Millikan with the help of Harvey Fletcher obtained the first measurement of the charge on an electron. Dividing the charge on a mole of electrons by the charge on a single electron provided a more accurate estimate of the Avogadro number.[20]

### SI definition of 1971

In 1971, in its 14th conference, the International Bureau of Weights and Measures (BIPM) decided to regard the amount of substance as an independent dimension of measurement, with the mole as its base unit in the International System of Units (SI).[17] Specifically, the mole was defined as an amount of a substance that contains as many elementary entities as there are atoms in 12 grams (0.012 kilograms) of carbon-12 (12C).[10] Thus, in particular, one mole of carbon-12 was exactly 12 grams of the element.

By this definition, one mole of any substance contained exactly as many molecules as one mole of any other substance. However, this number N0 (about 6.022×1023) was a physical constant that had to be experimentally determined, since it depended on the mass (in grams) of one atom of 12C, and therefore it was known only to a limited number of decimal digits.[17] The common rule of thumb that "one gram of matter contains N0 nucleons" was exact for carbon-12, but slightly inexact for other elements and isotopes.

In the same conference, the BIPM also named NA (the factor that converted moles into number of particles) the "Avogadro constant. However, the term "Avogadro number" continued to be used, especially in introductory works.[21] As a consequence of this definition, NA was not a pure number, but had the metric dimension of reciprocal of amount of substance (mol-1).

### SI redefinition of 2019

In its 26th Conference, the BIPM adopted a different approach: effective 20 May 2019, it defined the Avogadro constant NA as the exact value 6.02214076×1023 mol−1, thus redefining the mole as exactly 6.02214076×1023 constituent particles of the substance under consideration.[22][8] One consequence of this change is that the mass of a mole of 12C atoms is no longer exactly 0.012 kg. On the other hand, the dalton (a.k.a. universal atomic mass unit) remains unchanged as 112 of the mass of 12C.[23][24] Thus, the molar mass constant remains very close to but no longer exactly equal to 1 g/mol, although the difference (4.5×10−10 in relative terms, as of March 2019) is insignificant for all practical purposes.[8][1]

## Connection to other constants

The Avogadro constant NA is related to other physical constants and properties.

## References

1. ^ a b c Bureau International des Poids et Mesures (2019): The International System of Units (SI), 9th edition, English version, p. 134. Available at the BIPM website.
2. ^ H. P. Lehmann, X. Fuentes-Arderiu, and L. F. Bertello (1996): "Glossary of terms in quantities and units in Clinical Chemistry (IUPAC-IFCC Recommendations 1996)"; p. 963, item "Avogadro constant". Pure and Applied Chemistry, vol. 68, iss. 4, pp. 957–1000. doi:10.1351/pac199668040957
3. ^ Newell, David B.; Tiesinga, Eite (2019). "The International System of Units (SI)". NIST Special Publication 330. Gaithersburg, Maryland: National Institute of Standards and Technology. doi:10.6028/nist.sp.330-2019. S2CID 242934226. {{cite journal}}: Cite journal requires |journal= (help)
4. ^ de Bievre, P.; Peiser, H. S. (1992). "Atomic Weight: The Name, Its History, Definition and Units". Pure and Applied Chemistry. 64 (10): 1535–1543. doi:10.1351/pac199264101535. S2CID 96317287.
5. ^ Michael Mosher, Paul Kelter (2023): An Introduction to Chemistry, 2nd edition. Springer Nature. ISBN 9783030902674, 1067 pages
6. ^ Richard P. Feynman: The Feynman Lectures on Physics, Volume II
7. ^ Max Born (1969): Atomic Physics, 8th ed., Dover ed., reprinted by Courier in 2013; 544 pages. ISBN 978-0486318585
8. David B. Newell and Eite Tiesinga (2019): The International System of Units (SI). NIST Special Publication 330, National Institute of Standards and Technology. doi:10.6028/nist.sp.330-2019 S2CID 242934226
9. ^ Okun, Lev B.; Lee, A. G. (1985). Particle Physics: The Quest for the Substance of Substance. OPA Ltd. p. 86. ISBN 978-3-7186-0228-5.
10. ^ a b International Bureau of Weights and Measures (2006), The International System of Units (SI) (PDF) (8th ed.), pp. 114–115, ISBN 92-822-2213-6, archived (PDF) from the original on 4 June 2021, retrieved 16 December 2021
11. ^ Linus Pauling (1970), General Chemistry, p. 96. Dover Edition, reprinted by Courier in 2014; 992 pages. ISBN 978-0486134659
12. ^ Marvin Yelles (1971): McGraw-Hill Encyclopedia of Science and Technology, Vol. 9, 3rd ed.; 707 pages. ISBN 978-0070797987
13. ^ Avogadro, Amedeo (1811). "Essai d'une maniere de determiner les masses relatives des molecules elementaires des corps, et les proportions selon lesquelles elles entrent dans ces combinaisons". Journal de Physique. 73: 58–76. English translation.
14. ^ Perrin, Jean (1909). "Mouvement brownien et réalité moléculaire". Annales de Chimie et de Physique. 8e Série. 18: 1–114. Extract in English, translation by Frederick Soddy.
15. ^ "Stanislao Cannizzaro | Science History Institute". Science History Institute. June 2016. Retrieved 2 June 2022.
16. ^ Loschmidt, J. (1865). "Zur Grösse der Luftmoleküle". Sitzungsberichte der Kaiserlichen Akademie der Wissenschaften Wien. 52 (2): 395–413. English translation.
17. ^ a b c Bureau International des Poids et Mesures (1971): 14th Conference Générale des Poids et Mesures Archived 2020-09-23 at the Wayback Machine Available at the BIPM website.
18. ^ Virgo, S.E. (1933). "Loschmidt's Number". Science Progress. 27: 634–649. Archived from the original on 4 April 2005.
19. ^ Oseen, C.W. (December 10, 1926). Presentation Speech for the 1926 Nobel Prize in Physics.
20. ^ (1974): Introduction to the constants for nonexperts, 1900–1920 From the Encyclopaedia Britannica, 15th ed.; reproduced by NIST. Accessed on 2019-07-03.
21. ^ Kotz, John C.; Treichel, Paul M.; Townsend, John R. (2008). Chemistry and Chemical Reactivity (7th ed.). Brooks/Cole. ISBN 978-0-495-38703-9. Archived from the original on 16 October 2008.
22. ^ International Bureau for Weights and Measures (2017): Proceedings of the 106th meeting of the International Committee for Weights and Measures (CIPM), 16-17 and 20 October 2017, p. 23. Available at the BIPM website Archived 2021-02-21 at the Wayback Machine.
23. ^ Pavese, Franco (January 2018). "A possible draft of the CGPM Resolution for the revised SI, compared with the CCU last draft of the 9th SI Brochure". Measurement. 114: 478–483. Bibcode:2018Meas..114..478P. doi:10.1016/j.measurement.2017.08.020. ISSN 0263-2241.
24. ^ "Unified atomic mass unit". The IUPAC Compendium of Chemical Terminology. 2014. doi:10.1351/goldbook.U06554.
25. ^ "2018 CODATA Value: atomic mass constant". The NIST Reference on Constants, Units, and Uncertainty. NIST. 20 May 2019. Retrieved 20 May 2019.