TheInfoList

## History

The Avogadro constant is named after the early 19th-century Italian scientist Amedeo Avogadro, 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. The French physicist Jean Perrin in 1909 proposed naming the constant in honor of Avogadro. Perrin won the 1926 Nobel Prize in Physics, largely for his work in determining the Avogadro constant by several different methods.

The value of the Avogadro constant was first indicated by Johann Josef Loschmidt, who in 1865 estimated the average diameter of the molecules in the air by a method that is equivalent to calculating the number of particles in a given volume of gas. This latter 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

$n_{0}={\frac {p_{0}N_{\rm {A}}}{RT_{0}}},$ where p0 is the pressure, R is the gas constant and T0 is the absolute temperature. The connection with Loschmidt is the origin of the symbol L sometimes used for the Avogadro constant, and German-language literature may refer to both constants by the same name, distinguished only by the units of measurement.

Accurate determinations of the Avogadro constant require the measurement of a single quantity on both the atomic and macroscopic scales using the same unit of measurement. This became possible for the first time when American physicist Robert Millikan measured the charge on an electron in 1910. The electric charge per mole of electrons is a constant called the Faraday constant and had been known since 1834 when Michael Faraday published his works on electrolysis. By dividing the charge on a mole of electrons by the charge on a single electron the value of Avogadro's number is obtained. Since 1910, newer calculations have more accurately determined the values for the Faraday constant and the elementary charge (see § Measurement below).

Perrin originally proposed the name Avogadro's number (N) to refer to the number of molecules in one gram-molecule of oxygen (exactly 32g of oxygen, according to the definitions of the period), and this term is still widely used, especially in introductory works. The change in name to Avogadro constant (NA) came with the introduction of the mole as a base unit in the International System of Units (SI) in 1971, which regarded amount of substance as an independent dimension of measurement. With this recognition, the Avogadro constant was no longer a pure number, but had a unit of measurement, the reciprocal mole (mol−1).

While it is rare to use units of amount of substance other than the mole, the Avogadro constant can also be expressed by pound mole and ounce mole.

## General role in science

The Avogadro constant is a scaling factor between macroscopic and microscopic (atomic scale) observations of nature. As such, it provides the relationship between other physical constants and properties. For example, based on CODATA values, it establishes the following relationship between the gas constant R and the Boltzmann constant kB,

$R=k_{\text{B}}N_{\text{A}}=8.314\,4598(48)\ {{\text{J}}{\cdot }{\text{mol}}^{-1}{\cdot }{\text{K}}^{-1}}$ and the Faraday constant F and the elementary charge e,

$F=N_{\text{A}}e=96\,485.33289(59)\ {{\text{C}}{\cdot }{\text{mol}}^{-1}}.\,$ The Avogadro constant also enters into the definition of the unified atomic mass unit, u,

$1\ {\text{u}}={\frac {M_{\text{u}}}{N_{\text{A}}}}=1.660\,539\,040(20)\times 10^{-27}\ {\text{kg}}$ where Mu is the molar mass constant.

## Measurement

### Coulometry

The earliest accurate method to measure the value of the Avogadro constant was based on coulometry. The principle is to measure the Faraday constant, F, which is the electric charge carried by one mole of electrons, and to divide by the elementary charge, e, to obtain the Avogadro constant.

$N_{\text{A}}={\frac {F}{e}}$ The classic experiment is that of Bower and Davis at NIST, and relies on dissolving silver metal away from the anode of an electrolysis cell, while passing a constant electric current I for a known time t. If m is the mass of silver lost from the anode and Ar the atomic weight of silver, then the Faraday constant is given by:

$F={\frac {A_{\rm {r}}M_{\rm {u}}It}{m}}.$ The NIST scientists devised a method to compensate for silver lost from the anode by mechanical causes, and conducted an isotope analysis of the silver used to determine its atomic weight. Their value for the conventional Faraday constant is F90 = 96485.39(13) C/mol, which corresponds to a value for the Avogadro constant of 6.0221449(78)×1023 mol−1: both values have a relative standard uncertainty of 1.3×10−6.

### Electron mass measurement

The Committee on Data for Science and Technology (CODATA) publishes values for physical constants for international use. It determines the Avogadro constant from the ratio of the molar mass of the electron Ar(e)Mu to the rest mass of the electron me:

$N_{\rm {A}}={\frac {A_{\rm {r}}({\rm {e}})M_{\rm {u}}}{m_{\rm {e}}}}.$ The relative atomic mass of the electron, Ar(e), is a directly measured quantity, and the molar mass constant, Mu, is a defined constant in the SI. The electron rest mass, however, is calculated from other measured constants:

$m_{\rm {e}}={\frac {2R_{\infty }h}{c\alpha ^{2}}}.$ As may be observed in the table below, the main limiting factor in the precision of the Avogadro constant is the uncertainty in the value of the Planck constant, as all the other constants that contribute to the calculation are known more precisely.

Constant Symbol 2014 CODATA value Relative standard uncertainty Correlation coefficient
with NA
Proton-electron mass ratio mp/me 1836.152 673 89(17) 9.5×10–11 −0.0003
Molar mass constant Mu 0.001 kg/mol = 1 g/mol 0 (defined)  —
Rydberg constant R 10 973 731.568 508(65) m−1 5.9×10–12 −0.0002
Planck constant h 6.626 070 040(81)×10–34 J s 1.2×10–8 −0.9993
Speed of light c 299 792 458 m/s 0 (defined)  —
Fine structure constant α 7.297 352 5664(17)×10–3 2.3×10–10 0.0193
Avogadro constant NA 6.022 140 857(74)×1023 mol−1 1.2×10–8 1

### X-ray crystal density (XRCD) methods

A modern method to determine the Avogadro constant is the use of X-ray crystallography. Silicon single crystals may be produced today in commercial facilities with extremely high purity and with few lattice defects. This method defines the Avogadro constant as the ratio of the molar volume, Vm, to the atomic volume Vatom:

$N_{\rm {A}}={\frac {V_{\rm {m}}}{V_{\rm {atom}}}}$ , where $V_{\rm {atom}}={\frac {V_{\rm {cell}}}{n}}$ and n is the number of atoms per unit cell of volume Vcell.

The unit cell of silicon has a cubic packing arrangement of 8 atoms, and the unit cell volume may be measured by determining a single unit cell parameter, the length of one of the sides of the cube, a.

In practice, measurements are carried out on a distance known as d220(Si), which is the distance between the planes denoted by the Miller indices {220}, and is equal to a/8. The 2006 CODATA value for d220(Si) is 192.0155762(50) pm, a relative standard uncertainty of 2.8×10−8, corresponding to a unit cell volume of 1.60193304(13)×10−28 m3.

The isotope proportional composition of the sample used must be measured and taken into account. Silicon occurs in three stable isotopes (28Si, 29Si, 30Si), and the natural variation in their proportions is greater than other uncertainties in the measurements. The atomic weight Ar for the sample crystal can be calculated, as the standard atomic weights of the three nuclides are known with great accuracy. This, together with the measured density ρ of the sample, allows the molar volume Vm to be determined:

$V_{\rm {m}}={\frac {A_{\rm {r}}M_{\rm {u}}}{\rho }}$ where Mu is the molar mass constant. The 2006 CODATA value for the molar volume of silicon is 12.0588349(11) cm3⋅mol−1, with a relative standard uncertainty of 9.1×10−8.

As of the 2006 CODATA recommended values, the relative uncertainty in determinations of the Avogadro constant by the X-ray crystal density method is 1.2×10−7, about two and a half times higher than that of the electron mass method. $h={\frac {c\alpha ^{2}A_{\rm {r}}({\rm {e}})M_{\rm {u}}}{2R_{\infty }N_{\rm {A}}}}.$ 