Unified atomic mass unit: Difference between revisions
imported>John R. Brews m (TOC template) |
imported>John R. Brews (rearrange historical text; give it its own header. Examples) |
||
| Line 1: | Line 1: | ||
{{subpages}} | {{subpages}} | ||
{{TOC|right}} | {{TOC|right}} | ||
The '''unified atomic mass unit''' ('''''u'''''), or '''dalton''' ('''Da'''), is a unit of atomic and molecular mass. By definition it is one twelfth of the mass of an unbound [[carbon]]-12 (<sup>12</sup>C) [[atom]], at rest and in its ground state. | The '''unified atomic mass unit''' ('''''u'''''), or '''dalton''' ('''''Da'''''), is a unit of atomic and molecular mass. By definition it is one twelfth of the mass of an unbound [[carbon]]-12 (<sup>12</sup>C) [[atom]], at rest and in its ground state. | ||
The relationship of the unified atomic mass unit to the macroscopic [[SI]] base unit of mass, the [[kilogram]], is given by [[Avogadro's number]] ''N''<sub>A</sub>. By the definition of Avogadro's number, the mass of ''N''<sub>A</sub> carbon-12 atoms, at rest and in their ground state, is 12 gram ( = 12×10<sup>−3</sup> kg). From the latest value of ''N''<sub>A</sub> follows the latest value of the unified atomic mass unit:<ref name=NISTu> | The relationship of the unified atomic mass unit to the macroscopic [[SI]] base unit of mass, the [[kilogram]], is given by [[Avogadro's number]] ''N''<sub>A</sub>. By the definition of Avogadro's number, the mass of ''N''<sub>A</sub> carbon-12 atoms, at rest and in their ground state, is 12 gram ( = 12×10<sup>−3</sup> kg). From the latest value of ''N''<sub>A</sub> follows the latest value of the unified atomic mass unit:<ref name=NISTu> | ||
| Line 21: | Line 21: | ||
</ref> But further confusion prevails: | </ref> But further confusion prevails: | ||
In the literature one still finds the obsolete unit ''amu'' (atomic mass unit). This is deplorable, not only because it is not a unit accepted for use with the [[SI]], but also because two ''different'' standard masses are denoted by ''amu''. There is the physicist's ''amu'' ( = 1/1.000 317 9 ''u'') and there is the chemist's ''amu'' ( = 1/1.000 043 ''u''). | In the literature one still finds the obsolete unit ''amu'' (atomic mass unit). This is deplorable, not only because it is not a unit accepted for use with the [[SI]], but also because two ''different'' standard masses are denoted by ''amu''. There is the physicist's ''amu'' ( = 1/1.000 317 9 ''u'') and there is the chemist's ''amu'' ( = 1/1.000 043 ''u''). Because chemists and physicists now use the same atomic mass unit, today it is referred to as ''unified''. It is a non-[[SI]] unit accepted for use with the SI, whose value in SI units is obtained experimentally. | ||
==History== | |||
The first standardization of atomic mass was | The different interpretations of the ''amu'' arose historically. Before 1960, in physics the amu was defined as 1/16 of the mass of one atom of oxygen-16, while in chemistry the amu was defined as 1/16 of the ''average'' mass of an oxygen atom (averaged over the natural abundance of the different oxygen [[isotope]]s). Both units are slightly smaller than the ''unified atomic mass unit'', sybol ''u'', that was adopted by the [[International Union of Pure and Applied Physics]] in 1960 and by the [[International Union of Pure and Applied Chemistry]] in 1961. | ||
Much earlier, the first standardization of atomic mass was made by the chemist [[John Dalton]] in the early nineteenth century, who introduced the mass of one atom of [[hydrogen]] as the atomic mass unit. Later [[Francis Aston]], inventor of the [[mass spectrometer]], replace it by one sixteenth of the mass of one atom of [[oxygen]]-16. | |||
==Examples== | |||
The atomic mass unit in MeV is (1 ''u'') [[speed of light|''c<sub>0</sub>''<sup>2</sup>]]: | |||
:1 ''u'' = 931.494 061(21) MeV.<ref name=NIST2> | |||
{{cite web |title=Fundamental physical constants: atomic mass unit-electron volt relationship 1 ''u'' (''c<sub>0</sub>''<sup>2</sup>)|url=http://physics.nist.gov/cgi-bin/cuu/Value?uev |publisher=NIST |work=The NIST reference on constants, units, and uncertainty |accessdate=2011-09-04}} | |||
</ref> | |||
The proton mass is: | |||
:''m<sub>p</sub>= 1.007 276 466 812(90) ''u''.<ref name=mpu> | |||
{{cite web |title=Fundamental physical constants: proton mass in ''u'': ''m<sub>p</sub>'' |url=http://physics.nist.gov/cgi-bin/cuu/Value?mpu |publisher=NIST |work=The NIST reference on constants, units, and uncertainty |accessdate=2011-09-04}} | |||
</ref> | |||
The neutron mass is: | |||
:''m<sub>n</sub>= 1.008 664 916 00(43) ''u''.<ref name=mnu> | |||
{{cite web |title=Fundamental physical constants: neutron mass in ''u'': ''m<sub>n</sub>'' |url=http://physics.nist.gov/cgi-bin/cuu/Value?mnu |publisher=NIST |work=The NIST reference on constants, units, and uncertainty |accessdate=2011-09-09}} | |||
</ref> | |||
The electron mass is: | |||
:''m<sub>e</sub> = 5.485 799 0946(22) × 10<sup>-4</sup> ''u''.<ref name=meu> | |||
{{cite web |title=Fundamental physical constants: electron mass in ''u'': ''m<sub>e</sub>'' |url=http://physics.nist.gov/cgi-bin/cuu/Value?meu |publisher=NIST |work=The NIST reference on constants, units, and uncertainty |accessdate=2011-09-04}} | |||
</ref> | |||
==Reference== | ==Reference== | ||
<references /> | <references /> | ||
Revision as of 11:58, 10 September 2011
The unified atomic mass unit (u), or dalton (Da), is a unit of atomic and molecular mass. By definition it is one twelfth of the mass of an unbound carbon-12 (12C) atom, at rest and in its ground state.
The relationship of the unified atomic mass unit to the macroscopic SI base unit of mass, the kilogram, is given by Avogadro's number NA. By the definition of Avogadro's number, the mass of NA carbon-12 atoms, at rest and in their ground state, is 12 gram ( = 12×10−3 kg). From the latest value of NA follows the latest value of the unified atomic mass unit:[1]
- 1 u ≈ 1.660 538 921(73) × 10−27 kg
Future refinements in Avogadro's number by future improvements in counting large (on the order of 1027) numbers of atoms, will give better accuracy of u. It is hoped that in the future the experimental accuracy of Avogadro's constant will improve so much that the unified atomic mass unit may replace the kilogram as the SI base unit, see this article.
The unit u is convenient because one hydrogen atom has a mass of approximately 1 u, and more generally an atom or molecule that contains p protons and n neutrons will have a mass approximately equal to (p + n) u. The mass of a nucleus is not exactly equal to p + n, because the nuclear binding energy gives rise to a relativistic mass defect.
Confusions
In the system of atomic units, the "atomic unit of mass" is the mass of the electron me.[2] But further confusion prevails:
In the literature one still finds the obsolete unit amu (atomic mass unit). This is deplorable, not only because it is not a unit accepted for use with the SI, but also because two different standard masses are denoted by amu. There is the physicist's amu ( = 1/1.000 317 9 u) and there is the chemist's amu ( = 1/1.000 043 u). Because chemists and physicists now use the same atomic mass unit, today it is referred to as unified. It is a non-SI unit accepted for use with the SI, whose value in SI units is obtained experimentally.
History
The different interpretations of the amu arose historically. Before 1960, in physics the amu was defined as 1/16 of the mass of one atom of oxygen-16, while in chemistry the amu was defined as 1/16 of the average mass of an oxygen atom (averaged over the natural abundance of the different oxygen isotopes). Both units are slightly smaller than the unified atomic mass unit, sybol u, that was adopted by the International Union of Pure and Applied Physics in 1960 and by the International Union of Pure and Applied Chemistry in 1961.
Much earlier, the first standardization of atomic mass was made by the chemist John Dalton in the early nineteenth century, who introduced the mass of one atom of hydrogen as the atomic mass unit. Later Francis Aston, inventor of the mass spectrometer, replace it by one sixteenth of the mass of one atom of oxygen-16.
Examples
The atomic mass unit in MeV is (1 u) c02:
- 1 u = 931.494 061(21) MeV.[3]
The proton mass is:
- mp= 1.007 276 466 812(90) u.[4]
The neutron mass is:
- mn= 1.008 664 916 00(43) u.[5]
The electron mass is:
- me = 5.485 799 0946(22) × 10-4 u.[6]
Reference
- ↑ Fundamental physical constants: atomic mass unit-kilogram relationship 1 u. NIST. Retrieved on 2011-09-09.
- ↑ Fundamental physical constants: atomic unit of mass me. NIST. Retrieved on 2011-09-09.
- ↑ Fundamental physical constants: atomic mass unit-electron volt relationship 1 u (c02). The NIST reference on constants, units, and uncertainty. NIST. Retrieved on 2011-09-04.
- ↑ Fundamental physical constants: proton mass in u: mp. The NIST reference on constants, units, and uncertainty. NIST. Retrieved on 2011-09-04.
- ↑ Fundamental physical constants: neutron mass in u: mn. The NIST reference on constants, units, and uncertainty. NIST. Retrieved on 2011-09-09.
- ↑ Fundamental physical constants: electron mass in u: me. The NIST reference on constants, units, and uncertainty. NIST. Retrieved on 2011-09-04.