mole

mole⁵

(mōl)

n. (Abbr. mol)

The amount of a substance that contains as many atoms, molecules, ions, or other elementary units as the number of atoms in 0.012 kilogram of carbon 12. The number is 6.0225 × 10²³, or Avogadro's number. Also called gram molecule.
The mass in grams of this amount of a substance, numerically equal to the molecular weight of the substance. Also called gram-molecular weight.

[German Mol, short for Molekulargewicht, molecular weight, from molekular, molecular, from French moléculaire, from molécule, molecule. See molecule.]

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mole

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Standard unit for measuring everyday quantities of such minute entities as atoms or molecules. For any substance, the number of atoms or molecules in a mole is Avogadro's number (6.02 ´ 10²³) of particles. Defined exactly, it is the amount of pure substance containing the same number of chemical units that there are in exactly 12 g of carbon-12. For each substance, a mole is its atomic weight, molecular weight, or formula weight in grams. The number of moles of a solute in a litre of solution is its molarity (M); the number of moles of solute in 1,000 g of solvent is its molality (m). The two measures differ slightly and have different uses. See also stoichiometry.

For more information on mole, visit Britannica.com.

McGraw-Hill Science & Technology Encyclopedia:

Mole

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A unit (symbolized mol) used to measure the amount of material in a chemical sample. The mole is defined by international agreement as the amount of substance (chemical amount) of a chemical system that contains as many molecules or entities as there are atoms in 12 g of carbon-12 (¹²C). When the mole is used, the elementary entities need not be molecules, but they must always be specified. They may be atoms, molecules, ions, electrons, or specified groups of such particles.

Three obvious ways of measuring the amount of material in a given sample are to measure the mass of the sample, to measure the volume, or to count the number of molecules in the sample. Although it is more difficult to devise an experiment to count molecules, this third way of measuring amount is of special interest to chemists because molecules react in simple rational proportions (for example, one molecule of A may react with one, or two, or three molecules of B, and so forth). However, to count molecules is inconvenient in practice because the numbers are so large. For any chemical, a mass of 1 kilogram of the sample contains a large number of molecules, of the order 10²³–10²⁴. The mole is defined so that 1 mole of any substance always contains the same number of molecules. This number approximately 6.02 × 10²³, and is known as the Avogadro number. The mole is a more convenient unit in which to measure the amount of a chemical than counting the number of molecules, and it has the same advantages. See also Avogadro number.

The amount of substance (chemical amount) of a sample, n, may be determined in practice by one of three methods.

The value of n (the amount of substance) may be determined from the mass m by dividing by the molar mass M of the sample, as in Eq. (1). If m is expressed in g and M in g/mol, then the value of n will be obtained in mol.
1. $n=\frac{m}{M}$

For a gas, the value of n may be determined from the volume V, pressure p, and absolute temperature T by using the ideal gas equation (2), where R is the gas constant
2. $n=\frac{pV}{RT}$
(R = 8.3145 J K⁻¹ mol⁻¹). If pV is expressed in (N m⁻²) × (m³) = J, and RT in J mol⁻¹, then pV/RT gives the value of n in mol.

For a solution, the amount of solute (or the amount concentration of solution) is frequently determined by titration: if ν_A molecules of A react with ν_B molecules of B in the titration, then at the end point the amount of A used (n_A) is related to the amount of B (n_B) by Eq. (3), so that if one is known the other may be determined.
3. $n_A=\frac{\nu_A}{\nu_B}n_B$
See also Titration.

The concentration of a solution may be recorded as (mass of solute)/(volume of solution), in units gram/liter; or as (chemical amount of solute)/(volume of solution) in units mol/liter. Because of the proportionality of chemical amount to number of molecules, the latter is the more useful measure of concentration and is generally used in chemistry and biochemistry. See also Concentration scales.

Oxford Dictionary of Units & Measures:

mole

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[Etymology: molecule] chemistry. Symbol mol. SI The base unit for an amount of a substance: the amount of a substance that contains as many of its basic entities (e.g. atoms for chemical elements, molecules for compounds) as there are atoms in 12 g of ¹²C.
[McGlashan M. L. Metrologia Vol. 31, 247-55 (1995)]

The relevant basic entity should be defined or clearly implied in any expression of mole measurement; besides the common atom and molecule, it can be ions, electrons, or other ‘elementary’ particles, or groups of such particles. For any pure substance, one mole has a mass in grams numerically equal to its molecular weight in daltons. (Despite the change in metric systems from gram to kilogram as the base unit for mass, the mole remains tied in this manner to the gram. This is sometimes emphasized by calling it the gram-mole, allowing the kilogram-mole to mean its SI- coherent thousand-fold multiple.)

The number of molecules of any substance, else, for an element, of atoms, contained in 1 mole of it is Avogadro's number, = 602.213 67(36) × 10²¹. This could provide a natural definition of the mole independent of the kilogram and, using the masses of electron, neutron, and proton, a natural definition of that unit of mass too.

See also dalton.

History

Originally introduced early in the 1900s as the gram-molecular weight, i.e. the number of grams of a substance that equalled its molecular weight, it was then defined as the amount of substance of a system which contains as many atoms as 16 g of oxygen; called also gram-molecule. However, this proved ambiguous because physicists interpreted it as referring to the common isotope of oxygen, while chemists used the heavier naturally occurring and somewhat variable mixture of isotopes 16, 17, and 18. In 1940 the International Commission on Atomic Weights standardized the ratio as being 1:1.000 275, then brought in the unifying carbon-based scheme in 1961.
[Wichers E. Nature Vol. 194, 621-4 (1962)] This gave values of 0.0043% less than the chemists', and 0.0315% less than the physicists'. The carbon base results in more elements having integer values than applied with oxygen, whose scale had similar merit over hydrogen.

See weight re usage of that word.

1950/60	‘relative amount of substance’ based on carbon 12.
1967	CIPM; 1969 CIPM; 1971 14th CGPM:
	‘1. The mole is the amount of substance of a system which contains as many atoms as 0.012 kilogram of carbon 12: its symbol is “mol”.
	2. When the mole is used, the elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles, or specified groups of such particles.
	3. The mole is a base unit of the International System of Units.’
1980	CIPM: ‘in this definition, it is understood that unbound atoms of carbon, at rest and in their ground state, are referred to.’see note below

[Le Système International d'Unités (Sèvres, France: Bureau International de Poids et Mesures, 1985)]

TechEncyclopedia:

mole

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A unit of measurement of molecular weight. Part of the SI system of measurement, one mole (mol) is equal to 6.02257 X 10 to the 23rd molecules. See SI units.

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Oxford Dictionary of Sports Science & Medicine:

mole

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The SI unit of amount of a substance expressed as its molecular weight in grams. Thus, 1 mole (M) of glucose, which has the formula C₆H₁₂O₆, weighs 180 g. where the atomic weight of carbon is 12, hydrogen 1, and oxygen 16.

Columbia Encyclopedia:

mole

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mole, in chemistry, a quantity of particles of any type equal to Avogadro's number, or 6.02×10²³ particles. One gram-molecular weight of any molecular substance contains exactly one mole of molecules. The term mole is often used in place of gram-molecular weight; e.g., one speaks of 18 grams of water as one mole of water rather than as one gram-molecular weight of water. The mole is a unit in the International System of Units (SI).

Science Q&A:

What is a mole in chemistry?

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A mole (symbol mol), a fundamental measuring unit for the amount of a substance, refers to either a gram atomic weight or a gram molecular weight of a substance. It is the quantity of a substance that contains 6.02 10²³ atoms, molecules, or formula units of that substance. This number is called Avogadro's number or constant after Amadeo Avogadro (1776-1856), who is considered to be one of the founders of physical science.

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Obscure Words:

mole

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Chem. the molecular weight of a substance expressed in grams; gram molecule

Oxford Dictionary of Modern Slang:

mole

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noun
noun, Austral, usu. derog

A woman. (1965 —) .
R. D. Jones Give us a hand you lazy mole! (1979)

[Perh. a variant of moll noun.]

Previous:	mokus, mokker, moke
Next:	moley, moll, mollock

Oxford Dictionary of Biochemistry:

gram-molecule

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or gram-molecular weight

symbol: g-mol; the molecular weight of a compound (or element) expressed in grams; it has now been replaced by the mole.

Previous:	gram-equivalent, gram-atom, gram
Next:	gramicidin, gramicidin S, grancalcin

Rhymes:

mol

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See words rhyming with "mol."

Wikipedia on Answers.com:

Mole (unit)

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The mole is a unit of measurement used in chemistry to express amounts of a chemical substance, defined as an amount of a substance that contains as many elementary entities (e.g., atoms, molecules, ions, electrons) as there are atoms in 12 grams of pure carbon-12 (¹²C), the isotope of carbon with atomic weight 12. This corresponds to a value of 6.02214179(30)×10²³ elementary entities of the substance. It is one of the base units in the International System of Units, and has the unit symbol mol.^[1]

The mole is widely used in chemistry, instead of units of mass or volume, as a convenient way to express the amounts of reactants and products of chemical reactions. For example, the chemical equation 2 H₂ + O₂ → 2 H₂O implies that 2 mol of dihydrogen and 1 mol of dioxygen react to form 2 mol of water. The mole may also be used to express the number of atoms, ions, or other elementary entities in some sample. The concentration of a solution is commonly expressed by its molarity, the number of moles of the dissolved substance per litre of solution.

The number of molecules in a mole (known as Avogadro's number) is defined so that the mass of one mole of a substance, expressed in grams, is exactly equal to the substance's mean molecular weight. For example, the mean molecular weight of natural water is about 18.015, so one mole of water is about 18.015 grams. This property considerably simplifies many chemical and physical computations.

The name gram-molecule was formerly used for essentially the same concept.^[1] The name gram-atom (abbreviated gat.) has been used for a related but distinct concept, namely a quantity of a substance that contains Avogadro's number of atoms, whether isolated or combined in molecules. Thus, for example, 1 mole of MgB₂ is 1 gram-molecule of MgB₂ but 3 gram-atoms of MgB₂.^[2]^[3]

Contents

1 Definition and related concepts
2 History
3 The mole as a unit
4 Other units called "mole"
5 Proposed future definition
6 Related units
7 The unit's holiday
8 See also
9 References
10 External links

Definition and related concepts

As of 2011^[update], the mole is defined by BIPM to be an amount of a substance that contains as many elementary entities (e.g. atoms, molecules, ions, electrons) as there are atoms in 12 grams of pure carbon-12 (¹²C), the isotope of carbon with atomic weight 12.^[1] Thus, by definition, one mole of pure ¹²C has a mass of exactly 12 g. It also follows from the definition that X moles of any substance will contain the same number of molecules as X moles of any other substance.

The mass per mole of a substance is called its molar mass. Since the standard unit for expressing the mass of molecules or atoms (the dalton or atomic mass unit) is defined as 1/12 of the mass of a ¹²C atom, it follows that the molar mass of a substance, measured in grams per mole, is exactly equal to its mean molecular or atomic mass, measured in daltons; which is to say, to the substance's mean molecular or atomic weight.

The number of elementary entities in a sample of a substance is technically called its (chemical) amount. Therefore, the mole is a convenient unit for that physical quantity. One can determine the chemical amount of a known substance, in moles, by dividing the sample's mass by the substance's molar mass.^[4] Other methods include the use of the molar volume or the measurement of electric charge.^[4]

It should be noted that the mass of one mole of a substance depends not only on its molecular formula, but also on the proportion of the isotopes of each element present in it. For example, one mole of calcium-40 is 39.96259098 ± 0.00000022 grams, whereas one mole of calcium-42 is 41.95861801 ± 0.00000027 grams, and one mole of calcium with the normal isotopic mix is 40.078 ± 0.004 grams.

Since the definition of the gram is not (as of 2011^[update]) mathematically tied to that of the dalton, the number N_A of molecules in a mole (Avogadro's number) must be determined experimentally. The value adopted by CODATA in 2006 is N_A = 6.02214179×10²³ ± 0.00000030×10²³.^[5] In 2011 the measurement was refined to 6.02214078×10²³ ± 0.00000018×10²³.^[6]

History

The history of the mole is intertwined with that of molecular mass, atomic mass unit, Avogadro's number and related concepts.

The first table of atomic weights was published by John Dalton (1766–1844) in 1805, based on a system in which the atomic weight of hydrogen was defined as 1. These atomic weights were based on the stoichiometric proportions of chemical reactions and compounds, a fact that greatly aided their acceptance: It was not necessary for a chemist to subscribe to atomic theory (an unproven hypothesis at the time) to make practical use of the tables. This would lead to some confusion between atomic weights (promoted by proponents of atomic theory) and equivalent weights (promoted by its opponents and which sometimes differed from atomic weights by an integer factor), which would last throughout much of the nineteenth century.

Jöns Jacob Berzelius (1779–1848) was instrumental in the determination of atomic weights to ever-increasing accuracy. He was also the first chemist to use oxygen as the standard to which other weights were referred. Oxygen is a useful standard, as, unlike hydrogen, it forms compounds with most other elements, especially metals. However, he chose to fix the atomic weight of oxygen as 100, an innovation that did not catch on.

Charles Frédéric Gerhardt (1816–56), Henri Victor Regnault (1810–78) and Stanislao Cannizzaro (1826–1910) expanded on Berzelius' works, resolving many of the problems of unknown stoichiometry of compounds, and the use of atomic weights attracted a large consensus by the time of the Karlsruhe Congress (1860). The convention had reverted to defining the atomic weight of hydrogen as 1, although at the level of precision of measurements at that time — relative uncertainties of around 1% — this was numerically equivalent to the later standard of oxygen = 16. However the chemical convenience of having oxygen as the primary atomic weight standard became ever more evident with advances in analytical chemistry and the need for ever more accurate atomic weight determinations.

Developments in mass spectrometry led to the adoption of oxygen-16 as the standard substance, in lieu of natural oxygen.^{[citation needed]} The current definition of the mole, based on carbon-12, was approved during the 1960s.^[1]^[7] The four different definitions were equivalent to within 1%.

Scale basis	Scale basis relative to ¹²C = 12	Relative deviation from the ¹²C = 12 scale
Atomic weight of hydrogen = 1	1.00794(7)	−0.788%
Atomic weight of oxygen = 16	15.9994(3)	+0.00375%
Relative atomic mass of ¹⁶O = 16	15.9949146221(15)	+0.0318%

The name mole is an 1897 translation of the German unit Mol, coined by the chemist Wilhelm Ostwald in 1894 from the German word Molekül (molecule).^[8]^[9]^[10] However, the related concept of equivalent mass had been in use at least a century earlier.^[11]

The mole as a unit

Since its adoption into the International System of Units, there have been a number of criticisms of the concept of the mole as a unit like the meter or the second:

the number of molecules, etc. in a given lump of material is a fixed dimensionless quantity that can be expressed simply as a number, so does not require its own base unit;^[7]
the SI thermodynamic mole is irrelevant to analytical chemistry and is causing avoidable costs to advanced economies;^[12]
the mole is not a true metric (i.e. measuring) unit, rather it is a parametric unit and amount of substance is a parametric base quantity;^[13]
the concepts of the SI quantity 'amount of substance' and unit 'mole' are confusing and difficult to teach.^[14]
the SI defines numbers of entities as quantities of dimension one, and thus ignores the ontological distinction between entities and units of continuous quantities.^[15]

In chemistry, it has been known since Proust's law of definite proportions (1794) that knowledge of the mass of each of the components in a chemical system is not sufficient to define the system. Amount of substance can be described as mass divided by Proust's "definite proportions", and contains information that is missing from the measurement of mass alone. As demonstrated by Dalton's law of partial pressures (1803), a measurement of mass is not even necessary to measure the amount of substance (although in practice it is usual). There are many physical relationships between amount of substance and other physical quantities, the most notable one being the ideal gas law (where the relationship was first demonstrated in 1857). The term "mole" was first used in a textbook describing these colligative properties.

Other units called "mole"

Chemical engineers use the concept extensively, but the unit is rather small for industrial use.^[16] For convenience in avoiding conversions, some American engineers adopted the pound-mole (noted lb-mol or lbmol), which is defined as the number of entities in 12 lb of ¹²C. One lb-mol is equal to 453.59237 mol.^[17] In the metric system, chemical engineers once used the kilogram-mole (noted kg-mol), which is defined as the number of entities in 12 kg of ¹²C, and often referred to the mole as the gram-mole (noted g-mol), when dealing with laboratory data.^[17] However modern chemical engineering practice is to use the kilomole (kmol), which is identical to the kilogram-mole, but whose name and symbol adopt the SI convention for standard multiples of metric units.

Proposed future definition

In 2011, the 24^th meeting of the General Conference on Weights and Measures (CGPM) agreed a plan for a possible revision of the SI base unit definitions on an as yet undetermined date. This plan, set forward in the meeting's first resolution, included a proposal to redefine the mole in a way that will fix “the Avogadro constant to be equal to exactly 6.022 14X ×10²³ when it is expressed in the SI unit mol^-1.”^[18]

Related units

The SI units for molar concentration are mol/m³. However, most chemical literature traditionally uses mol/dm³, or mol dm⁻³, which is the same as mol/L. These traditional units are often denoted by a capital letter M (pronounced "molar"), sometimes preceded by an SI prefix, for example, millimoles per litre (mmol/L) or millimolar (mM), micromoles/litre (µmol/L) or micromolar (µM), or nanomoles/L (nmol/L) or nanomolar (nM).

The unit's holiday

October 23 is called Mole Day.^[19] It is an informal holiday in honour of the unit among chemists in North America. The date is derived from Avogadro's number, which is approximately 6.022×10²³. It officially starts at 6:02 A.M. and ends at 6:02 P.M.

References

^ ^a ^b ^c ^d International Bureau of Weights and Measures (2006), The International System of Units (SI) (8th ed.), pp. 114–15, ISBN 92-822-2213-6, http://www.bipm.org/utils/common/pdf/si_brochure_8_en.pdf
^ Wang, Yuxing et al.; Bouquet, Fr d ric; Sheikin, Ilya; Toulemonde, Pierre; Revaz, Bernard; Eisterer, Michael; Weber, Harald W; Hinderer, Joerg et al (2003). "Specific heat of MgB2 after irradiation". Journal of Physics: Condensed Matter 15 (6): 883–893. arXiv:cond-mat/0208169. Bibcode 2003JPCM...15..883W. doi:10.1088/0953-8984/15/6/315.
^ Lortz, R. et al.; Wang, Y.; Abe, S.; Meingast, C.; Paderno, Yu.; Filippov, V.; Junod, A. (2005). "Specific heat, magnetic susceptibility, resistivity and thermal expansion of the superconductor ZrB12". Phys. Rev. B 72 (2): 024547. arXiv:cond-mat/0502193. Bibcode 2005PhRvB..72b4547L. doi:10.1103/PhysRevB.72.024547.
^ ^a ^b International Bureau of Weights and Measures. "Realising the mole." Retrieved 25 September 2008.
^ Mohr, Peter J.; Taylor, Barry N.; Newell, David B. (2008). "CODATA Recommended Values of the Fundamental Physical Constants: 2006". Rev. Mod. Phys. 80 (2): 633–730. Bibcode 2008RvMP...80..633M. doi:10.1103/RevModPhys.80.633. http://physics.nist.gov/cuu/Constants/index.html. Direct link to value.
^ Andreas, Birk; et al (2011). "Determination of the Avogadro Constant by Counting the Atoms in a ²⁸Si Crystal". Physical Review Letters 106 (3). Bibcode 2011PhRvL.106c0801A. doi:10.1103/PhysRevLett.106.030801. http://physics.aps.org/synopsis-for/10.1103/PhysRevLett.106.030801.
^ ^a ^b de Bièvre, P.; Peiser, H.S. (1992). "'Atomic Weight'—The Name, Its History, Definition, and Units". Pure Appl. Chem. 64 (10): 1535–43. doi:10.1351/pac199264101535. http://www.iupac.org/publications/pac/1992/pdf/6410x1535.pdf
^ Helm, Georg (1897). The Principles of Mathematical Chemistry: The Energetics of Chemical Phenomena. transl. by Livingston, J.; Morgan, R.. New York: Wiley. p. 6.
^ Some sources place the date of first usage in English as 1902. Merriam–Webster proposes an etymology from Molekulärgewicht (molecular weight).
^ Ostwald, Wilhelm (1893). Hand- und Hilfsbuch zur Ausführung Physiko-Chemischer Messungen. Leipzig. p. 119.
^ mole, n.⁸, Oxford English Dictionary, Draft Revision Dec. 2008
^ Price, Gary (2010). "Failures of the global measurement system. Part 1: the case of chemistry". Accreditation and Quality Assurance 15 (7): 421–427. doi:10.1007/s00769-010-0655-z. http://www.springerlink.com/content/p63w663v127t5g0q/. [1].
^ Johansson, Ingvar (2010). "Metrological thinking needs the notions of parametric quantities, units, and dimensions.". Metrologia 47 (3): 219–230. Bibcode 2010Metro..47..219J. doi:10.1088/0026-1394/47/3/012. http://stacks.iop.org/0026-1394/47/i=3/a=012.
^ Furio, C; Azcona, R;Guisasola, J. (2002). "The learning and teaching of the concepts 'amount of substance' and mole - a review of the literature". Chemistry Education: Research and Practice in Europe 3 (3): 277–292. http://www.uoi.gr/cerp/2002_October/pdf/02Furio.pdf. [2]
^ Cooper, G; Humphry, S (2010). "The ontological distinction between units and entities". Synthese. doi:10.1007/s11229-010-9832-1.
^ In particular, when the mole is used, alongside the SI unit of volume of a cubic metre, in thermodynamic calculations such as the ideal gas law, a factor of 1000 is introduced which engineering practice chooses to simplify by adopting the kilomole.
^ ^a ^b Himmelblau, David (1996). Basic Principles and Calculations in Chemical Engineering (6 ed.). pp. 17–20. ISBN 0-13-305798-4.
^ "RESOLUTIONS ADOPTED BY THE 24TH MEETING OF THE GENERAL CONFERENCE ON WEIGHTS AND MEASURES (CGPM)". Paris: BIPM. 17-21 Oct, 2011. http://www.bipm.org/utils/common/pdf/24_CGPM_Resolutions.pdf.
^ History of National Mole Day Foundation, Inc

External links

ChemTeam: The Origin of the Word 'Mole' at the Wayback Machine (archived December 22, 2007)

v d e SI units

Base units	Ampere · Candela · Kelvin · Kilogram · Metre · Mole · Second

Derived units	Becquerel · Coulomb · degree Celsius · Farad · Gray · Henry · Hertz · Joule · Katal · Lumen · Lux · Newton · Ohm · Pascal · Radian · Siemens · Sievert · Steradian · Tesla · Volt · Watt · Weber

Accepted for use with SI	Dalton (Atomic mass unit) · Astronomical unit · Day · Decibel · Degree of arc · Electronvolt · Hectare · Hour · Litre · Minute · Minute of arc · Neper · Second of arc · Tonne Atomic units · Natural units

See also	SI prefixes · Systems of measurement · Conversion of units · New SI definitions · History of the metric system

Book:International System of Units · Category:SI base units

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Translations:

Mole

Top

Dansk (Danish)
1.
n. - [zool.] muldvarp

2.
n. - modermærke, skønhedsplet

3.
n. - mole, havnedæmning

4.
n. - mol

5.
n. - mola (vævssamling i livmoderen)

6.
n. - krydret sauce af mexicansk oprindelse med chokolade, chilier og krydderier

Nederlands (Dutch)
mol, golfbreker, geheim agent, beschutte haven, moedervlek, mol (scheikunde)

Français (French)
1.
n. - (Zool) taupe, (fig) taupe

2.
n. - grain de beauté

3.
n. - jetée, brise-lames

4.
n. - (Phys, Chim) mole

5.
n. - (Méd) môle

6.
n. - sauce au chili

Deutsch (German)
1.
n. - Maulwurf

2.
n. - Leberfleck, Muttermal

3.
n. - Mole, Hafendamm

4.
n. - (Chem.) Mol, Grammmoleküle

5.
n. - Mole

6.
n. - mexikanische scharfe Chilisoße

Ελληνική (Greek)
n. - κρεατοελιά, (ζωολ.) τυφλοπόντικας, μόλος, κυματοθραύστης, τεχνητό λιμάνι

Italiano (Italian)
talpa, neo

Português (Portuguese)
n. - sinal congênito na pele (m), toupeira (f) Zool., quebra-mar (f)

Русский (Russian)
родинка, крот, дамба, моль, агент, внедрившийся в иностранную разведку

Español (Spanish)
1.
n. - topo

2.
n. - lunar

3.
n. - rompeolas, dársena, malecón

4.
n. - mol

5.
n. - fibroma

6.
n. - salsa de chile picante

Svenska (Swedish)
n. - (födelse)märke, vågbrytare, mullvad, grammolekyl

中文（简体）(Chinese (Simplified))
1. 鼹鼠, 钱鼠, 隧道全断面掘进机, 长期潜伏的间谍

2. 痣

3. 胎块

4. 防波堤

5. 摩尔, 克分子

6. 鼹鼠, 钱鼠, 隧道全断面掘进机, 长期潜伏的间谍

中文（繁體）(Chinese (Traditional))
1.
n. - 鼴鼠, 錢鼠, 隧道全斷面掘進機, 長期潛伏的間諜

2.
n. - 摩爾, 克分子

3.
n. - 痣

4.
n. - 胎塊

5.
n. - 防波堤

6.
n. - 鼴鼠, 錢鼠, 隧道全斷面掘進機, 長期潛伏的間諜

한국어 (Korean)
1.
n. - 두더지

2.
n. - (피부의) 검은 점

3.
n. - 방파제

4.
n. - (화학의) 몰

5.
n. - 자궁조직의 비정상적인 덩어리

6.
n. - 매운 칠리소스

日本語 (Japanese)
n. - モグラ, ほくろ, 防波堤

العربيه (Arabic)
‏(الاسم) شامه, خال‏

עברית (Hebrew)
n. - ‮חפרפרת, חולד‬
n. - ‮שומה, בהרת‬
n. - ‮מזח, שובר-גלים‬
n. - ‮יחידת-כמות תקנית של חומר‬
n. - ‮כמות לא רגילה של רקמה ברחם‬
n. - ‮סוג של רטוב צ'ילי‬

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		American Heritage Dictionary. The American Heritage® Dictionary of the English Language, Fourth Edition Copyright © 2007, 2000 by Houghton Mifflin Company. Updated in 2009. Published by Houghton Mifflin Company. All rights reserved. Read more
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		McGraw-Hill Science & Technology Encyclopedia. McGraw-Hill Encyclopedia of Science and Technology. Copyright © 2005 by The McGraw-Hill Companies, Inc. All rights reserved. Read more
		Oxford Dictionary of Units & Measures. A Dictionary of Weights, Measures, and Units. Copyright © Donald Fenna 2002, 2004. All rights reserved. Read more
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		Oxford Dictionary of Sports Science & Medicine. The Oxford Dictionary of Sports Science & Medicine. Copyright © Michael Kent 1998, 2006, 2007. All rights reserved. Read more
		Columbia Encyclopedia. The Columbia Electronic Encyclopedia, Sixth Edition Copyright © 2012, Columbia University Press. Licensed from Columbia University Press. All rights reserved. www.cc.columbia.edu/cu/cup/. Read more
		Science Q&A. The Handy Science Answer Book. 2003 ©Visible Ink Press (handyanswers.com). All rights reserved. Read more
		Obscure Words. © 2008 by Michael A. Fischer http://home.comcast.net/~wwftd. Read more
		Oxford Dictionary of Modern Slang. Oxford University Press. © 1997, 2008, 2010 All rights reserved. Read more
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	Why do they call the number mole a mole? Read answer...
	What is the mole? Read answer...
	What is the mole ratio that can convert from moles of a to moles of b? Read answer...

	Is maurie mole really a mole?
	How do you do mole mole conversions?
	What are Stoichiometric mole to mole conversions?

mole

mole5

mole

Mole

mole

mole

mole

mole

What is a mole in chemistry?

mole

mole

gram-molecule

mol

Mole (unit)

Definition and related concepts

History

The mole as a unit

Other units called "mole"

Proposed future definition

Related units

The unit's holiday

See also

References

External links

Mole

mole⁵