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| In [[thermodynamics]], '''chemical potential''', also known as '''partial molar free energy''', is a form of [[potential energy]] that can be absorbed or released during a chemical reaction. It may also change during a [[phase transition]]. The chemical potential of a species in the mixture can be defined as the slope of the [[Thermodynamic free energy|free energy]] of the system with respect to a change in the number of moles of just that species. Thus, it is the [[partial derivative]] of the free energy with respect to the amount of the species, all other species' concentrations in the mixture remaining constant, and at constant temperature. When pressure is constant, chemical potential is the partial molar [[Gibbs free energy]]. At [[chemical equilibrium]] or in [[phase equilibrium]] the total sum of chemical potentials is zero, as the free energy is at a minimum.<ref>
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| {{cite book |last1=Atkins |first1=Peter |last2=de Paula |first2=Julio |title=Atkins' Physical Chemistry|edition=8th |year=2006 |publisher= Oxford University Press|isbn=978-0-19-870072-2}} Page references in this article refer specifically to the 8th edition of this book.</ref><ref>
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| {{cite journal | last = Baierlein| first = Ralph |date=April 2001 | title = The elusive chemical potential| journal = American Journal of Physics | volume = 69| issue = 4| pages = 423–434| doi = 10.1119/1.1336839 | url = http://www.physics.udel.edu/~bnikolic/teaching/phys624/PDF/chemical_potential.pdf|bibcode = 2001AmJPh..69..423B }}</ref><ref>
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| {{cite journal| last = Job| first = G.| coauthors = Herrmann, F. |date=February 2006 | title = Chemical potential–a quantity in search of recognition| journal = European Journal of Physics | volume = 27| pages = 353–371| doi = 10.1088/0143-0807/27/2/018 | url = http://www.physikdidaktik.uni-karlsruhe.de/publication/ejp/chem_pot_ejp.pdf | format = PDF|bibcode = 2006EJPh...27..353J| issue = 2 }}</ref>
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| In [[semiconductor]] physics, the chemical potential of a system of electrons at a temperature of zero Kelvin is known as the [[Fermi level]].<ref name=Kittel1980>{{cite book | last = Kittel | first = Charles | authorlink = Charles Kittel | coauthors = [[Herbert Kroemer]] | title = Thermal Physics (2nd Edition) | publisher = W. H. Freeman | date = 1980-01-15 | location = | page = 357 | url = http://books.google.com/?id=c0R79nyOoNMC&pg=PA357 | doi = | id = | isbn = 978-0-7167-1088-2 }}</ref>
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| ==Overview==
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| Particles tend to move from higher chemical potential to lower chemical potential. In this way, chemical potential is a generalization of [[potential energy|"potentials" in physics]] such as [[gravitational potential]]. When a ball rolls down a hill, it is moving from a higher gravitational potential (higher elevation) to a lower gravitational potential (lower elevation). In the same way, as molecules move, react, dissolve, melt, etc., they will always tend naturally to go from a higher chemical potential to a lower one, changing the [[particle number]], which is [[conjugate variables (thermodynamics)|conjugate variable]] to chemical potential.
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| A simple example is a system of dilute molecules [[molecular diffusion|diffusing]] in a homogeneous environment. In this system, the molecules tend to move from areas with high [[concentration]] to low concentration, until eventually the concentration is the same everywhere.
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| The microscopic explanation for this is based in [[kinetic theory]] and the random motion of molecules. However, it is simpler to describe the process in terms of chemical potentials: For a given temperature, a molecule has a higher chemical potential in a higher-concentration area, and a lower chemical potential in a low concentration area. Movement of molecules from higher chemical potential to lower chemical potential is accompanied by a release of free energy. Therefore it is a [[spontaneous process]].
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| Another example is a glass of liquid water with ice cubes in it. Above 0°C, an H<sub>2</sub>O molecule in the liquid phase has a lower chemical potential than a water molecule in an ice cube (solid phase). When some ice melts H<sub>2</sub>O molecules migrate from solid to liquid where their chemical potential is lower. Below 0°C, the molecules in ice have a lower chemical potential, so the ice cubes grow. At the temperature of the [[melting point]], 0°C, the chemical potentials in water and ice are the same; the ice cubes neither grow nor shrink, and the system is in [[thermodynamic equilibrium|equilibrium]].
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| A third example is illustrated by the chemical reaction of [[dissociation (chemistry)|dissociation]] of a [[weak acid]], such as [[acetic acid]], HA, A=CH<sub>3</sub>COO<sup>-</sup>.
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| :HA {{eqm}} H<sup>+</sup> + A<sup>-</sup>
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| [[Vinegar]] contains acetic acid. When acid molecules dissociate, the concentration of the undissociated acid molecules (HA) decreases and the concentrations of the product ions (H<sup>+</sup> and A<sup>-</sup>) increase. Thus the chemical potential of HA decreases and the sum of the chemical potentials of H<sup>+</sup> and A<sup>-</sup> increases. When the sums of chemical potential of reactants and products are equal the system is at equilibrium and there is no tendency for the reaction to proceed in either the forward or backward direction. This explains why vinegar is acidic, because acetic acid dissociates to some extent, releasing [[hydrogen ion]]s into the solution.
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| Chemical potentials are important in many aspects of [[equilibrium chemistry]], including [[melting point|melting]], [[boiling point|boiling]], [[evaporation]], [[solubility]], [[osmosis]], [[partition coefficient]], [[liquid-liquid extraction]] and [[chromatography]]. In each case there is a characteristic constant which is a function of the chemical potentials of the species at equilibrium.
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| In [[electrochemistry]], [[ion]]s do ''not'' always tend to go from higher to lower chemical potential, but they ''do'' always go from higher to lower ''[[electrochemical potential]]''. The electrochemical potential completely characterizes all of the influences on an ion's motion, while the chemical potential includes everything ''except'' the [[electric force]]. (See [[#Internal, external, and total chemical potential|below]] for more on this terminology.)
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| ==Thermodynamic definitions==
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| The fundamental equation of [[chemical thermodynamics]] for a system containing ''n'' constituent species, with the ''i''-th species having ''N''<sub>i</sub> particles is, in terms of Gibbs energy
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| :<math> dG = -SdT + VdP + \sum_{i=1}^n \mu_i dN_i \,</math>
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| At constant temperature and pressure this simplifies to
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| :<math> dG = \sum_{i=1}^n \mu_i dN_i = \mu_1dN_1 + \mu_2dN_2 + ...\,</math>
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| The definition of chemical potential of the ''i''-th species, ''μ<sub>i</sub>'', follows by setting all the numbers ''N'', apart from one, to be constant.
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| :<math>\mu_i=\left(\frac{\partial G}{\partial N_i}\right)_{T,P,N_{j\neq i}}</math>
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| When temperature and volume are taken to be constant chemical potential relates to the [[Helmholtz free energy]], ''A''.
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| :<math>\mu_i = \left(\frac{\partial A}{\partial N_i}\right)_{T,V, N_{j \ne i}}</math>
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| The chemical potential of a species is the slope of the free energy with respect to the number of particles of that species. It reflects the change in free energy when the number of particles of one species changes. Each chemical species, be it an atom, ion or molecule, has its own chemical potential. At equilibrium free energy is at its minimum for the system, that is, d''G''=0. It follows that the sum of chemical potentials is also zero.
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| :<math> \mu_1dN_1 + \mu_2dN_2 + ... = 0\,</math>
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| Use of this equality provides the means to establish the [[equilibrium constant]] for a chemical reaction.
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| Other definition are sometimes used.
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| :<math>\mu_i = \left(\frac{\partial H}{\partial N_i} \right)_{S,P, N_{j \ne i}} or \ \mu_i = \left(\frac{\partial U}{\partial N_i} \right)_{S,V, N_{j \ne i}}</math>
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| Here ''U'' is [[internal energy]], ''H'' is [[enthalpy]] and the [[entropy]], ''S'', is taken to be constant (see [[#History]]). Keeping the entropy fixed requires perfect [[thermal insulation]], so these definitions have limited practical applications.
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| === Dependence on concentration (particle number) ===
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| The variation of chemical potential with particle number is most easily expressed in terms relating quantities to their [[concentration]]s. The concentration of a species in a given volume, v, is simply N<sub>i</sub> / v, so chemical potential can be defined in terms of concentration rather than particle number. For species in solution
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| :μ<sub>i</sub> = μ<sub>i</sub><sup>std</sup> + RT ln a<sub>i</sub>
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| where μ<sub>i</sub><sup>std</sup> is the potential in a given [[standard state]] and a<sub>i</sub> is the [[chemical activity|activity]] of the species in solution. Activity can be expressed as a product of concentration and an [[activity coefficient]], so if activity coefficients are ignored, chemical potential is proportional to the logarithm of the concentration of the species.
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| For species in the gaseous state the variation is expressed as
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| :μ<sub>i</sub> = μ<sub>i</sub><sup>std</sup> + RT ln f<sub>i</sub>
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| where f<sub>i</sub> is the [[fugacity]]. If the [[ideal gas]] law applies fugacity is equal to [[partial pressure]] and chemical potential is proportional to the logarithm of the partial pressure.
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| ===Dependence on temperature and pressure===
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| The [[Maxwell relation]]
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| :<math> \left( \frac{\partial \mu}{\partial T} \right)_{p,n} =- \left( \frac{\partial S}{\partial n} \right)_{T,p}</math>
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| shows that the temperature variation of chemical potential depends on entropy. If entropy increases as the particle number increases, then chemical potential will decrease as temperature increases.
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| Similarly
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| :<math> \left( \frac{\partial \mu}{\partial p} \right)_{T,n} = \left( \frac{\partial V}{\partial n} \right)_{T,p}</math>
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| shows that the pressure coefficient depends on volume. If volume increases with particle number, chemical potential also increases as pressure increases.
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| == Applications ==
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| The [[Gibbs-Duhem equation]] is useful because it relates individual chemical potentials. For example, in a binary mixture, at constant temperature and pressure, the chemical potentials of the two participants are related by
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| :<math>d\mu_B=-\frac{n_A}{n_B}d\mu_A</math>
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| Every instance of phase or chemical equilibrium is characterized by a constant. For instance, the melting of ice is characterized by a temperature, known as the [[melting point]] at which solid and liquid phases are in equilibrium with each other. Chemical potentials can be used to explain the slopes of lines on a [[phase diagram]] by using the [[Clapeyron equation]], which in turn can be derived from the [[Gibbs-Duhem]] equation.<ref>Atkins, Section 4.1, p 126</ref> They are used to explain [[colligative property|colligative properties]] such as [[melting point depression]] by the application of pressure.<ref>Atkins, Section 5.5, pp 150-155</ref> Both [[Raoult's law]] and [[Henry's law]] can be derived in a simple manner using chemical potentials.<ref>Atkins, Section 5.3, pp 143-145</ref>
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| ==History==
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| Chemical potential was first described by the American engineer, chemist and mathematical physicist [[Willard Gibbs|Josiah Willard Gibbs]]. He defined it as follows:
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| {{quote|If to any [[wiktionary:homogeneous|homogeneous]] mass in a [[Thermodynamic state|state]] of [[hydrostatic stress]] we suppose an infinitesimal quantity of any substance to be added, the mass remaining homogeneous and its [[entropy]] and [[volume]] remaining unchanged, the increase of the [[internal energy|energy]] of the mass divided by the quantity of the substance added is the ''potential'' for that substance in the mass considered.}}
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| Gibbs later noted{{citation needed|date=September 2011}} also that for the purposes of this definition, any [[chemical element]] or combination of elements in given proportions may be considered a substance, whether capable or not of existing by itself as a homogeneous body. This freedom to choose the boundary of the system allows chemical potential to be applied to a huge range of systems. The term can be used in [[thermodynamics]] and [[physics]] for any system undergoing change. Chemical potential is also referred to as '''partial molar Gibbs energy''' (see also [[partial molar property]]). Chemical potential is measured in units of energy/particle or, equivalently, energy/[[Mole (unit)|mole]].
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| In his 1873 paper ''A Method of Geometrical Representation of the Thermodynamic Properties of Substances by Means of Surfaces'', Gibbs introduced the preliminary outline of the principles of his new equation able to predict or estimate the tendencies of various natural processes to ensue when bodies or systems are brought into contact. By studying the interactions of homogeneous substances in contact, i.e. bodies, being in composition part solid, part liquid, and part vapor, and by using a three-dimensional [[volume]]–[[entropy]]–[[internal energy]] graph, Gibbs was able to determine three states of equilibrium, i.e. "necessarily stable", "neutral", and "unstable", and whether or not changes will ensue. In 1876, Gibbs built on this framework by introducing the concept of chemical potential so to take into account chemical reactions and states of bodies that are chemically different from each other. In his own words, to summarize his results in 1873, Gibbs states:{{citation needed|date=September 2011}}
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| {{quote|If we wish to express in a single equation the necessary and sufficient condition of thermodynamic equilibrium for a substance when surrounded by a medium of constant pressure ''P'' and temperature ''T'', this equation may be written:
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| :<math>\displaystyle \delta (\epsilon - T\eta + P\nu) = 0</math>
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| where ''δ'' refers to the variation produced by any variations in the state of the parts of the body, and (when different parts of the body are in different states) in the proportion in which the body is divided between the different states. The condition of stable equilibrium is that the value of the expression in the parenthesis shall be a minimum.}}
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| In this description, as used by Gibbs, ''ε'' refers to the [[internal energy]] of the body, ''η'' refers to the [[entropy]] of the body, and ''ν'' is the [[volume]] of the body.
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| ==Electrochemical, internal, external, and total chemical potential==
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| The abstract definition of chemical potential given above—total change in free energy per extra mole of substance—is more specifically called '''total chemical potential'''.<ref name=Kittel>''[http://books.google.com/books?id=c0R79nyOoNMC&pg=PA124 Thermal Physics]'' by Kittel and Kroemer, second edition, page 124.</ref><ref>''Thermodynamics in Earth and Planetary Sciences'' by Jibamitra Ganguly, [http://books.google.com/books?id=aD6TJAuCTVsC&pg=PA240 google books link]. This text uses "internal", "external", and "total chemical potential" as in this article.</ref> If two locations have different total chemical potentials for a species, some of it may be due to potentials associated with "external" force fields ([[Electric potential energy]] differences, [[gravitational potential energy]] differences, etc.), while the rest would be due to "internal" factors (density, temperature, etc.)<ref name=Kittel/> Therefore the total chemical potential can be split into '''internal chemical potential''' and '''external chemical potential''':
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| :<math>\mu_{\mathrm{tot}} = \mu_{\mathrm{int}} + \mu_{\mathrm{ext}} \,</math>
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| where
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| :<math>\mu_{\mathrm{ext}} = qV + mgh + \cdots</math>
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| i.e., the external potential is the sum of electric potential, gravitational potential, etc. (q and m are the charge and mass of the species, respectively, V and h are the [[voltage]] and height of the container, respectively, and g is the [[Standard gravity|acceleration due to gravity]].) The internal chemical potential includes everything else besides the external potentials, such as density, temperature, and enthalpy.
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| The phrase "chemical potential" sometimes means "total chemical potential", but that is not universal.<ref name=Kittel/> In some fields, in particular [[electrochemistry]], [[semiconductor physics]], and [[solid-state physics]], the term "chemical potential" means ''internal'' chemical potential, while the term [[electrochemical potential]] is used to mean ''total'' chemical potential.<ref>''Electrochemical Methods'' by Bard and Faulkner, 2nd edition, Section 2.2.4(a),4-5.</ref><ref>''Electrochemistry at Metal and Semiconductor Electrodes'', by Norio Sato, pages 4-5, [http://books.google.com/books?id=olQzaXNgM74C&pg=PA4 google books link]</ref><ref>''Physics Of Transition Metal Oxides'', by Sadamichi Maekawa, p323, [http://books.google.com/books?id=iyNzfufnkBgC&pg=PA323 google books link]</ref><ref>''The Physics of Solids: Essentials and Beyond'', by Eleftherios N. Economou, page 140, [http://books.google.com/books?id=SyGsHxH071MC&pg=PA140 google books link]. In this text, total chemical potential is usually called as "electrochemical potential", but sometimes as just "chemical potential". The internal chemical potential is referred to by the unwieldy phrase "chemical potential in the absence of the [electric] field".</ref><ref>''Solid State Physics'' by Ashcroft and Mermin, page 257 note 36. Page 593 of the same book uses, instead, an unusual "flipped" definition where "chemical potential" is the total chemical potential which is constant in equilibrium, and "electrochemical potential" is the internal chemical potential; presumably this unusual terminology was an unintentional mistake.</ref>
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| ==Systems of particles==
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| ===Chemical potential of electrons in solids===
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| {{main|Fermi level}}
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| Electrons in solids have a chemical potential, defined the same way as the chemical potential of a chemical species: The change in free energy when electrons are added or removed from the system. In the case of electrons, the chemical potential is usually expressed in energy per particle rather than energy per mole, and the energy per particle is conventionally given in units of [[electron-volt]] (eV).
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| Chemical potential plays an especially important role in [[semiconductor physics]]. For example, [[doping (semiconductor)|n-type]] silicon has a higher chemical potential of electrons than [[doping (semiconductor)|p-type]] silicon. Therefore, when p-type and n-type silicon are put into contact–called a p–n junction–electrons will spontaneously flow from the n-type to the p-type. This transfer of charge causes a "built-in" electric field, which is central to how [[p–n diode]]s and [[photovoltaics]] work. In the diode at equilibrium the [[chemical potential]] (''internal'' chemical potential) varies from the p-type to the n-type side, while the [[total chemical potential]] (electrochemical potential) is constant throughout the diode.
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| Chemical potential of electrons in solids is closely related to the concepts of [[work function]], [[fermi level]], [[electronegativity]], and [[ionization potential]]. In fact, the chemical potential of an atom is sometimes said to be the negative of the atom's [[electronegativity]]. Likewise, the process of chemical potential equalization is sometimes referred to as the process of ''electronegativity equalization''. This connection comes from the [[Mulliken scale|Mulliken]] definition of electronegativity. By inserting the energetic definitions of the [[ionization potential]] and [[electron affinity]] into the Mulliken electronegativity, it is possible to show that the Mulliken chemical potential is a finite difference approximation of the electronic energy with respect to the number of electrons., i.e.,
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| :<math>\mu_{\mathrm{Mulliken}}=-\chi_{\mathrm{Mulliken}}=-\frac{IP+EA}{2}=\left[\frac{\delta E[N]}{\delta N}\right]_{N=N_0}</math>
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| where ''IP'' and ''EA'' are the ionization potential and electron affinity of the atom, respectively.
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| As described above, when describing chemical potential, one has to say "relative to what". In the case of electrons in solids, chemical potential is often specified "relative to vacuum", i.e. relative to an electron sitting isolated in empty space. This definition is somewhat delicate, however, as [[Fermi_level#Why_it_is_not_advisable_to_use_.22the_energy_in_vacuum.22_as_a_reference_zero|not all points in the vacuum are equivalent]].
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| In practice, the [[electrochemical potential]] of electrons is even more important than the chemical potential. The electrochemical potential of electrons in a solid is called the [[Fermi level]].
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| ===Sub-nuclear particles===
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| In recent years, [[thermal physics]] has applied the definition of chemical potential to systems in [[particle physics]] and its associated processes. For example, in a [[quark-gluon plasma]] or other [[QCD matter]], at every point in space there is a chemical potential for [[photon]]s, a chemical potential for electrons, a chemical potential for [[baryon number]], [[electric charge]], and so forth.
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| In the case of photons, photons are [[boson]]s and can very easily and rapidly appear or disappear. Therefore the chemical potential of photons is always and everywhere zero. The reason is, if the chemical potential somewhere was higher than zero, photons would spontaneously disappear from that area until the chemical potential went back to zero; likewise if the chemical potential somewhere was less than zero, photons would spontaneously appear until the chemical potential went back to zero. Since this process occurs extremely rapidly (at least, it occurs rapidly in the presence of dense charged matter), it is safe to assume that the photon chemical potential is never different from zero.
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| Electric charge is different, because it is conserved, i.e. it can be neither created nor destroyed. It can, however, diffuse. The "chemical potential of electric charge" controls this diffusion: Electric charge, like anything else, will tend to diffuse from areas of higher chemical potential to areas of lower chemical potential.<ref>{{cite book|author= Baierlein, Ralph|title=Thermal Physics|publisher=Cambridge University Press|year=2003|isbn=0-521-65838-1|oclc= 39633743}}</ref> Other conserved quantities like [[baryon number]] are the same. In fact, each conserved quantity is associated with a chemical potential and a corresponding tendency to diffuse to equalize it out.<ref>[http://books.google.com/books?id=SAlbKkdor1gC&pg=PA91&lpg=PA91 Hadrons and Quark-Gluon Plasma], by Jean Letessier, Johann Rafelski, p91</ref>
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| In the case of electrons, the behavior depends on temperature and context. At low temperatures, with no [[positron]]s present, electrons cannot be created or destroyed. Therefore there is an electron chemical potential that might vary in space, causing diffusion. At very high temperatures, however, electrons and positrons can spontaneously appear out of the vacuum ([[pair production]]), so the chemical potential of electrons by themselves becomes a less useful quantity than the chemical potential of the conserved quantities like (electrons minus positrons).
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| The chemical potentials of [[boson]]s and [[fermion]]s is related to the number of particles and the temperature by [[Bose–Einstein statistics]] and [[Fermi–Dirac statistics]] respectively.
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| ==See also==
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| *[[Activity (chemistry)]]
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| *[[Chemical equilibrium]]
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| *[[Electrochemical potential]]
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| *[[Equilibrium chemistry]]
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| *[[Excess chemical potential]]
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| *[[Fugacity]]
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| *[[Partial molar property]]
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| *[[Thermodynamic equilibrium]]
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| ==References==
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| {{Reflist}}
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| <!-- * {{cite journal | last = Kaplan| first = T. A. |date=March 2006
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| | title = The Chemical Potential| journal = Journal of Statistical Physics
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| | volume = 122| issue = 6| pages = 1237–1260| doi = 10.1007/s10955-005-8067-x|bibcode = 2006JSP...122.1237K }} -->
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| ==External links==
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| *[http://www.tf.uni-kiel.de/matwis/amat/def_en/kap_2/advanced/t2_4_1.html Chemical Potential]
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| *[http://www.phasediagram.dk/chemical_potentials.htm Chemical Potentials]
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| *[http://www.job-stiftung.de/index.php?id=54,0,0,1,0,0 Values of the chemical potential of 1300 substances]
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| <!-- (not relevant) *[http://www.job-stiftung.de/index.php?id=31,0,0,1,0,0 Chemical potential in experiments:] Demonstration experiments "dissolution of marble", "ammonia fountain", "carbide lamp" (instructions and videos) -->
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| [[Category:Physical chemistry]]
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| [[Category:Potentials]]
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| [[Category:Thermodynamics]]
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| [[Category:Thermodynamic properties]]
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| {{Link GA|es}}
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