Geochemistry

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Geochemistryis thesciencethat uses the tools and principles ofchemistryto explain the mechanisms behind major geological systems such as theEarth's crustand itsoceans.^[1]: 1The realm of geochemistry extends beyond theEarth, encompassing the entireSolar System,^[2]and has made important contributions to the understanding of a number of processes includingmantle convection, the formation ofplanetsand the origins ofgraniteandbasalt.^[1]: 1It is an integrated field of chemistry andgeology.

The termgeochemistrywas first used by the Swiss-German chemistChristian Friedrich Schönbeinin 1838: "a comparative geochemistry ought to be launched, before geognosy can become geology, and before the mystery of the genesis of our planets and their inorganic matter may be revealed."^[3]However, for the rest of the century the more common term was "chemical geology", and there was little contact betweengeologistsandchemists.^[3]

Geochemistry emerged as a separate discipline after major laboratories were established, starting with theUnited States Geological Survey(USGS) in 1884, which began systematic surveys of the chemistry of rocks and minerals. The chief USGS chemist,Frank Wigglesworth Clarke, noted that the elements generally decrease in abundance as their atomic weights increase, and summarized the work on elemental abundance inThe Data of Geochemistry.^[3][4]: 2

The composition ofmeteoriteswas investigated and compared to terrestrial rocks as early as 1850. In 1901,Oliver C. Farringtonhypothesised that, although there were differences, the relative abundances should still be the same.^[3]This was the beginnings of the field ofcosmochemistryand has contributed much of what we know about the formation of the Earth and the Solar System.^[5]

In the early 20th century,Max von LaueandWilliam L. Braggshowed that X-ray scattering could be used to determine the structures of crystals. In the 1920s and 1930s,Victor Goldschmidtand associates at theUniversity of Osloapplied these methods to many common minerals and formulated a set of rules for how elements are grouped. Goldschmidt published this work in the seriesGeochemische Verteilungsgesetze der Elemente[Geochemical Laws of the Distribution of Elements].^{[4]: 2 [6]}

The research ofManfred Schidlowskifrom the 1960s to around the year 2002 was concerned with the biochemistry of theEarly Earthwith a focus on isotope-biogeochemistry and the evidence of the earliest life processes inPrecambrian.^[7][8]

Some subfields of geochemistry are:^[9]

• Aqueous geochemistrystudies the role of various elements in watersheds, includingcopper,sulfur,mercury, and how elemental fluxes are exchanged through atmospheric-terrestrial-aquatic interactions.^[10]
• Biogeochemistryis the field of study focusing on the effect of life on the chemistry of the Earth.^[11]: 3
• Cosmochemistryincludes the analysis of the distribution of elements and their isotopes in thecosmos.^[2]: 1
• Isotope geochemistryinvolves the determination of the relative and absolute concentrations of theelementsand theirisotopesin the Earth and on Earth's surface.^[12]
• Organic geochemistry, the study of the role of processes and compounds that are derived from living or once-living organisms.^[13]
• Photogeochemistryis the study of light-induced chemical reactions that occur or may occur among natural components of the Earth's surface.^[14]
• Regional geochemistryincludes applications to environmental, hydrological and mineral exploration studies.^[15]

The building blocks of materials are thechemical elements. These can be identified by theiratomic numberZ, which is the number ofprotonsin thenucleus. An element can have more than one value for N, thenumber of neutronsin the nucleus. The sum of these is themass number, which is roughly equal to theatomic mass. Atoms with the same atomic number but different neutron numbers are calledisotopes. A given isotope is identified by a letter for the element preceded by a superscript for the mass number. For example, two common isotopes ofchlorineare³⁵Cl and³⁷Cl. There are about 1700 known combinations of Z and N, of which only about 260 are stable. However, most of the unstable isotopes do not occur in nature. In geochemistry, stable isotopes are used to trace chemical pathways and reactions, while radioactive isotopes are primarily used to date samples.^{[4]: 13–17}

The chemical behavior of an atom – itsaffinity for other elementsand the type ofbondsit forms – is determined by the arrangement of electrons inorbitals, particularly the outermost (valence) electrons. These arrangements are reflected in the position of elements in theperiodic table.^{[4]: 13–17}Based on position, the elements fall into the broad groups ofalkali metals,alkaline earth metals,transition metals, semi-metals (also known asmetalloids),halogens,noble gases,lanthanidesandactinides.^{[4]: 20–23}

Another useful classification scheme for geochemistry is theGoldschmidt classification, which places the elements into four main groups.Lithophilescombine easily with oxygen. These elements, which includeNa,K,Si,Al,Ti,MgandCa, dominate in theEarth's crust, formingsilicatesand other oxides.Siderophileelements (Fe,Co,Ni,Pt,Re,Os) have an affinity forironand tend to concentrate in thecore.Chalcophileelements (Cu,Ag,Zn,Pb,S) formsulfides; andatmophileelements (O,N,Hand noble gases) dominate the atmosphere. Within each group, some elements arerefractory, remaining stable at high temperatures, while others arevolatile, evaporating more easily, so heating can separate them.^{[1]: 17 [4]: 23}

The chemical composition of the Earth and other bodies is determined by two opposing processes: differentiation and mixing. In the Earth'smantle, differentiation occurs atmid-ocean ridgesthroughpartial melting, with more refractory materials remaining at the base of thelithospherewhile the remainder rises to formbasalt. After an oceanic plate descends into the mantle,convectioneventually mixes the two parts together.Erosiondifferentiatesgranite, separating it intoclayon the ocean floor,sandstoneon the edge of the continent, and dissolved minerals in ocean waters.Metamorphismandanatexis(partial melting of crustal rocks) can mix these elements together again. In the ocean, biological organisms can cause chemical differentiation, while dissolution of the organisms and their wastes can mix the materials again.^{[1]: 23–24}

A major source of differentiation isfractionation, an unequal distribution of elements and isotopes. This can be the result of chemical reactions,phase changes, kinetic effects, orradioactivity.^[1]: 2–3On the largest scale,planetary differentiationis a physical and chemical separation of a planet into chemically distinct regions. For example, the terrestrial planets formed iron-rich cores and silicate-rich mantles and crusts.^[16]: 218In the Earth's mantle, the primary source of chemical differentiation ispartial melting, particularly near mid-ocean ridges.^{[17]: 68, 153}This can occur when the solid is heterogeneous or asolid solution, and part of the melt is separated from the solid. The process is known asequilibriumorbatchmelting if the solid and melt remain in equilibrium until the moment that the melt is removed, andfractionalorRayleighmelting if it is removed continuously.^[18]

Isotopic fractionationcan have mass-dependent and mass-independent forms. Molecules with heavier isotopes have lowerground state energiesand are therefore more stable. As a result, chemical reactions show a small isotope dependence, with heavier isotopes preferring species or compounds with a higher oxidation state; and in phase changes, heavier isotopes tend to concentrate in the heavier phases.^[19]Mass-dependent fractionation is largest in light elements because the difference in masses is a larger fraction of the total mass.^[20]: 47

Ratios between isotopes are generally compared to a standard. For example, sulfur has four stable isotopes, of which the two most common are³²S and³⁴S.^[20]: 98The ratio of their concentrations,R=³⁴S/³²S, is reported as

${\displaystyle \delta {}^{34}\mathrm {S} =1000\left({\frac {R}{R_{\mathrm {s} }}}-1\right),}$

whereR_sis the same ratio for a standard. Because the differences are small, the ratio is multiplied by 1000 to make it parts per thousand (referred to as parts per mil). This is represented by the symbol‰.^[19]: 55

Equilibrium fractionationoccurs between chemicals or phases that are in equilibrium with each other. In equilibrium fractionation between phases, heavier phases prefer the heavier isotopes. For two phases A and B, the effect can be represented by the factor

${\displaystyle a_{\mathrm {A-B} }={\frac {R_{\mathrm {A} }}{R_{\mathrm {B} }}}.}$

In the liquid-vapor phase transition for water,a_l-vat 20 degreesCelsiusis 1.0098 for¹⁸O and 1.084 for²H. In general, fractionation is greater at lower temperatures. At 0 °C, the factors are 1.0117 and 1.111.^[19]: 59

When there is no equilibrium between phases or chemical compounds,kinetic fractionationcan occur. For example, at interfaces between liquid water and air, the forward reaction is enhanced if the humidity of the air is less than 100% or the water vapor is moved by a wind. Kinetic fractionation generally is enhanced compared to equilibrium fractionation and depends on factors such as reaction rate, reaction pathway and bond energy. Since lighter isotopes generally have weaker bonds, they tend to react faster and enrich the reaction products.^[19]: 60

Biological fractionation is a form of kinetic fractionation since reactions tend to be in one direction. Biological organisms prefer lighter isotopes because there is a lower energy cost in breaking energy bonds. In addition to the previously mentioned factors, the environment and species of the organism can have a large effect on the fractionation.^[19]: 70

Through a variety of physical and chemical processes, chemical elements change in concentration and move around in what are calledgeochemical cycles. An understanding of these changes requires both detailed observation and theoretical models. Each chemical compound, element or isotope has a concentration that is a functionC(r,t)of position and time, but it is impractical to model the full variability. Instead, in an approach borrowed fromchemical engineering,^[1]: 81geochemists average the concentration over regions of the Earth calledgeochemical reservoirs. The choice of reservoir depends on the problem; for example, the ocean may be a single reservoir or be split into multiple reservoirs.^[21]In a type of model called abox model, a reservoir is represented by a box with inputs and outputs.^{[1]: 81 [21]}

Geochemical models generally involve feedback. In the simplest case of a linear cycle, either the input or the output from a reservoir is proportional to the concentration. For example,saltis removed from the ocean by formation ofevaporites, and given a constant rate of evaporation in evaporite basins, the rate of removal of salt should be proportional to its concentration. For a given componentC, if the input to a reservoir is a constantaand the output iskCfor some constantk, then themass balanceequation is

${\displaystyle {\frac {dC}{dt}}=a-kC.}$

(1)

This expresses the fact that any change in mass must be balanced by changes in the input or output. On a time scale oft= 1/k, the system approaches asteady statein whichC^steady=a/k. Theresidence timeis defined as

${\displaystyle \tau _{\mathrm {res} }=C^{\text{steady}}/I=C^{\text{steady}}/O,}$

whereIandOare the input and output rates. In the above example, the steady-state input and output rates are both equal toa, soτ_res= 1/k.^[21]

If the input and output rates are nonlinear functions ofC, they may still be closely balanced over time scales much greater than the residence time; otherwise, there will be large fluctuations inC. In that case, the system is always close to a steady-state and the lowest order expansion of the mass balance equation will lead to a linear equation like Equation (1). In most systems, one or both of the input and output depend onC, resulting in feedback that tends to maintain the steady-state. If an external forcing perturbs the system, it will return to the steady-state on a time scale of1/k.^[21]

The composition of the solar system is similar to that of many other stars, and aside from small anomalies it can be assumed to have formed from asolar nebulathat had a uniform composition, and the composition of theSun'sphotosphereis similar to that of the rest of the Solar System. The composition of the photosphere is determined by fitting theabsorption linesin itsspectrumto models of the Sun's atmosphere.^[23]By far the largest two elements by fraction of total mass are hydrogen (74.9%) andhelium(23.8%), with all the remaining elements contributing just 1.3%.^[24]There is a general trend ofexponential decreasein abundance with increasing atomic number, although elements with even atomic number are more common than their odd-numbered neighbors (theOddo–Harkins rule). Compared to the overall trend,lithium,boronandberylliumare depleted and iron is anomalously enriched.^{[25]: 284–285}

The pattern of elemental abundance is mainly due to two factors. The hydrogen, helium, and some of the lithium wereformed in about 20 minutes after the Big Bang, while the rest werecreated in the interiors of stars.^{[4]: 316–317}

Meteoritescome in a variety of compositions, but chemical analysis can determine whether they were once inplanetesimalsthatmeltedordifferentiated.^[23]: 45Chondritesare undifferentiated and have round mineral inclusions calledchondrules. With the ages of 4.56 billion years, they date to theearly solar system. A particular kind, theCI chondrite, has a composition that closely matches that of the Sun's photosphere, except for depletion of some volatiles (H, He, C, N, O) and a group of elements (Li, B, Be) that are destroyed by nucleosynthesis in the Sun.^{[4]: 318 [23]}Because of the latter group, CI chondrites are considered a better match for the composition of the early Solar System. Moreover, the chemical analysis of CI chondrites is more accurate than for the photosphere, so it is generally used as the source for chemical abundance, despite their rareness (only five have been recovered on Earth).^[23]

The planets of the Solar System are divided into two groups: the four inner planets are theterrestrial planets(Mercury,Venus,EarthandMars), with relatively small sizes and rocky surfaces. The four outer planets are thegiant planets, which are dominated by hydrogen and helium and have lower mean densities. These can be further subdivided into thegas giants(JupiterandSaturn) and theice giants(UranusandNeptune) that have large icy cores.^{[26]: 26–27, 283–284}

Most of our direct information on the composition of the giant planets is fromspectroscopy. Since the 1930s, Jupiter was known to contain hydrogen,methaneandammonium. In the 1960s,interferometrygreatly increased the resolution and sensitivity of spectral analysis, allowing the identification of a much greater collection of molecules includingethane,acetylene, water andcarbon monoxide.^{[27]: 138–139}However, Earth-based spectroscopy becomes increasingly difficult with more remote planets, since the reflected light of the Sun is much dimmer; and spectroscopic analysis of light from the planets can only be used to detect vibrations of molecules, which are in theinfraredfrequency range. This constrains the abundances of the elements H, C and N.^[27]: 130Two other elements are detected: phosphorus in the gasphosphine(PH₃) and germanium ingermane(GeH₄).^[27]: 131

The helium atom has vibrations in theultravioletrange, which is strongly absorbed by the atmospheres of the outer planets and Earth. Thus, despite its abundance, helium was only detected once spacecraft were sent to the outer planets, and then only indirectly through collision-induced absorption in hydrogen molecules.^[27]: 209Further information on Jupiter was obtained from theGalileoprobewhen it was sent into the atmosphere in 1995;^[28][29]and thefinal missionof theCassini probein 2017 was to enter the atmosphere of Saturn.^[30]In the atmosphere of Jupiter, He was found to be depleted by a factor of 2 compared to solar composition and Ne by a factor of 10, a surprising result since the other noble gases and the elements C, N and S were enhanced by factors of 2 to 4 (oxygen was also depleted but this was attributed to the unusually dry region that Galileo sampled).^[29]

Spectroscopic methods only penetrate the atmospheres of Jupiter and Saturn to depths where the pressure is about equal to 1bar, approximately Earth'satmospheric pressureatsea level.^[27]: 131The Galileo probe penetrated to 22 bars.^[29]This is a small fraction of the planet, which is expected to reach pressures of over 40 Mbar. To constrain the composition in the interior, thermodynamic models are constructed using the information on temperature from infrared emission spectra and equations of state for the likely compositions.^[27]: 131High-pressure experiments predict that hydrogen will be a metallic liquid in the interior of Jupiter and Saturn, while in Uranus and Neptune it remains in the molecular state.^{[27]: 135–136}Estimates also depend on models for the formation of the planets. Condensation of the presolar nebula would result in a gaseous planet with the same composition as the Sun, but the planets could also have formed when a solid core captured nebular gas.^[27]: 136

In current models, the four giant planets have cores of rock and ice that are roughly the same size, but the proportion of hydrogen and helium decreases from about 300 Earth masses in Jupiter to 75 in Saturn and just a few in Uranus and Neptune.^[27]: 220Thus, while the gas giants are primarily composed of hydrogen and helium, the ice giants are primarily composed of heavier elements (O, C, N, S), primarily in the form of water, methane, and ammonia. The surfaces are cold enough for molecular hydrogen to be liquid, so much of each planet is likely a hydrogen ocean overlaying one of heavier compounds.^[31]Outside the core, Jupiter has a mantle of liquid metallic hydrogen and an atmosphere of molecular hydrogen and helium. Metallic hydrogen does not mix well with helium, and in Saturn, it may form a separate layer below the metallic hydrogen.^[27]: 138

Terrestrial planets are believed to have come from the same nebular material as the giant planets, but they have lost most of the lighter elements and have different histories. Planets closer to the Sun might be expected to have a higher fraction of refractory elements, but if their later stages of formation involved collisions of large objects with orbits that sampled different parts of the Solar System, there could be little systematic dependence on position.^{[32]: 3–4}

Direct information on Mars, Venus and Mercury largely comes from spacecraft missions. Usinggamma-ray spectrometers, the composition of the crust of Mars has been measured by theMars Odysseyorbiter,^[33]the crust of Venus by some of theVeneramissions to Venus,^[32]and the crust of Mercury by theMESSENGERspacecraft.^[34]Additional information on Mars comes from meteorites that have landed on Earth (theShergottites,Nakhlites, andChassignites, collectively known as SNC meteorites).^[35]: 124Abundances are also constrained by the masses of the planets, while the internal distribution of elements is constrained by their moments of inertia.^[4]: 334

The planets condensed from the solar nebula, and much of the details of their composition are determined by fractionation as they cooled. The phases that condense fall into five groups. First to condense are materials rich in refractory elements such as Ca and Al. These are followed by nickel and iron, thenmagnesium silicates. Below about 700kelvins(700 K),FeSand volatile-rich metals and silicates form a fourth group, and in the fifth groupFeOenter the magnesium silicates.^[36]The compositions of the planets and the Moon arechondritic, meaning that within each group the ratios between elements are the same as in carbonaceous chondrites.^[4]: 334

The estimates of planetary compositions depend on the model used. In theequilibrium condensationmodel, each planet was formed from afeeding zonein which the compositions of solids were determined by the temperature in that zone. Thus, Mercury formed at 1400 K, where iron remained in a pure metallic form and there was little magnesium or silicon in solid form; Venus at 900 K, so all the magnesium and silicon condensed; Earth at 600 K, so it contains FeS and silicates; and Mars at 450 K, so FeO was incorporated into magnesium silicates. The greatest problem with this theory is that volatiles would not condense, so the planets would have no atmospheres and Earth no atmosphere.^{[4]: 335–336}

Inchondritic mixingmodels, the compositions of chondrites are used to estimate planetary compositions. For example, one model mixes two components, one with the composition of C1 chondrites and one with just the refractory components of C1 chondrites.^[4]: 337In another model, the abundances of the five fractionation groups are estimated using an index element for each group. For the most refractory group,uraniumis used; iron for the second; the ratios of potassium andthalliumto uranium for the next two; and the molar ratio FeO/(FeO+MgO) for the last. Using thermal and seismic models along with heat flow and density, Fe can be constrained to within 10 percent on Earth, Venus, and Mercury. U can be constrained within about 30% on Earth, but its abundance on other planets is based on "educated guesses". One difficulty with this model is that there may be significant errors in its prediction of volatile abundances because some volatiles are only partially condensed.^{[36][4]: 337–338}

The more common rock constituents are nearly alloxides;chlorides,sulfidesandfluoridesare the only important exceptions to this and their total amount in any rock is usually much less than 1%. By 1911,F. W. Clarkehad calculated that a little more than 47% of the Earth's crust consists ofoxygen. It occurs principally in combination as oxides, of which the chief aresilica,alumina,iron oxides, and variouscarbonates(calcium carbonate,magnesium carbonate,sodium carbonate, andpotassium carbonate). The silica functions principally as an acid, forming silicates, and all the commonest minerals ofigneous rocksare of this nature. From a computation based on 1672 analyses of numerous kinds of rocks Clarke arrived at the following as the average percentage composition of the Earth's crust: SiO₂=59.71, Al₂O₃=15.41, Fe₂O₃=2.63, FeO=3.52, MgO=4.36, CaO=4.90, Na₂O=3.55, K₂O=2.80, H₂O=1.52, TiO₂=0.60, P₂O₅=0.22, (total 99.22%). All the other constituents occur only in very small quantities, usually much less than 1%.^[37]

These oxides combine in a haphazard way. For example,potash(potassium carbonate) and soda (sodium carbonate) combine to producefeldspars. In some cases, they may take other forms, such asnepheline,leucite, andmuscovite, but in the great majority of instances they are found as feldspar.Phosphoric acidwithlime(calcium carbonate) formsapatite.Titanium dioxidewithferrous oxidegives rise toilmenite. Part of the lime forms lime feldspar. Magnesium carbonate and iron oxides with silica crystallize asolivineorenstatite, or with alumina and lime form the complex ferromagnesian silicates of which thepyroxenes,amphiboles, andbiotitesare the chief. Any excess of silica above what is required to neutralize thebaseswill separate out asquartz; excess of alumina crystallizes ascorundum. These must be regarded only as general tendencies. It is possible, by rock analysis, to say approximately what minerals the rock contains, but there are numerous exceptions to any rule.^[37]

Except inacidor siliceous igneous rocks containing greater than 66% ofsilica, known asfelsicrocks, quartz is not abundant in igneous rocks. In basic rocks (containing 20% of silica or less) it is rare for them to contain as much silicon, these are referred to asmaficrocks. Ifmagnesiumandironare above average while silica is low,olivinemay be expected; where silica is present in greater quantity over ferromagnesian minerals, such asaugite,hornblende,enstatiteorbiotite, occur rather than olivine. Unlesspotashis high and silica relatively low,leucitewill not be present, for leucite does not occur with free quartz.Nepheline, likewise, is usually found in rocks with much soda and comparatively little silica. With highalkalis, soda-bearingpyroxenesandamphibolesmay be present. The lower the percentage of silica and alkali's, the greater is the prevalence ofplagioclase feldsparas contracted with soda or potash feldspar.^[37]

Earth's crust is composed of 90% silicate minerals and their abundance in the Earth is as follows:plagioclase feldspar(39%),alkali feldspar(12%), quartz (12%),pyroxene(11%),amphiboles(5%),micas(5%),clay minerals(5%); the remaining silicate minerals make up another 3% of Earth's crust. Only 8% of the Earth is composed of non-silicate minerals such ascarbonates,oxides, andsulfides.^[38]

The other determining factor, namely the physical conditions attending consolidation, plays, on the whole, a smaller part, yet is by no means negligible. Certain minerals are practically confined to deep-seated intrusive rocks, e.g., microcline, muscovite, diallage. Leucite is very rare in plutonic masses; many minerals have special peculiarities in microscopic character according to whether they crystallized in-depth or near the surface, e.g., hypersthene, orthoclase, quartz. There are some curious instances of rocks having the same chemical composition, but consisting of entirely different minerals, e.g., the hornblendite of Gran, in Norway, which contains only hornblende, has the same composition as some of thecamptonitesof the same locality that contain feldspar and hornblende of a different variety. In this connection, we may repeat what has been said above about the corrosion of porphyritic minerals in igneous rocks. In rhyolites and trachytes, early crystals of hornblende and biotite may be found in great numbers partially converted into augite and magnetite. Hornblende and biotite were stable under the pressures and other conditions below the surface, but unstable at higher levels. In the ground-mass of these rocks, augite is almost universally present. But the plutonic representatives of the same magma, granite, and syenite contain biotite and hornblende far more commonly than augite.^[37]

Those rocks that contain the most silica, and on crystallizing yield free quartz, form a group generally designated the "felsic" rocks. Those again that contain the least silica and most magnesia and iron, so that quartz is absent whileolivineis usually abundant, form the "mafic" group. The "intermediate" rocks include those characterized by the general absence of both quartz and olivine. An important subdivision of these contains a very high percentage of alkalis, especially soda, and consequently has minerals such asnephelineandleucitenot common in other rocks. It is often separated from the others as the "alkali" or "soda" rocks, and there is a corresponding series of mafic rocks. Lastly, a small sub-group rich in olivine and without feldspar has been called the "ultramafic" rocks. They have very low percentages of silica but much iron and magnesia.

Except these last, practically all rocks contain felspars or feldspathoid minerals. In the acid rocks, the common feldspars are orthoclase, perthite, microcline, and oligoclase—all having much silica and alkalis. In the mafic rocks labradorite, anorthite, and bytownite prevail, being rich in lime and poor in silica, potash, and soda. Augite is the most common ferromagnesian in mafic rocks, but biotite and hornblende are on the whole more frequent in felsic rocks.^[37]

Most Common Minerals	Felsic	Intermediate		Mafic	Ultramafic
	Quartz Orthoclase (and Oligoclase), Mica, Hornblende, Augite	Little or no Quartz: Orthoclase hornblende, Augite, Biotite	Little or no Quartz: Plagioclase Hornblende, Augite, Biotite	No Quartz Plagioclase Augite, Olivine	No Felspar Augite, Hornblende, Olivine
Plutonic or Abyssal type	Granite	Syenite	Diorite	Gabbro	Peridotite
Intrusive orHypabyssaltype	Quartz-porphyry	Orthoclase-porphyry	Porphyrite	Dolerite	Picrite
Lavas or Effusive type	Rhyolite,Obsidian	Trachyte	Andesite	Basalt	Komatiite

Rocks that contain leucite or nepheline, either partly or wholly replacing felspar, are not included in this table. They are essentially of intermediate or of mafic character. We might in consequence regard them as varieties of syenite, diorite, gabbro, etc., in which feldspathoid minerals occur, and indeed there are many transitions between syenites of ordinary type and nepheline — or leucite — syenite, and between gabbro or dolerite and theralite or essexite. But, as many minerals develop in these "alkali" rocks that are uncommon elsewhere, it is convenient in a purely formal classification like that outlined here to treat the whole assemblage as a distinct series.^[37]

Nepheline and Leucite-bearing Rocks

Most Common Minerals	Alkali Feldspar, Nepheline or Leucite, Augite, Hornblend, Biotite	Soda Lime Feldspar, Nepheline or Leucite, Augite, Hornblende (Olivine)	Nepheline or Leucite, Augite, Hornblende, Olivine
Plutonic type	Nepheline-syenite, Leucite-syenite, Nepheline-porphyry	Essexite and Theralite	Ijolite and Missourite
Effusive type or Lavas	Phonolite, Leucitophyre	Tephrite and Basanite	Nepheline-basalt, Leucite-basalt

This classification is based essentially on the mineralogical constitution of the igneous rocks. Any chemical distinctions between the different groups, though implied, are relegated to a subordinate position. It is admittedly artificial, but it has grown up with the growth of the science and is still adopted as the basis on which more minute subdivisions are erected. The subdivisions are by no means of equal value. The syenites, for example, and the peridotites, are far less important than the granites, diorites, and gabbros. Moreover, the effusive andesites do not always correspond to the plutonic diorites but partly also to the gabbros. As the different kinds of rock, regarded asaggregatesof minerals, pass gradually into one another, transitional types are very common and are often so important as to receive special names. The quartz-syenites and nordmarkites may be interposed between granite and syenite, the tonalites and adamellites between granite and diorite, the monzonites between syenite and diorite, norites and hyperites between diorite and gabbro, and so on.^[37]

Trace metalsreadily formcomplexeswith majorionsin the ocean, includinghydroxide,carbonate, andchlorideand their chemical speciation changes depending on whether the environment isoxidized or reduced.^[39]Benjamin (2002) defines complexes of metals with more than one type ofligand, other than water, as mixed-ligand-complexes. In some cases, a ligand contains more than onedonoratom, forming very strong complexes, also calledchelates(the ligand is the chelator). One of the most common chelators is EDTA (ethylenediaminetetraacetic acid), which can replace six molecules of water and form strong bonds with metals that have a plus two charge.^[40]With stronger complexation, loweractivityof the free metal ion is observed. One consequence of the lower reactivity of complexed metals compared to the same concentration of free metal is that the chelation tends to stabilize metals in the aqueous solution instead of in solids.^[40]

Concentrationsof the trace metalscadmium,copper,molybdenum,manganese,rhenium,uraniumandvanadiumin sediments record the redox history of the oceans.^[41]Within aquatic environments, cadmium(II) can either be in the form CdCl⁺_(aq)inoxicwaters or CdS(s) in a reduced environment. Thus, higher concentrations of Cd in marine sediments may indicate low redox potential conditions in the past. For copper(II), a prevalent form is CuCl⁺(aq) within oxic environments and CuS(s) and Cu₂S within reduced environments. The reduced seawater environment leads to two possible oxidation states of copper, Cu(I) and Cu(II).^[41]Molybdenum is present as the Mo(VI) oxidation state as MoO₄²⁻_(aq)in oxic environments. Mo(V) and Mo(IV) are present in reduced environments in the forms MoO₂⁺_(aq)and MoS_2(s).^[41]Rhenium is present as the Re(VII) oxidation state as ReO₄⁻within oxic conditions, but is reduced to Re(IV) which may form ReO₂or ReS₂. Uranium is in oxidation state VI in UO₂(CO₃)₃⁴⁻(aq) and is found in the reduced form UO₂(s).^[41]Vanadium is in several forms in oxidation state V(V); HVO₄²⁻and H₂VO₄⁻. Its reduced forms can include VO₂⁺, VO(OH)₃⁻, and V(OH)₃.^[41]These relative dominance of these species depends onpH.

In the water column of the ocean or deep lakes, vertical profiles of dissolved trace metals are characterized as followingconservative–type,nutrient–type, orscavenged–typedistributions. Across these three distributions, trace metals have different residence times and are used to varying extents byplanktonicmicroorganisms. Trace metals with conservative-type distributions have high concentrations relative to their biological use. One example of a trace metal with a conservative-type distribution is molybdenum. It has a residence time within the oceans of around 8 x 10⁵years and is generally present as themolybdateanion (MoO₄²⁻). Molybdenum interacts weakly with particles and displays an almost uniform vertical profile in the ocean. Relative to the abundance of molybdenum in the ocean, the amount required as a metal cofactor forenzymesin marinephytoplanktonis negligible.^[42]

Trace metals with nutrient-type distributions are strongly associated with the internal cycles of particulate organic matter, especially the assimilation by plankton. The lowest dissolved concentrations of these metals are at the surface of the ocean, where they are assimilated by plankton. As dissolution and decomposition occur at greater depths, concentrations of these trace metals increase. Residence times of these metals, such as zinc, are several thousand to one hundred thousand years. Finally, an example of a scavenged-type trace metal isaluminium, which has strong interactions with particles as well as a short residence time in the ocean. The residence times of scavenged-type trace metals are around 100 to 1000 years. The concentrations of these metals are highest around bottom sediments,hydrothermal vents, and rivers. For aluminium, atmospheric dust provides the greatest source of external inputs into the ocean.^[42]

Iron and copper show hybrid distributions in the ocean. They are influenced by recycling and intense scavenging. Iron is a limiting nutrient in vast areas of the oceans and is found in high abundance along with manganese near hydrothermal vents. Here, many iron precipitates are found, mostly in the forms of iron sulfides and oxidized iron oxyhydroxide compounds. Concentrations of iron near hydrothermal vents can be up to one million times the concentrations found in the open ocean.^[42]

Using electrochemical techniques, it is possible to show that bioactive trace metals (zinc, cobalt, cadmium, iron, and copper) are bound by organic ligands in surface seawater. These ligand complexes serve to lower the bioavailability of trace metals within the ocean. For example, copper, which may be toxic to open ocean phytoplankton and bacteria, can form organic complexes. The formation of these complexes reduces the concentrations of bioavailable inorganic complexes of copper that could be toxic to sea life at high concentrations. Unlike copper, zinc toxicity in marine phytoplankton is low and there is no advantage to increasing the organic binding of Zn²⁺. Inhigh-nutrient, low-chlorophyll regions, iron is the limiting nutrient, with the dominant species being strong organic complexes of Fe(III).^[42]

• The Geochemistry of Igneous Rocks(Gunn Interactive Ltd.)