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Heritage Science
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  • Review
  • Open Access

Isotopes in cultural heritage: present and future possibilities

Heritage Science20186:25

https://doi.org/10.1186/s40494-018-0192-3

©  The Author(s) 2018

  • Received: 10 January 2018
  • Accepted: 16 April 2018
  • Published:

Abstract

This paper is focused on methodology and scientific interpretations by use of isotopes in heritage science—what can be done today, and what may be accomplished in the near future? Generally, isotopic compositions could be used to set time constraints on processes and manufacturing of objects (e.g. the 14C technique). Furthermore, isotopic compositions (e.g. Sr and Pb isotopes) are useful for tracing the origin of a component or a metal. The concepts isotope and isotopic fractionation are explained, and the use of stable respectively radioactive isotopes is exemplified. Elements which today have a large potential in heritage research are reviewed, and some recent and less known applications from the literature are summarized. Useful types of mass spectrometers are briefly described, and the need for reliable standards as well as accurate measurements and corrections is stressed. In future, further chemical elements may be utilized for isotope studies in heritage science, and possible candidates are discussed. The paper may in particular be valuable to readers less acquainted with the use of isotopic measurements. The many examples from referenced papers and also results from the authors’ studies in this field may inspire imaginative and inquisitive scientists to try new applications utilizing isotope data in heritage science.

Keywords

  • Isotopes
  • Standards
  • Dating
  • Measurement
  • Mass spectrometer
  • Archaeology
  • History
  • Art

Brief history and introduction

Some 100 years ago, the knowledge concerning the composition of atoms was elucidated by brilliant scientists such as Ernest Rutherford, J. J. Thomson, Marie Curie, Henri Bequerel, Niels Bohr, F. W. Aston, Frederick Soddy and many others [1]. Much of the early work was concentrated on radioactivity. During studies on the radioactive decay of uranium and thorium, a confusing discovery was that there seemed to be several kinds of thorium atoms which decayed at different rates. The American chemist T. W. Richards showed in 1913 that lead produced from the decay of uranium had a different atomic weight as compared with “ordinary” lead from lead ore. Soddy showed that a radioactive element may have different atomic masses although with identical chemical properties. Francis W. Aston showed with his so-called mass spectrograph that neon gas is composed of two different kinds of atoms, having atomic weights around 20 respectively 22. The different atoms were named “isotopes” after the Greek name which means “the same place” (i.e. in the Periodic Table of Elements). Many of the scientists were rewarded with a Nobel Prize in chemistry or physics: J. J. Thomson (1906), Ernest Rutherford (1908), Marie Curie (1911), Niels Bohr (1922), Frederick Soddy (1921), Francis Aston (1922), Harold Urey (1934) and James Chadwick (1935).

Today, the concept isotope is well known to the scientific world, and numerous applications have for almost a century been used in science. Geologists were among the first to use this technique when attempting to date rocks. Among the earliest works is a helium isotope study [2] where uranium minerals were dated, which a few years later was followed by a radiogenic Pb study aimed to date the mineral uraninite [3]. Some decades later, isotopes were used also in other fields, e.g. medicine and archaeology. In 1943, Georges de Hevesy was awarded a Nobel Prize for his isotopic methods to trace chemical reactions and processes in the human body. Still most important in archaeology is the well-known radiocarbon dating technique [4], for which Willard F. Libby in 1960 received the Nobel Prize in Chemistry. Today’s archaeologists can benefit from a number of scientific techniques to investigate excavated objects [e.g. 5–8], among them various isotopic techniques. Isotope measurements are also applied in many other fields such as forensics, food and beverage industry, environmental sciences, history, heritage science, and also utilized to detect forgeries in art. The present paper gives examples of factors controlling isotopic compositions and gives prominence to chemical elements which are apt to applications in heritage science research, today and in the future. A brief description of useful measuring instruments is included.

Fundamentals of isotopes

Each element is built of atoms. However, for most elements their atoms may have different masses, and the variants are called isotopes. The isotopic distribution for a specific element is almost uniform in the lithosphere and atmosphere. However, small variations of the isotopic compositions of certain elements in nature do occur, and isotope studies are concerned with the interpretations of such variations. These variations are due to two mechanisms: (i) isotopic fractionation—which essentially is due to the breaking of physical bonds of different strengths; and (ii) radioactive decay—whereby one unstable (parent) isotope spontaneously disintegrates and eventually results in a stable (daughter) isotope. The first mechanism concerns stable (non-radiogenic) isotopes and is above all important for light elements, as will be explained below.

Most chemical elements in nature exist with two or more isotopes. The various isotopes of each element have the same number of protons (Z), but this is not true for the number of neutrons (N) or the mass (M = Z + N). For example, carbon (always with Z = 6) has three isotopes: the two stable isotopes 12C (with six neutrons) and 13C (seven neutrons), and (with only about one part per trillion) the radioactive (non-stable) isotope 14C (with eight neutrons), often denoted C-14. Tin is outstanding with its ten stable isotopes. On the other hand, 20 elements exist in nature with only one stable isotope. Among these elements are gold and phosphorus, which is unfortunate since both are important to archaeologists and museum curators. It should also be added that no element with an atomic number Z > 83 is stable, i.e. containing only stable isotopes. There are basically two ways of applying isotopic techniques: one to track the background of objects or human remains (origin, provenance, diet, migration), and another for dating of investigated objects or sites. Some isotope systems have been utilized for many decades, while others have only recently been tested or used for certain applications. The stable isotopes of carbon have a unique archaeological potential, since analyses of carbon isotopes allow evaluations of both provenance and diet pattern. A brief summary of isotope systems and their possible use in heritage science is presented in Table 1.
Table 1

Isotope systems which have been used in archaeology and cultural heritage

Element

Dating

Provenance

Diet for humans

Migration among humans

Other

H

  

X

  

B

 

X

   

C

XX (C-14)

 

XX

  

N

  

X

  

O

 

(X)

X

(X)

Paleothermometry

Mg

  

(X)

  

Si

 

(X)

   

S

 

(X)

X

 

Ore prospecting, pollution

Cl

(X)

    

Ar

X

    

Ca

  

(X)

  

Fe

 

(X)

   

Cu

 

(X)

   

Zn

 

(X)

   

Sr

 

XX

 

X

 

Ag

 

(X)

   

Sn

 

(X)

   

Nd

 

X

   

Hg

 

(X)

   

Pb

 

XX

   

Th

X

    

U

X

    

The most commonly used systems are marked XX, those often used X, and those recently tested or used (X)

Stable isotopes and isotopic fractionation

Local variations in the proportions of stable isotopes of an element are brought about by isotopic fractionation. Each element’s isotopes have identical chemical properties, whereas physical properties such as melting and boiling points display very slight differences. This is the basis for isotopes of different elements to behave differently during natural processes, and therefore the ratio of these isotopes changes or “fractionates”. As early as 1931, Harold Urey discovered the deuterium isotope (2H or “D”) and demonstrated discrepancies in vapor pressure among the isotopes of gaseous elements. Accordingly, evaporation, condensation, rain, snow, melting, crystallization, adsorption, diffusion etcetera may give rise to a small but (sometimes) measurable isotopic differentiation [9]. For example, “ordinary” water, H2O, boils at 100.00 °C at 1 bar, while “heavy” water, D2O, has a boiling point of 101.42 °C. Complicated biochemical processes may also induce a slight isotopic fractionation, for example in photosynthesis, during the synthesis of amino acids or lipids, and processes in bacteria [10–16]. In these processes, the isotopic fractionation is due to physical processes such as diffusion. Occasionally, so called mass-independent fractionation (MIF) can be important in e.g. biochemical reactions as shown for a number of light elements [17]. Generally, a light element induces larger isotopic fractionation because the relative difference in mass between its isotopes is greater than for a heavy element. For instance, deuterium (D, 2H) is twice as heavy as 1H, i.e. 100% heavier, while 181Ta is only 0.56% heavier than 180Ta. The light elements, hydrogen, carbon, nitrogen and oxygen to mention a few, are therefore especially susceptible to natural isotopic fractionation, while much less physical differences are observed for the heavier elements. The reason that the heavy elements strontium and lead have large and easily measurable differences among their isotopes is principally due to radioactive decay processes (cf. below).

Measuring techniques

Fundamentally, there are two methods to determine the amount of various isotopes in a special material. The first is to directly measure the radioactivity of the isotope in question, by counting particles (of α, β, or γ type) that are produced by a specific decay. This method has been used when applying the Carbon-14 dating technique and for other systems such as U-He and Tritium-3He, and have been described to detail in the literature [18]. The prevailing way of analyzing isotopes is to make use of some kind of mass spectrometer that is designed to determine the distribution of an element’s isotopes. The working principle behind this technique is that different types of atoms or molecules can be separated according to their masses, and the ratios between the isotopes of interest can be subsequently measured. Most mass spectrometers are designed for the analysis of organic compounds. However, several types of mass spectrometers have been developed to determine isotope ratios and the basic features of a few commonly used types are presented here. The first generation of magnetic sector instruments in the 1940:s are often named “Nier spectrometer” after its inventor Alfred Nier [19], cf. Fig. 1. This type is sometimes abbreviated Isotope Ratio Mass Spectrometer (IRMS) and another acronym is Stable Isotope Ratio Analysis (SIRA), often used for analysis of gaseous compounds of light stable elements. During the latest decades, more advanced mass spectrometers have been developed, producing increasingly better precision for sample sizes becoming smaller and smaller (nanogram to picogram levels) [e.g. 20–23]. The amount of sample is therefore rarely a problem, but their purity is of the greatest importance. For solid samples, a Thermal Ionization Mass Spectrometer (TIMS) is often used, e.g. for strontium and neodymium specimens, and generates very precise results. It utilizes a minute solid sample, previously isolated in a clean laboratory following standard ion exchange procedures. Certain spectrometers, like a MC-ICP-MS spectrometer (Multiple Collector—Inductively Coupled Plasma—Mass Spectrometer; cf. Fig. 2) are equipped with a laser system. Such laser-based systems remove (ablate) particles from the surface of a sample which are led to an analyzer. This technique as well as the ion microprobe (SIMS; secondary ion mass spectrometry) are capable of analyzing samples in situ, which eliminates the need for tedious laboratory treatment. The latter techniques are versatile and can be used for a range of elements, allowing both stable and radioactive isotopes to be analyzed in very small samples; besides, the sample through-put is large compared to e.g. the TIMS technique. The precision obtained with in situ techniques is, however, not as good as for TIMS-analyzed samples. Irrespective of the instrumentation used, samples must be handled with care and thorough analytical protocols need to be followed in order to obtain precise and accurate results. A feature in common for isotopic measurements is the need for standardization, and this is accomplished in different ways and is method-specific. It is common practice to run samples in duplicate to ensure a good reproducibility.
Fig. 1
Fig. 1

Schematic picture of a Nier-type isotope ratio mass spectrometer using a gas source analytical medium (in this example carbon dioxide, CO2). Reproduced after chemical sciences: a manual for CSIR-UGC National Eligibility Test, http://wikibooks.org

Fig. 2
Fig. 2

An MC-ICP-MS spectrometer (Nu Plasma II) at the Department of Geological Sciences, Swedish Museum of Natural History, Stockholm. Photo: Melanie Schmitt

Light stable isotope applications

Stable isotopes of light elements are utilized in many fields. The archaeological applications dominate, for instance to investigate changes in habitat, food, animal herding, dietary tendencies and migration patterns for humans. A commonly used division is between “traditional” stable isotopes of the light elements of primarily H, C, O, N and S, which are further discussed below. Heavier elements such as lead and strontium, as well as “non-traditional” elements (such as Mg, Cl, Fe and Cu) are considered in a subsequent paragraph.

Standards and data for H, C, N, O, S

The lightest of all elements, hydrogen (Z = 1), has two stable isotopes: 1H (major part) and 2H (deuterium; often denoted D), which constitutes only 0.015% of all hydrogen atoms. Carbon (Z = 6) has two stable isotopes, 12C (ca 98.9%) and 13C (ca 1.1%). The ratio 13C/12C, here denoted R13, varies within a small range in an organism mainly due to consumed food (“you are what you eat”), referring to the stable isotope signature of the body [24]. The value of the sample (s) is usually given relative to a standard (std) by the expression δ13C = [R13s/R13std − 1] × 1000. This gives a number (in ‰), easier to handle, which is either positive or negative relative to a standard. The international standard was for many years PDB, a belemnite from the Cretaceous Pee-Dee formation in South Carolina. It is now exhausted, and therefore a V-prefix is used (e.g. V-PDB), following the nomenclature suggested at a conference held in Vienna in 1993 [25].

Nitrogen (Z = 7) exists in nature with two stable isotopes, 14N (ca 99.64%) and 15N (0.36%). The 15N/14N isotopic ratio is usually given as δ15N (in ‰) relative to a standard, commonly nitrogen in the air. Oxygen (Z = 8) exists with three stable isotopes: 16O (99.76%), 17O (0.04%) and 18O (0.20%). Usually the 18O/16O ratio is determined, and its value is conventionally given as δ18O relative to an international standard (V-SMOW or V-PDB). Sulfur (Z = 16) exists in nature with four stable isotopes with mass numbers 32, 33, 34 and 36. Their relative abundances are around 95.0, 0.76, 4.2 and 0.015%, respectively. Usually the 34S/32S ratio is determined which is expressed as a δ34S value versus the Canyon Diablo troilite (CDT), an iron sulfide standard.

Common light elements—archaeology

Among the light elements, carbon has the largest impact of modern archaeological science. Organic carbon is isotopically “light” (i.e. with a comparatively large proportion of 12C) with strongly negative δ13C values, for pit coal as low as − 25‰ and for methane even lower. In archaeology, δ13C values can usually give information on a human’s diet [e.g. 26, 27]. δ13C changes with the trophic level; lowest for green plants (ca. − 27‰), less negative for terrestrial animals (ca. − 22‰), and highest for marine animals (ca. − 16‰). Even degraded lipids preserved in ancient pottery may be analyzed [28]. Nitrogen isotopes are useful in archaeology to establish a probable diet pattern. An organism can integrate nitrogen from nitrates, ammonium or (rarely) free nitrogen in the air. The δ15N value of green plants is around 2–4‰, while herbivorous animals have values around 6‰, i.e., a higher trophic level gives a higher value [29]. Marine organisms may have still higher values, and Inuit’s whose main food is marine protein can have δ15N values as high as 18‰ [30].

Oxygen is mainly integrated in humans through ingestion of water, the isotopes of which depend on altitude and latitude, and its isotopes may thus be used to verify a hypothetical geographic origin. In humans and animals, sulfur is found in collagen and keratin. These proteins are relatively resistant towards acids and can be retrieved even in prehistoric graves in regions now suffering from acidification [31]. Marine, freshwater and terrestrial ecosystems often display distinctly different sulfur isotope compositions, and accordingly sulfur isotope data in human and faunal tissues can infer the consumption pattern of foods [32–34]. The proportion of deuterium in bone collagen of humans and animals shows a trophic level effect, with increasing values from herbivores to omnivores to humans [35]. A pioneering study of remains of humans, animals and plants from archaeological sites by means of hydrogen isotopes has been published by Yang and Leng [36]. As hydrogen and oxygen are constituents in water, a combined O–H isotope systematics may be useful to trace the origin of water found in e.g. plants and living organisms. Studies involving hydrogen isotopes in hair have been published [37–39].

By combining different isotope systems of light elements, such as carbon, nitrogen, oxygen, sulfur and hydrogen, a detailed understanding can often be reached regarding the origin and diets of e.g. archeological human remains. In particular, sulfur and hydrogen isotope data can be a valuable complement to other stable isotope (C and N) data obtained on human bone. Many studies involving human diets, nutritional ecology, extraction methods and also sheep’s wool have been published [40–46], and also a study combining stable isotopes and ancient DNA analyses [47]. Extensive review concerning mammalian proteins has been published by Wilkinson [42]. An interesting multi-isotope study of the remains of King Richard III has been published by Lamb et al. [48]. For instance, there was a significant shift noted in the nitrogen, but not carbon, isotope values towards the end of his life, which may be explained by an increase of luxury food and drink such as game birds, freshwater fish and wine. This is the first suggestion of wine affecting the isotope composition of an individual and thus has wider implications for isotope-based palaeodietary and migration reconstructions.

Common light elements—other applications

The study of light stable elements is also used in many other fields of heritage science. Some of these applications have a geological background. For instance, geologists measure carbon isotopes while prospecting for fossil fuel and to interpret the origin of carbonates. Marble is of great interest in heritage science. It is a metamorphic product of limestone (a carbonate rock), whose dominant mode of formation is from various organisms living in water. Accordingly, its carbon and oxygen isotope compositions have been used to determine the provenance of marble in buildings and monuments in the Mediterranean area. An early study was published in 1972 by Craig & Craig and was later followed by others [49–53].

Oxygen isotopes may also be utilized in studying the origin of e.g. groundwater. For instance, δ18O for meteorological precipitations shows seasonal variations—those deposited during the summer are less negative than the winter values [54, 55]. Accordingly, δ18O data can be used for paleo-thermometry [56]. An interesting study has been made by Dansgaard et al. [57]. Cores drilled from Greenland ice were cut into small fractions, which were analyzed for δ18O. In this way, “age rings” similar to tree rings were obtained. The cores could thus be dated, and the age could often be verified from deposits of ashes emitted from known volcanic eruptions. Inversely, earlier unknown eruptions could be identified. Similar applications may as well be used in heritage science where e.g. ash layers are present at excavation sites. Oxygen may also be extracted from silicates, which define the predominant mineral group in nature, by means of a powerful chemical reagent such as bromine pentafluoride [58], and such isotopic compositions can be used to relate an archaeological object to a specific environment, for instance in gemmological applications [59] and potentially to determine the provenience of silica-rich artefacts (e.g. obsidian tools) to a specific rock quarry. Sulfur isotopes have been used in environmental studies of damaged outdoor cultural monuments and buildings [60–65]. In many cases the origin of sulfur in the gaseous oxides was due to the impact of fossil fuels.

Provenancing objects using heavy isotopes (Pb, Sr, Nd)

Numerous examples demonstrate that Pb and Sr (and also e.g. Nd) isotopes may be used to set constraints on the source or provenance of cultural objects. Such applications are based on the long-lived decay series exemplified above for age dating. The difference is that instead of measuring a ratio between parent and daughter isotopes, appropriate isotope ratios including only the daughter element are used for the provenance. For strontium and neodymium, the radioactive decays of interest are 87Rb to 87Sr and 147Sm to 143Nd, and the relevant isotope ratios used are 87*Sr/86Sr and 143*Nd/144Nd (the asterixis denotes an isotope formed from radiogenic decay). These elements, along with lead, are advantageous because their isotopic variations are comparatively large and easily measured, and their isotope systems are well characterized.

Lead is typically a trace element in bronze, coins and many other metal objects, and a major constituent of crystal glass and lead pigments. This enables lead isotopes to be used to determine the provenance of these objects. Lead exists with four stable isotopes having mass numbers 204, 206, 207 and 208. The three latter isotopes are successively added as a result of decay of U and Th isotopes, and their relative isotopic abundance is often given by the ratios 206Pb/204Pb, 207Pb/204Pb and 208Pb/204Pb, using 204Pb as a reference isotope [54, 55]. Since these decays are extremely slow, the geological age of a mineral deposit is an important factor for its lead isotopic composition. For Pb-rich ores no significant in situ decay of U and Th takes place after their formation, thus implying that their Pb isotope ratios carry a “fossil record” which represents their time of formation. The isotopic variations in the lithosphere may therefore be considerable, which is favorable when attempting to use Pb isotopes to reveal the provenance of the lead in an object. For example, during the Middle Ages several lead-bearing ore deposits were mined in south Sweden in the so called Bergslagen area west and north-west of Lake Mälaren. This region is geologically very old, around 1900-1800 Ma (million years), which gives quite different lead isotope distributions (206Pb/204Pb values cluster around 15.70) as compared with ores from the European continent exhibiting much younger Palaeozoic to Mesozoic (545-65 Ma) terrains, where 206Pb/204Pb ore values usually are in the range 17.5–19.0.

When using lead isotopes to provenance an object, it is often customary to display data in 206Pb/204Pb versus 207Pb/206Pb or 208Pb/206Pb diagrams, respectively. Numerous reference data from ancient mining districts are reported in this way, and the isotopic compositions of discrete ores or regions may provide characteristic “fingerprints”. A disagreement between data for sample and ore deposit, respectively, definitely shows that the analyzed lead cannot originate from the deposit in question. An agreement (“isotopic match”) indicates that the lead may originate from that specific deposit. It must also be remembered that an overlap of isotopic fingerprints may exist between different ore districts, and that lead isotope data are not available for all conceivable mines. However, lead isotope abundances in combination with other observations such as trace elements can often help pin-pointing a possible origin of the lead. Efforts to compile an extensive database for lead isotopes have been made by a group in Oxford (the OXALID database) [66], and currently work is in progress for further published data [67]. Strontium, neodymium and oxygen isotopes have been used to provenance ancient glass, for instance in the Mediterranean area [68–74]. Chinese glazes have been examined with strontium isotopes [75]. The results on some of these studies also have relevance for manufacturing techniques.

Lead pigments have also been analyzed for their isotopic composition. In this way ancient Chinese and central Asian pigments have been examined [76]. Fortunato et al. [77] have determined lead isotope abundance ratios in lead white, a common constituent in seventeenth century oil paintings. Works of art by Rubens, van Dyck and other Flemish masters gave very similar lead isotope distributions, which indicates a distinct origin of raw materials. Also Fleming [78] has described how lead pigments in oil paintings by old masters may be used to settle doubts on genuineness. With respect to Swedish material, studies of mediaeval lead pigments from mural paintings, church portals and baptismal stone fonts have been performed with the aim to determine their origin [79–81]. Most lead pigments were found to originate from the Harz and Erzgebirge regions in Germany, but also lead pigments from Russia and Sweden (the Bergslagen ore district) were identified.

A large number of archaeological bronze artefacts excavated in Scandinavia have also been analyzed [82, 83]. In these studies, it was definitely shown that the lead in the bronzes did not originate from Swedish ores, but rather from ore regions mainly in Austria, Spain and Sardinia. Ancient silver coins have been studied elsewhere, as well as ancient bronze artefacts, and their origin and authenticity examined with the aid of lead isotopes [78, 84–87]. The ancient plumbing system in Pompeii has been examined for lead isotopes, indicating multiple sources for the lead [88]. The ship Batavia, belonging to the Dutch East India Company, was shipwrecked outside Australia in 1628. Some of their copper objects have been analyzed for lead isotopes [89], showing that the metal originated from various sources, among them the Swedish Bergslagen region with its very distinct isotopic signature. A final example concerns the murder of the Swedish warrior king Karl XII in 1718. He was shot in Norway with a bullet containing lead to make it heavier. The lead isotope study gave no clear evidence for the lead provenance—however, it was certainly not lead from the Swedish Bergslagen region [90].

As regards strontium, the 87Sr/86Sr ratio differs for various geological environments, and the local variations can be appreciable. Since strontium is chemically related to calcium, it is partly integrated in teeth and bone in humans and animals. Dental enamel is mainly formed during the childhood and this part does not exchange its strontium subsequent after its formation, while other parts of the body are affected later in life. Strontium and other isotopes can therefore be used to study the migration of humans or animals during their life-time [91–94]. Famous examples are given by various isotopic analyses of the remains of “Ötzi the Ice-man” [95, 96]. There are also examples of multi-isotopic approach in Swedish archaeology, such as “The man from Granhammar”, who seems to have travelled a lot before he was finally murdered [97], and there are many further examples [e.g. 98, 99].

Provenancing with less common stable isotope systems

With the advent of new generations of ICP-MS and SIMS instruments, it is today possible to detect and measure natural isotope variations among numerous “non-traditional” elements such as boron, magnesium, silicon, chlorine, iron, nickel, copper, zinc, tin and many others. These have recently attracted a large interest in the scientific community [17, 100, 101]. However, several factors obstruct a general usage in heritage science. Apart from problems with infinitesimal fractionations induced in nature for the heavier elements, as well as uncertainties about the nature of processes leading to measurable fractionations, reference data are still relatively few, and the analytical challenges are large and their common usage in cultural sciences remains to be proven.

Be that as it may, the recent decade has witnessed a steadily increasing interest for isotope studies regarding the above-mentioned elements. Among these boron is the lightest element, with an atomic number Z = 5, which is advantageous since relatively large isotopic differences may be expected. Boron is a trace element present in natron glass, and a study of Roman glass has recently been published and proven boron to be a provenance indicator for glass [102]. In that paper it could be concluded that the Greco-Roman glasses showed a rather homogeneous isotopic composition, expressed as δ11B.

Magnesium (Z = 12) has three stable isotopes, and in a recent study Mg isotopes were measured in mammal tooth enamel [103]. It was found that δ26Mg increases from herbivores to higher-level consumers, discriminating most of the trophic steps. This, combined with values for Ba/Ca, δ13C and δ34Ca may prove useful in paleodietary studies. Also, silicon (Z = 14) isotopes have been studied, usually with a geological focus [104] but has also been used as a proxy for environmental change [105]. Calcium (Z = 20) is a main constituent of bone. Pilot studies have been undertaken by Reynard et al. [106], using bones from humans and animals from three archaeological sites. There was a significant difference in the 44Ca/42Ca isotope ratios between humans and animals, which was attributed to differences in metabolic processes rather than due to dairy consumption among the adult humans. It was also concluded that the bone calcium isotope ratios were not substantially affected by diagenetic changes. Even a preliminary study of selenium (Z = 34) isotopes in organic Se-bearing species has been published [107].

Some isotope studies of metallic elements will be considered. Isotopes of copper and iron (having two respectively four stable isotopes) have been measured in artefacts [108–114]. A great challenge is that both metals are ubiquitous in the lithosphere, so the task to provenance from their isotopic abundance may be anywhere from difficult to hopeless. A more promising candidate within the isotope field may be zinc with its five stable isotopes. Copper and zinc isotope ratios in human bone and enamel have been examined by Jaouen et al. [115, 116]. Tin, with ten stable isotopes, is interesting being a constituent in many bronze artefacts, but the analysis is indeed complicated. Nevertheless, some interesting studies have been published by Pernicka et al. [e.g. 117–119] and Balliana et al. and others [120, 121]. Mercury (with seven stable isotopes) is also likely to be difficult to use for isotope measurements because of minor fractionation in nature, but it may have a potential as a tracer of organic matter [17]. Analyses of cinnabar pigments (HgS) have actually been undertaken [122], but in this study the provenance was based on the pigments’ sulfur isotopes, and fortunately the number of cinnabar sources in Europe is limited. However, this necessitates that the pigment certainly is the mineral minimum, and not a synthetic product (called vermilion) made from mercury and sulfur. In the latter case the sulfur may originate from anywhere in Europe. With the aim to trace the provenance of coinage through variations in isotopic abundances, silver, copper, and lead isotopes were measured in 91 coins from the East Mediterranean Antiquity and Roman world, medieval western Europe, sixteenth to eighteenth century Spain, Mexico, and the Andes [123]. The isotope measurements demonstrate that also silver isotopes has a large potential for provenance studies. Pre-1492 European silver can be distinguished from Mexican and Andean metal. European silver dominated Spanish coinage until Philip III, but had, 80 years later after the reign of Philip V, been flushed from the monetary mass and replaced by Mexican silver.

Radioactive isotopes used for age dating

Radiocarbon dating

There are separate classes of radioactive decay systems on which different isotopic dating methods are based; cosmogenic nuclides (e.g. C-14, tritium and Cl-36), the uranium/thorium-series disequilibria systems (e.g. the 230Th-232Th and 210Pb methods), long-lived systems (e.g. the U–Pb, K–Ar and Ar–Ar methods), and radiation damage methods (e.g. thermoluminescence and fission track methods). The systematics behind these techniques are very different and, with the exception of the carbon-14 method, the reader is referred to text books for more detailed information. The most frequently used archaeological dating technique is the well-known C-14 “radiocarbon” method [4, 6, 18, 124–127]. Successful applications include dating of e.g. human and animal remains, mummies, wood artefacts, parchment, textiles, cereals, charcoal, peat and slag. The method is based on the fact that cosmic neutrons react with atmospheric 14N to form radioactive 14C, which decays by β-emission with a half-life (T1/2) of 5730 ± 40 years. (After a half-life, 50% of the radioactive isotopes have decayed). Almost all living matter is constantly exchanging 14C with their environment, mainly by food or atmospheric CO2. This exchange expires when the organism dies, and the 14C decay can consequently be used as an “archaeological chronometer”. The age is determined by measuring the proportion of 14C in relation to 12C and comparing this with corresponding theoretical value for “modern” carbon.

Initially, the organic material to be dated was burned to CO2 in oxygen, whereupon its radioactivity was determined in a relatively tedious process where the 14C activity was estimated from the measurements of β-particles emitted during decay of 14C to 14N. The procedure also involved a conventional gas mass spectrometer to obtain the 13C/12C ratio needed for corrections (cf. below). Accordingly, radiocarbon ages determined some decades ago may suffer from low accuracy. Today the number of 14C atoms in relation to the stable carbon isotopes can be directly measured with an Accelerator Mass Spectrometer (AMS) in samples with as little as 100 μg of carbon, and yet producing precise ages of around ± 40 years for samples being a few 1000 years old. However, there are several sources of error to be considered. For instance, it is imperative to avoid contamination from modern material, which would otherwise give a much too low (“young”) age. Likewise, an organism having absorbed carbon dioxide from fossil fuel would cause a much too high age. If trees growing near a high-way would be radiocarbon dated, their “age” would erroneously amount to several million years. Furthermore, a number of corrections are necessary for a reliable result. The 14C/12C ratio in the atmosphere has shown small fluctuations with time and locality, and certain calibration curves should therefore be employed. Furthermore, the CO2 uptake in an organism is affected by isotopic fractionation. It is assumed that in relation to C-12, all organisms discriminate against C-14 about twice as much as against C-13, and this can be accounted for in a procedure involving the determination of the 13C/12C ratio. Therefore, many corrections are necessary to the raw radiocarbon age to yield a calendar date [124–128]. Another correction is necessary to compensate for the so-called Suess effect. This is a change in the ratio of the atmospheric concentrations of 13C and 14C by the admixture of fossil-fuel derived carbon dioxide, which is depleted in 13C and contains no 14C. The effect is named after the Austrian chemist Hans Suess, who noted the influence of this effect on the accuracy of radiocarbon dating [129, 130].

Numerous famous and successful C-14 age dating’s have been published during the last half-century on materials such as the Dead Sea scrolls, the Shroud of Turin, Egyptian mummies, and Ötzi the Iceman. It must also be remembered that the C-14 technique is only applicable for organic material. However, iron artefacts may be dated because they contain small amounts of the carbon (charcoal) once used for reduction of the iron oxide ore. Bone material can often be dated from its collagen, which is remarkably stable, even in soil suffering from atmospheric acidification [31]. A number of corrections are necessary for a reliable result (cf. below).

Dating with other isotope systems

Dating with the C-14 techniques has its limitations when older artefacts are to be dated. After ten half-lives (about 60,000 years) only one per mil of the original amount of 14C atoms remains, which is challenging for a high-quality analysis. In this case, radioactive isotopes with longer half-life’s can be considered. For instance, 36Cl with a half-life of 301,000 years may be utilized for very old materials in specific cases [131]. Tritium (3H), decaying to 3He with a half-life of about 12 years, is produced from cosmic-ray neutrons interacting with 14N. Tritium is a minor constituent of water molecules on the surface of the earth due to fall-out from meteoric precipitation. The tritium component in water can be used to determine the age of a water mass (e.g. groundwater). Tritium analyses, based on the measurement of emitted β-particles, combined with analyses of 3He (tritium—3He method) have been applied on problems in archeology [132]. However, because of atmospheric testing of nuclear weapons, the amount of tritium in the atmosphere rose and this may obstruct the interpretation of data. In this context also the 90Sr isotope may be mentioned which originates in a similar manner as tritium. Nuclear accidents like that in Chernobyl (1986) have influenced the concentration of 90Sr in the atmosphere.

The effect of so called uranium/thorium-series disequilibria give rise to a number of dating methods. Briefly, these disequilibria occur when biologic and inorganic reactions break the complex chains which define the decay of U and Th parent isotopes. This, in turn, leads to an interplay between various processes and for instance the application of the 238U/234U—230Th series methods enable events up to 500,000 years to be dated. Examples include dating of lake sediments, corals, dropstones and early human species, archeological sites [55; and references therein]. Obviously, this may be applied in studies of anthropology and ancient mining. In geology, where long time scales often are considered, rocks are dated by using decay series like A (parent isotope) → B (daughter isotope), where element A has a very long half-life. The common principle of these systems is that time can be determined by measuring the ratio between newly formed daughters and remaining parent isotopes. For instance, 238U decays to stable 206Pb with a half-life of ca. 4.5 billion years, but despite this slow decay it has been shown that the technique is capable of dating carbonate samples as young as 250,000 years [133, 134]. The age of fossil enamel has been successfully determined with U–Pb dating techniques [135]. Another useful decay series, with applications to archeological finds, is K–Ar (and a variant known as the Ar–Ar method which is based on the same decay of 40K to 40Ar). For instance, the fossil remains of “Lucy” from Awash Valley in Ethiopia could be dated to 3.2 million years by use of K–Ar and Ar–Ar dating of a surrounding layer of volcanic ashes [136]. Another well-known example utilizing the Ar–Ar isotope technique is the dating of the Vesuvius eruption (AD 79). Despite the slow decay of 40K to 40Ar (half-life 1250 million years), which therefore entails large analytical challenges to date young events, Renne et al. [137] were able to obtain an Ar–Ar age indistinguishable from the historical age of the eruption.

Finally, fission track dating and thermoluminescence are two dating methods which have been applied on glass objects and on dating ceramics [138, 139]. The former method relies on counting tracks caused by spontaneous fission of 238U atoms, whereas the latter is based on electromagnetic emission from non-conducting crystalline solids. Dating of fossil bones and teeth has been tested by means of fission tracks [140].

Limitations

This paper has exemplified how certain isotope systems can be used to reveal a human’s diet, migration patterns or age. However, there are often limitations which can make the results uncertain. A determined age may be if not erroneous so at least questionable. The problems with the C-14 dating technique has already been discussed. Following the first enthusiasm over this remarkable method, it has been shown that a number of corrections are necessary to get a reliable result, and that older dating’s might be questioned. It is of the greatest importance that no trace of “modern” carbon has polluted the sample used for the dating. Uncertainty how to validate other experimental isotope data is discussed below. An example worth considering is the dating of the Turin shroud, discussed by Meacham [141].

Many isotope studies are focused on archaeological examinations of human remains in order to ascertain information on diet or diseases. A body may have rested in the ground for centuries or thousands of years and may have been affected by the surrounding soil. In particular, diagenetic effects on bone and teeth have been studied. The problem is important because bone apatite yields dietary information about various life-stages. Most authors agree that diagenesis is a problem for these materials, and that the conditions at archaeological sites must be evaluated in each case [142–145]. Also a study of modern and ancient buried wood has been published, showing a linear correlation between carbohydrate content and the stable carbon isotope composition, because the carbohydrates are preferentially degraded during early diagenesis [146]. Usually an inorganic compound is more stable than organic and biological material, so the problem of diagenesis is likely to be smaller for metal artefacts, ceramics etc. However, also weathering may potentially alter the original isotopic composition of an object, and it may be essential to compare analytical results from both inner and outer parts of the artefacts. Furthermore, contamination from modern material that accidently got mixed with an object of some kind, and also conservation treatments, may jeopardize a judicial interpretation of the results obtained. Occasionally, it is of outermost importance to avoid the destruction of an object which may imply that a technique like SIMS (in situ technique affecting only a very tiny surficial area) is recommendable.

The provenance of an artefact can be determined or at least suggested from the isotope analysis of elements like lead, strontium and neodymium. Many other elements have also been used, like boron, copper, tin etc. The technical developments during the last decades allows extremely small sample volumes to be investigated which, however, make tough demands regarding the analytical protocols used at isotope laboratories. In particular, it is crucial to maintain very low levels of laboratory contamination and consider appropriate standardization procedures to master instrumental isotopic fractionation and use precautions not to alter the isotopic composition during pre-analysis sample treatment. For those heavy elements, for which isotopic differences among samples are notoriously small, optimized laboratory procedures are especially important. It may be difficult to convincingly prove, based on e.g. neodymium isotopes, that certain samples have a different provenance than others, due to the minor isotopic differences that are developed. Yet, it may still be possible to group samples by claiming that one set of samples has an isotopic signature that is distinct from that of another set. Lead isotope provenancing of objects is governed by relative large isotopic differences developed among potential source areas, but a complication is that there might be an isotopic overlap between geographical regions. There is a problem with isotopic overlap also for e.g. Cu and Zn and a further hinder for a successful provenancing when using these systems is that there are typically numerous potential regions sharing a specific type of metal deposit. At the best, some conceivable deposits can be dismissed.

Possible future applications

Isotope measurements are now routinely used in many fields such as geology, medicine, heritage science, archaeology, forensics, environmental studies and in the food and beverage industry. At present about ten elements, or isotope systems, are currently used on a routine basis for investigations in the field of heritage science (Table 1). The technical development of spectrometers has now reached a stage where so called compound-specific type of analysis is possible. Data from this approach is normally obtained by using a gas chromatograph (GC) which allows a controlled introduction of a certain molecular species into a MC-ICP-MS system and then e.g. analyzes the isotopic composition of carbon in organic species, or chlorine contained in e.g. pesticides. Another interesting technique utilizing specific isotopic properties is NMR, Nuclear Magnetic Resonance, today commonly used in medicine to study anomalies in human tissues. The method is based on the weak magnetic field of the nuclei of certain isotopes such as 1H and 13C, which in a strong magnetic field may cause resonance with low-frequency radio waves. The technique has also been used to investigate old human remains [147].

In the future, probably many more elements’ isotope systems may be used. Hypothetically, for instance elements such as potassium, titanium, chromium, manganese, nickel and the platinum metals group are of interest in the study of cultural objects, preferably as components in multi-isotope studies. Moreover, isotope studies may successfully be combined with analytical data for trace elements. Although not based on isotopes, the hydration method is also worth mentioning in this context. This method allows dating of obsidian, a dense volcanic rock often used for producing stone tools [148]. Dating of microfossils in flint artefacts with the aid of palynological techniques is also possible at many instances. Understanding isotope systematics has also proven useful when investigating the effect of human activities on the environment. Considering the constantly growing field of applications and the fact that each new generation of mass spectrometers induce a much better accuracy, the future use of isotopes in heritage science is certainly likely to grow with time.

Declarations

Authors’ contributions

AN and KB have together written the manuscript. Both authors read and approved the final manuscript.

Authors’ information

Anders G. Nord (born in 1942). At the University of Stockholm he acquired a sound knowledge of chemistry, physics, mathematics, and mineralogy. He graduated in chemistry (1974) and was later associate professor. During employment at the Swedish Museum of Natural History, a system for analysis of light stable elements was built in cooperation with Kjell Billström. Other fields were carbon-14 dating and lead isotope analyses. For 20 years he was finally employed at the National Heritage Board of Sweden as a conservation scientist, with focus on the degradation of archaeological artefacts and museum objects, as well as analysis of medieval murals. Helping colleagues regarding isotope data for provenance and other interpretations was another important task. Anders Nord is still active as a research scientist and has so far published about 200 scientific papers and contributed to eight books.

Kjell Billström (born in 1954) studied geology at the University of Stockholm, where he graduated. Since 1978 he has been employed at the Department of Geosciences at the Swedish Museum of Natural History. He first worked with light stable isotopes, but has later concentrated on ore formation, development of the earth crust, and geological dating using heavy radioactive elements. He has also a wide experience in problems where lead isotopes have been of certain importance, and of testing and running various models of mass spectrometers.

Acknowledgements

The authors will express their sincere gratitude to the staff at the Swedish Museum of Natural History for many valuable discussions and useful improvements of the manuscript. We are also grateful to Inga Ullén (Swedish Museum of National Antiquities), Kerstin Lidén (Archaeological Research Laboratory, University of Stockholm), and Adrian Boyce (SUERC, Glasgow) for useful examples concerning isotope studies in archaeology. Finally we want to thank the Torsten Söderberg Foundation, which has provided economic support for many of our earlier investigations where isotope data have been of crucial importance.

Competing interests

The authors declare that they have no competing interests.

Availability of data and materials

Available upon request.

Consent for publication

Not applicable.

Ethics approval and consent to participate

Not applicable.

Funding

There is no funding for this summarizing paper.

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Authors’ Affiliations

(1)
National Heritage Board of Sweden, Kevingeringen 10, 182 50 Danderyd, Sweden
(2)
Dept. of Geosciences, Swedish Museum of Natural History, P.O. Box 50007, 104 50 Stockholm, Sweden

References

  1. Faure G. Principles of isotope geology. New York: J. Wiley & Sons; 1977.Google Scholar
  2. Campbell J. Rutherford—a brief biography. Canterbury; 2001.Google Scholar
  3. Boltwood B. The ultimate disintegration product of the radio-active elements. Am J Sci. 1907;24:77–88.Google Scholar
  4. Arnold JR, Libby WF. Age determinations by radiocarbon content: checks with samples of known age. Science. 1949;110:678–80.View ArticleGoogle Scholar
  5. Meschel SV. Chemistry and archaeology: a creative bond. Chicago: University of Chicago, Dept. of Chemistry; 1979.Google Scholar
  6. Wintle AG. Archaeologically-relevant dating techniques for the next century: small, hot and identified by acronyms. J Archaeol Sci. 1996;23:123–38.View ArticleGoogle Scholar
  7. Pollard AM, Batt CM, Stern B, Young SMM. Analytical chemistry in archaeology. Cambridge: Cambridge University Press; 2007.View ArticleGoogle Scholar
  8. Artioli G, editor. Scientific methods and cultural heritage. Oxford: Oxford University Press; 2010.Google Scholar
  9. Hoefs J. Stable isotope geochemistry. 6th ed. Berlin: Springer; 2008.Google Scholar
  10. Park R, Epstein S. Carbon isotope fractionation during photosynthesis. Geochim Cosmochim Acta. 1960;21:110–26.View ArticleGoogle Scholar
  11. Farquhar GD, Ehlinger JR, Hubick KT. Carbon isotope discrimination and photosynthesis. Annu Rev Plant Physiol. 1989;40:503–37.View ArticleGoogle Scholar
  12. Macko SA, Fogel ML. Isotopic fractionation of nitrogen and carbon in the synthesis of amino acids by microorganisms. Chem Geol Isot Geosci Sect. 1987;65:79–92.View ArticleGoogle Scholar
  13. Chambers LA, Trudinger PA, Smith JW, Burns MS. Fractionation of sulfur isotopes by continuous cultures of Desulfovibrio desulfuricans. Can J Microbiol. 1975;21:1602–7.View ArticleGoogle Scholar
  14. DeNiro MJ, Epstein S. Mechanisms of carbon isotope fractionation associated with lipid synthesis. Science. 1977;197:261–3.View ArticleGoogle Scholar
  15. O’Leary MH. Carbon isotope fractionation in plants. Phytochemistry. 1981;20:553–67.View ArticleGoogle Scholar
  16. Hoch AR, Lever DA, Shaw G. A review of literature in support of experimental and modelling of Carbon-14 behaviour in the biosphere. Nottingham: University of Nottingham Publ. AMEC/Nott/004041/001.Google Scholar
  17. Teng FZ, Watkins JM, Dauphas N, editors. Non-traditional stable isotopes. Reviews in mineralogy and geochemistry, vol. 82; 2017.Google Scholar
  18. McDougall D. Nature’s clock—how scientists measure the age of almost everything Radiocarbon Dating. Oakland: University of California Press; 2008.Google Scholar
  19. De Laeter J, Kurz MD. Alfred Nier and the sector field mass spectrometer. J Mass Spectrom. 2006;41:847–54.View ArticleGoogle Scholar
  20. Brenna JT, Corso TN, Tobias HJ, Caimi RJ. High-precision continuous-flow isotope ratio mass spectrometry. Mass Spectr. Rev. 1997;16:227–58.View ArticleGoogle Scholar
  21. Meier-Augenstein W. Applied gas chromatography coupled to isotope ratio mass spectometry. J. Chromatogr. 1999;A842:351–71.View ArticleGoogle Scholar
  22. De Groot A, editor. Handbook of stable isotope analytical techniques, vol. 1. New York: Elsevier; 2004.Google Scholar
  23. Muccio Z, Jackson GP. Isotope ratio mass spectrometry. Analyst. 2009;134:213–22.View ArticleGoogle Scholar
  24. Tykot RH. Stable isotope and diet—you are what you eat. In: Proceedings international school of physics enrico fermi, CLIV. Amsterdam: IOS Press; 2004.Google Scholar
  25. Povince PP, Sanchez-Caboze JA. In: International conference on isotopes and environmental studies. VPDB conference Vienna 1993. Amsterdam: Elsevier.Google Scholar
  26. Tauber H. 13C evidence for dietary habits of prehistoric man in Denmark. Nature. 1981;292:332–3.View ArticleGoogle Scholar
  27. Lidén K, Nelson ED. Stable carbon isotopes as dietary indicator in the Baltic area. Fornvännen. 1994;89:13–21.Google Scholar
  28. Mottram HR, Dudd SN, Lawrence GJ, Stott AW, Evershed RP. New chromatographic, mass spectrometric and stable isotope approaches to the classification of degraded animal fats preserved in archaeological pottery. J Chromatogr A. 1999;833:209–21.View ArticleGoogle Scholar
  29. Hedges REM, Reynard LM. Nitrogen isotopes and the trophic level of humans in archaeology. J Archaeol Sci. 2007;34:1240–51.View ArticleGoogle Scholar
  30. Buchardt B, Bunch V, Helin P. Fingernails and diet: stable isotope signatures of a marine community from Uummannaq, North Greenland. Chem Geol. 2007;244:316–29.View ArticleGoogle Scholar
  31. Nielsen-Marsh CM, Smith CI, Jans M, Collins MJ, Nord AG, Kars H. Bone diagenesis in the European Holocene II: taphonomic and environmental considerations and the long-term preservation of archaeological bone. J Archaeol Sci. 2006;34:1523–31.View ArticleGoogle Scholar
  32. Richards MP, Fuller BT, Sponheimer M, Robinson T, Ayliffe L. Sulphur isotopes in palaeodietary studies—a review and results from a controlled feeding experiment. Int J Osteoarchaeol. 2003;13:37–45.View ArticleGoogle Scholar
  33. Nehlich O, Borić D, Stefanivić S, Richards MP. Sulphur isotope evidence for freshwater fish consumption: a case study from the Danube Gorges, SE Europe. J Archaeol Sci. 2010;37:1131–9.View ArticleGoogle Scholar
  34. Privat KL, O’Connell T, Hedges REM. The distinction between freshwater and terrestrial-based diets: methodological concerns and archaeological applications of sulphur stable isotope analysis. J Archaeol Sci. 2007;34:1197–204.View ArticleGoogle Scholar
  35. Reynard LM, Hedges REM. Stable hydrogen isotopes of bone collagen in palaeo-dietary and palaeo-environmental reconstruction. J Archaeol Sci. 2008;35:1934–42.View ArticleGoogle Scholar
  36. Yang H, Leng Q. Molecular hydrogen isotope analysis of living and fossil plants—metasequoia as an example. Prog Nat Sci. 2009;19:901–12.View ArticleGoogle Scholar
  37. Sharp ZD, Atudorei V, Panarello HO, Fernandez J, Douthitt C. Hydrogen isotope systematics of hair: archaeological and forensic applications. J Archaeol Sci. 2003;30:1709–16.View ArticleGoogle Scholar
  38. O’Grady SP, Valenzuela LO, Remien CH, Enright LE, Jorgensen MJ, Kaplan JR, Wagner JD, Cerling TE, Ehlinger JR. Hydrogen and oxygen ratios in body, water and hair—modelling isotope dynamics in nonhuman primates. Am J Primatol. 2012;74:651–60.View ArticleGoogle Scholar
  39. Bol R, Pflieger C. Stable isotope (C, N and S) analysis of hair in modern humans and their domestic animals. Rapid Comm. Mass Spectrometry. 2002;16:2195–200.View ArticleGoogle Scholar
  40. Hobson KA. Tracing origin and migration of wildlife using stable isotopes: a review. Oecologia. 1999;20:314–26.View ArticleGoogle Scholar
  41. Schwartz HP, Schoeninger HP. Stable isotope analyses in human nutritional ecology. Am J Phys Anthropol. 1991;34:283–321.View ArticleGoogle Scholar
  42. Wilkinson DJ. Historical and contemporary stable isotope tracer approaches to studying mammalian protein metabolism. Mass Spectrom Rev. 2018;37:57–80.View ArticleGoogle Scholar
  43. White CD, Schwarcz HP. Ancient Maya diet as inferred from isotopic and elemental analysis of human bone. J Archaeol Sci. 1989;16:451–74.View ArticleGoogle Scholar
  44. Sealy J, Johnson H, Richards M, Nehlich O. Comparison of two methods of extracting collagen for stable carbon and nitrogen isotope analysis: comparing whole bone demineralization with gelatinization and ultrafiltration. J Archaeol Sci. 2014;47:64–9.View ArticleGoogle Scholar
  45. Iacumin P, Bocherens H, Chaix L, Marioth A. Stable carbon and nitrogen isotopes as dietary indicators of ancient Nubian populations (Northern Sudan). J Archaeol Sci. 1998;25:293–301.View ArticleGoogle Scholar
  46. von Holstein IC, Makarewicz CA. Geographical variability in northern European sheep wool isotopic composition (C, N, H values). Rapid Commun Mass Spectr. 2016;30:1423–34.View ArticleGoogle Scholar
  47. Naumann E, Krzewinska M, Götherström A, Eriksson G. Slaves as burial gifts in Viking Age Norway? Evidence from stable isotope and ancient DNA analysis. J Archaeol Sci. 2014;41:533–40.View ArticleGoogle Scholar
  48. Lamb AL, Evans JE, Buckley R, Appleby J. Multi-isotope analysis demonstrates significant lifestyle changes in King Richard III. J Archaeol Sci. 2014;50:559–65.View ArticleGoogle Scholar
  49. Craig H, Craig V. Greek marbles—determination of provenance by isotopic analysis. Science. 1972;76:401–3.View ArticleGoogle Scholar
  50. Pearl Z, Mogaritz M. Stable isotopes and the Roman marble trade—evidence from Scythopolis and Caesarea, Israel. In: Taylor HP, O’Neil JR, Kaplan IR, editors. Stable isotope geochemistry—geological society, Spec. Ed; 1991, No. 3.Google Scholar
  51. Herz N. Provenance determination of Neolithic to classical Mediterranean marbles by stable isotopes. Archaeometry. 1992;34:186–94.View ArticleGoogle Scholar
  52. Maniatis Y, Tambakopoulos D, Dotsika E, Stafanidou-Tiveriou Th. Marble provenance investigation of Roman sarcophagi from Thessaloniki. Archaeometry. 2009;52:45–58.View ArticleGoogle Scholar
  53. Tambakopoulos D, Maniatis Y. The marble of the Cyclades and its use in the Early Bronze Age. In: Marthari M, Renfrew C, Boyd MJ, editors. Early cycladic sculpture in context. Oxbow: Oxford and Philadelphia; 2017. p. 468–82.Google Scholar
  54. Faure G. Principles and applications of isotope geology. 2nd ed. Upper Saddle River: Prentice Hall; 1998.Google Scholar
  55. Faure G, Mensing TM. Isotopes: principles and applications. 3rd ed. Hoboken: John Wiley & Sons Inc; 2005.Google Scholar
  56. Donner J, Nord AG. Carbon and oxygen stable isotope composition of Mytilus Edulis and Modiolus Modiolus shells from Holocene-raised beaches at the outer coast of the Varanger peninsula, north Norway. J Palaeogeogr Palaeoclim Palaeoecol. 1986;56:35–50.View ArticleGoogle Scholar
  57. Dansgaard W, Johnson SJ, Möller J, Langway CC. One thousand centuries of climatic record from Camp Century on the Greenland ice sheet. Science. 1969;166:377–80.View ArticleGoogle Scholar
  58. Clayton RN, Mayeda TK. The use of bromine pentafluoride in the extraction of oxygen from oxides and silicates for isotopic analysis. Geochim Cosmochim Acta. 1963;27:43–52.View ArticleGoogle Scholar
  59. Cheilletz A, Branquet Y, Giar D, Martin-Izard A, Alexandrov P, Piat DH. Oxygen isotope systematics of emerald: relevance for its origin and geological significance. Miner Deposita. 1998;33:513–9.View ArticleGoogle Scholar
  60. Longinelli A, Bartelloni M. Atmospheric pollution in Venice, Italy, as indicated by isotopic analyse. Water Air Soil Pollut. 1978;10:335–41.View ArticleGoogle Scholar
  61. Krouse HR. Stable isotopes: Natural and anthropogenic sulfur in the environment. Scientific Committee on Problems of the Environment (SCOPE). Paris: United Nations Development Programme; 1983.Google Scholar
  62. Bužek F, Srámek J. Sulfur isotopes in the study of stone monument conservation. Stud Conserv. 1985;30:171–8.Google Scholar
  63. Pye K, Schiavon N. The effects of air pollution on the built environment. Nature. 1989;342:663–4.View ArticleGoogle Scholar
  64. Nord AG. Analysis of sandstone at the Royal Palace, Stockholm. Geologiska Föreningens i Stockholm Förhandlingar. 1995;117:43–8.Google Scholar
  65. Nord AG, Tronner K, Boyce A. Atmospheric bronze and copper corrosion as environmental indicator. A study based on chemical and sulphur isotope data. Water Air Soil Pollut. 2001;127:193–204.View ArticleGoogle Scholar
  66. Stos-Gale ZA, Gale NH. Metal provenancing using isotopes and the Oxford archaeological lead isotope database (OXALID). J Archaeol Anthropol Sci. 2009;1:195–213.View ArticleGoogle Scholar
  67. Blichert-Toft J, Delile H, Lee CT, Stos-Gale Z, Billström K, Andersen TH, Huhma H, Albarède F. Large-scale tectonic cycles in Europe revealed by distinct Pb isotope studies. AGU Publ Geochem Geophys Geosyst Res Article. 2016. https://doi.org/10.1002/2016GC006524.View ArticleGoogle Scholar
  68. Henderson J, Evans JA, Sloan HJ, Leng J, Doherty C. The use of oxygen, strontium and lead isotopes to provenance ancient glasses in the Middle East. J Archaeol Sci. 2005;32:665–73.View ArticleGoogle Scholar
  69. Henderson J, Evans J, Nikita K. Isotopic evidence for the primary production, provenance and trade of late bronze age glass in the Mediterranian. Mediterr Archaeol Archaeom. 2010;10:1–24.Google Scholar
  70. Freestone IC, Leslie KA, Thirlwall M, Gorin-Rosen M. Strontium isotopes in the investigation of early Islamic glass production: byzantine and Early Islamic glass from the near East. Archaeometry. 2003;45:19–32.View ArticleGoogle Scholar
  71. Degryse P, Schneider J. Pliny the Elder and Sr-Nd isotopes: tracing the provenance of raw materials for Roman glass production. J Archaeol Sci. 2008;35:1993–2000.View ArticleGoogle Scholar
  72. Gallo F, Silvestri A, Degrysa P, Ganio M, Longinelli A, Molin G. Roman and Late-Roman glass from north-eastern Italy: the isotopic perspective to provenance its raw materials. J Archaeol Sci. 2015;62:55–65.View ArticleGoogle Scholar
  73. Knaf ACS, Koornneef JM, Davies GR. Non-invasive portable laser ablation sampling of art and archaeological materials with subsequent Sr-Nd isotope analysis by TIMS using 1013 Ω amplifiers. J Anal At Spectrum. 2017;32:2210–6.View ArticleGoogle Scholar
  74. Brems D, Degryse P. Trace element analysis in provenancing Roman glass-making. Archaeometry. 2013;56:116–36.View ArticleGoogle Scholar
  75. Ma H, Henderson J, Evans J. The exploration of Sr isotopic analysis applied to Chinese glazes: part one. J Archaeol Sci. 2014;50:551–8.View ArticleGoogle Scholar
  76. Brill RH, Felker-Dennis CC, Shirahata H, Joel EC. Lead isotope analysis of some Chinese and central Asian pigments. Los Angeles: The Getty Conservation Institute; 1997. p. 369–78.Google Scholar
  77. Fortunato G, Ritter A, Fabian D. Old Masters’ lead white pigments: investigations of paintings from the 16th to 17th century using high precision lead isotope abundance ratios. Analyst. 2005;130:898–906.View ArticleGoogle Scholar
  78. Fleming JS. Authenticity in art—the scientific detection of forgery. London: Institute of Physics; 1975.Google Scholar
  79. Nord AG, Billström K, Tronner K, Björling Olausson K. Lead isotope data for provenancing mediaeval pigments in Swedish mural paintings. J Cult Herit. 2015;16:856–61.View ArticleGoogle Scholar
  80. Nord AG, Tronner K, Billström K, Strandberg Zerpe B. Analysis of mediaeval Swedish paintings influenced by Russian-Byzantine art. J Cult Herit. 2017;23:162–9.View ArticleGoogle Scholar
  81. Nord AG, Tronner K, Billström K, Gustafsson Belzacq M. Pigment traces on mediaeval stornework in Gotland’s churches—examination of seven 12th century baptismal fonts and a limestone pew. Fornvännen. 2016;111:17–26.Google Scholar
  82. Ling J, Hjärthner-Holdar E, Grandin L, Billström K, Persson PO. Moving metals or indigenous mining? Provenancing Scandinavian bronze age artefacts by lead isotopes and trace elements. J Archaeol Sci. 2013;40:291–304.View ArticleGoogle Scholar
  83. Ling J, Stos-Gale Z, Grandin L, Billström K, Hjärthner-Holdar E, Persson PO. Moving metals II: provenancing Scandinavian bronze Age artefacts by lead isotope and elemental analyses. J Archaeol Sci. 2014;41:106–32.View ArticleGoogle Scholar
  84. Rehren T, Pernicka E. Coins, artefacts and isotopes–archaeometallurgy and archaeometry. Archaeometry. 2008;50:232–48.View ArticleGoogle Scholar
  85. Niederschlag E, Perncika E, Seifert T, Bartelheim M. The determination of lead isotope ratios by multiple collector ICP-MS: a case study of Early Bronze age artefacts and their possible relation with ore deposits of Germany and Bohemia. Archaeometry. 2003;45:61–100.View ArticleGoogle Scholar
  86. Molofsky LJ, Killick D, Ducea MN, Macovei M, Chesley JT, Ruiz J, Thibodeau A, Popescu GC. A novel approach to lead isotope provenance studies of tin and bronze applications to South African and Romanian artifacts. J Archaeol Sci. 2014;50:440–50.View ArticleGoogle Scholar
  87. Pointing M, Evans JA, Pashley V. Fingerprinting of Roman mints, using laser ablation MC-ICP-MS lead isotope analysis. Archaeometry. 2003;45:591–7.View ArticleGoogle Scholar
  88. Boni M, Dima G, Frei R, Villa IM. Lead isotope evidence for a mixed provenance for Roman water pipes from Pompeii. Archaeometry. 2000;42:201–8.View ArticleGoogle Scholar
  89. van Duivenvoorde W. Batavia shipwreck: study of the Batavia ship’s hull remains. Dissertation, Western Australia Museum, Perth; 2008.Google Scholar
  90. Johansson Å. Isotopic analyses of the Karl XII brass bullet. The Varberg Museum Yearbook 1992. Varberg; 1992. (In Swedish with English summary).Google Scholar
  91. Schweissing MM, Grupe G. Local or non-local? A research of strontium isotope ratios of teeth and bones on skeletal remains. Anthroposophische Anzeigen. 2000;58:99–103.Google Scholar
  92. Hodell DA, Quinn RL, Brenner M, Kamenov G. Spatial variation of strontium isotopes in the Maya region: a tool for tracking ancient human migration. J Archaeol Sci. 2004;31:585–601.View ArticleGoogle Scholar
  93. Bentley RA. Strontium isotopes from the Earth to the archaeological skeleton—a review. J Archaeol Method Theory. 2006;13:135–87.View ArticleGoogle Scholar
  94. Åberg G, Fosse G, Stray H. Man, nutrition and mobility: a comparison of teeth and bone from the Medieval era and the present from Pb and Sr isotopes. Sci Total Environ. 1998;224:109–19.View ArticleGoogle Scholar
  95. Fowler B. Iceman—uncovering the life and times of a Prehistoric man found in an Alpine glacier. New York: Random House; 2000.Google Scholar
  96. Der Spindler K. Mann im Eis. München: Neue sensationelle Erkenntnisse über die Mumie der Ötztaler Alpen. Goldmann Verlag; 2000.Google Scholar
  97. Lindström J. The Bronze Age murder. Stockholm: Norstedt Publ; 2009 (in Swedish).Google Scholar
  98. Ericsson G, Papmehl-Dufay L, Lidén K. Cultural interaction and change: a multi-isotopic approach to the Neolithization in coastal areas. World Archaeol. 2013. https://doi.org/10.1080/00438243.2013.820651.View ArticleGoogle Scholar
  99. Fjellström M. Isotope analyses of the so-called Birka girl. Archaeological Research Laboratory, University of Stockholm, Report 208; 2012.Google Scholar
  100. Albarède E, Beard B. Analytical methods for non-traditional isotopes. Rev Miner Geochem. 2004;55:113–52.View ArticleGoogle Scholar
  101. Young ED, Manning CT, Schauble EA, Shahar A, Macris CA, Lazar C, Jordan M. High-temperature equilibrium isotope fractionation of non-traditional stable isotopes: experiments, theory, and applications. Chem Geol. 2015;395:176–95.View ArticleGoogle Scholar
  102. Devulder V, Vanhaecke F, Shortland A, Mattingly D, Jackson C, Degryse P. Boron isotope composition as a provenance indicator for the flux raw material in Roman natron glass. J Archaeol Sci. 2014;46:107–13.View ArticleGoogle Scholar
  103. Martin JE, Vance D, Balter V. Magnesium stable isotope ecology using mammal tooth enamel. In: Proceedings of the National Academy of Sciences of the USA. Ecology, Earth, Atmospheric, and Planetary Sciences. 2015; 112:430–435.Google Scholar
  104. Li YH, Wan DF, Jiang SY. Silicon isotope study on the Meishucum Precambrium-Cambrium boundary section, Yunnan. Geol Rev. 1995;41:179–87.Google Scholar
  105. Leng MJ, Swann GEA, Hodson MJ, Tyler JJ, Patwardhan SV, Sloane HJ. The potential use of silicon isotope composition of biogenic silica as a proxy for environmental change. Silicon. 2009;1:65–77.View ArticleGoogle Scholar
  106. Reynard LM, Henderson GM, Hedges REM. Calcium isotopes in archaeological bones and their relationship to dairy consumption. J Archaeol Sci. 2010;38:657–64.View ArticleGoogle Scholar
  107. Li XF, Lin Y. Equilibrium Se isotope fractionation parameters: a first-principle study. Earth Planet Sci. 2011;304:113–20.View ArticleGoogle Scholar
  108. Gale AP, Woodhead ZA, Walder A, Bowen I. Natural variations detected in the isotopic composition of copper—possible applications to archaeology and geochemistry. Int J Mass Spectrom. 1999;184:1–9.View ArticleGoogle Scholar
  109. Jaouen K, Balter V, Herrscher E, Lamboux A, Telouk P, Albarède F. Fe and Cu stable isotopes in archaeological human bones and their relationship to sex. Am J Anthropol. 2012;148:334–40.View ArticleGoogle Scholar
  110. Powell W, Mathur R, Bankoff HA, Mason A, Bulatovic A, Filipovic V, Godfrey L. Digging deeper: insights into metallurgical transitions in European prehistory through copper isotopes. J Archaeol Sci. 2017;88:37–46.View ArticleGoogle Scholar
  111. Powell W, Mathur R, Bankoff AH, John J, Chvojka O, Tisucká M, Bulatovic A, Filipovic V. Copper isotopes as a means of determining regional metallurgical practices in European prehistory: a reply to Jansen (2018). J Archaeol Sci. 2018;89:1–6.View ArticleGoogle Scholar
  112. Lazarov M, Weyer S, Pacevski A, Horn I. Cu isotope fractionation in primary and secondary copper minerals from the Coka Marin and Bor mining areas (east Serbia). Miner Mag. 2011;75:1279–85.Google Scholar
  113. Baron S. Iron isotopes as a potential tool for ancient iron metal tracing. J Archaeol Sci. 2016;76:9–20.View ArticleGoogle Scholar
  114. Pernicka E, Begemann F, Schmidt-Strecker S, Günther AW. Eneolithic and Early Bronze age copper artefacts from the Balkans and their relation to Serbian copper ores. Praehistorische Zeitschrift. 1993;68:1–54.View ArticleGoogle Scholar
  115. Jaouen K, Herrscher E, Balter V. Copper and zinc isotope ratios in human bone and enamel. Am J Phys Anthropol. 2017;162:491–500.View ArticleGoogle Scholar
  116. Jaouen K, Szpak P, Richards MP. Zinc Isotope Ratios as Indicators of Diet and Trophic Level in Arctic Marine Mammals. PLOS 2016, Paper 11(3), PMC 4806842.Google Scholar
  117. Haustein M, Gillis C, Pernicka E. Tin isotopy—a new method for solving old questions. Archaeometry. 2010;52:816–32.View ArticleGoogle Scholar
  118. Brügmann G, Berger D, Pernicka E. Determination of the tin stable isotopic composition in tin-bearing metals and minerals by MC-ICP-MS. Geostand Geoanal Res. 2017;41:437–48.View ArticleGoogle Scholar
  119. Nickel D, Haustein H, Lampke T, Pernicka E. Identification of forgeries by measuring tin isotopes in corroded bronze. Archaeometry. 2012;54:167–74.View ArticleGoogle Scholar
  120. Balliana E, Aramendia M, Resano M, Barbante C, Vanhaecke F. Copper and tin isotope analysis of ancient bronzes for archaeological investigation: development and validation of a suitable analytical methodlogy. Anal Bioanal Chem. 2013;405:2973–86.View ArticleGoogle Scholar
  121. Mason AH, Powell W, Bankoff A, Ruiz J. The isotope characterization of bronze artifacts in central Balkans. J Archaeol Sci. 2016;69:110–7.View ArticleGoogle Scholar
  122. Spangenberg JE, Lavrič JV, Meisser N, Serneels V. Sulfur isotope analysis of cinnabar from Roman wall paintings by IRMS—tracking the origin of archaeological red pigments and their authenticity. Rapid Comm Mass Spectr. 2010;24:2812–6.View ArticleGoogle Scholar
  123. Desaulty AM, Telouk P, Albalat E, Albarède F. Isotopic Ag-Cu-Pb record of silver circulating through 16th to 18th century Spain. In: Proceedings of the national academie of sciences of the USA. 2011; 108:9002–9007.Google Scholar
  124. Münich KO, Östlund KG, de Vries K. Carbon-14 activity during the past 5000 years. Nature. 1958;182:1432–5.View ArticleGoogle Scholar
  125. Olson EA, Broecker WS. Lamont radiocarbon measurements VIII. Radiocarbon. 1961;3:141–8.View ArticleGoogle Scholar
  126. Olsson IU. Radiocarbon dating history: early days, questions, and problems. Radiocarbon. 2009;51:1–43.View ArticleGoogle Scholar
  127. Taylor RE. Radiocarbon dating—an archaeological perspective. 2nd ed. London: Taylor & Francis; 2014.Google Scholar
  128. Clark FM, Renfrew C. Tree-ring calibration of radiocarbon data and the chronology of ancient Egypt. Nature. 1973;249:266–70.View ArticleGoogle Scholar
  129. Keeling CD. The Suess effect: 13Carbon/14Carbon interrelations. Environ Int. 1979;2:229–300.View ArticleGoogle Scholar
  130. Tans PP, de Jong AFM, Mook WG. Natural 14C variation and the Suess effect. Nature. 1979;280:826–8.View ArticleGoogle Scholar
  131. Alfimov V. Accelerator mass spectrometry of 36Cl and 129I. Dissertation. Uppsala: University of Uppsala; 2005.Google Scholar
  132. Melcher L, Zimmerman DW. Tritium-helium dating in the Sargasso Sea. J Archaeol Sci. 1996;23:123–38.View ArticleGoogle Scholar
  133. Rasbury ET, Cole JM. Directly dating geologic events: U-Pb dating of carbonates. Rev Geophys. 2009;47:3.View ArticleGoogle Scholar
  134. Parrish R, Rasbury T. Direct in situ dating of carbonates by LA-ICM-(MC)-MS and its applications to chronostratigraphy. Search and Discovery 2014, Article #41269.Google Scholar
  135. Balter V, Blichert-Toft J, Braga J, Telouk P, Thackerey F, Albarède F. U-Pb dating of fossil enamel from the Swartkrans Pleistocene hominid site, South Africa. Earth Planet Sci Lett. 2008;267:236–46.View ArticleGoogle Scholar
  136. Walter RC. Age of Lucy and the First Family: single-crystal 40Ar/39Ar dating of the Denen Dora and lower Kada Hadar members of the Hadar formation, Ethiopia. Geology. 1994;22:6–10.View ArticleGoogle Scholar
  137. Renne PR, Sharp WD, Deino AL, Orsi G, Civeta L. 40Ar/39Ar dating into the historical realm: calibration against pliny the younger. Science. 1997;277:1279–80.View ArticleGoogle Scholar
  138. Fleische RL, Price PB, Walker RM. Nuclear tracks in solids. Oakland: University of California, Berkely Press; 1975.Google Scholar
  139. Naeser CW. Fission-track dating and geologic annealing of fission tracks. In: Jäger E, Hunziker JC, editors. Lectures in isotope geology. Berlin: Springer; 1979. p. 154.View ArticleGoogle Scholar
  140. Jolivet M, Lebatard AE, Reyss JL, Brunet M. Can fossil bones and teeth be dated using fission track analysis? Chem Geol. 2008;247:81–99.View ArticleGoogle Scholar
  141. Meacham W. Radiocarbon measurement and age of the Turin Shroud: possibilities and uncertainties. In: Proceedings of the symposium “Turin shroud—image of Christ?”. Hongkong, March 1986.Google Scholar
  142. Nelson BK, DeNiro MJ, Schoeninger MJ, DePaolo DJ, Hare PE. Effects if diagenesis on strintium, carbon, nitrogen and oxygen concentration and isotopic composition of bone. Geochim Cosmochim Acta. 1986;50:1941–9.View ArticleGoogle Scholar
  143. Kohn MJ, Schoeninger MJ, Barker WW. Altered states: effects of diagenesis on fossil tooth chemistry. Geochim Cosmochim Acta. 1999;63:2737–47.View ArticleGoogle Scholar
  144. Lee-Thorpe J, Sponheimer M. Three case studies used to reassess the reliability of fossil bone and enamel isotope signals for paleodietary studies. J Anthropol Archaeol. 2003;22:208–16.View ArticleGoogle Scholar
  145. Snoek C, Lee-Thorpe J, Schulting R, de Jong J, Debouge W, Mattielli N. Calcined bone provides a reliable substrate for strontium isotope ratios shown by an enrichment experiment. Rapid Commun Mass Spectr. 2015;29:107–14.View ArticleGoogle Scholar
  146. Spiker EC, Hatcher PG. The effects of early diagenesis on the chemical and stable carbon isotope composition of wood. Geochim Cosmochim Acta. 1987;51:1385–91.View ArticleGoogle Scholar
  147. Ghisalberti EL, Godfrey IM. Application of Nuclear Magnetic Resonance spectroscopy to the analysis of organic archaeological materials. Stud Conserv. 1998;43:215–30.Google Scholar
  148. Friedman I, Trembour FW, Hughes RE. Obsidian hydration dating. In: Taylor RE, Aitken MJ, editors. Chronometric dating in archaeology. New York: Plenum Press; 1997. p. 297–322.View ArticleGoogle Scholar

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