Environmental and Low-Temperature Geochemistry

Peter Ryan

• Éditeur: Wiley-Blackwell
• Année: 2019
• ISBN:
  9781119568612
• Édition: 2
• Sujet: Sciences physiques
• Sous-sujet: Minéralogie

Environmental and Low-Temperature Geochemistry presents conceptual and quantitative principles of geochemistry in order to foster understanding of natural processes at and near the earth's surface, as well as anthropogenic impacts and remediation strategies. It provides the reader with principles that allow prediction of concentration, speciation, mobility and reactivity of elements and compounds in soils, waters, sediments and air, drawing attention to both thermodynamic and kinetic controls. The scope includes atmosphere, terrestrial waters, marine waters, soils, sediments and rocks in the shallow crust; the temporal scale is present to Precambrian, and the spatial scale is nanometers to local, regional and global.

This second edition of Environmental and Low-Temperature Geochemistry provides the most up-to-date status of the carbon cycle and global warming, including carbon sources, sinks, fluxes and consequences, as well as emerging evidence for (and effects of) ocean acidification. Understanding environmental problems like this requires knowledge based in fundamental principles of equilibrium, kinetics, basic laws of chemistry and physics, empirical evidence, examples from the geological record, and identification of system fluxes and reservoirs that allow us to conceptualize and understand. This edition aims to do that with clear explanations of fundamental principles of geochemistry as well as information and approaches that provide the student or researcher with knowledge to address pressing questions in environmental and geological sciences.

New content in this edition includes:

• Focus Boxes – one every two or three pages – providing case study examples (e.g. methyl isocyanate in Bhopal, origins and health effects of asbestiform minerals), concise explanations of fundamental concepts (e.g. balancing chemical equations, isotopic fractionation, using the K eq to predict reactivity), and useful information (e.g. units of concentration, titrating to determine alkalinity, measuring redox potential of natural waters);
• Sections on emerging contaminants for which knowledge is rapidly increasing (e.g. perfluorinated compounds, pharmaceuticals and other domestic and industrial chemicals);
• Greater attention to interrelationships of inorganic, organic and biotic phases and processes;
• Descriptions, theoretical frameworks and examples of emerging methodologies in geochemistry research, e.g. clumped C-O isotopes to assess seawater temperature over geological time, metal stable isotopes to assess source and transport processes, X-ray absorption spectroscopy to study oxidation state and valence configuration of atoms and molecules;
• Additional end-of-chapter problems, including more quantitatively based questions.
• Two detailed case studies that examine fate and transport of organic contaminants (VOCs, PFCs), with data and interpretations presented separately. These examples consider the chemical and mineralogical composition of rocks, soils and waters in the affected system; microbial influence on the decomposition of organic compounds; the effect of reduction-oxidation on transport of Fe, As and Mn; stable isotopes and synthetic compounds as tracers of flow; geological factors that influence flow; and implications for remediation.

The interdisciplinary approach and range of topics – including environmental contamination of air, water and soil as well as the processes that affect both natural and anthropogenic systems – make it well-suited for environmental geochemistry courses at universities as well as liberal arts colleges.

1
Background and Basic Chemical Principles: Elements, Ions, Bonding, Reactions

1.1 An Overview Of Environmental Geochemistry – History, Scope, Questions, Approaches, Challenges for the Future

The best way to have a good idea is to have a lot of ideas. (Linus Pauling)

All my life through, the new sights of nature made me rejoice like a child. (Marie Curie)

I must speak of the soil hiding the rocks, of the lasting river destroyed by time. (Pablo Neruda)

Environmental and low‐temperature geochemistry encompasses research at the intersection of geology, environmental studies, chemistry, and biology, and at its most basic level is designed to answer questions about the behavior of natural and anthropogenic substances at or near the surface of earth. The scope includes topics as diverse as trace metal pollution, soil formation, acid rain, sequestration of atmospheric carbon, and pathways of human–plant–wildlife exposure to contaminants. Most problems in environmental geochemistry require understanding of the relationships among aqueous solutions, geological processes, minerals, organic compounds, gases, thermodynamics and kinetics, and microbial influences, to name a few.

A good example to lay out some of the basic considerations in environmental and low‐temperature geochemistry is the fate and transport of lead (Pb) in the environment. In many regions of the Earth, Pb in the earth surface environment is (was) derived from combustion of leaded gasoline, because even in places where it has been banned (most of the world), Pb tends to persist in soil. The original distribution of Pb was controlled at least in part by atmospheric processes ranging from advection (i.e. wind) to condensation and precipitation.

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Focus Box 1.1
Defining “Low‐Temperature”

In the world of geochemistry and mineralogy, “low‐temperature” environments generally refer to those at or near the Earth's surface, whereas “high‐temperature” environments include those deeper in the crust, i.e. igneous and metamorphic systems. Most geochemists consider tropical soils with mean annual temperature of 25 °C, alpine or polar systems with mean annual temperature of <5 °C, and sediments buried 1 km below the surface with a temperature of 50 °C, all as low‐temperature systems.

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Once deposited on Earth's surface, the fate and transport of Pb is controlled by interactions and relationships among lead atoms, solids compounds (e.g. inorganic minerals or organic matter), plants or other organisms, and the composition of water in soils, lakes, or streams (including dissolved ions like Cl⁻ and CO₃ ²⁻ and gases like O₂ and CO₂). In cases where Pb falls on soils bearing the carbonate anion (CO₃ ²⁻), the formation of lead carbonate (PbCO₃) can result in sequestration of lead in a solid state where it is largely unavailable for uptake by organisms. If the PbCO₃ is thermodynamically stable, the lead can remain sequestered (i.e. in a solid state and relatively inert), but changes in chemical regime can destabilize carbonates. For example, acidic precipitation that lowers the pH of soil can cause dissolution of PbCO₃, but how much of the carbonate will dissolve? How rapidly? Much like the melting of snow on a spring day, geochemical processes are kinetically controlled (some more than others), so even in cases where phases exist out of equilibrium with their surroundings, we must kn...