Porosity or void fraction is a measure of the void spaces in a material, is a fraction of the volume of voids over the total volume, between 0 and 1, or as a percentage between 0% and 100%. Speaking, some tests measure the "accessible void", the total amount of void space accessible from the surface. There are many ways to test porosity in a part, such as industrial CT scanning; the term porosity is used in multiple fields including pharmaceutics, metallurgy, manufacturing, earth sciences, soil mechanics and engineering. In gas-liquid two-phase flow, the void fraction is defined as the fraction of the flow-channel volume, occupied by the gas phase or, alternatively, as the fraction of the cross-sectional area of the channel, occupied by the gas phase. Void fraction varies from location to location in the flow channel, it fluctuates with time and its value is time averaged. In separated flow, it is related to volumetric flow rates of the gas and the liquid phase, to the ratio of the velocity of the two phases.
Used in geology, soil science, building science, the porosity of a porous medium describes the fraction of void space in the material, where the void may contain, for example, air or water. It is defined by the ratio: ϕ = V V V T where VV is the volume of void-space and VT is the total or bulk volume of material, including the solid and void components. Both the mathematical symbols ϕ and n are used to denote porosity. Porosity is a fraction between 0 and 1 ranging from less than 0.01 for solid granite to more than 0.5 for peat and clay. The porosity of a rock, or sedimentary layer, is an important consideration when attempting to evaluate the potential volume of water or hydrocarbons it may contain. Sedimentary porosity is a complicated function of many factors, including but not limited to: rate of burial, depth of burial, the nature of the connate fluids, the nature of overlying sediments. One used relationship between porosity and depth is given by the Athy equation: ϕ = ϕ 0 e − k z where ϕ 0 is the surface porosity, k is the compaction coefficient and z is depth.
A value for porosity can alternatively be calculated from the bulk density ρ bulk, saturating fluid density ρ fluid and particle density ρ particle: ϕ = ρ particle − ρ bulk ρ particle − ρ fluid If the void space is filled with air, the following simpler form may be used: ϕ = 1 − ρ bulk ρ particle Normal particle density is assumed to be 2.65 g/cm3, although a better estimation can be obtained by examining the lithology of the particles. Porosity can be proportional to hydraulic conductivity; the principal complication is that there is not a direct proportionality between porosity and hydraulic conductivity but rather an inferred proportionality. There is a clear proportionality between hydraulic conductivity. There tends to be a proportionality between pore throat radii and pore volume. If the proportionality between pore throat radii and porosity exists a proportionality between porosity and hydraulic conductivity may exist. However, as grain size or sorting decreases the proportionality between pore throat radii and porosity begins to fail and therefore so does the proportionality between porosity and hydraulic conductivity.
For example: clays have low hydraulic conductivity but have high porosities, which means clays can hold a large volume of water per volume of bulk material, but they do not release water and therefore have low hydraulic conductivity. Well sorted materials have higher porosity than sized poorly sorted materials; the graphic illustrates how some smaller grains can fill the pores, drastically reducing porosity and hydraulic conductivity, while only being a small fraction of the total volume of the material. For tables of common porosity values for earth materials, see the "further reading" section in the Hydrogeology article. Consolidated roc
Fluorine is a chemical element with symbol F and atomic number 9. It is the lightest halogen and exists as a toxic pale yellow diatomic gas at standard conditions; as the most electronegative element, it is reactive, as it reacts with all other elements, except for helium and neon. Among the elements, fluorine ranks 24th in universal 13th in terrestrial abundance. Fluorite, the primary mineral source of fluorine which gave the element its name, was first described in 1529. Proposed as an element in 1810, fluorine proved difficult and dangerous to separate from its compounds, several early experimenters died or sustained injuries from their attempts. Only in 1886 did French chemist Henri Moissan isolate elemental fluorine using low-temperature electrolysis, a process still employed for modern production. Industrial production of fluorine gas for uranium enrichment, its largest application, began during the Manhattan Project in World War II. Owing to the expense of refining pure fluorine, most commercial applications use fluorine compounds, with about half of mined fluorite used in steelmaking.
The rest of the fluorite is converted into corrosive hydrogen fluoride en route to various organic fluorides, or into cryolite, which plays a key role in aluminium refining. Molecules containing a Carbon–fluorine bond have high chemical and thermal stability. Pharmaceuticals such as atorvastatin and fluoxetine contain C-F bonds, the fluoride ion inhibits dental cavities, so finds use in toothpaste and water fluoridation. Global fluorochemical sales amount to more than US$15 billion a year. Fluorocarbon gases are greenhouse gases with global-warming potentials 100 to 20,000 times that of carbon dioxide. Organofluorine compounds persist in the environment due to the strength of the carbon–fluorine bond. Fluorine has no known metabolic role in mammals. Fluorine atoms have nine electrons, one fewer than neon, electron configuration 1s22s22p5: two electrons in a filled inner shell and seven in an outer shell requiring one more to be filled; the outer electrons are ineffective at nuclear shielding, experience a high effective nuclear charge of 9 − 2 = 7.
Fluorine's first ionization energy is third-highest among all elements, behind helium and neon, which complicates the removal of electrons from neutral fluorine atoms. It has a high electron affinity, second only to chlorine, tends to capture an electron to become isoelectronic with the noble gas neon. Fluorine atoms have a small covalent radius of around 60 picometers, similar to those of its period neighbors oxygen and neon; the bond energy of difluorine is much lower than that of either Cl2 or Br2 and similar to the cleaved peroxide bond. Conversely, bonds to other atoms are strong because of fluorine's high electronegativity. Unreactive substances like powdered steel, glass fragments, asbestos fibers react with cold fluorine gas. Reactions of elemental fluorine with metals require varying conditions. Alkali metals cause; some solid nonmetals react vigorously in liquid air temperature fluorine. Hydrogen sulfide and sulfur dioxide combine with fluorine, the latter sometimes explosively. Hydrogen, like some of the alkali metals, reacts explosively with fluorine.
Carbon, as lamp black, reacts at room temperature to yield fluoromethane. Graphite combines with fluorine above 400 °C to produce non-stoichiometric carbon monofluoride. Carbon dioxide and carbon monoxide react at or just above room temperature, whereas paraffins and other organic chemicals generate strong reactions: fully substituted haloalkanes such as carbon tetrachloride incombustible, may explode. Although nitrogen trifluoride is stable, nitrogen requires an electric discharge at elevated temperatures for reaction with fluorine to occur, due to the strong triple bond in elemental nitrogen. Oxygen does not combine with fluorine under ambient conditions, but can be made to react using electric discharge at low temperatures and pressures. Heavier halogens react with fluorine as does the noble gas radon. At room temperature, fluorine is a gas of diatomic molecules, pale yellow, it has a characteristic halogen-like biting odor detectable at 20 ppb. Fluorine condenses into a bright yellow liquid at −188 °C, a transition temperature similar to those of oxygen and nitrogen.
Fluorine has two solid forms, α- and β-fluorine. The latter crystallizes at −220 °C and is transparent and sof
In crystallography, a vacancy is a type of point defect in a crystal. Crystals inherently possess imperfections, sometimes referred to as crystalline defects. A defect in which an atom is missing from one of the lattice sites is known as a "vacancy" defect, it is known as a Schottky defect, although in ionic crystals the concepts are not identical. Vacancies occur in all crystalline materials. At any given temperature, up to the melting point of the material, there is an equilibrium concentration. At the melting point of some metals the ratio can be 1:1000; this temperature dependence can be modelled by N v = N exp where Nv is the vacancy concentration, Qv is the energy required for vacancy formation, kB is the Boltzmann constant, T is the absolute temperature, N is the concentration of atomic sites i.e. N = ρ N A / A where ρ is density, NA Avogadro constant, A the atomic mass, it is the simplest point defect. In this system, an atom is missing from its regular atomic site. Vacancies are formed during solidification due to vibration of atoms, local rearrangement of atoms, plastic deformation and ionic bombardments.
The creation of a vacancy can be modeled by considering the energy required to break the bonds between an atom inside the crystal and its nearest neighbor atoms. Once that atom is removed from the lattice site, it is put back on the surface of the crystal and some energy is retrieved because new bonds are established with other atoms on the surface. However, there is a net input of energy because there are fewer bonds between surface atoms than between atoms in the interior of the crystal. Crystallographic defect Schottky defect Frenkel defect Crystalline Defects in Silicon
Wayne State University
Wayne State University is an American public research university located in Detroit, Michigan. Founded in 1868, WSU consists of 13 schools and colleges offering nearly 350 programs to more than 27,000 graduate and undergraduate students. Wayne State University is Michigan's third-largest university; the WSU main campus comprises 195 acres linking more than 100 research buildings. The Wayne State Warriors compete in the NCAA Division II Great Lakes Intercollegiate Athletic Conference; the first component of the modern Wayne State University was established in 1868 as the Detroit College of Medicine. In 1885, the Detroit College of Medicine merged with its competitor, the Michigan College of Medicine and its consolidated buildings. In 1913 the school was restructured as the Detroit College of Medicine and Surgery, passing under that name into the control of the Detroit Board of Education; these institutions are incarnated today as the Wayne State University School of Medicine. In 1881, the Detroit Normal Training School for Teachers was established by the Detroit Board of Education.
In 1920, after several re-locations to larger quarters, the school became the Detroit Teachers College. The Board of Education voted in 1924 to make the college a part of the new College of the City of Detroit; this became the Wayne State University College of Education. In 1917, the Detroit Board of Education founded the Detroit Junior College and would make Detroit Central High School's Old Main Hall its campus. Detroit's College of Pharmacy and the Detroit Teachers College were added to the campus in 1924, were organized into the College of the City of Detroit; the original junior college became the College of Liberal Arts. The first bachelor's degrees were awarded in 1925; the College of Liberal Arts of the College of the City of Detroit is today the Wayne State University College of Liberal Arts and Sciences. Recognizing the need for a good public law school, a group of lawyers, including Allan Campbell, the school's founding dean, established Detroit City Law School in 1927 as part of the College of the City of Detroit.
Structured as a part-time, evening program, the school graduated its first class with the bachelor of laws degree in 1928 and achieved full American Bar Association in 1939. The school is known today as Wayne State University Law School. In 1933, the Detroit Board of Education voted to unify the colleges. In January 1934, that institution was named Wayne University, taking its name from Wayne County in which the University and the City of Detroit reside, as well as Major General "Mad" Anthony Wayne. Continuing to grow, Wayne University added its School of Social Work in 1935, the School of Business Administration in 1946. Wayne University was renamed Wayne State University in 1956 and the institution became a constitutionally mandated university by a popularly adopted amendment to the Michigan Constitution in 1959; the Wayne State University Board of Governors created the Institute of Gerontology in 1965 in response to a State of Michigan mandate. The primary mission in that era was to engage in research and service in the field of aging.
Wayne State University grew again in 1973 with the addition of the College of Lifelong Learning. In 1985, the School of Fine and the Performing Arts, the College of Urban and Metropolitan Affairs grew the university further. In the 2000s, WSU constructed several new buildings, including the Integrative Biosciences Center, a 207,000-square-foot facility for interdisciplinary work in the biosciences. More than 500 researchers and principal investigators work out of the building, which opened in 2016. On June 5, 2013, the Board of Governors unanimously elected M. Roy Wilson as Wayne State's 12th president, he was sworn in on August 1, 2013. In 2015, WSU bestowed its first posthumous honorary doctorate degree on Viola Liuzzo. In 2015, the School of Business administration was renamed the Mike Ilitch School of Business; the name was changed in recognition of a $40 million grant from Marian Ilitch. This gift was used towards building a new business school facility in Detroit, which opened in late August 2018.
The new Mike Ilitch School of Business building is located on Woodward in the emerging'District Detroit' development. Wayne State's academic offerings are divided among 13 schools and colleges: the Mike Ilitch School of Business. Fall 2018 enrollment for the university consisted of 27,053 students. Wayne State University is Michigan's only urban research university and is classified as a research university with the highest research activity by the Carnegie Foundation. Under the Michigan Constitution, the boards of governors of WSU are elected by the citizens of Michigan statewide. Wayne State University, Michigan State University, the University of Michigan are the three institutional members of the State of Michigan's University Research Corridor. Wayne State offers more than 350 undergraduate, post-graduate and certificate programs in 13 schools and colleges. Mike Ilitch School of Business The Mike Ilitch School of Business offers undergraduate degrees in accounting, global supply chain, information systems
Diffusion is the net movement of molecules or atoms from a region of higher concentration to a region of lower concentration. Diffusion is driven by a gradient in chemical potential of the diffusing species. A gradient is the change in the value of a quantity e.g. concentration, pressure, or temperature with the change in another variable distance. A change in concentration over a distance is called a concentration gradient, a change in pressure over a distance is called a pressure gradient, a change in temperature over a distance is called a temperature gradient; the word diffusion derives from the Latin word, which means "to spread way out.” A distinguishing feature of diffusion is that it depends on particle random walk, results in mixing or mass transport without requiring directed bulk motion. Bulk motion, or bulk flow, is the characteristic of advection; the term convection is used to describe the combination of both transport phenomena. An example of a situation in which bulk motion and diffusion can be differentiated is the mechanism by which oxygen enters the body during external respiration known as breathing.
The lungs are located in the thoracic cavity, which expands as the first step in external respiration. This expansion leads to an increase in volume of the alveoli in the lungs, which causes a decrease in pressure in the alveoli; this creates a pressure gradient between the air outside the body at high pressure and the alveoli at low pressure. The air moves down the pressure gradient through the airways of the lungs and into the alveoli until the pressure of the air and that in the alveoli are equal i.e. the movement of air by bulk flow stops once there is no longer a pressure gradient. The air arriving in the alveoli has a higher concentration of oxygen than the “stale” air in the alveoli; the increase in oxygen concentration creates a concentration gradient for oxygen between the air in the alveoli and the blood in the capillaries that surround the alveoli. Oxygen moves by diffusion, down the concentration gradient, into the blood; the other consequence of the air arriving in alveoli is that the concentration of carbon dioxide in the alveoli decreases.
This creates a concentration gradient for carbon dioxide to diffuse from the blood into the alveoli, as fresh air has a low concentration of carbon dioxide compared to the blood in the body. The pumping action of the heart transports the blood around the body; as the left ventricle of the heart contracts, the volume decreases, which increases the pressure in the ventricle. This creates a pressure gradient between the heart and the capillaries, blood moves through blood vessels by bulk flow down the pressure gradient; as the thoracic cavity contracts during expiration, the volume of the alveoli decreases and creates a pressure gradient between the alveoli and the air outside the body, air moves by bulk flow down the pressure gradient. The concept of diffusion is used in: physics, biology, sociology and finance. However, in each case, the object, undergoing diffusion is “spreading out” from a point or location at which there is a higher concentration of that object. There are two ways to introduce the notion of diffusion: either a phenomenological approach starting with Fick's laws of diffusion and their mathematical consequences, or a physical and atomistic one, by considering the random walk of the diffusing particles.
In the phenomenological approach, diffusion is the movement of a substance from a region of high concentration to a region of low concentration without bulk motion. According to Fick's laws, the diffusion flux is proportional to the negative gradient of concentrations, it goes from regions of higher concentration to regions of lower concentration. Sometime various generalizations of Fick's laws were developed in the frame of thermodynamics and non-equilibrium thermodynamics. From the atomistic point of view, diffusion is considered as a result of the random walk of the diffusing particles. In molecular diffusion, the moving molecules are self-propelled by thermal energy. Random walk of small particles in suspension in a fluid was discovered in 1827 by Robert Brown; the theory of the Brownian motion and the atomistic backgrounds of diffusion were developed by Albert Einstein. The concept of diffusion is applied to any subject matter involving random walks in ensembles of individuals. Biologists use the terms "net movement" or "net diffusion" to describe the movement of ions or molecules by diffusion.
For example, oxygen can diffuse through cell membranes so long as there is a higher concentration of oxygen outside the cell. However, because the movement of molecules is random oxygen molecules move out of the cell; because there are more oxygen molecules outside the cell, the probability that oxygen molecules will enter the cell is higher than the probability that oxygen molecules will leave the cell. Therefore, the "net" movement of oxygen molecules is into the cell. In other words, there is a net movement of oxygen molecules down the concentration gradient. In the scope of time, diffusion in solids was used. For example, Pliny the Elder had described the cementation process, which produces steel from the element iron through carbon diffusion. Another example is well known for many centuries, the diffusion of colors of stained glass or earthenware and Chinese ceramics. In modern science, the first systematic experimental study of di
An alloy is a combination of metals and of a metal or another element. Alloys are defined by a metallic bonding character. An alloy may be a mixture of metallic phases. Intermetallic compounds are alloys with a defined crystal structure. Zintl phases are sometimes considered alloys depending on bond types. Alloys are used in a wide variety of applications. In some cases, a combination of metals may reduce the overall cost of the material while preserving important properties. In other cases, the combination of metals imparts synergistic properties to the constituent metal elements such as corrosion resistance or mechanical strength. Examples of alloys are steel, brass, duralumin and amalgams; the alloy constituents are measured by mass percentage for practical applications, in atomic fraction for basic science studies. Alloys are classified as substitutional or interstitial alloys, depending on the atomic arrangement that forms the alloy, they can be heterogeneous or intermetallic. An alloy is a mixture of chemical elements, which forms an impure substance that retains the characteristics of a metal.
An alloy is distinct from an impure metal in that, with an alloy, the added elements are well controlled to produce desirable properties, while impure metals such as wrought iron are less controlled, but are considered useful. Alloys are made by mixing two or more elements, at least one of, a metal; this is called the primary metal or the base metal, the name of this metal may be the name of the alloy. The other constituents may or may not be metals but, when mixed with the molten base, they will be soluble and dissolve into the mixture; the mechanical properties of alloys will be quite different from those of its individual constituents. A metal, very soft, such as aluminium, can be altered by alloying it with another soft metal, such as copper. Although both metals are soft and ductile, the resulting aluminium alloy will have much greater strength. Adding a small amount of non-metallic carbon to iron trades its great ductility for the greater strength of an alloy called steel. Due to its very-high strength, but still substantial toughness, its ability to be altered by heat treatment, steel is one of the most useful and common alloys in modern use.
By adding chromium to steel, its resistance to corrosion can be enhanced, creating stainless steel, while adding silicon will alter its electrical characteristics, producing silicon steel. Like oil and water, a molten metal may not always mix with another element. For example, pure iron is completely insoluble with copper; when the constituents are soluble, each will have a saturation point, beyond which no more of the constituent can be added. Iron, for example, can hold a maximum of 6.67% carbon. Although the elements of an alloy must be soluble in the liquid state, they may not always be soluble in the solid state. If the metals remain soluble when solid, the alloy forms a solid solution, becoming a homogeneous structure consisting of identical crystals, called a phase. If as the mixture cools the constituents become insoluble, they may separate to form two or more different types of crystals, creating a heterogeneous microstructure of different phases, some with more of one constituent than the other phase has.
However, in other alloys, the insoluble elements may not separate until after crystallization occurs. If cooled quickly, they first crystallize as a homogeneous phase, but they are supersaturated with the secondary constituents; as time passes, the atoms of these supersaturated alloys can separate from the crystal lattice, becoming more stable, form a second phase that serve to reinforce the crystals internally. Some alloys, such as electrum, an alloy consisting of silver and gold, occur naturally. Meteorites are sometimes made of occurring alloys of iron and nickel, but are not native to the Earth. One of the first alloys made by humans was bronze, a mixture of the metals tin and copper. Bronze was an useful alloy to the ancients, because it is much stronger and harder than either of its components. Steel was another common alloy. However, in ancient times, it could only be created as an accidental byproduct from the heating of iron ore in fires during the manufacture of iron. Other ancient alloys include pewter and pig iron.
In the modern age, steel can be created in many forms. Carbon steel can be made by varying only the carbon content, producing soft alloys like mild steel or hard alloys like spring steel. Alloy steels can be made by adding other elements, such as chromium, vanadium or nickel, resulting in alloys such as high-speed steel or tool steel. Small amounts of manganese are alloyed with most modern steels because of its ability to remove unwanted impurities, like phosphorus and oxygen, which can have detrimental effects on the alloy. However, most alloys were not created until the 1900s, such as various aluminium, titanium and magnesium alloys; some modern superalloys, such as incoloy and hastelloy, may consist of a multitude of different elements. As a noun, the term alloy is used to describe a mixture of atoms in which the primary constituent is a metal; when used as a verb, the term refers to the act of mixing a metal with other elements. The primary metal is called the matrix, or the solvent; the secondary constituents are called s
Zinc is a chemical element with symbol Zn and atomic number 30. It is the first element in group 12 of the periodic table. In some respects zinc is chemically similar to magnesium: both elements exhibit only one normal oxidation state, the Zn2+ and Mg2+ ions are of similar size. Zinc has five stable isotopes; the most common zinc ore is sphalerite, a zinc sulfide mineral. The largest workable lodes are in Australia and the United States. Zinc is refined by froth flotation of the ore and final extraction using electricity. Brass, an alloy of copper and zinc in various proportions, was used as early as the third millennium BC in the Aegean, the United Arab Emirates, Kalmykia and Georgia, the second millennium BC in West India, Iran, Syria and Israel/Palestine. Zinc metal was not produced on a large scale until the 12th century in India, though it was known to the ancient Romans and Greeks; the mines of Rajasthan have given definite evidence of zinc production going back to the 6th century BC. To date, the oldest evidence of pure zinc comes from Zawar, in Rajasthan, as early as the 9th century AD when a distillation process was employed to make pure zinc.
Alchemists burned zinc in air to form what they called "philosopher's wool" or "white snow". The element was named by the alchemist Paracelsus after the German word Zinke. German chemist Andreas Sigismund Marggraf is credited with discovering pure metallic zinc in 1746. Work by Luigi Galvani and Alessandro Volta uncovered the electrochemical properties of zinc by 1800. Corrosion-resistant zinc plating of iron is the major application for zinc. Other applications are in electrical batteries, small non-structural castings, alloys such as brass. A variety of zinc compounds are used, such as zinc carbonate and zinc gluconate, zinc chloride, zinc pyrithione, zinc sulfide, dimethylzinc or diethylzinc in the organic laboratory. Zinc is an essential mineral, including to postnatal development. Zinc deficiency affects about two billion people in the developing world and is associated with many diseases. In children, deficiency causes growth retardation, delayed sexual maturation, infection susceptibility, diarrhea.
Enzymes with a zinc atom in the reactive center are widespread in biochemistry, such as alcohol dehydrogenase in humans. Consumption of excess zinc may cause ataxia and copper deficiency. Zinc is a bluish-white, diamagnetic metal, though most common commercial grades of the metal have a dull finish, it is somewhat less dense than iron and has a hexagonal crystal structure, with a distorted form of hexagonal close packing, in which each atom has six nearest neighbors in its own plane and six others at a greater distance of 290.6 pm. The metal is hard and brittle at most temperatures but becomes malleable between 100 and 150 °C. Above 210 °C, the metal can be pulverized by beating. Zinc is a fair conductor of electricity. For a metal, zinc has low melting and boiling points; the melting point is the lowest of all the d-block metals aside from cadmium. Many alloys contain zinc, including brass. Other metals long known to form binary alloys with zinc are aluminium, bismuth, iron, mercury, tin, cobalt, nickel and sodium.
Although neither zinc nor zirconium are ferromagnetic, their alloy ZrZn2 exhibits ferromagnetism below 35 K. A bar of zinc generates a characteristic sound when bent, similar to tin cry. Zinc makes up about 75 ppm of Earth's crust. Soil contains zinc in 5–770 ppm with an average 64 ppm. Seawater has only 30 ppb and the atmosphere, 0.1–4 µg/m3. The element is found in association with other base metals such as copper and lead in ores. Zinc is a chalcophile, meaning the element is more to be found in minerals together with sulfur and other heavy chalcogens, rather than with the light chalcogen oxygen or with non-chalcogen electronegative elements such as the halogens. Sulfides formed as the crust solidified under the reducing conditions of the early Earth's atmosphere. Sphalerite, a form of zinc sulfide, is the most mined zinc-containing ore because its concentrate contains 60–62% zinc. Other source minerals for zinc include smithsonite, hemimorphite and sometimes hydrozincite. With the exception of wurtzite, all these other minerals were formed by weathering of the primordial zinc sulfides.
Identified world zinc resources total about 1.9–2.8 billion tonnes. Large deposits are in Australia and the United States, with the largest reserves in Iran; the most recent estimate of reserve base for zinc was made in 2009 and calculated to be 480 Mt. Zinc reserves, on the other hand, are geologically identified ore bodies whose suitability for recovery is economically based at the time of determination. Since exploration and mine development is an ongoing process, the amount of zinc reserves is not a fixed number and sustainability of zinc ore supplies cannot be judged by extrapolating the combined mine life of today's zinc mines; this concept is well supported by data from the United States Geol