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. Aluminium ( aluminum in and ) is a with the Al and 13. It is a silvery-white, soft, and in the. By mass, aluminium makes up about 8% of the, where it is the third most abundant element (after and ) and also the most abundant metal. Occurrence of aluminium decreases in the Earth's mantle below, however. The chief of aluminium is.

Aluminium metal is highly reactive, such that are rare and limited to extreme environments. Instead, it is found combined in over 270 different.Aluminium is remarkable for its low and its ability to resist through the phenomenon of. Aluminium and its are vital to the industry and important in and building industries, such as building facades and window frames. The and are the most useful compounds of aluminium.Despite its prevalence in the environment, no known form of life uses aluminium, but aluminium is well tolerated by plants and animals.

Because of these salts' abundance, the potential for a biological role for them is of continuing interest, and studies continue. Main article:Of aluminium isotopes, only 27Alis stable. This is consistent with aluminium having an odd atomic number.

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It is the only aluminium isotope, i.e. The only one that has existed on Earth in its current form since the creation of the planet. Nearly all aluminium on Earth is present as this isotope, which makes it a and means that its is the same as that of the isotope. The standard atomic weight of aluminium is low in comparison with many other metals, which has consequences for the element's properties (see ). This makes aluminium very useful in (NMR), as its single stable isotope has a high NMR sensitivity.All other isotopes of aluminium are. The most stable of these is ( 717,000 years) and therefore could not have survived since the formation of the planet.

However, minute traces of 26Al are produced from in the by caused by protons. The ratio of 26Al to has been used for of geological processes over 10 5 to 10 6 year time scales, in particular transport, deposition, storage, burial times, and erosion.

Most meteorite scientists believe that the energy released by the decay of 26Al was responsible for the melting and of some after their formation 4.55 billion years ago.The remaining isotopes of aluminium, with ranging from 22 to 43, all have half-lives well under an hour. Three states are known, all with half-lives under a minute. Electron shellAn aluminium atom has 13 electrons, arranged in an of  3s 2 3p 1, with three electrons beyond a stable noble gas configuration. Accordingly, the combined first three of aluminium are far lower than the fourth ionization energy alone. Such an electron configuration is shared with the other well-characterized members of its group, and; it is also expected for. Aluminium can relatively easily surrender its three outermost electrons in many chemical reactions (see ). The of aluminium is 1.61 (Pauling scale).

High-resolution - micrograph of Al atoms viewed along the 001 zone axis.A free aluminium atom has a of 143. With the three outermost electrons removed, the shrinks to 39 pm for a 4-coordinated atom or 53.5 pm for a 6-coordinated atom. At, aluminium atoms (when not affected by atoms of other elements) form a bound by provided by atoms' outermost electrons; hence aluminium (at these conditions) is a metal. This crystal system is shared by many other metals, such as and; the size of a unit cell of aluminium is comparable to that of those other metals. It is however not shared by the other members of its group; boron has ionization energies too high to allow metallization, thallium has a structure, and gallium and indium have unusual structures that are not close-packed like those of aluminium and thallium. Since few electrons are available for, aluminium metal is soft with a low melting point and low, as is common for. BulkAluminium metal has an appearance ranging from silvery white to dull gray, depending on the.

A fresh film of aluminium serves as a good (approximately 92%) of and an excellent reflector (as much as 98%) of medium and far radiation.The density of aluminium is 2.70 g/cm 3, about 1/3 that of steel, much lower than other commonly encountered metals, making aluminium parts easily identifiable through their lightness. Aluminium's low density compared to most other metals arises from the fact that its nuclei are much lighter, while difference in the unit cell size does not compensate for this difference. The only lighter metals are the metals of and, which apart from and are too reactive for structural use (and beryllium is very toxic). Aluminium is not as strong or stiff as steel, but the low density makes up for this in the industry and for many other applications where light weight and relatively high strength are crucial.Pure aluminium is quite soft and lacking in strength. In most applications various are used instead because of their higher strength and hardness. The of pure aluminium is 7–11, while have yield strengths ranging from 200 MPa to 600 MPa.

Aluminium is, and allowing it to be easily. It is also easily, and the low melting temperature of 660 °C allows for easy.Aluminium is an excellent and, having 59% the conductivity of, both thermal and electrical, while having only 30% of copper's density. Aluminium is capable of, with a superconducting critical temperature of 1.2 and a critical magnetic field of about 100 (10 ). It is and thus essentially unaffected by static magnetic fields. The high electrical conductivity, however, means that it is strongly affected by changing magnetic field through the induction of. Main article:Aluminium combines characteristics of pre- and post-transition metals.

Since it has few available electrons for metallic bonding, like its heavier group 13 congeners, it has the characteristic physical properties of a post-transition metal, with longer-than-expected interatomic distances. Furthermore, as Al 3+ is a small and highly charged cation, it is strongly polarizing and aluminium compounds tend towards covalency; this behaviour is similar to that of (Be 2+), and the two display an example of a.Unlike all other post-transition metals, the underlying core under aluminium's valence shell is that of the preceding, whereas those of its heavier congeners, and also include a filled d-subshell and in some cases an f-subshell. Hence, inner electrons of aluminium shield the valence electrons completely, unlike those of aluminium's heavier congeners.

Aluminium's electropositive behavior, high affinity for oxygen, and highly negative are all more similar to those of, and, which have ds 2 configurations of three valence electrons outside a noble gas core: aluminium is the most electropositive metal in its group. Aluminium also bears minor similarities to the metalloid boron in the same group: AlX 3 compounds are valence to BX 3 compounds (they have the same valence electronic structure), and both behave as and readily from. Additionally, one of the main motifs of boron chemistry is structures, and aluminium forms an important part of many icosahedral alloys, including the Al–Zn–Mg class.Aluminium has a high to oxygen, which renders it suitable for use as a in the reaction. A fine powder of aluminium metal reacts explosively on contact with; under normal conditions, however, aluminium forms a thin oxide layer that protects the metal from further corrosion by oxygen, water, or dilute acid, a process termed. Because of its general resistance to corrosion, aluminium is one of the few metals that retains silvery reflectance in finely powdered form, making it an important component of paints. Aluminium is not attacked by oxidizing acids because of its passivation. This allows aluminium to be used to store reagents such as, concentrated, and some organic acids.In hot concentrated, aluminium reacts with water with evolution of hydrogen, and in aqueous or at room temperature to form —protective passivation under these conditions is negligible.

Also dissolves aluminium. Aluminium is corroded by dissolved, such as common, which is why household plumbing is never made from aluminium. The oxide layer on aluminium is also destroyed by contact with due to or with salts of some electropositive metals. As such, the strongest aluminium alloys are less corrosion-resistant due to reactions with alloyed, and aluminium's corrosion resistance is greatly reduced by aqueous salts, particularly in the presence of dissimilar metals.Aluminium reacts with most nonmetals upon heating, forming compounds such as (AlN), (Al 2S 3), and the aluminium halides (AlX 3).

It also forms a wide range of involving metals from every group on the periodic table. Inorganic compoundsThe vast majority of compounds, including all aluminium-containing minerals and all commercially significant aluminium compounds, feature aluminium in the oxidation state 3+. The of such compounds varies, but generally Al 3+ is either six- or four-coordinate. Almost all compounds of aluminium(III) are colorless. Mechanism of the Friedel–Crafts acylation, using AlCl 3 as a catalystWith heavier halides, the coordination numbers are lower. The other trihalides are or with tetrahedral four-coordinate aluminium centers. (AlCl 3) has a layered polymeric structure below its melting point of 192.4 °C (378 °F), but transforms on melting to Al 2Cl 6 dimers with a concomitant increase in volume by 85% and a near-total loss of electrical conductivity.

These still predominate in the gas phase at low temperatures (150–200 °C), but at higher temperatures increasingly dissociate into trigonal planar AlCl 3 monomers similar to the structure of. And form Al 2X 6 dimers in all three phases and hence do not show such significant changes of properties upon phase change. These materials are prepared by treating aluminium metal with the halogen. The aluminium trihalides form many or complexes; their nature makes them useful as catalysts for the. Aluminium trichloride has major industrial uses involving this reaction, such as in the manufacture of and; it is also often used as the precursor for many other aluminium compounds and as a reagent for converting nonmetal fluorides into the corresponding chlorides (a ).Aluminium forms one stable oxide with the Al 2O 3, commonly called. It can be found in nature in the mineral, α-alumina; there is also a γ-alumina phase.

As corundum is very hard ( 9), has a high melting point of 2,045 °C (3,713 °F), has very low volatility, is chemically inert, and a good electrical insulator, it is often used in abrasives (such as toothpaste), as a refractory material, and in cermanics, as well as being the starting material for the electrolytic production of aluminium metal. And are impure corundum contaminated with trace amounts of other metals. The two main oxide-hydroxides, AlO(OH), are. There are three main trihydroxides:, and, which differ in their crystalline structure.

Many other intermediate and related structures are also known. Most are produced from ores by a variety of wet processes using acid and base. Heating the hydroxides leads to formation of corundum. These materials are of central importance to the production of aluminium and are themselves extremely useful. Some mixed oxide phases are also very useful, such as (MgAl 2O 4), Na-β-alumina (NaAl 11O 17), and (Ca 3Al 2O 6, an important mineral phase in ).The only stable under normal conditions are (Al 2S 3), (Al 2Se 3), and (Al 2Te 3). All three are prepared by direct reaction of their elements at about 1,000 °C (1,832 °F) and quickly hydrolyse completely in water to yield aluminium hydroxide and the respective. As aluminium is a small atom relative to these chalcogens, these have four-coordinate tetrahedral aluminium with various polymorphs having structures related to, with two-thirds of the possible metal sites occupied either in an orderly (α) or random (β) fashion; the sulfide also has a γ form related to γ-alumina, and an unusual high-temperature hexagonal form where half the aluminium atoms have tetrahedral four-coordination and the other half have trigonal bipyramidal five-coordination.

Four: (AlN), (AlP), (AlAs), and (AlSb), are known. They are all isoelectronic to and, all of which but AlN have the structure. All four can be made by high-temperature (and possibly high-pressure) direct reaction of their component elements. Rarer oxidation states. See also:Although the great majority of aluminium compounds feature Al 3+ centers, compounds with lower oxidation states are known and are sometimes of significance as precursors to the Al 3+ species.AlF, AlCl, AlBr, and AlI exist in the gaseous phase when the respective trihalide is heated with aluminium, and at cryogenic temperatures. Their instability in the condensed phase is due to their ready to aluminium and the respective trihalide: the reverse reaction is favored at high temperature (although even then they are still short-lived), explaining why AlF 3 is more volatile when heated in the presence of aluminium metal, as is aluminium metal when heated in the presence of AlCl 3. A stable derivative of aluminium monoiodide is the cyclic formed with, Al 4I 4(NEt 3) 4.

Also of theoretical interest but only of fleeting existence are Al 2O and Al 2S. Al 2O is made by heating the normal oxide, Al 2O 3, with silicon at 1,800 °C (3,272 °F) in a. Such materials quickly disproportionate to the starting materials.Very simple Al(II) compounds are invoked or observed in the reactions of Al metal with oxidants. For example, AlO, has been detected in the gas phase after explosion and in stellar absorption spectra. More thoroughly investigated are compounds of the formula R 4Al 2 which contain an Al–Al bond and where R is a large organic. Organoaluminium compounds and related hydrides.

Structure of, a compound that features five-coordinate carbon.A variety of compounds of empirical formula AlR 3 and AlR 1.5Cl 1.5 exist. The aluminium trialkyls and triaryls are reactive, volatile, and colorless liquids or low-melting solids. They catch fire spontaneously in air and react with water, thus necessitating precautions when handling them. They often form dimers, unlike their boron analogues, but this tendency diminishes for branched-chain alkyls (e.g., Me 3CCH 2); for example, exists as an equilibrium mixture of the monomer and dimer. These dimers, such as (Al 2Me 6), usually feature tetrahedral Al centers formed by dimerization with some alkyl group bridging between both aluminium atoms. They are and react readily with ligands, forming adducts.

In industry, they are mostly used in alkene insertion reactions, as discovered by, most importantly in 'growth reactions' that form long-chain unbranched primary alkenes and alcohols, and in the low-pressure polymerization of. There are also some and cluster organoaluminium compounds involving Al–N bonds.The industrially most important aluminium hydride is (LiAlH 4), which is used in as a reducing agent in. It can be produced from and: 4 LiH + AlCl 3 → LiAlH 4 + 3 LiClThe simplest hydride, or alane, is not as important.

It is a polymer with the formula (AlH 3) n, in contrast to the corresponding boron hydride that is a dimer with the formula (BH 3) 2. Natural occurrence. See also: In spaceAluminium's per-particle abundance in the is 3.15 (parts per million). It is the twelfth most abundant of all elements and third most abundant among the elements that have odd atomic numbers, after hydrogen and nitrogen. The only stable isotope of aluminium, 27Al, is the eighteenth most abundant nucleus in the Universe. It is created almost entirely after fusion of carbon in massive stars that will later become: this fusion creates 26Mg, which, upon capturing free protons and neutrons becomes aluminium. Some smaller quantities of 27Al are created in shells of evolved stars, where 26Mg can capture free protons.

Essentially all aluminium now in existence is 27Al; 26Al was present in the early Solar System but is currently. However, the of 26Al that do exist are the most common emitter in the. A major aluminium ore. The red-brown color is due to the presence of minerals.Overall, the Earth is about 1.59% aluminium by mass (seventh in abundance by mass). Aluminium occurs in greater proportion in the Earth than in the Universe because aluminium easily forms the oxide and becomes bound into rocks and aluminium stays in the while less reactive metals sink to the core. In the Earth's crust, aluminium is the most abundant (8.3% by mass) metallic element and the third most abundant of all elements (after oxygen and silicon).

A large number of silicates in the Earth's crust contain aluminium. In contrast, the Earth's is only 2.38% aluminium by mass.Because of its strong affinity for oxygen, aluminium is almost never found in the elemental state; instead it is found in oxides or silicates., the most common group of minerals in the Earth's crust, are aluminosilicates. Aluminium also occurs in the minerals,. Impurities in Al 2O 3, such as and, yield the and, respectively.

Native aluminium metal can only be found as a minor phase in low oxygen environments, such as the interiors of certain volcanoes. Native aluminium has been reported in in the northeastern of the. It is possible that these deposits resulted from of tetrahydroxoaluminate Al(OH) 4 −.Although aluminium is a common and widespread element, not all aluminium minerals are economically viable sources of the metal.

Almost all metallic aluminium is produced from the (AlO x(OH) 3–2 x). Bauxite occurs as a product of low iron and silica bedrock in tropical climatic conditions. In 2017, most bauxite was mined in Australia, China, Guinea, and India. World production of aluminium since 1900Throughout the 20th century, the production of aluminium rose rapidly: while the world production of aluminium in 1900 was 6,800 metric tons, the annual production first exceeded 100,000 metric tons in 1916; 1,000,000 tons in 1941; 10,000,000 tons in 1971. In the 1970s, the increased demand for aluminium made it an exchange commodity; it entered the, the oldest industrial metal exchange in the world, in 1978. The output continued to grow: the annual production of aluminium exceeded 50,000,000 metric tons in 2013.The for aluminium declined from $14,000 per metric ton in 1900 to $2,340 in 1948 (in 1998 United States dollars). Extraction and processing costs were lowered over technological progress and the scale of the economies.

However, the need to exploit lower-grade poorer quality deposits and the use of fast increasing input costs (above all, energy) increased the net cost of aluminium; the real price began to grow in the 1970s with the rise of energy cost. Production moved from the industrialized countries to countries where production was cheaper. Production costs in the late 20th century changed because of advances in technology, lower energy prices, exchange rates of the United States dollar, and alumina prices. The countries' combined share in primary production and primary consumption grew substantially in the first decade of the 21st century. China is accumulating an especially large share of world's production thanks to abundance of resources, cheap energy, and governmental stimuli; it also increased its consumption share from 2% in 1972 to 40% in 2010. In the United States, Western Europe, and Japan, most aluminium was consumed in transportation, engineering, construction, and packaging. EtymologyAluminium is named after alumina, or aluminium oxide in modern nomenclature.

The word 'alumina' comes from 'alum', the mineral from which it was collected. The word 'alum' comes from alumen, a word meaning 'bitter salt'. The word alumen stems from the root.alu- meaning 'bitter' or 'beer'. 1897 American advertisement featuring the aluminum spellingBritish chemist, who performed a number of experiments aimed to isolate the metal, is credited as the person who named the element. In 1808, he suggested the metal be named alumium.

This suggestion was criticized by contemporary chemists from France, Germany, and Sweden, who insisted the metal should be named for the oxide, alumina, from which it would be isolated. In 1812, Davy chose aluminum, thus producing the modern name. However, its spelling and pronunciation varies: aluminum is in use in the United States and Canada while aluminium is in use elsewhere.

SpellingThe -ium suffix followed the precedent set in other newly discovered elements of the time: potassium, sodium, magnesium, calcium, and (all of which Davy isolated himself). Nevertheless, element names ending in -um were known at the time; for example, (known to Europeans since the 16th century), (discovered in 1778), and (discovered in 1802).

The -um suffix is consistent with the universal spelling for the (as opposed to aluminia); compare to, the oxide of, and, and, the oxides of, and, respectively.In 1812, British scientist wrote an anonymous review of Davy's book, in which he objected to aluminum and proposed the name aluminium: 'for so we shall take the liberty of writing the word, in preference to aluminum, which has a less classical sound.' This name did catch on: while the -um spelling was occasionally used in Britain, the American scientific language used -ium from the start. Most scientists used -ium throughout the world in the 19th century; it still remains the standard in most other languages. In 1828, American lexicographer used exclusively the aluminum spelling in his. In the 1830s, the -um spelling started to gain usage in the United States; by the 1860s, it had become the more common spelling there outside science.

In 1892, Hall used the -um spelling in his advertising handbill for his new electrolytic method of producing the metal, despite his constant use of the -ium spelling in all the patents he filed between 1886 and 1903. It was subsequently suggested this was a typo rather than intended. By 1890, both spellings had been common in the U.S. Overall, the -ium spelling being slightly more common; by 1895, the situation had reversed; by 1900, aluminum had become twice as common as aluminium; during the following decade, the -um spelling dominated American usage. In 1925, the adopted this spelling.The (IUPAC) adopted aluminium as the standard international name for the element in 1990. In 1993, they recognized aluminum as an acceptable variant; the most recent acknowledges this spelling as well. IUPAC official publications use the -ium spelling as primary but list both where appropriate.

Production and refinement. See also: World's top producers of primary aluminium, 2016 CountryOutput(thousandtons)31,8733,5613,2082,8962,4711,631700World total58,800Aluminium production is highly energy-consuming, and so the producers tend to locate smelters in places where electric power is both plentiful and inexpensive. As of 2012, the world's largest of aluminium are located in China, Russia, Bahrain, United Arab Emirates, and South Africa.In 2016, China was the top producer of aluminium with a world share of fifty-five percent; the next largest producing countries were Russia, Canada, India, and the United Arab Emirates.According to the 's, the global stock of aluminium in use in society (i.e. In cars, buildings, electronics, etc.) is 80 kg (180 lb). Much of this is in more-developed countries (350–500 kg (770–1,100 lb) per capita) rather than less-developed countries (35 kg (77 lb) per capita). Bayer process.

Main article:Recovery of the metal through has become an important task of the aluminium industry. Recycling was a low-profile activity until the late 1960s, when the growing use of aluminium brought it to public awareness. Recycling involves melting the scrap, a process that requires only 5% of the energy used to produce aluminium from ore, though a significant part (up to 15% of the input material) is lost as (ash-like oxide). An aluminium stack melter produces significantly less dross, with values reported below 1%.White dross from primary aluminium production and from secondary recycling operations still contains useful quantities of aluminium that can be. The process produces aluminium billets, together with a highly complex waste material. This waste is difficult to manage. It reacts with water, releasing a mixture of gases (including, among others, and ), which spontaneously ignites on contact with air; contact with damp air results in the release of copious quantities of ammonia gas.

Despite these difficulties, the waste is used as a filler in. The major uses for aluminium metal are in:. Transportation (, aircraft, marine vessels, spacecraft, etc.).

Aluminium is used because of its low density;. Packaging (, foil, frame etc.). Aluminium is used because it is non-toxic , non-, and -proof;. Building and construction (, building wire, sheathing, roofing, etc.).

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Since steel is cheaper, aluminium is used when lightness, corrosion resistance, or engineering features are important;. Electricity-related uses (conductor alloys, motors and generators, transformers, capacitors, etc.). Aluminium is used because it is relatively cheap, highly conductive, has adequate mechanical strength and low density, and resists corrosion;. A wide range of items, from to. Low density, good appearance, ease of fabrication, and durability are the key factors of aluminium usage;. Machinery and equipment (processing equipment, pipes, tools).

Aluminium is used because of its corrosion resistance, non-pyrophoricity, and mechanical strength.CompoundsThe great majority (about 90%) of is converted to metallic aluminium. Being a very hard material ( 9), alumina is widely used as an abrasive; being extraordinarily chemically inert, it is useful in highly reactive environments such as lamps. Aluminium oxide is commonly used as a catalyst for industrial processes; e.g. The to convert to sulfur in and to. Many industrial are by alumina, meaning that the expensive catalyst material is dispersed over a surface of the inert alumina.

Another principal use is as a drying agent or absorbent. Laser deposition of alumina on a substrateSeveral sulfates of aluminium have industrial and commercial application. (in its hydrate form) is produced on the annual scale of several millions of metric tons. About two-thirds is consumed in. The next major application is in the manufacture of paper. It is also used as a in dyeing, in pickling seeds, deodorizing of mineral oils, in, and in production of other aluminium compounds.

Two kinds of alum, and, were formerly used as and in leather tanning, but their use has significantly declined following availability of high-purity aluminium sulfate. Anhydrous is used as a catalyst in chemical and petrochemical industries, the dyeing industry, and in synthesis of various inorganic and organic compounds. Aluminium hydroxychlorides are used in purifying water, in the paper industry, and as antiperspirants. Schematic of aluminium absorption by human skin.Despite its widespread occurrence in the Earth's crust, aluminium has no known function in biology.

At pH 6–9 (relevant for most natural waters), aluminium precipitates out of water as the hydroxide and is hence not available; most elements behaving this way have no biological role or are toxic. Aluminium salts are remarkably nontoxic, having an of 6207 mg/kg (oral, mouse), which corresponds to 500 grams for an 80 kg (180 lb) person. ToxicityIn most people, aluminium is not as toxic as. Aluminium is classified as a non-carcinogen by the. There is little evidence that normal exposure to aluminium presents a risk to healthy adult, and there is evidence of no toxicity if it is consumed in amounts not greater than 40 mg/day per kg of.

Most aluminium consumed will leave the body in feces; most of the small part of it that enters the bloodstream, will be excreted via urine. EffectsAluminium, although rarely, can cause vitamin D-resistant, -resistant, and central nervous system alterations. People with kidney insufficiency are especially at a risk. Chronic ingestion of hydrated aluminium silicates (for excess gastric acidity control) may result in aluminium binding to intestinal contents and increased elimination of other metals, such as or; sufficiently high doses (50 g/day) can cause anemia.

There are five major aluminium forms absorbed by human body: the free solvated trivalent cation (Al 3+ (aq)); low-molecular-weight, neutral, soluble complexes (LMW-Al 0 (aq)); high-molecular-weight, neutral, soluble complexes (HMW-Al 0 (aq)); low-molecular-weight, charged, soluble complexes (LMW-Al(L) n +/− (aq)); nano and micro-particulates (Al(L) n(s)). They are transported across cell membranes or cell epi-/ through five major routes: (1); (2); (3); (4) channels; (5) adsorptive or receptor-mediated.During the 1988 people in had their drinking water contaminated with for several weeks. A final report into the incident in 2013 concluded it was unlikely that this had caused long-term health problems.Aluminium has been suspected of being a possible cause of, but research into this for over 40 years has found, as of 2018, no good evidence of causal effect.Aluminium increases -related in human cells cultured in the laboratory. In very high doses, aluminium is associated with altered function of the blood–brain barrier. A small percentage of people have contact to aluminium and experience itchy red rashes, headache, muscle pain, joint pain, poor memory, insomnia, depression, asthma, irritable bowel syndrome, or other symptoms upon contact with products containing aluminium.Exposure to powdered aluminium or aluminium welding fumes can cause. Fine aluminium powder can ignite or explode, posing another workplace hazard.

Exposure routesFood is the main source of aluminium. Drinking water contains more aluminium than solid food; however, aluminium in food may be absorbed more than aluminium from water.

Major sources of human oral exposure to aluminium include food (due to its use in food additives, food and beverage packaging, and cooking utensils), drinking water (due to its use in municipal water treatment), and aluminium-containing medications (particularly antacid/antiulcer and buffered aspirin formulations). Dietary exposure in Europeans averages to 0.2–1.5 mg/kg/week but can be as high as 2.3 mg/kg/week. Higher exposure levels of aluminium are mostly limited to miners, aluminium production workers, and patients.Consumption of, and cosmetics provide possible routes of exposure. Consumption of acidic foods or liquids with aluminium enhances aluminium absorption, and has been shown to increase the accumulation of aluminium in nerve and bone tissues. TreatmentIn case of suspected sudden intake of a large amount of aluminium, the only treatment is which may be given to help eliminate aluminium from the body.

However, this should be applied with caution as this reduces not only aluminium body levels, but also those of other metals such as copper or iron. Environmental effects. As aluminium technically does not come after any in the periodic table, it is excluded by some authors from the set of post-transition metals.

Nevertheless its weakly metallic behaviour is similar to that of its heavier congeners in group 13, and, which are post-transition metals by all definitions. No elements with odd atomic numbers have more than two stable isotopes; even-numbered elements have multiple stable isotopes, with tin (element 50) having the highest number of isotopes of all elements, ten. See for more details.

Most other metals have greater standard atomic weights: for instance, that of iron is 55.8; copper 63.5; lead 207.2. Abundances in the source are listed relative to silicon rather than in per-particle notation.

The sum of all elements per 10 6 parts of silicon is 2.6682 ×10 10 parts; aluminium comprises 8.410 ×10 4 parts. For instance, see the November–December 2013 issue of Chemistry International: in a table of (some) elements, the element is listed as 'aluminium (aluminum)'.References.