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Pb Intim kaufen - Die besten Pb Intim verglichen! TOMES I ET II. TOME I. Lead production declined after the fall of Rome and did not reach comparable levels until the Industrial Revolution.

In , the annual global production of lead was about ten million tonnes, over half of which was from recycling. Lead's high density, low melting point, ductility and relative inertness to oxidation make it useful.

These properties, combined with its relative abundance and low cost, resulted in its extensive use in construction, plumbing , batteries , bullets and shot , weights, solders , pewters , fusible alloys , white paints , leaded gasoline , and radiation shielding.

In the late 19th century , lead's toxicity was recognized, and its use has since been phased out of many applications.

However, many countries still allow the sale of products that expose humans to lead, including some types of paints and bullets. Lead is a neurotoxin that accumulates in soft tissues and bones; it damages the nervous system and interferes with the function of biological enzymes , causing neurological disorders, such as brain damage and behavioral problems.

A lead atom has 82 electrons , arranged in an electron configuration of [ Xe ]4f 14 5d 10 6s 2 6p 2. The sum of lead's first and second ionization energies —the total energy required to remove the two 6p electrons—is close to that of tin , lead's upper neighbor in the carbon group.

This is unusual; ionization energies generally fall going down a group, as an element's outer electrons become more distant from the nucleus , and more shielded by smaller orbitals.

The similarity of ionization energies is caused by the lanthanide contraction —the decrease in element radii from lanthanum atomic number 57 to lutetium 71 , and the relatively small radii of the elements from hafnium 72 onwards.

This is due to poor shielding of the nucleus by the lanthanide 4f electrons. The sum of the first four ionization energies of lead exceeds that of tin, [3] contrary to what periodic trends would predict.

Relativistic effects , which become significant in heavier atoms, contribute to this behavior. Lead's lighter carbon group congeners form stable or metastable allotropes with the tetrahedrally coordinated and covalently bonded diamond cubic structure.

The energy levels of their outer s- and p-orbitals are close enough to allow mixing into four hybrid sp 3 orbitals.

In lead, the inert pair effect increases the separation between its s- and p-orbitals, and the gap cannot be overcome by the energy that would be released by extra bonds following hybridization.

Lead consequently has a face-centered cubic structure [7] like the similarly sized [8] divalent metals calcium and strontium. Pure lead has a bright, silvery appearance with a hint of blue.

Characteristic properties of lead include high density , malleability, ductility, and high resistance to corrosion due to passivation. Lead's close-packed face-centered cubic structure and high atomic weight result in a density [16] of Lead is a very soft metal with a Mohs hardness of 1.

In comparison, that of aluminium is The melting point of lead—at Natural lead consists of four stable isotopes with mass numbers of , , , and , [30] and traces of five short-lived radioisotopes.

With its high atomic number, lead is the heaviest element whose natural isotopes are regarded as stable; lead is the heaviest stable nucleus. This distinction formerly fell to bismuth , with an atomic number of 83, until its only primordial isotope , bismuth, was found in to decay very slowly.

Three of the stable isotopes are found in three of the four major decay chains : lead, lead, and lead are the final decay products of uranium, uranium, and thorium, respectively.

As uranium decays into lead, their relative amounts change; this is the basis for uranium—lead dating. Apart from the stable isotopes, which make up almost all lead that exists naturally, there are trace quantities of a few radioactive isotopes.

One of them is lead; although it has a half-life of only Lead, , and are present in the decay chains of uranium, thorium, and uranium, respectively, so traces of all three of these lead isotopes are found naturally.

Minute traces of lead arise from the very rare cluster decay of radium, one of the daughter products of natural uranium, and the decay chain of neptunium, traces of which are produced by neutron capture in uranium ores.

Lead is particularly useful for helping to identify the ages of samples by measuring its ratio to lead both isotopes are present in a single decay chain.

In total, 43 lead isotopes have been synthesized, with mass numbers — Bulk lead exposed to moist air forms a protective layer of varying composition.

Lead II carbonate is a common constituent; [46] [47] [48] the sulfate or chloride may also be present in urban or maritime settings.

Fluorine reacts with lead at room temperature, forming lead II fluoride. The reaction with chlorine is similar but requires heating, as the resulting chloride layer diminishes the reactivity of the elements.

Lead metal resists sulfuric and phosphoric acid but not hydrochloric or nitric acid ; the outcome depends on insolubility and subsequent passivation of the product salt.

The tetravalent state is common for the carbon group. The divalent state is rare for carbon and silicon , minor for germanium, important but not prevailing for tin, and is the more important of the two oxidation states for lead.

The result is a stronger contraction of the lead 6s orbital than is the case for the 6p orbital, making it rather inert in ionic compounds.

The inert pair effect is less applicable to compounds in which lead forms covalent bonds with elements of similar electronegativity, such as carbon in organolead compounds.

In these, the 6s and 6p orbitals remain similarly sized and sp 3 hybridization is still energetically favorable. Lead, like carbon, is predominantly tetravalent in such compounds.

There is a relatively large difference in the electronegativity of lead II at 1. Lead II compounds are characteristic of the inorganic chemistry of lead.

Even strong oxidizing agents like fluorine and chlorine react with lead to give only PbF 2 and PbCl 2. As the chloride salt is sparingly soluble in water, in very dilute solutions the precipitation of lead II sulfide is achieved by bubbling hydrogen sulfide through the solution.

Litharge is the most commonly used inorganic compound of lead. Lead sulfide is a semiconductor , a photoconductor , and an extremely sensitive infrared radiation detector.

The other two chalcogenides, lead selenide and lead telluride , are likewise photoconducting. They are unusual in that their color becomes lighter going down the group.

Lead dihalides are well-characterized; this includes the diastatide [64] and mixed halides, such as PbFCl. The relative insolubility of the latter forms a useful basis for the gravimetric determination of fluorine.

The difluoride was the first solid ionically conducting compound to be discovered in , by Michael Faraday. Lead II sulfate is insoluble in water, like the sulfates of other heavy divalent cations.

Lead II nitrate and lead II acetate are very soluble, and this is exploited in the synthesis of other lead compounds.

Few inorganic lead IV compounds are known. They are only formed in highly oxidizing solutions and do not normally exist under standard conditions.

Lead dioxide is a strong oxidizing agent, capable of oxidizing hydrochloric acid to chlorine gas.

Lead disulfide [72] and lead diselenide [73] are only stable at high pressures. Lead tetrafluoride , a yellow crystalline powder, is stable, but less so than the difluoride.

Lead tetrachloride a yellow oil decomposes at room temperature, lead tetrabromide is less stable still, and the existence of lead tetraiodide is questionable.

Lead III may be obtained, as an intermediate between lead II and lead IV , in larger organolead complexes; this oxidation state is not stable, as both the lead III ion and the larger complexes containing it are radicals.

Numerous mixed lead II,IV oxides are known. A further sesquioxide , Pb 2 O 3 , can be obtained at high pressure, along with several non-stoichiometric phases.

Many of them show defective fluorite structures in which some oxygen atoms are replaced by vacancies: PbO can be considered as having such a structure, with every alternate layer of oxygen atoms absent.

Lead can form multiply-bonded chains , a property it shares with its lighter homologs in the carbon group. Its capacity to do so is much less because the Pb—Pb bond energy is over three and a half times lower than that of the C—C bond.

The lead analog of the simplest organic compound , methane , is plumbane. Plumbane may be obtained in a reaction between metallic lead and atomic hydrogen.

These compounds are relatively stable: tetraethyllead only starts to decompose if heated [88] or if exposed to sunlight or ultraviolet light.

Lead's per-particle abundance in the Solar System is 0. Primordial lead—which comprises the isotopes lead, lead, lead, and lead—was mostly created as a result of repetitive neutron capture processes occurring in stars.

The two main modes of capture are the s- and r-processes. In the s-process s is for "slow" , captures are separated by years or decades, allowing less stable nuclei to undergo beta decay.

Further captures result in lead, lead, and lead On capturing another neutron, lead becomes lead, which quickly decays into bismuth On capturing another neutron, bismuth becomes bismuth, and this beta decays to polonium, which alpha decays to lead The cycle hence ends at lead, lead, lead, and bismuth In the r-process r is for "rapid" , captures happen faster than nuclei can decay.

The neutron flux involved may be on the order of 10 22 neutrons per square centimeter per second. Lead is classified as a chalcophile under the Goldschmidt classification , meaning it is generally found combined with sulfur.

This accounts for lead's relatively high crustal abundance of 14 ppm; it is the 38th most abundant element in the crust.

The main lead-bearing mineral is galena PbS , which is mostly found with zinc ores. Arsenic , tin, antimony, silver , gold, copper, and bismuth are common impurities in lead minerals.

World lead resources exceed two billion tons. Significant deposits are located in Australia, China, Ireland, Mexico, Peru, Portugal, Russia, and the United States.

Global reserves—resources that are economically feasible to extract—totaled 88 million tons in , of which Australia had 35 million, China 17 million, and Russia 6.

Typical background concentrations of lead do not exceed 0. This word is related to the Latin plumbum , which gave the element its chemical symbol Pb.

Metallic lead beads dating back to — BCE have been found in Asia Minor and may represent the first example of metal smelting. These three regions collectively dominated production of mined lead until c.

Rome's territorial expansion in Europe and across the Mediterranean, and its development of mining, led to it becoming the greatest producer of lead during the classical era , with an estimated annual output peaking at 80, tonnes.

Like their predecessors, the Romans obtained lead mostly as a by-product of silver smelting. Lead tablets were commonly used as a material for letters.

In Roman times, lead sling bullets were amply used, and were effective at a distance of between and meters.

The Balearic slingers, used as mercenaries in Carthaginian and Roman armies, were famous for their shooting distance and accuracy.

Lead was used for making water pipes in the Roman Empire ; the Latin word for the metal, plumbum , is the origin of the English word " plumbing ".

Its ease of working and resistance to corrosion [] ensured its widespread use in other applications, including pharmaceuticals, roofing, currency, and warfare.

The lead conferred an agreeable taste due to the formation of "sugar of lead" lead II acetate , whereas copper or bronze vessels could impart a bitter flavor through verdigris formation.

Heinz Eschnauer and Markus Stoeppler "Wine—An enological specimen bank", []. The Roman author Vitruvius reported the health dangers of lead [] and modern writers have suggested that lead poisoning played a major role in the decline of the Roman Empire.

By association, lead was considered the father of all metals. During the classical era and even up to the 17th century , tin was often not distinguished from lead: Romans called lead plumbum nigrum "black lead" , and tin plumbum candidum "bright lead".

Pliny incorrectly wrote that stibnite would give lead on heating, instead of antimony. Lead mining in Western Europe declined after the fall of the Western Roman Empire , with Arabian Iberia being the only region having a significant output.

In Europe, lead production began to increase in the 11th and 12th centuries, when it was again used for roofing and piping. Starting in the 13th century, lead was used to create stained glass.

The use of such wine was forbidden for use in Christian rites by a papal bull in , but it continued to be imbibed and resulted in mass poisonings up to the late 18th century.

It was less damaging to iron gun barrels, had a higher density which allowed for better retention of velocity , and its lower melting point made the production of bullets easier as they could be made using a wood fire.

A similar fashion appeared in Japan in the 18th century with the emergence of the geishas , a practice that continued long into the 20th century.

The white faces of women "came to represent their feminine virtue as Japanese women", [] with lead commonly used in the whitener.

In the New World , lead production was recorded soon after the arrival of European settlers. The earliest record dates to in the English Colony of Virginia , fourteen years after its foundation.

In the second half of the 18th century, Britain, and later continental Europe and the United States, experienced the Industrial Revolution.

This was the first time during which lead production rates exceeded those of Rome. This led to research into the effects of lead intake.

Lead was proven to be more dangerous in its fume form than as a solid metal. Lead poisoning and gout were linked; British physician Alfred Baring Garrod noted a third of his gout patients were plumbers and painters.

The effects of chronic ingestion of lead, including mental disorders, were also studied in the 19th century. The first laws aimed at decreasing lead poisoning in factories were enacted during the s and s in the United Kingdom.

Further evidence of the threat that lead posed to humans was discovered in the late 19th and early 20th centuries. Mechanisms of harm were better understood, lead blindness was documented, and the element was phased out of public use in the United States and Europe.

The United Kingdom introduced mandatory factory inspections in and appointed the first Medical Inspector of Factories in ; as a result, a fold decrease in lead poisoning incidents from to was reported.

The last major human exposure to lead was the addition of tetraethyllead to gasoline as an antiknock agent , a practice that originated in the United States in It was phased out in the United States and the European Union by In the s, the United States and Western European countries introduced legislation to reduce lead air pollution.

As of , production of lead is increasing worldwide due to its use in lead—acid batteries. In , 4. The top three producers of mined lead concentrate in that year were China, Australia, and the United States.

The primary and secondary lead production processes are similar. Some primary production plants now supplement their operations with scrap lead, and this trend is likely to increase in the future.

Given adequate techniques, lead obtained via secondary processes is indistinguishable from lead obtained via primary processes. Scrap lead from the building trade is usually fairly clean and is re-melted without the need for smelting, though refining is sometimes needed.

There are two main ways of doing this: a two-stage process involving roasting followed by blast furnace extraction, carried out in separate vessels; or a direct process in which the extraction of the concentrate occurs in a single vessel.

The latter has become the most common route, though the former is still significant. First, the sulfide concentrate is roasted in air to oxidize the lead sulfide: [].

As the original concentrate was not pure lead sulfide, roasting yields not only the desired lead II oxide, but a mixture of oxides, sulfates, and silicates of lead and of the other metals contained in the ore.

Impurities are mostly arsenic, antimony, bismuth, zinc, copper, silver, and gold. Typically they are removed in a series of pyrometallurgical processes.

The melt is treated in a reverberatory furnace with air, steam, and sulfur, which oxidizes the impurities except for silver, gold, and bismuth.

Oxidized contaminants float to the top of the melt and are skimmed off. Zinc, which is immiscible in lead, dissolves the silver and gold.

The zinc solution can be separated from the lead, and the silver and gold retrieved. The resulting bismuth dross can be skimmed off.

Alternatively to the pyrometallurgical processes, very pure lead can be obtained by processing smelted lead electrolytically using the Betts process.

Anodes of impure lead and cathodes of pure lead are placed in an electrolyte of lead fluorosilicate PbSiF 6. Once electrical potential is applied, impure lead at the anode dissolves and plates onto the cathode, leaving the majority of the impurities in solution.

In this process, lead bullion and slag is obtained directly from lead concentrates. The lead sulfide concentrate is melted in a furnace and oxidized, forming lead monoxide.

Carbon as coke or coal gas [p] is added to the molten charge along with fluxing agents. The lead monoxide is thereby reduced to metallic lead, in the midst of a slag rich in lead monoxide.

For a low-grade feed, all of the lead can be oxidized to a high-lead slag. Research on a cleaner, less energy-intensive lead extraction process continues; a major drawback is that either too much lead is lost as waste, or the alternatives result in a high sulfur content in the resulting lead metal.

Hydrometallurgical extraction, in which anodes of impure lead are immersed into an electrolyte and pure lead is deposited onto a cathode, is a technique that may have potential, but is not currently economical except in cases where electricity is very cheap.

Smelting, which is an essential part of the primary production, is often skipped during secondary production. It is only performed when metallic lead has undergone significant oxidation.

Of the sources of lead for recycling, lead—acid batteries are the most important; lead pipe, sheet, and cable sheathing are also significant.

Contrary to popular belief, pencil leads in wooden pencils have never been made from lead. When the pencil originated as a wrapped graphite writing tool, the particular type of graphite used was named plumbago literally, act for lead or lead mockup.

Lead metal has several useful mechanical properties, including high density, low melting point, ductility, and relative inertness.

Many metals are superior to lead in some of these aspects but are generally less common and more difficult to extract from parent ores.

Lead's toxicity has led to its phasing out for some uses. Lead has been used for bullets since their invention in the Middle Ages. It is inexpensive; its low melting point means small arms ammunition and shotgun pellets can be cast with minimal technical equipment; and it is denser than other common metals, which allows for better retention of velocity.

It remains the main material for bullets, alloyed with other metals as hardeners. Lead's high density and resistance to corrosion have been exploited in a number of related applications.

It is used as ballast in sailboat keels; its density allows it to take up a small volume and minimize water resistance, thus counterbalancing the heeling effect of wind on the sails.

Lead has many uses in the construction industry; lead sheets are used as architectural metals in roofing material, cladding , flashing , gutters and gutter joints, and on roof parapets.

Lead is added to copper alloys, such as brass and bronze, to improve machinability and for its lubricating qualities. Being practically insoluble in copper the lead forms solid globules in imperfections throughout the alloy, such as grain boundaries.

In low concentrations, as well as acting as a lubricant, the globules hinder the formation of swarf as the alloy is worked, thereby improving machinability.

Copper alloys with larger concentrations of lead are used in bearings. The lead provides lubrication, and the copper provides the load-bearing support.

Lead's high density, atomic number, and formability form the basis for use of lead as a barrier that absorbs sound, vibration, and radiation.

The largest use of lead in the early 21st century is in lead—acid batteries. The lead in batteries undergoes no direct contact with humans, so there are fewer toxicity concerns.

Lead is used in high voltage power cables as sheathing material to prevent water diffusion into insulation; this use is decreasing as lead is being phased out.

In addition to being the main application for lead metal, lead-acid batteries are also the main consumer of lead compounds. Other applications of lead compounds are very specialized and often fading.

Lead-based coloring agents are used in ceramic glazes and glass, especially for red and yellow shades. Lead is frequently used in the polyvinyl chloride coating of electrical cords.

Because of its toxicity, European and North American manufacturers use alternatives such as zinc. Lead has no confirmed biological role, and there is no confirmed safe level of lead exposure.

Only about a third of lead is excreted by a child. Continual exposure may result in the bioaccumulation of lead. Lead is a highly poisonous metal whether inhaled or swallowed , affecting almost every organ and system in the human body.

It does so by binding to the sulfhydryl groups found on many enzymes, [] or mimicking and displacing other metals which act as cofactors in many enzymatic reactions.

Lead can cause severe damage to the brain and kidneys and, ultimately, death. By mimicking calcium, lead can cross the blood—brain barrier.

It degrades the myelin sheaths of neurons , reduces their numbers, interferes with neurotransmission routes, and decreases neuronal growth.

This causes ineffective heme synthesis and microcytic anemia. Symptoms of lead poisoning include nephropathy , colic -like abdominal pains, and possibly weakness in the fingers, wrists, or ankles.

Small blood pressure increases, particularly in middle-aged and older people, may be apparent and can cause anemia. Several studies, mostly cross-sectional, found an association between increased lead exposure and decreased heart rate variability.

Chronic, high-level exposure has been shown to reduce fertility in males. In a child's developing brain, lead interferes with synapse formation in the cerebral cortex , neurochemical development including that of neurotransmitters , and the organization of ion channels.

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