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Metals Mahum Mujeeb 8A

+Aluminum (Al)

Discoverer: Hans Christian Oersted

Discovery Location: Copenhagen, Denmark

Discovery Year: 1825

Ancient Greeks and Romans used alum as an astringent, for medicinal purposes, and as a

mordant in dyeing. It is used in kitchen utensils, exterior decorations, and thousands of industrial applications. Although the electrical conductivity of aluminum is only about 60% that of copper per

area of cross section, aluminum is used in electrical transmission lines because of its light weight. The alloys of aluminum are used in the construction of aircraft and rockets. Reflective

aluminum coatings are used for telescope mirrors, making decorative paper, packaging, and many other uses. Alumina is used in glassmaking and refractoriness. Synthetic ruby and sapphire have

applications in producing coherent light for lasers.

Aluminum has a melting point of 660.37°C, boiling point of 2467°C, specific gravity of

2.6989 (20°C), and valence of 3. Pure aluminum is a silvery-white metal. It is soft, light, relatively nontoxic, with a high thermal conductivity, and high corrosion resistance. It

can be easily formed, machined, or cast. Aluminum is nonmagnetic and nonspeaking. It

is second among metals in terms of malleability and sixth in ductility. Aluminum coatings are highly reflective of both visible and radiant heat. The coatings form a thin

layer of protective oxide and do not deteriorate like silver coatings.

The alumina must be molten for electrolysis to work,Unfortunately, alumina has a high melting point (2040 °C)and it is not practical to do electrolysis at such a high temperature. A solution of alumina in cryolite melts at about 900 °Cand electrolysis is done at about 950 °C.

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AluminumOn the right are some pictures of Aluminum and where they can be used.

+Calcium (Ca)

Discoverer: Sir Humphy DavyDiscovery Location: London

Year: 1808

Calcium is essential for human nutrition. Animals skeletons get their rigidity primarily

from calcium phosphate. The eggs of birds and shells of mollusks are comprised of calcium

carbonate. Calcium is also necessary for plant growth. Calcium is used as a reducing agent

when preparing metals from their halogen and oxygen compounds; as a reagent in

purification of inert gases; to fix atmospheric nitrogen; as a scavenger and decarbonizes in metallurgy; and for making alloys. Calcium compounds are used in making lime, bricks, cement, glass, paint, paper, sugar, glazes, as

well as for many other uses.

The melting point of calcium is 839 +/- 2°C, boiling point is 1484°C, specific gravity is 1.55

(20°C), with a valence of 2. Calcium is a silvery white, soft alkaline earth metal.

Although none of the alkaline earths occur free in nature, calcium compounds are abundant.

1. Grinding, crushing , wet milling and screening, particle size fractionation. The calcium carbonate so obtained is normally delivered to the consumer (such as paper mills

for paper coating, wet end filler for the production of neutral or alkaline sized papers) in slurry form. The solids

content of the slurry is high, near to 65 - 70%, various deflocculates are used to maintain a very low viscosity

even with the high solids.2. 2. The limestone is fired in a furnace to convert the calcium carbonate to calcium oxide. The CaO is delivered to the customer as a bulk powder where it is made into a Ca(OH)2 slurry with water. Carbon dioxide is then added

to the slurry to reform Calcium Carbonate, This latter process yields a carbonate with controlled characteristics

such as particle size and particle size distribution. This method is used for calcium carbonate used in the

pharmaceutical industry as a vey pure carbonate is obtained.

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CalciumOn the right are some pictures of Calcium and where they can be used.

+Iron (Fe)

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Unfortunately, no one knows who was the first person to discover iron. Iron has been used since prehistory. The Ancient Egyptians and Sumerians began using iron on the tips of

spears and in some ornaments around 4000 BC. They obtained the iron from meteorites that hit the earth. Sometime between 2000 and 1200 BC the smelting of iron (that is,

obtaining iron metal from iron ore) began in either India, Anatolia or Caucasus. We don’t

know who was the first to invent this process as artifacts containing iron are found

throughout the history of these civilizations

Iron is vital to plant and animal life. In humans, it appears in the hemoglobin molecule. Iron metal is usually alloyed with other metals and carbon for commercial uses. Pig iron is an alloy containing

about 3-5% carbon, with varying quantities of Si, S, P, and Mn. Pig iron is brittle, hard, and fairly fusible and is used to produce other iron alloys, including steel. Wrought iron contains only a few tenths of a percent of carbon and is malleable,

tough, and less fusible than pig iron. Wrought iron typically has a fibrous structure. Carbon steel is an iron alloy with carbon and small amounts of S, Si,

Mn, and P. Alloy steels are carbon steels that contain additives such as chromium, nickel,

vanadium, etc. Iron is the least expensive, most abundant, and most used of all metals.

The melting point of iron is 1535°C, boiling point is 2750°C, specific gravity is 7.874

(20°C), with a valence of 2, 3, 4, or 6. Pure iron is chemically reactive and corrodes

rapidly, especially in moist air or at elevated temperatures. Four allotropic forms, or ferrites, are known: a, b, g, and d, with

transition points at 770, 928, and 1530°C. The a form is magnetic, but when iron is

transformed into the b form, the magnetism disappears, although the lattice remains

unchanged.

Iron ore consists mostly of oxygen and iron atoms bonded together into molecules. To convert these

oxides of iron to metallic iron, they must be smelted or sent through a direct reduction process to remove

the oxygen. Oxygen-iron bonds are strong, and to remove the iron from the oxygen, a stronger

elemental bond must be presented to attach to the oxygen. Carbon is used because the strength of a

carbon-oxygen bond is greater than that of the iron-oxygen bond, and the process is done at high

temperatures. The iron ore must be powdered and mixed with coke, which is essentially carbon, and

the combination must be burnt in the smelting process. The carbon dioxide byproduct goes off into the atmosphere and what is left is almost pure iron.

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IronOn the right are some pictures of Iron and where they can be used.

+Mercury (Hg)

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The Babylonians, among the first people groups of early civilization, is credited to be

the first to put on record the use of the element mercury. This was some 3000 years

ago when it was mixed freely with other products. It was then sometimes added in

creams and ointments in dangerous proportions because it was not yet known then as a chemical element. At times poisoning was

the result. The discovery of mercury as an element was in the 18th century.

Mercury is amalgamated with gold to facilitate the recovery of gold from its ores. Mercury is used to make thermometers, diffusion pumps,

barometers, mercury vapor lamps, mercury switches, pesticides, batteries, dental preparations,

antifouling paints, pigments, and catalysts. Many of the salts and organic mercury compounds are

important.Mercury has a melting point of -38.842°C, boiling point

of 356.58°C, specific gravity of 13.546 (20°C), and a valence of 1 or 2. Mercury is one of the few elements

that is liquid at ordinary room temperatures. Mercury is a heavy, silvery-white metal. It is a relatively poor

conductor of heat, but a fair conductor of electricity. Mercury readily forms alloys with other metals, called

amalgams. An electrical discharge will cause mercury to combine with the noble gases argon, krypton, neon, and

xenon. Mercury and its compounds are highly poisonous. Mercury is readily absorbed across unbroken skin or though the respiratory or gastrointestinal tract. It acts as a cumulative poison. Mercury is very volatile in

air. When room temperature air (20°C) is saturated with mercury vapor, the concentration greatly exceeds the

toxic limit. The concentration, and thus the danger, increases at higher temperatures.

1. Cinnabar ore occurs in concentrated deposits located at or near the surface. About 90% of these deposits are deep enough to require underground mining with tunnels. The remaining 10% can be

excavated from open pits.1 Cinnabar is dislodged from the surrounding rocks by drilling and blasting with explosives or by the use of power equipment.

The ore is brought out of the mine on conveyor belts or in trucks or trains.

2. Commercial-grade mercury is poured into wrought-iron or steel flasks and sealed. Each flask contains 76 lb (34.5 kg) of mercury. Higher purity mercury is usually sealed in smaller glass or plastic containers

for shipment.

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MercuryOn the right are some pictures of Mercury and where they can be used.

+Potassium (K)

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Discoverer: Sir Humphrey Davy

Discover Location: LondonYear: 1807

Potash is in high demand as a fertilizer. Potassium, found in most

soils, is an element that is essential for plant growth. An alloy of potassium and sodium is used

as a heat transfer medium. Potassium salts have many

commercial uses.

Potassium's melting point is 63.25°C, boiling point is 760°C, specific gravity is

0.862 (20°C), with a valence of 1. Potassium is one of the most reactive and electropositive of metals. The only metal that is lighter than potassium is lithium. The silvery white metal is soft (easily cut

with a knife). The metal must be stored in a mineral oil, such as kerosene, as it oxidizes

rapidly in air and catches fire spontaneously when exposed to water. Its decomposition in water evolves hydrogen.

Potassium and its salts will color flames violet.

Potassium is gained either immediately by electrolysis of Potassium salts or

by reaction of Na with Potassium salts. Potassium is relatively easy to purify once it has been produced by

either method, though "crude" commercial potassium is often sold directly after electrolysis. Obviously,

both processes require very high temperature, as Potassium salts

have to be molten to conduct electricity.

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PotassiumOn the right are some pictures of Potassium and where they can be used.

+Magnesium (Mg)

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Discoverer: Joseph BlackDiscovered Location: Bordeux ,

FranceYear: 1755

Magnesium is used in pyrotechnic and incendiary devices. It is alloyed with other metals to make

them lighter and more easily welded, with applications in the aerospace industry. Magnesium

is added to many propellants. It is used as a reducing agent in the preparation of uranium and

other metals that are purified from their salts. Magnetite is used in refectories. Magnesium hydroxide (milk of magnesia), sulfate (Epsom

salts), chloride, and citrate are used in medicine. Organic magnesium compounds have many uses.

Magnesium is essential for plant and animal nutrition. Chlorophyll is a magnesium-centered

porphyry.

Magnesium has a melting point of 648.8°C, boiling point of 1090°C, specific gravity of 1.738 (20°C), and valence of 2. Magnesium metal is light (one-third lighter

than aluminum), silvery-white, and relatively tough. The metal

tarnishes slightly in air. Finely divided magnesium ignites upon

heating in air, burning with a bright white flam

Magnesium metal is strong reducing agent and therefore, cannot be obtained by chemical reduction

method. It is extracted by electrolysis of fused anhydrous salts. A number of methods are available

for the extraction of magnesium metal from its ores. The most widely

used method is based on the electrolysis of magnesium chloride

obtained from the seawater.

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MagnesiumOn the right are some pictures of Magnesium and where they can be used.

+Titanium (Ti)

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Discoverer: William GregorDiscovered Location: England

Year: 1791

Titanium is important for alloying with aluminum, molybdenum, iron, manganese, and other metals. Titanium alloys are used in situations

where lightweight strength and ability to withstand temperature extremes are required (e.g., aerospace applications). Titanium may

be used in desalination plants. The metal is frequently used for components which must be exposed to seawater. A titanium anode

coated with platinum may be used to provide cathodic corrosion protection from seawater. Because it is inert in the body, titanium metal has surgical applications. Titanium dioxide is used to make

man-made gemstones, although the resulting stone is relatively soft. The asterism of star sapphires and rubies is a result of the present of

TiO2. Titanium dioxide is used in house paint and artist paint. The paint is permanent and provides good coverage. It is an excellent

reflector of infrared radiation. The paint is also used in solar observatories. Titanium oxide pigments account for the largest use of

the element. Titanium oxide is used in some cosmetics to disperse light. Titanium tetrachloride is used to iridize glass. Since the

compound fumes strongly in air, it is also used to produce smoke screens.

Titanium has a melting point of 1660 +/- 10°C, boiling point of 3287°C, specific gravity of 4.54, with a valence of 2, 3, or 4. Pure titanium is a lustrous white metal with low density, high strength, and high corrosion resistance. It is resistant to dilute

sulfuric and hydrochloric acids, moist chlorine gas, most organic acids, and chloride solutions. Titanium is only ductile when it is free of oxygen. Titanium burns in air and is the only

element that burns in nitrogen. Titanium is dimorphic, with the hexagonal a form slowly changing to the cubic be form around 880°C. The metal combines with oxygen at red heat

temperatures and with chlorine at 550°C. Titanium is as strong as steel, but it is 45% lighter. The metal is 60% heavier

than aluminum, but it is twice as strong. Titanium metal is considered to be physiologically inert. Pure titanium dioxide is reasonably clear, with an extremely high index of refraction

and an optical dispersion higher than that of diamond. Natural titanium becomes highly radioactive upon bombardment with

deuterons.

Conversion of titanium (IV) oxide, TiO2, into titanium(IV) chloride, TiCl4The ore rutile (impure titanium(IV) oxide) is heated with chlorine and coke at a temperature of about 900°C. Other metal chlorides are formed as well because of other metal compounds in the ore. Very pure liquid titanium (IV) chloride can be separated from the other chlorides by fractional distillation under an argon or nitrogen atmosphere, and is stored in totally dry tanks.

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TitaniumOn the right are some pictures of Titanium and where they can be used.

+Zinc (Zn)

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Discoverer: Andreas MarggrafDiscovered Location: Germany

Year: 1746

Zinc is used to form numerous alloys, including brass, bronze, nickel silver, soft solder, Geman silver, spring brass, and aluminum solder. Zinc is used to make die

castings for use in the electrical, automotive, and hardware industries. The alloy Prestal, consisting of 78% zinc and 22% aluminum, is nearly as strong as steel yet exhibits

super plasticity. Zinc is used to galvanize other metals to prevent corrosion. Zinc oxide is used in paints, rubbers,

cosmetics, plastics, inks, soap, batteries, pharmaceuticals, and many other products. Other zinc compounds are also

widely used, such as zinc sulfide (luminous dials and fluorescent lights) and ZrZn2 (ferromagnetic materials).

Zinc is an essential element for humans and other animal nutrition. Zinc-deficient animals require 50% more food to gain the same weight as animals with sufficient zinc. Zinc

metal is not considered toxic, but if fresh zinc oxide is inhaled it can cause a disorder referred to as zinc chills or

oxide shakes.

Zinc has a melting point of 419.58°C, boiling point of 907°C, specific gravity of 7.133 (25°C),

with a valence of 2. Zinc is a lustous blue-white metal. It is

brittle at low temperatures, but becomes malleable at 100-150°C. It is a fair electrical conductor. Zinc

burns in air at high red heat, evolving white clouds of zinc oxide.

Add hydrochloric acid. The zinc will form zinc chloride and the sand will remain unchanged. You can then filter it to get the zinc chloride dissolved in the filtered solution and the sand left in the filter.

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ZincOn the right are some pictures of Titanium and where they can be used.

+Extractions

+ Chemical series produced by arranging the

metals in order of their ease of reaction with reagents such as oxygen, water, and acids. An example of such an arrangement, starting with the most reactive, is: potassium, sodium, calcium, magnesium, aluminum, zinc, iron, tin, lead, copper, silver, gold. This arrangement aids the understanding of the properties of metals, helps to explain differences between them, and enables predictions to be made about a metal's behavior, based on a knowledge of its position or properties. It also allows prediction of the relative stability of the compounds formed by an element: the more reactive the metal, the more stable its compounds are likely to be.

The position of a metal in the series determines the reactions of the metal with various reagents, the displacement of one metal from its compound by another metal, and the method of extraction of a metal from its ore.

Reactivity Series

+Timeline Of Events This is the timeline of the metals I did just before. As you can see from above going down it shows which time period each metal was discovered. First Mercury was discovered by the Babylonians and then Iron was later discovered by the Egyptians. We do not know the exact time periods but we do the the tribes and civilizations which discovered it. Next Zinc and Magnesium were discovered only 9 years away from each other. Later in 1791, Titanium was discovered. In 1807 Calcium was discovered and a year after that Potassium was discovered. In 1826 Aluminum was discovered.

Metal: Date Discovered:Mercury BabylonianIron EgyptianZinc 1746Magnesium 1755Titanium 1791Calcium 1807Potassium 1808Aluminum 1825

+AOI Relating to Metals Metals are well suited to sustainable development goals. They are not biodegradable

and have virtually an unlimited lifespan and the potential for unlimited recyclability. Thus metals can be considered as renewable materials. However mineral resources, the source of primary metals, are “non-renewable” as their supply is finite, but this does not necessarily mean scarcity. In this paper the results from a series of Life Cycle Assessments of primary metal production processes for copper, nickel, lead, zinc, aluminum and steel have been used to examine how metals may contribute to society’s transition to sustainable development. Particular issues considered include: •

Current metal reserves and how these may change in the future,

Some of the environmental impacts (Total Energy, Global Warming Potential and Acidification Potential) associated with primary metal production and how they will be exacerbated by declining ore grades

New processing technologies with lower energy consumptions and improved metal extraction efficiencies that will reduce reserve depletion and environmental impacts,

Increasing the utilization of “metals in use” by recycling, with particular reference to aluminum, •

The potential impact of a carbon tax on metal prices and how this may influence the ways in which metals are used in the future.

Human Ingenuity

+The End By Mahum Mujeeb 8A