Aluminum–a.k.a.Aluminium
Atomic Number: 13
Symbol: Al
History: In 1761, Guyton de Morveau suggested calling the base alum alumine. In 1808, Humphry Davy identified the existence of a metal base of alum, which he at first termed aluminum and later aluminum.
Applications/Uses: Aluminum and its alloys are used because they are easy to form, readily available, inexpensive, and recyclable.
Copper
Atomic Number: 29
Symbol: Cu
History: Copper and its alloys have been used for thousands of years. In the Roman era, copper was principally mined on Cyprus, hence the origin of the name of the metal as cyprium (metal of Cyprus), later shortened to cuprum.
Applications/Uses: Copper and copper alloys have a number of properties that make them useful, including high electrical and thermal conductivity, high ductility, and good corrosion resistance.
Brass
Atomic Number:
Symbol:
History: Brass, which is an alloy of copper and zinc, has been used since at least the 10th century BC.
Applications/Uses: Brass is a substitutional alloy. It is used for decoration for its bright gold-like appearance; for applications where low friction is required such as locks, gears, bearings, doorknobs, ammunition, and valves; for plumbing and electrical applications; and extensively in musical instruments such as horns and bells for its acoustic properties. It is also used in zippers.
Invar
Atomic Number:
Symbol: FeNi36
History: Invar, also known generically as FeNi36 (64FeNi in the US), is a nickel iron alloy. The name, Invar, comes from the word invariable, referring to its lack of expansion or contraction with temperature changes.
Applications/Uses: Invar is used where high dimensional stability is required, such as precision instruments, clocks, seismic creep gauges, television shadow-mask frames, valves in motors, and antimagnetic watches.
Iron
Atomic Number:26
Symbol: Fe
History: Iron metal has been used since ancient times.
Applications/Uses: Iron is the most widely used of all the metals and is used for construction of machinery and machine tools, automobiles, the hulls of large ships, and structural components for buildings. Since pure iron is quite soft, it is most commonly used in the form of steel.
Chromium
Atomic Number:24
Symbol: Cr
History: The name of the element is derived from the Greek word ‘chroma’, meaning colour,[2] because many of its compounds are intensely coloured. Chromium oxide was used by the Chinese in the Qin dynasty over 2,000 years ago to coat weapons such as bronze crossbow bolts and steel swords found at the Terracotta Army.
Applications/Uses: Steel is made highly resistant to corrosion and discoloration by adding chromium to form stainless steel. Chrome plating (electroplating with chromium) is another major use. Dye and pigment – like chrome yellow & chrome red. Chromium is used in producing synthetic rubies. Preservation of wood. Tanning of leather.
Vanadium
Atomic Number:23
Symbol: V
History: Vanadium occurs naturally in about 65 different minerals and in fossil fuel deposits. Although Berzelius claimed to have first isolated vanadium in the 1830s, in 1867 Henry Enfield Roscoe showed that he had only obtained the oxide, and finally in 1869 Roscoe demonstrated a method to obtain the pure element.
Applications/Uses: Vanadium pentoxide is used as a catalyst for the production of sulfuric acid. Vanadium forms stable nitrides and carbides, resulting in a significant increase in the strength of the steel.
Tungsten
Atomic Number:74
Symbol: W
History: Tungsten is also known as wolfram.The word tungsten comes from the Swedish language ‘tung sten’ directly translatable to heavy stone, though the name is volfram in Swedish to distinguish it from Scheelite, in Swedish alternatively named tungsten. It was identified as a new element in 1781, and first isolated as a metal in 1783.
Applications/Uses: Tungsten’s alloys are used in incandescent light bulb filaments, X-ray tubes (as both the filament and target), electrodes in TIG welding, and superalloys. High speed steel can contain as much as 18% tungsten. Superalloys containing tungsten, such as Hastelloy and Stellite, are used in turbine blades and wear-resistant parts and coatings.
Lead
Atomic Number:82
Symbol: Pb
History: Lead’s symbol Pb is an abbreviation of its Latin name plumbum for soft metals; the English words “plumbing”, “plumber”, “plumb”, and “plumb-bob” also derive from this Latin root.
Applications/Uses: Lead has been commonly used for thousands of years because it is widespread, easy to extract and easy to work with. It is highly malleable as well as easy to smelt. It has been commonly used for small arms ammunition and shotgun pellets. lead is used for the ballast keel of sailboats. It is used in solder for electronics.
Magnesium
Atomic Number:12
Symbol: Mg
History: The name magnesium originates from the Greek word for a district in Thessaly called Magnesia. The metal itself was first produced by Sir Humphry Davy in England in 1808 using electrolysis of a mixture of magnesia and mercuric oxide.
Applications/Uses: In vegetation magnesium is the metallic ion at the center of chlorophyll, and is thus a common additive to fertilizers. Magnesium compounds are used medicinally as common laxatives, antacids (e.g., milk of magnesia). Magnesium ions help to impart a natural tartness to fresh mineral waters.
Manganese
Atomic Number:25
Symbol: Mn
History: Johan Gottlieb Gahn was the first to isolate an impure sample of manganese metal in 1774. It is found as a free element in nature (often in combination with iron), and in many minerals.
Applications/Uses: Manganese is a metal with important industrial metal alloy uses, particularly in stainless steels.
Tin
Atomic Number:50
Symbol: Sn
History: Tin is known as stannum in Latin. Tin extraction and use can be dated to the beginnings of the Bronze Age around 3000 BC. After 600 BC pure metallic tin was produced.
Applications/Uses: Tin is used in many alloys, most notably tin/lead soft solders. A large application for tin is corrosion-resistant tin plating of steel. Because of its low toxicity, tin-plated metal is also used for food packaging, giving the name to tin cans, which are made mostly of steel.
Titanium
Atomic Number:22
Symbol: Ti
History: Titanium was discovered in Cornwall, Great Britain, by William Gregor in 1791 and named by Martin Heinrich Klaproth for the Titans of Greek mythology.
Applications/Uses: Titanium alloys are used for strength in higher temperature (~1000° F) application, when component weight is a concern, or when good corrosion resistance is required. Titanium can be alloyed with iron, aluminium, vanadium, molybdenum, among other elements, to produce strong lightweight alloys for aerospace (jet engines, missiles, and spacecraft), military, industrial process (chemicals and petro-chemicals, desalination plants, pulp, and paper), automotive, agri-food, medical prostheses, orthopedic implants, dental and endodontic instruments and files, dental implants, sporting goods, jewelry, mobile phones, and other applications.
Bronze
Atomic Number:
Symbol:
History: Bronze is a metal alloy consisting primarily of copper, usually with tin as the main additive. The earliest tin-alloy bronzes date to the late 4th millennium BC in Susa (Iran) and some ancient sites in China, Luristan (Iran) and Mesopotamia (Iraq).
Applications/Uses: Bronze was especially suitable for use in boat and ship fittings prior to the wide employment of stainless steel owing to its combination of toughness and resistance to salt water corrosion. Bronze is still commonly used in ship propellers and submerged bearings. Indian Hindu artisans from the period of the Chola empire in Tamil Nadu, used bronze to create intricate statues via the lost wax casting method with ornate detailing depicting the Gods. Bronze is the preferred metal for top-quality bells, particularly bell metal, which is about 23% tin.
Pewter
Atomic Number:
Symbol:
History: Pewter was first used around the beginning of the Bronze Age in the Near East (Middle East). The earliest piece of pewter found is from an Egyptian tomb from 1450 BCE. Pewter is a malleable metal alloy, traditionally 85–99% tin, with the remainder consisting of copper, antimony, bismuth and (sometimes, and less commonly today) lead.
Applications/Uses: Pewter is used for items including porringers, plates, dishes, basins, spoons, measures, flagons, communion cups, teapots, sugar bowls, beer steins, and cream jugs. In the early 19th century, changes in fashion caused a decline in the use of pewter flatware. Today, pewter is used in decorative objects, mainly collectible statuettes and figurines, game figures, aircraft and other models, (replica) coins, pendants, plated jewelry.
Nickel
Atomic Number: 28
Symbol: Ni
History: The use of nickel (as a natural meteoric nickel–iron alloy) has been traced as far back as 3500 BC. Nickel was first isolated and classified as a chemical element in 1751 by Axel Fredrik Cronstedt.
Applications/Uses: Nickel alloys are used for still higher temperatures (~1500-2000° F) applications or when good corrosion resistance is required. 60% of world production is used in nickel-steels (particularly stainless steel). Other uses include alnico magnets, coinage, rechargeable batteries, electric guitar strings, microphone capsules, and special alloys. It is used as a catalyst for hydrogenation. Enzymes of some microorganisms and plants contain nickel as an active site, which makes the metal an essential nutrient for them.
Antimony
Atomic Number:51
Symbol:Sb
History: Antimony is known as ‘stibium’ in Latin. Antimony compounds have been known since ancient times and were used for cosmetics; metallic antimony was also known, but it was erroneously identified as lead. It was established to be an element around the 17th century.
Applications/Uses: The largest applications for metallic antimony are as alloying material for lead and tin and for lead antimony plates in lead-acid batteries. Antimony compounds are prominent additives for chlorine- and bromine-containing fire retardants found in many commercial and domestic products. An emerging application is the use of antimony in microelectronics. Normally the compounds of S and P-Block elements are colours block Red, Green, Pure Red, Yellow, and Grey etc. While those of transition metals in the solid or in solution states are usually coloured.
The colours of hydrated captions of transition metals of the first transition series are: Sc3+, Ti4+(3D, N=O- colourless: Ti3_(3D1, N=1)-Block Red: V3+(3D2+N=2)- Green: V2 ( 3D3, N=3)-pure Red CR3+(3D3;N=3)- Yellow: CR2+ (3D4, N=4) Blue: Mn3+(3D4, N=4) Grey: Mn2 + (3D5, N=5)- Yellow: Fe2_(3D6, N=4) here n denotes the number of coloures.
For simplicity water molecules associated with each cation have not been shown. It may be seen from colours given above that the captions (e.g. Sc3+Ti4,+CU+,Zn2+) having vacant or completely felted D-Orbitals (D0 and D10 Orbital’s) are colourless while those 9E.G. Ti3+ V3+, Cr3+ etc) having partially-filled D-Orbitals (D1,D2,D3 etc, Orbital’s) are coloured.
In other words the captions having called the trichloride paired in D-Orbital’s (i.e. empty D-Orbitals) are colourless while those having some or all the electrons unpaired in D-Orbitals are coloured. Ih N is the number of unpaired electrons in D-Orbitals, then the Ions having N=0 are colourless while those having N=1, 2etc. are coloured.
M+ 2H+ (from acid)-------------------M2 +H2(G) in actual practice, the rate with which most of these metals react with acid and liberate H2 gas is wary slow.
Some of the metals get protected from further attack of the acids due to the formation of a thin protective layer of their oxide which prevents the acid to come in further contact with the metal, e.g., although the electrode potential of CR is much less than that of trichloride(eD cR3+=-0.71 volt), it gets coated with is non-reactive oxide, cR203 which makes it so uncreative that can be used as a protective non-oxidising metal (II) in spite of the fact that all the metals of first transition series expecting Cu, have high negative values of standard electrode potentials, these are not as good reducing agents as the metal of groups IA, IIA and IIIA.
The poor reducing capacity of the transition metals is due to high heats of vaporization, high ionization potentials and low heats of hydration of their ions.