Copper properties and uses. Introduction. Picture 7. Copper's anti-bacterial and corrosion resistant properties help make it ideal for beer brewing vessels. Corrosion resistant Copper is low in the reactivity series . This means that it doesn't tend to corrode. Again, this is important for its use for pipes, electrical cables, saucepans and radiators. However, it also means that it is well suited to decorative use. Jewellery, statues and parts of buildings can be made from copper, brass or bronze and remain attractive for thousands of years. Antibacterial Copper is a naturally hygienic metal that slows down the growth of germs such as E-coli (the “burger bug”), MRSA (the hospital “superbug”) and legionella. This is important for applications such as food preparation, hospitals, coins (see biocidal copper ), door knobs and plumbing systems. Picture 8. Brazing copper pipes to make a strong joint. Picture 9. Brass can be polished up to give an attractive gold finish. Easily joined Copper can be joined easily by soldering or brazing . This is useful for pipework and for making sealed copper vessels. Ductile Copper is a ductile metal.

This means that it can easily be shaped into pipes and drawn into wires. Copper pipes are lightweight because they can have thin walls. They don't corrode and they can be bent to fit around corners. The pipes can be joined by soldering and they are safe in fires because they don't burn or support combustion. Tough Copper and copper alloys are tough . This means that they were well suited to being used for tools and weapons. Imagine the joy of ancient man when he discovered that his carefully formed arrowheads no longer shattered on impact. The property of toughness is vital for copper and copper alloys in the modern world. They do not shatter when they are dropped or become brittle when cooled below 0 °C. Non magnetic Copper is non magnetic and non sparking. Because of this, it is used in special tools and military applications. Attractive colour Copper and its alloys , such as brass, are used for jewellery and ornaments. They have an attractive golden colour which varies with the copper content. They have a good resistance to tarnishing making them last a long a time. Picture 10. Roll over the properties above to see which metals give copper alloys those properties. Alloys easily Copper can be combined with other metals to make alloys .

The most well known are brass and bronze . Although copper has excellent electrical and thermal properties, it needs to be hardened and strengthened for many industrial applications. It is therefore mixed with other metals and melted. The liquid metals form a solution which, when they solidify, are called alloys. Some copper alloys are: brass: copper + zinc Picture 11. Copper hot water cylinders (background) are shredded and compressed into bales (front right) for recycling. Recyclable Copper can be recycled without any loss of quality. 40% of the world's demand is met by recycled copper (see extracting copper ). Catalytic compounds Copper can act as a catalyst . For example, it speeds up the reaction between zinc and dilute sulphuric acid. It is found in some enzymes , one of which is involved in respiration . So it really is a vital element. Question 5 The table shows some uses of copper. In each case, the use relies on particular properties. Click on the buttons to show which properties each use should have.

Use Ductility | Define Ductility at Dictionary.com C14: from Old French, from Latin ductilis, from dūcere to lead Collins English Dictionary - Complete & Unabridged 2012 Digital Edition © William Collins Sons & Co. Ltd. 1979, 1986 © HarperCollins Publishers 1998, 2000, 2003, 2005, 2006, 2007, 2009, 2012 Word Origin and History for ductility Expand ductile adj. mid-14c., from Old French ductile or directly from Latin ductilis "that may be led or drawn," from past participle of ducere "to lead" (see duke (n.)). Related: Ductility. Online Etymology Dictionary, © 2010 Douglas Harper Ductile - definition of ductile by The Free Dictionary Ductile - definition of ductile by The Free Dictionary 1. Easily drawn into wire or hammered thin: ductile metals. 2. Easily molded or shaped. See Synonyms at malleable . 3.

Capable of being readily persuaded or influenced; tractable: a ductile young mind. [Middle English ductil, from Old French, from Latin ductilis, from ductus, past participle of dūcere, to lead; see deuk- in the Appendix of Indo-European roots.] duc·til′i·ty (-tĭl′ĭ-tē), duc′ti·li·bil′i·ty (-lə-bĭl′ĭ-tē) n. ductile (ˈdʌktaɪl) adj 1. (Metallurgy) (of a metal, such as gold or copper) able to be drawn out into wire 2. able to be moulded; pliant; plastic 3. easily led or influenced; tractable [C14: from Old French, from Latin ductilis, from dūcere to lead] ˈductilely adv 1. capable of being hammered out thin, as certain metals; malleable. 2. capable of being drawn out into wire or threads, as gold. 3. able to undergo change of form without breaking. 4. capable of being molded or shaped; plastic.

[1300–50; Middle English < Latin ductilis=duc-, variant s. of dūcere (see duct ) + -tilis -tile ] duc′tile•ly, adv. duc•til′i•ty, duc′tile•ness, n. duc·tile (dŭk′təl) 1. Easily drawn out into a fine strand or wire. Gold and silver are ductile metals. Compare brittle . 2. Relating to rock or other materials that are capable of withstanding a certain amount of force by changing form before fracturing or breaking. ThesaurusAntonymsRelated WordsSynonymsLegend: manipulable , tractable - easily managed (controlled or taught or molded); "tractable young minds"; "the natives...being...of an intelligent tractable disposition"- Samuel Butler 2.

ductile - capable of being shaped or bent or drawn out; "ductile copper"; "malleable metals such as gold"; "they soaked the leather to made it pliable"; "pliant molten glass"; "made of highly tensile steel alloy" formed - having or given a form or shape ductile [ˈdʌktaɪl] ADJ (Tech) [metal] → dúctil ductile (fig liter) person → leicht lenkbar ductile ductile (ˈdaktail) adjective (of metals) able to be drawn out into wire etc.

buigbaar قابِل للتَّمَدُّد мек dúctil kujný, tažný biegsam smidig; kan formes όλκιμος (για μέταλλο) dúctil venitatav چکش خوار venyvä ductile רקיע लचीला rastezljiv, savitljiv képlékeny duktil teygjanlegur; auðmótanlegur duttile 引き伸ばせる (금속 등이) 가단성(可鍛性)인 tamprus, elastingas (par metālu) elastīgs; stiepjams mulur rekbaar formbar ; smidig ciągliwy هغه شى چى په سيم بدليداى شى dúctil ductil ковкий kujný raztezen rastegljiv tänjbar, utdragbar ซึ่งทำให้เป็นแผ่นบางได้ haddeden çekilip tel haline getirilebilen 有延性的(指金屬)

 гнучкий; ковкий نرم، دھات جس کا تار کھینچا جا سکے dễ uốn nắn 易拉长的（指金属） duc·tile a.

dúctil, que tiene la propiedad de admitir deformaciones sin romperse. Want to thank TFD for its existence? Tell a friend about us , add a link to this page, or visit the webmaster's page for free fun content . Link to this page: atomic number 58 References in classic literature ? This metal, in fact, is the most tenacious, the most ductile, and the most malleable, and consequently suitable for all moulding operations; and when smelted with pit coal, is of superior quality for all engineering works requiring great resisting power, such as cannon, steam boilers, hydraulic presses, and the like.

View in context In one well-marked instance, I put the comb back into the hive, and allowed the bees to go on working for a short time, and again examined the cell, and I found that the rhombic plate had been completed, and had become perfectly flat: it was absolutely impossible, from the extreme thinness of the little rhombic plate, that they could have effected this by gnawing away the convex side; and I suspect that the bees in such cases stand in the opposed cells and push and bend the ductile and warm wax (which as I have tried is easily done) into its proper intermediate plane, and thus flatten it. Basic Metals Element Group Properties By Anne Marie Helmenstine, Ph.D. Updated April 01, 2016. Several groups of elements can be termed metals. Here is look at the location of the metals on the periodic table and their common properties: Examples of Metals Most of the elements on the periodic table are metals, including gold, silver, platinum, mercury, uranium, aluminum, sodium and calcium. Alloys, such as brass and bronze, also are metals.

Location of Metals on the Periodic Table Metals are located on the left side and the middle of the periodic table . Group IA and Group IIA (the alkali metals ) are the most active metals. The transition elements , groups IB to VIIIB, are also considered metals. The basic metals are the element to the right of the transition metals. The bottom two rows of elements beneath the body of the periodic table are the lanthanides and actinides , which are also metals. Properties of Metals Metals are shiny solids are room temperature (except mercury, which is a shiny liquid element ), with characteristic high melting points and densities. continue reading below our video Trends in the Periodic Table Many of the properties of metals, including large atomic radius, low ionization energy , and low electronegativity , are due to the fact that the electrons in the valence shell of a metal atoms can be removed easily. One characteristic of metals is their ability to be deformed without breaking. Malleability is the ability of a metal to be hammered into shapes. Ductility is the ability of a metal to be drawn into wire. Because the valence electrons can move freely, metals are good heat conductors and electrical conductors.

Summary of Common Properties Solids at room temperature (except mercury) High melting points Metal | Define Metal at Dictionary.com metal noun 1. any of a class of elementary substances, as gold, silver, or copper, all of which are crystalline when solid and many of which are characterized by opacity, ductility, conductivity, and a unique luster when freshly fractured. 2. such a substance in its pure state, as distinguished from alloys. an element yielding positively charged ions in aqueous solutions of its salts. 3. an alloy or mixture composed wholly or partly of such substances, as brass. 4. an object made of metal. 5. the state of being set in type. 8. molten glass in the pot or melting tank. 9. verb (used with object), metaled, metaling or (especially British) metalled, metalling. 10. to furnish or cover with metal. 11. British. to pave or surface (a road) with broken stone.

Origin of metal 1250-1300; Middle English (< Old French) < Latin metallum quarry, metal < Greek métallon mine, quarry, metal Related forms Examples from the Web for metal Expand Contemporary Examples Without any warning, dozens of black-clad riot police armed with rifles and metal sticks stormed the garden. Trevethlan: Volume 1 William Davy Watson I had reached down, picked up a metal cylinder and showed it to him. The Blue Wall Richard Washburn Child They were a stalwart people, versed in agriculture and working in metal. British Dictionary definitions for metal Expand noun 1. any of a number of chemical elements, such as iron or copper, that are often lustrous ductile solids, have basic oxides, form positive ions, and are good conductors of heat and electricity an alloy, such as brass or steel, containing one or more of these elements 2. (printing) type made of metal 3. the substance of glass in a molten state or as the finished product 4. (informal) short for heavy metal (sense 1) 6.

(navy) the total weight of projectiles that can be shot by a ship's guns at any one time the total weight or number of a ship's guns 7. (astronomy) Also called heavy element. any element heavier than helium 8. (pl) the rails of a railway adjective verb (transitive) -als, -alling, -alled (US) -als, -aling, -aled 11. to fit or cover with metal 12. to make or mend (a road) with road metal Derived Forms C13: from Latin metallum mine, product of a mine, from Greek metallon metal. Collins English Dictionary - Complete & Unabridged 2012 Digital Edition © William Collins Sons & Co. Ltd. 1979, 1986 © HarperCollins Publishers 1998, 2000, 2003, 2005, 2006, 2007, 2009, 2012 Word Origin and History for metal Expand n.

mid-13c., from Old French metal "metal; material, substance, stuff" (12c.), from Latin metallum "metal; mine, quarry, mineral, what is got by mining," from Greek metallon "metal, ore" (senses only in post-classical texts; originally "mine, quarry, pit"), probably from metalleuein "to mine, to quarry," of unknown origin, but related somehow to metallan "to seek after." Cf. Greek metalleutes "a miner," metalleia "a searching for metals, mining." adj. late 14c., from metal (n.). Online Etymology Dictionary, © 2010 Douglas Harper metal met·al (mět'l) n. Any of a category of electropositive elements that usually reflect light, are generally good conductors of heat and electricity, and can be melted or fused, hammered into thin sheets, or drawn into wires. Typical metals form salts with nonmetals, basic oxides with oxygen, and alloys with one another. An alloy of two or more metallic elements. An object made of metal.

The American Heritage® Stedman's Medical Dictionary Copyright © 2002, 2001, 1995 by Houghton Mifflin Company. Published by Houghton Mifflin Company. metal (mět'l) Any of a large group of chemical elements, including iron, gold, copper, lead, and magnesium, that readily become cations and form ionic bonds, having relatively free valence electrons (electrons in the outer shells). Metals are generally good conductors of electricity because of the freedom of their valence electrons. Metals generally conduct heat well, and in solid form are relatively malleable and ductile compared to other solids. They are usually shiny and opaque. All metals except mercury are solid at room temperature. An alloy, such as steel or bronze, made of two or more metals. In astronomy, any atom except hydrogen and helium. Small stones or gravel, mixed with tar to form tarmac for the surfacing of roads. Our Living Language : Most metallic elements are lustrous or colorful solids that are good conductors of heat and electricity, and readily form ionic bonds with other elements.

Many of their properties are due to the fact that their outermost electrons, called valence electrons, are not tightly bound to the nucleus. For instance, most metals form ionic bonds easily because they readily give up valence electrons to other atoms, thereby becoming positive ions (cations). The electrical conductivity of metals also stems from the relative freedom of valence electrons. In a substance composed of metals, the atoms are in a virtual "sea" of valence electrons that readily jump from atom to atom in the presence of an electric potential, creating electric current. With the exception of hydrogen, which behaves like a metal only at very high pressures, the elements that appear in the left-hand column of the Periodic Table are called alkali metals. Alkali metals, such as sodium and potassium, have only one electron in their outermost shell, and are chemically very reactive. (Hydrogen is exceptional in that, although it is highly reactive, its other metallic properties are manifest only at very high pressures.) Metals farther toward the right side of the Periodic Table, such as tin and lead, have more electrons in their outermost shell, and are not as reactive.

The somewhat reactive elements that fall between the two extremes are the transition elements, such as iron, copper, tungsten, and silver. In most atoms, inner electron shells must be maximally occupied by electrons before an outer shell will accept electrons, but many transition elements have electron gaps in the shell just inside the valence shell. This configuration leads to a wide variety of available energy levels for electrons to move about in, so in the presence of electromagnetic radiation such as light, a variety of frequencies are readily emitted or absorbed. Thus transition metals tend to be very colorful, and each contributes different colors to different compounds. The American Heritage® Science Dictionary Copyright © 2002. Published by Houghton Mifflin. All rights reserved. Slang definitions & phrases for metal Expand metal structures METALLIC STRUCTURES This page decribes the structure of metals, and relates that structure to the physical properties of the metal. The structure of metals The arrangement of the atoms Metals are giant structures of atoms held together by metallic bonds. "Giant" implies that large but variable numbers of atoms are involved - depending on the size of the bit of metal.

Note: Before you go on, it might be a good idea to read the page on bonding in metals unless you are reasonably happy about the idea of the delocalised electrons ("sea of electrons") in metals. 12-co-ordination Most metals are close packed - that is, they fit as many atoms as possible into the available volume. Each atom in the structure has 12 touching neighbours. Such a metal is described as 12-co-ordinated. Each atom has 6 other atoms touching it in each layer. There are also 3 atoms touching any particular atom in the layer above and another 3 in the layer underneath. This second diagram shows the layer immediately above the first layer. There will be a corresponding layer underneath. (There are actually two different ways of placing the third layer in a close packed structure, but that goes beyond the requirements of current A'level syllabuses.) 8-co-ordination Some metals (notably those in Group 1 of the Periodic Table) are packed less efficiently, having only 8 touching neighbours. These are 8-co-ordinated. The left hand diagram shows that no atoms are touching each other within a particular layer . They are only touched by the atoms in the layers above and below.

The right hand diagram shows the 8 atoms (4 above and 4 below) touching the darker coloured one. Crystal grains It would be misleading to suppose that all the atoms in a piece of metal are arranged in a regular way. Any piece of metal is made up of a large number of "crystal grains", which are regions of regularity. At the grain boundaries atoms have become misaligned. Note: Within a crystal grain you get rather subtle irregularities known as dislocations. It isn't important to know about these for UK A level Chemistry (or equivalent) purposes, although they turn out to be essential in discussing the workability of metals at a higher level. I haven't included a description of them here because it is quite difficult to visualise how they work, and I don't want to add unnecessary complications. The physical properties of metals Melting points and boiling points Metals tend to have high melting and boiling points because of the strength of the metallic bond. The strength of the bond varies from metal to metal and depends on the number of electrons which each atom delocalises into the sea of electrons, and on the packing.

Group 1 metals like sodium and potassium have relatively low melting and boiling points mainly because each atom only has one electron to contribute to the bond - but there are other problems as well: Group 1 elements are also inefficiently packed (8-co-ordinated), so that they aren't forming as many bonds as most metals. They have relatively large atoms (meaning that the nuclei are some distance from the delocalised electrons) which also weakens the bond. Electrical conductivity Metals conduct electricity. The delocalised electrons are free to move throughout the structure in 3-dimensions. They can cross grain boundaries. Even though the pattern may be disrupted at the boundary, as long as atoms are touching each other, the metallic bond is still present. Liquid metals also conduct electricity, showing that although the metal atoms may be free to move, the delocalisation remains in force until the metal boils. Thermal conductivity Metals are good conductors of heat. Heat energy is picked up by the electrons as additional kinetic energy (it makes them move faster). The energy is transferred throughout the rest of the metal by the moving electrons.

Strength and workability Malleability and ductility Metals are described as malleable (can be beaten into sheets) and ductile (can be pulled out into wires). This is because of the ability of the atoms to roll over each other into new positions without breaking the metallic bond. If a small stress is put onto the metal, the layers of atoms will start to roll over each other. If the stress is released again, they will fall back to their original positions. Under these circumstances, the metal is said to be elastic. If a larger stress is put on, the atoms roll over each other into a new position, and the metal is permanently changed. The hardness of metals This rolling of layers of atoms over each other is hindered by grain boundaries because the rows of atoms don't line up properly. It follows that the more grain boundaries there are (the smaller the individual crystal grains), the harder the metal becomes. Offsetting this, because the grain boundaries are areas where the atoms aren't in such good contact with each other, metals tend to fracture at grain boundaries. Increasing the number of grain boundaries not only makes the metal harder, but also makes it more brittle.

Controlling the size of the crystal grains If you have a pure piece of metal, you can control the size of the grains by heat treatment or by working the metal. Heating a metal tends to shake the atoms into a more regular arrangement - decreasing the number of grain boundaries, and so making the metal softer. Banging the metal around when it is cold tends to produce lots of small grains. Cold working therefore makes a metal harder. To restore its workability, you would need to reheat it. You can also break up the regular arrangement of the atoms by inserting atoms of a slightly different size into the structure. Alloys such as brass (a mixture of copper and zinc) are harder than the original metals because the irregularity in the structure helps to stop rows of atoms from slipping over each other. Questions to test your understanding If this is the first set of questions you have done, please read the introductory page before you start. You will need to use the BACK BUTTON on your browser to come back here afterwards. Copper, Chemical Element - reaction, water, uses, elements, metal, number, name, symbol Tools for working with copper, made in about 5000 B.C. , have also been found.

In the New World, Native Americans used copper objects as early as 2000 B.C. The symbol for copper, Cu, comes from the Latin word cuprum. Cuprum is the ancient name of the island of Cyprus. The Romans obtained much of their copper from Cyprus. Bronze was one of the first alloys produced. It is primarily copper and tin. The two metals can be melted together rather easily. Humans discovered methods for making the alloy as early as 4000 B.C. Over the next thousand years, bronze was used for a great variety of tools, weapons, jewelry, and other objects. It was such an important metal that the period from 4000 to 3000 B.C. is now known as the Bronze Age. The Iron Age followed the Bronze Age when iron began to replace bronze in tools and weapons. Physical properties An important physical property of copper is its color. In fact, people often refer to anything with a reddish-brown tint as being copper colored. Copper metal is fairly soft and ductile. Ductile means capable of being drawn into wires. Both heat and electricity pass through copper very easily. The high electrical conductivity makes it ideal for many electrical purposes.

Copper has a melting point of 1,083°C (1,982°F) and a boiling point of 2,595°C (4,703°F). Its density is 8.96 grams per cubic centimeter. Chemical properties Copper is a moderately active metal. It dissolves in most adds and in alkalis. An alkali is a chemical with properties opposite those of an acid. Sodium hydroxide, commonly found in bleach and drain cleaners like Drano, is an example of an alkali. An important chemical property of copper is the way it reacts with oxygen. In moist air, it combines with water and carbon dioxide. The product of this reaction is called hydrated copper carbonate Copper samples from northern Michigan. (Cu 2 (OH) 2 CO 3 ). This compound has a beautiful greenish color, called a patina. Copper roofs eventually develop this color. Occurrence in nature The abundance of copper in the Earth's crust is estimated to be about 70 parts per million. It ranks in the upper quarter among elements present in the Earth's crust. Small amounts (about 1 part per billion) also occur in seawater.

At one time, it was not unusual to find copper lying on the ground. However, this is no longer true. Today, copper is obtained from minerals such as azurite, or basic copper carbonate (Cu 2 (OH) 2 CO 3 ); chalcocite, or copper glance or copper sulfide (Cu 2 S); chalcopyrite, or copper pyrites or copper iron sulfide (CuFeS 2 ); cuprite, or copper oxide (Cu 2 O); and malachite, or basic copper carbonate (Cu 2 (OH) 2 CO 3 ). Bronze, a copper alloy, was such an important metal from 4000 to 3000 B.C. that the era is now known as the Bronze Age. Copper is mined in more than 50 nations, from Albania and Argentina to Zambia and Zimbabwe. The leading producers are Chile and the United States. Nearly half of the world's copper comes from these two countries. The next largest producers are Canada, Peru, Australia, Russia, and Indonesia. About 98 percent of copper mined in the United States comes from Arizona, Utah, New Mexico, Nevada, and Montana.

Isotopes There are two naturally occurring isotopes of copper, copper-63 and copper-65. Isotopes are two or more forms of an element. Isotopes differ from each other according to their mass number. The number written to the right of the element's name is the mass number. The mass number represents the number of protons plus neutrons in the nucleus of an atom of the element. The number of protons determines the element, but the number of neutrons in the atom of any one element can vary. Each variation is an isotope. Nine radioactive isotopes of copper are known also. A radioactive isotope is one that breaks apart and gives off some form of radiation. Radioactive isotopes are produced when very small particles are fired at atoms. These particles stick in the atoms and make them radioactive. The color of the Statue of Liberty A n important physical property of copper is the element's color—reddish-brown. An important chemical property is the way copper reacts with oxygen. It turns the reddish-brown tint green. This change of color is a result of the copper combining with water and carbon dioxide in moist air. The product of this reaction is called hydrated copper carbonate.

Perhaps the most famous and dramatic example of this phenomenon is the Statue of Liberty on Ellis Island near New York City. The Statue, or Lady Liberty as it is often called, was a gift to the United States from France. It was dedicated on October 28, 1886. It symbolizes political freedom and democracy. The Statue of Liberty is covered with copper plates. When it was new, Lady Liberty was copper in color. Over time, the plates slowly turned green. The statue was given a thorough cleaning for its 100th birthday party on July 4, 1986. But the color stayed green. It would take a lot of elbow grease to return the Lady to its original copper color! Two radioactive isotopes of copper are used in medicine. One is copper-64. This isotope is used to study brain function and to detect Wilson's disease. This disease is the inability to eliminate copper from one's body. The second isotope is copper-67. This isotope can be used to treat cancer. The isotope is injected into the body. It then goes to cells that have become cancerous. In these cells, the isotope gives off radiation that can kill the cancerous cells.

Extraction Converting copper ore to copper metal often involves many steps. First, the ore is crushed into small pieces. Then the crushed pieces are mixed with water to form a slurry, a soup-like mixture of crushed ore and water. The slurry is spun around in large vats with steel balls to crush/the ore to an even finer powder. Next, blasts of air are passed through the slurry. Impure copper rises to the top of the mixture and unwanted earthy materials sink to the bottom. The copper mixture is skimmed off the top of the slurry and dissolved in sulfuric acid (H 2 SO 4 ). Bars of iron are added to the copper/sulfuric acid mixture. Iron is a more active metal than copper. It replaces the copper from the sulfuric acid solution. Copper deposits on the surface of the iron bar where it is easily scraped off. The copper is still not pure enough for most purposes. The most common method for copper purification relies on electrolysis, which is the process by which an electrical current is used to cause a chemical change, usually the breakdown of some substance. The copper is dissolved in sulfuric acid again and an electric current is passed through the solution.

Pure copper metal is deposited on one of the metal electrodes. By repeating this process, the copper is 99.9 percent pure. Other methods are also used to remove copper from its ores. The method chosen depends on the kind of ore used. People often refer to anything with a reddish-brown tint as being copper colored. Uses The most important application of copper metal is electrical wiring. Nearly every electrical device relies on copper wiring because copper metal is highly conductive and inexpensive. These devices include electric clocks, stoves, portable CD players, and transmission wires that carry electricity. A large skyscraper contains miles of copper wiring for all its electrical needs. Older telephone lines are thick bundles of copper wires. And computers depend on circuit boards imprinted with minute copper pathways. Alloys of copper, such as bronze and brass, are also used in construction. These alloys find their way into roofs, heating and plumbing systems, and the skeleton of the building itself. A number of copper alloys have been developed for special purposes. For example, gun metal is an alloy used to make guns. It contains about 90 percent copper and 10 percent tin. Monel metal is an alloy of nickel and copper that is resistant to corrosion (rusting).

Coinage metal is a copper alloy from which U.S. coins are made. How much is a penny worth? The core of a penny used to be copper. From its introduction in 1909 to 1982, the penny was 95 percent copper. Depending on the year, the other 5 percent was either all zinc or a combination of zinc and tin (bronze). In 1943—during World War II (1939-45)—the penny consisted of zinc-plated steel. This penny was a failure. The steel was magnetic (so it got stuck in vending machines), the zinc corroded easily, and the public often confused it with a dime. By the 1980s, copper had become more valuable than the one cent that the penny was worth. So in 1982, the U.S. mint switched the penny's core to art inexpensive zinc coated with copper. The rest of that pocket change—dimes, nickels, and quarters—have a core of coinage metal with a thin coating of a silvery metal. Coinage metal is a copper alloy. A large skyscraper contains miles of copper wiring for all its electrical needs.

Compounds A number of copper compounds are used as pesticides, chemicals that kill insects and rodents like rats and mice: basic copper acetate (Cu 2 O(C 2 H 3 O 2 ) 2 ): insecticide (kills insects) and fungicide (kills fungi) copper chromate (CuCrO 4 ○ 2CuO): fungicide for the treatment of seeds copper fluorosilicate (CuSiF 6 ): grapevine fungicide copper methane arsenate (CuCH 3 AsO 3 ): algicide (kills algae) copper-8-quinolinolate (Cu(C 9 H 6 ON) 2 ): protects fabric from mildew copper oxalate (CuC 2 O 4 ): seed coating to repel rats copper oxychloride (3CuO ○ CuCl 2 ): grapevine fungicide tribasic copper sulfate (CuSO 4 ○ 3Cu(OH) 2 ): fungicide, used as a spray or dust on crops Other copper compounds are found in battery fluid; fabric dye; fire retardants; food additives for farm animals; fireworks (bright emerald color); manufacture of ceramics and enamels; photographic film; pigments (coloring agents) in paints

, metal preservatives, and marine paints; water purification; and wood preservatives.

Turquoise and malachite are semi-precious gemstones made up of copper compounds. Turquoise ranges in color from green to blue. The color of blood In humans, the blood that comes from the lungs to the cells is bright red. The red color is caused by oxyhemoglobin (the compound hemoglobin combined with oxygen). Hemoglobin carries oxygen through the blood and is red because of the iron it carries. Compounds of iron are often red or reddish-brown. Blood returning from cells to the lungs (which flows through the veins) is purplish-red because the hemoglobin has lost its oxygen. Some animals, however, do not have hemoglobin to carry oxygen through the blood. For example, crustaceans (shellfish like lobsters, shrimps, and crabs) use a compound called hemocyanin. Hemocyanin is similar to hemoglobin but contains copper instead of iron. Many copper compounds, including hemocyanin, are blue. Therefore, the blood of a crustacean is blue, not red. Health effects Copper is an essential micronutrient for both plants and animals.

A micronutrient is an element needed in minute amounts Crustaceans, such as this Giant Tasmanian lobster, have blue blood because of a copper compound called hemocyanin. to maintain good health in an organism. A healthy human has no more than about 2 milligrams of copper for every kilogram of body weight. Copper is critical to enzyme production. An enzyme is a substance that stimulates certain chemical reactions in the body. Without enzymes, the reactions would be too slow. Copper enzymes function in the production of blood vessels, tendons, bones, and nerves. Animals seldom become ill from a lack of copper, but copper-deficiency disorders (problems because of lack of copper) can occur with animals who live on land that lacks copper. Large amounts of copper in the human body are usually not a problem either. One exception is the condition known as Wilson's disease. Some people are born without the ability to eliminate copper from their bodies. The amount of copper they retain increases. The copper level can become so great it begins to affect a person's brain, liver, or kidneys. Mental illness and death can result. Fortunately, this problem can be treated. The person is given a chemical that combines with the copper.

The copper's damaging effects on the body are reduced or eliminated. Also read article about Copper from Wikipedia User Contributions: PROPERTIES OF METALS This section is devoted primarily to the terms used in describing various properties and characteristics of metals in general. Of primary concern in aircraft maintenance are such general properties of metals and their alloys as hardness, brittleness, malleability , ductility , elasticity, toughness, density, fusibility, conductivity, and contraction and expansion. You must know the definition of the terms included here because they form the basis for further discussion of aircraft metals. Hardness Hardness refers to the ability of a metal to resist abrasion, penetration, cutting action, or permanent distortion. Hardness may be increased by working the metal and, in the case of steel and certain titanium and aluminum alloys, by heat treatment and cold-working (discussed later). Structural parts are often formed from metals in their soft state and then heat treated to harden them so that the finished shape will be retained. Hardness and strength are closely associated properties of all metals. Brittleness Brittleness is the property of a metal that allows little bending or deformation without shattering. In other words, a brittle metal is apt to break or crack without change of shape.

Because structural metals are often subjected to shock loads, brittleness is not a very desirable property. Cast iron , cast aluminum, and very hard steel are brittle metals. Malleability A metal that can be hammered, rolled, or pressed into various shapes without cracking or breaking or other detrimental effects is said to be malleable. This property is necessary in sheet metal that is to be worked into curved shapes such as cowlings, fairings, and wing tips. Copper is one example of a malleable metal. Ductility Ductility is the property of a metal that permits it to be permanently drawn, bent, or twisted into various shapes without breaking. This property is essential for metals used in making wire and tubing. Ductile metals are greatly preferred for aircraft use because of their ease of forming and resistance to failure under shock loads. For this reason, aluminum alloys are used for cowl rings, fuselage and wing skin, and formed or extruded parts, such as ribs, spars, and bulkheads. Chrome-molybdenum steel is also easily formed into desired shapes. Ductility is similar to malleability .

Elasticity Elasticity is that property that enables a metal to return to its original shape when the force that causes the change of shape is removed. This property is extremely valuable, because it would be highly undesirable to have a part permanently distorted after an applied load was removed. Each metal has a point known as the elastic limit, beyond which it cannot be loaded without causing permanent distortion. When metal is loaded beyond its elastic limit and permanent distortion does result, it is referred to as strained. In aircraft construction, members and parts are so designed that the maximum loads to which they are subjected will never stress them beyond their elastic limit. NOTE: Stress is the internal resistance of any metal to distortion. Toughness A material that possesses toughness will withstand tearing or shearing and may be stretched or otherwise deformed without breaking. Toughness is a desirable property in aircraft metals. Density Density is the weight of a unit volume of a material. In aircraft work, the actual weight of a material per cubic inch is preferred, since this figure can be used in determining the weight of a part before actual manufacture. Density is an important consideration when choosing a material to be used in the design of a part and still maintain the proper weight and balance of the aircraft.

Fusibility Fusibility is defined as the ability of a metal to become liquid by the application of heat. Metals are fused in welding. Steels fuse at approximately 2,500�F, and aluminum alloys at approximately 1, 110�F. Conductivity Conductivity is the property that enables a metal to carry heat or electricity . The heat conductivity of a metal is especially important in welding, because it governs the amount of heat that will be required for proper fusion. Conductivity of the metal, to a certain extent, determines the type of jig to be used to control expansion and contraction. In aircraft, electrical conductivity must also be considered in conjunction with bonding , which is used to eliminate radio interference . Metals vary in their capacity to conduct heat. Copper, for instance, has a relatively high rate of heat conductivity and is a good electrical conductor.

Question: What word describes the property of a metal that allows it to be drawn out into wire?
Answer: DUCTILITY