What is a good explanation of metallic corrosion?
491586
Metallic corrosion is basically a redox reaction where the metal is oxidised by the oxygen in the air and sometimes assisted by the presence of water.
316653
Depends on the application you have for the copper. You can shield it from oxygen and other corrosive agents using a protective atmosphere.\n\nAt 500°C exposed to atmospheric oxygen you will want a solid metal with a stable passivizing surface or too noble to react. Titanium or platinum will probably be overkill, stainless steel may discolour.\n\nOr you might be thinking about a sacrificial anode, leaving the copper intact but dissolving the connected material (e.g. zinc or magnesium).
186001
u forgot to put the foloowings to choose from...\nbut still here are some ideas for u...\nTO PREVENT RUST, KEEP METAL SURFACE DRY - OR ADD A COATING \nRust is corrosion that affects ferrous metals such as iron and steel. In many cases, water vapor must be in the air before rust can occur. With iron, for example, 40 percent humidity must be present before rust will start to occur. The best way to prevent corrosion is to keep metal surfaces dry. Isolating the metal by coating it with paint, lacquer or wax is another good way to prevent corrosion. \n\nBefore coating a metal surface, remove all traces of rust. Then apply a primer and finish with paint. It's best if the paint and primer are the same brand; they usually are formulated to work together. Metals such as brass, copper or aluminum are best protected with either wax or by spraying them with lacquer or clear varnish. \n\nRust also can attack metal in inaccessible areas. Corrosion occurs inside a home hot-water heater, for example, because the ions circulating in the water make it easy for dissolved oxygen to pull the electrons from the interior surface of the metal tank. \n\nRust that occurs in localized areas is called localized corrosion. There are three types: galvanic, crevice and pitting. \n\n- Galvanic corrosion: It occurs whenever two dissimilar metals contact each other. This creates a flow of electrons between the metals that eventually causes them to disintegrate. One way to prevent this corrosion is to replace one metal piece with another that is compatible with the mating piece.\n\nFor example, many aluminum storm doors have steel rivets holding the hinges or closing piston in place. Often, corrosion starts around these fasteners, then works to the adjacent aluminum panels. Drilling the corroded fasteners out and replacing them with aluminum pop-rivets will stop the galvanic corrosion before it spreads.\n\n- Crevice corrosion: It occurs around the joints and seams of metal fixtures where dirt accumulates. By itself the dirt is not particularly harmful, but it allows moisture to collect; this causes corrosion. Joint and seam corrosion is a common occurrence on gutters and downspouts. Clean them often to keep dirt and leaves, which retain moisture, from building up. If rust is present, remove it with a flexible sanding wheel chucked in an electric drill, then prime and paint the bare metal.\n\n- Pitting corrosion: It occurs outdoors when the wind bombards metal surfaces with minute particles of dirt, salt or sand and creates microscopic craters that retain moisture. At first, the corrosion is limited, then quickly escalates into a formidable problem. Outdoor electrical conduits, television antenna masts, metal windows and doors, and children's play equipment are a few of the items that receive constant assault from air-borne particles and are subject to pit corrosion. This type of corrosion is severe near the seashore and is most noticeable on the side of the house that faces the prevailing winds. Check exposed metal surfaces often; sand and paint them if they show signs of pitting.
550877
Well my man fatigue limit cannot tend to infinity... you joking??????? anyways non ferrous metals have higher fatigue limit coz no other metal corrodes as fast as iron.... got it?
1165893
sometimes, your own perspiration causes metals to corrode.  This has to do with the composition on your sweat.  It's the same reason that some jewelry that isn't gold turns green after a while.
79044
Here is a centralized page of information, with several links along the left side for more information:\nhttp://www.webelements.com/webelements/elements/text/Cu/key.html
146495
if metal rusts, the iron is being oxidized so it is a chemical change.
1090211
Galvanized metal is a tin and carbon steel alloy. It corrodes at a slower rate of speed.
524355
I'm a metallurgist - weld material is more highly 'strained' than the parent material, so it is more prone to acidic corrosion relative to the parent material.\n\nThere is another possibility:  how do know the "weld metal" was the same as the parent material?  Perhaps the weld material was had fewer alloying elements so corroded sooner...  (cheap filler metal)\n\nOne more thing to consider:  if the part was hooked up to any electrical source, the corrosion could be caused by electrolysis rather than acidic corrosion (no kidding! happens more than you think).  Check with a voltmeter to ground; I've had batteries just eat right through stainless over a weekend; if so, insulate!
876346
Corrosion is defined as: the chemical or electrochemical reaction between a material (usually a metal) and its environment that produces a deterioration of the material and its properties.\n\nAny chemical (or electrochemical) that will deteriorate one or more properties of the composite will be sufficient.\n\nTake a simple electrochemical reaction, for example - without a UV coating, fiberglass (which happens to be a composite) loses tensile strength on prolonged exposure to sunlight.
939721
If it's metallic, it could be sodium or potassium.
40274
The magnesium metal buried nearby provides protection from corrosion.  “Corrosion” is the technical name for the chemical reaction that takes place when a metal combines with oxygen.  Magnesium acts as an anode and protects the iron or steel tank by corroding in preference to the iron or steel tank.  This means that instead of Iron giving up electrons that attach to the oxygen atoms(which causes corrosion), the Magnesium releases the electrons.  The Magnesium and Oxygen atoms combine to form magnesium oxide while Iron does not take part in the chemical reaction and is thus protected.\n\nThe corrosion of a magnesium anode in preference to steel is an example of galvanic protection.
255218
If you are asking how to reverse the corrosion, you could use an electrical cell to reduce the iron, but the product would not be carbon steel as you originally had.  The best way to deal with corrosion is toprevent it, either through coating or the use of a sacrificial anode depending on your situation.
443053
Metals are shiny and are good conductors of heat and electric current. They are malleable and ductile.\nNon-metals are dull, and are poor conductors of heat and electric current. They're brittle and unmalleable.
783824
Rusting or corroding is the wearing away of a metal layer that leads to formation of metal compounds on the surface. Rust is a compound that forms on top of iron. Blackening of silver is another example
934645
I'm no expert in this field.\nCheck out:\nhttp://www.railway-technology.com/contractors/door/mkb/\nhttp://www.key-to-metals.com/Article31.htm\n\nThere are umpteen others.
1131804
You have the potential for galvanic corrosion.  Essentially, two metals at different potentials share electrons and one metal (the one with the higher potential) will start to erode and "plate" the other metal.\n\nTypically, using some sort of material that is a non-conductor (ceramics, rubber, etc) between the two or passivating the metal surfaces or coating the metal surfaces (prime and paint per ANSI standards) are your best options to prevent this.