what happens to iron when heated?
959853
The atoms of iron begin to move at a more rapid pace, causing the material to expand.  Once it expands enough there is so much energy that it can turn into liquid form, allowing it to flow freely so long as another force isn't standing in it's way.  The same thing happens to all matter when heated up.  You may even notice that the metal will begin to glow.  This is because of radiation in the form of photon particles.  It will also become highly ductile and maliable, which are two characteristics that iron have.  Heck, if iron were to be heated up far enough it could even become a gas.  However, I doubt you would ever be able to do it without both heat and compression with current technology.  You might even cause the gasses in the atmosphere around it to gain enough energy to start a fusion reaction, which could cause one yucky mess out of our atmosphere if they don't cool down.
58800
Iron produces rust by chemically reacting with Oxygen from the atomosphere. Oxygen can easily form Ferrous/ or ferric oxide (i.e., oxides of iron) reacting with iron. We call these iron oxides as rust. The coating of tin protects iron from contact of atomospheric oxygen. That is how tin coatings prevent iron from rust.
394719
Rust is a chemical reaction involving iron and oxygen.  Melting metal is simply a physical reaction changing the state of its matter, so melting the metal wouldn't get rid of the rust to the best of my knowledge.  IT might however make it easy for you to seperate the rusted and non rusted parts of the metal, but then again it might make it a total mess lol
644673
They get cold. \n\nThere are some effects on magnetic properties when you go very cold (search on magnetism AND temperature) especailly for electromagnets. Some things which aren't magnetic start to become so and things which are magnetic become more so. You wouldn`t notice much if you used a home freezer, you need to get much closer to absolute zero.    \n\nMaking it hot has a more important effect. A permanent magnet heated to above its Curie temperature will lose its properties.
1052987
All of the above.\n\nActually even Magnetism is affected by heat.  Heat a magnet and it will lose its magnetism.\n\nChemical composition will also change.
1024027
Copper in the metal spark and flame apparatus of the lighter.  The metal is heated by the flame, and electrons in the metal are excited and jump up a few orbitals (energy levels), and on the way back down to the ground state, they release the energy in the form of light correpsonding to green wavelengths.
451605
Anything warmer than the air temperature will be affected\n\nMeaning more heat will be lost from the warm object if there is  wind. The wind moves the lost heat away from the object.
646871
since,wateris a compound and a compound can never show the properties of its constituents.that's why water neither burns itself nor supports combustion.similar example is of iron fillings and sulphur.when we make a mixture of them,they do show their their properties But when a chemical reaction occurs and they together make ironsulphate,the new substanse doesn't show their properties that is ironsulphate is not attracted by magnet.
1070520
Try this. Iron when combined with other metal elements becomes non-magnetic, yet with varying of the same elements is quite attracted to the magnet.Name the divisions of the metals and explain why.
297607
If they are heated under really hot temperatures, they will melt.
181969
It loses electrons, so it gets a higher oxidation state. An example would be iron going to rust (Fe(s) --> Fe+3).
869402
D. Mg, because it will oxidize instead of the iron.
883128
Use a magnet. Iron is attracted to it, lead is not.
1161988
No.\n\nBut it can when it is heated.\n\nIf you heat a magnetic material above its Curie temperature, it depolarises and stops being magnetic.
1030054
You would find, if you had a sensitive enough measuring system, that the energy is dispersed through the acid as heat. \n\nWhen acid oxidises metal there is an initial activation energy required to break the metal lattice and that energy nromally comes from the heat already in the system. When the lattice is under stress sit requires far less energy to break down and the activation energy is lower. That means that more heat is retained by the system as heat.\n\nYou can see for yourself that a metal lattice under stress breaks down and oxidises more readily by simply bending an iron nail and dropping it in a few mm of salt water for a few days. The iron will rust almost exclusively where it was bent. That is because the  bend represents a point of stress in the lattice.\n\nWith less energy required to break down the metal alttice the overall reaction becomes more energetically positive and the amount of heat in the system increases.\n\nThe amount of additional heat this represents is tiny, but with an incredibly stable atmosphere and a very sensitive thermometer you would regeister the lost energy as a higher temperature than an identical beaker of acid with an uncompressed spring.
749307
amount of heat lost by iron bar = heat gained by water\n500x0.449x(212-T) = 2000x4.18(T-24)\nT is the equilibrium temp for bare and water.\nrearrange the equality and you will get T = 28.9 C\nso, the temp difference = 28.9 - 24 = 4.9 C.
1039654
Extraction Of Iron   \n      \n  Like the majority of metal ores, iron ores are not pure compounds. Rather, most iron ore compounds are polluted with sand, rock and silica.\n\nThe process of extracting iron involves a number of steps.\n\nThe first step to concentrate the iron ore and remove its contents of silica.\n\nTo further remove any existing impurities, a complex process takes place in a blast furnace. The charge is where materials are placed into the blast furnace. These materials are:\n\nOre \nLimestone \nCoke\nA burst of hot, oxygen enriched air is blown into the air-blast nozzle located at the near bottom of the furnace. What follows are a number of oxidation and reduction type reactions which ultimately produce the metallic iron.\n\nOne of these reactions is the coke being burnt. The heat generated by this reaction increases the bottom of the furnace to a temperature near 19000° C. This reaction is represented in a chemical equation:\n\nC(s) + O2(g) ® CO2(g) + heat\nThe carbon dioxide generated rises halfway up the furnace, where it reacts with the hotter coke. This causes the carbon dioxide to reduce into carbon monoxide. This reaction absorbs some heat and lowers the temperature of the upper part of the furnace to roughly 1300° C.\n\nCO2(g) + C(s) + heat ® 2CO(g)\nThis carbon monoxide then reduces the iron oxide to a metallic iron, which is molten at the temperature of the reaction. This takes place in middle and upper parts of the furnace.\n\n3CO(g) + Fe2O3(s) ® 2Fe(l) + 3CO2(g)\nThe limestone in the charge is to remove any existing silica left in the enriched ore. There are two steps in this process.\n\nThe first step is heating the limestone in the furnace to produce lime, CaO. This takes place in the middle of the furnace.\n\nCaCO3(s) ® CaO(s) + CO2(g)\nThe second step in this process is when the lime reacts with the silica, resulting in calcium silicate.\n\nCaO(s) ® SiO2(s) + CaSiO2(l)\nAt this point, the calcium silicate is a liquid which seems to mean that the lime has served as a flux. The term flux refers to a substance that cause mineral impurities in an ore to melt more readily. The melting process that takes place in the furnace is called smelting. In this process of smelting, the products in the furnace are separated into layers. In this way, the molten iron is the bottom layer and molten calcium silicate is the layer above it. Being that the molten iron is more dense than the molten calcium silicate. \n\nThe calcium silicate is a kind of slag, formed in a smelting process by the lime combining with the calcium silicate. As a slag, the calcium is easily separated from the more dense molten iron. This is done simply by tapping the slag with an outlet.\n\nWhen cooled, the molten iron from the blast furnace becomes pig iron. It still contains a number of impurities; \n\nSulfur \nPhosphorus \nBoron\nThese lower the iron's tensile strength and make it more brittle. However, it has such impurities at much lower levels.\n\nFrom here, most iron is processed further to make steel or cast iron.