examples of compund formed by aluminum?
447091
sodium aluminum sulfate (alum)- ingredient in baking powder.\n\n\nGarnets!\nIncluding the stuff on sandpaper.\n\ningredients in antiperspirant that makes it work: \nAluminum chloride, Aluminum zirconium tricholorohydrex glycine, Aluminum chlorohydrate, Aluminum hydroxybromide
513571
http://www.versafittings.com/images/BrsCatPg85-92.pdf#search='aluminum%20tubing%20working%20press%20ure'\n\nThis offers an I.D. and O.D> reference.
488112
http://chemistry.allinfoabout.com/features/nonmetals.html
471526
I suspect that the product is AlSO4.\n\nI'm thinking that the Al swaps with the Cu.  That would leave a free Cu+ which might displace the H from H20 and form either CuOH or CuO, either one of which would probably produce H2.  \n\nSo, I guess you would first get CuOH and AlOH, as intermediate reactions.\n\nI think the equation is:\n\n                          NaCl (goes over the arrow)\n6CuSO4 + 4Al + 12H2O ---------------> 2Al2(SO4)3 + 6Cu(OH)2 + 6H2
816061
It is tough to answer this question without knowing what the experimental procedure was or what the aluminum foil was used for.  More detail please.
457637
Aluminum Nitrate, Al(NO3)3, since, in a neutralization you take off any acidic hydrogen's, and any hydroxyls, and you combine the remaining ions in a way that the product molecule has no net charge. So\n Al(OH)3=Al(+3) + 3OH(-) \n HNO3 = H(+) + NO3(-)\nThe H(+) ions and OH(-) ions combine to form water, and each Al(+3) ion combines with 3 NO3(-) ions to produce Al(NO3)3 \n\nFormic acid (CHOOH) and sodium hydroxide(NaOH) produce Sodium formate, CHOONa, for the same reason as above.\n\nNote: The other H in Formic Acid is non-acidic, and so is not replaced by Na
599695
Aluminum is 2.9 times as dense as iron. On the other hand, iron has roughly half the specific heat as aluminum.\n\nSpecific heat is measured in terms of how many calories of energy it takes to raise the temperature of one gram one degree centigrade. \n\nGiven two equal masses of aluminum and iron, the aluminum with the higher specific heat will take more energy to heat and give of more energy cooling. As a result, it will take longer to heat and cool. \n\nHowever, given two equal volumes of aluminum and iron, the aluminum will have only 1/3 the mass and therefore will need throw off only 2/3s as much heat to cool as the iron.
399458
"A thermite reaction (a type of aluminothermic reaction) is one in which aluminium metal is oxidized by the oxide of another metal, most commonly iron oxide. The name thermite is also used to refer to a mixture of two such chemicals. The products are aluminium oxide, free elemental iron, and a great deal of heat. The reactants are commonly powdered and mixed with a binder to keep the material solid and prevent separation."\n\n"Uses:Thermite reactions have many uses. It was originally used for repair welding in-place such things as locomotive axle-frames where the repair can take place without removing the part from its installed location. Thermite grenades are used in war to destroy sensitive equipment or documents when at imminent risk of capture by the enemy. Thermite grenades and bombs have been used in combat as incendiary devices, able to burn through heavy armor or other fireproof barriers. Thermite can also be used for quickly cutting or welding metal such as rail tracks, without requiring complex or heavy equipment. It also enables infantry to destroy enemy artillery without the use of loud explosive charges and therefore operate with stealth. The mixture has been sold for many years under the trademark name Thermit for use in railroad welding."
367193
Draino is essential NaOH add that to aluminum and you will get NaOH + Al --> Al(OH)3 + Na2O + H2. So I guess hydrogen gas.
135714
I have done some research on this because my mom has been stricken with Alztiemers. Drs dont think its aluminium. They say most the time its triggered from stroke or stress. They dont know for sure the cause.
913792
I found a very informative essay at the below address, which covers the removal of Alumina from Its Bauxite Ore.  The process is very complex because Alumina is not actually found in its raw state as part of the Bauxite compound.  Bauxite is heated and then through a process of chemical electrolysis alumina is extracted and forms aluminium.  More precise explanation can be found at below address.     \n\nhttp://www.patana.ac.th/parents/curriculum/Chemistry/units/LR803.html
360182
Heavy Metal! Just joking. http://www.scienceproject.com/projects/intro/elementary/EX057.asp Go here, they have a lot of information.\n\nhttp://www.science.ca/askascientist/viewquestion.php?qID=1216 And this one. It is clear that aluminum conducts the best heat.
971763
1) Fe(s) +Cu^2+(aq) --> Fe^2+(aq) + Cu(s)  Single replacement, redox reaction where iron is oxidized and copper is reduced\n\n2) 2Al(s)+(3/2)O2(g)-->Al2O3(s)\nredox reaction, oxygen is reduced (neutral to -2) and aluminum is oxidized (neutral to +3)
1063042
Used to be aluminum. Some are acrylic now.
29972
Try Wikipedia...the link is below:\nhttp://en.wikipedia.org/wiki/Rust\n\nBut generally speaking:\n-Iron rusts to form Iron Oxide (Fe2O3)-numbers are all in subscripts\n- Aluminium oxides forming Aluminium Oxide, which is concidered as rust as well\n\nNot all metals rust the way iron does
936613
Of course, aluminum wins as it has the lowest density.  The passivating oxide film makes aluminum non-corrosive, which is a great comfort to the metallurists and structural engineers responsible for keeping these birds in flight, rather than cracked up over an ocean.
1178077
Scientists suspected that an unknown metal existed in alum as early as 1787, but they did not have a way to extract it until 1825. Hans Christian Oersted, a Danish chemist, was the first to produce tiny amounts of aluminum.\n\nDuring that time, the method to extract aluminum was so costly that aluminum once was considered more precious than gold. \n\nThe plant, owned by J.G. Neher & Sons (aluminum manufacturers) started in 1886 in Schaffhausen, Switzerland, at the foot of the Rhine Falls - capturing the falls’ energy to produce aluminum. Neher's sons together with Dr. Lauber discovered the endless rolling process and the use of aluminum foil as a protective barrier. From there began the wide use of aluminum foil in the packaging of chocolate bars and tobacco products. Processes evolved over time to include the use of print, color, lacquer, laminate and the embossing of the aluminum. \n\nAlthough the technology to extract aluminum improved greatly, it still is a energy extensive process.  If you, as a chemist can figure out a way to reduce the amount of energy needed to extract aluminum even by 1%, your method can make you a millionaire overnight.  There is a thought to motivate you to study Chem.  =)