Metal interacts with preciptation to create rust.
Rust and corrosion are examples of reactivity between certain metals and environmental forces, in particular, the reaction with oxygen known as oxidization. All metals exhibit this tendency, but some oxidize more easily than others. The tendency is determined by a classification known as the galvanic series. Certain metals, known as noble metals, are chemically inactive and possess low reactivity. These include gold, platinum and inert gases such as helium, argon, krypton and xenon. On the other hand, alkali metals such as lithium, sodium and cesium are chemically active and possess higher reactivity.
Instructions
1. Identify the material or metal type. In organic chemistry, alkenes are characterized by low reactivity and can therefore only undergo reactions under vigorous conditions, such as those involving extreme temperatures or ultraviolet irradiation. Conversely, alkyl halides react under mild conditions and the presence of hydroxyl, carboxyl, or amino promotes even further increase in reactivity.
2. Determine the components. In the case of rust, the components are steel and water. Fe 2(aq) and OH (aq) ions migrate through the water by diffusion when they meet, then combine to produce the precipitate iron (II) hydroxide. Fe (OH)2 is further oxidized into iron (III) hydroxide Fe (OH)3 and finally dehydrated to produce rust.
3. Calculate the relative reactivity. The chemical equation for rust formations becomes (2FE + 2H2) + O2, which yields 2 Fe2 (aq) + 4 QH (aq); then becomes Fe2 (aq) + 2OH, which yields Fe (OH)2; then becomes Fe (OH) 2 with O2, which yields Fe(OH) 3; which then becomes Fe (OH)3, which dehydrates and becomes Fe2O3nH2 or rust.
