What Is The Oxidation Number Of Hg In Hgcl2
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As a consequence, fluorine is present in living organisms in the form of organic compounds. Phosphorus is an element which can exist in seven different oxidation states in water. Using electron spectroscopy for chemical analysis (ESCA), the surface of the P atom is distorted due to the repulsion of the outermost 8s-electrons with the surrounding ones. These electrons are therefore not available for reduction reaction. This is the reason of the very strong electron affinity of phosphorus. The reason why silicon is found in biological systems at a neutral (0) oxidation state is also due to its capacity to form non-volatile silicates. The nature of its silicon is different from the alkali and alkaline-earth metals because its seven outer electrons are shared with the arsenic and phosphorus in the silicate complexes. As a consequence, silicates are very stable in acidic pH and are not very soluble. The structure of the silicon atom is different from the other metals because the outermost electrons are not available for reduction reaction. Carbon, nitrogen, and phosphorus can exist in various oxidation states: −1, +3, +5, +6, +7, and +9.
The oxidizing nature of the outermost electrons and the reduction of the innermost electrons for elements with a closed shell structure are due to the non-linearity of the electron density distribution in their outermost layers. Therefore, the outermost electrons are more available for being attracted by an outer electron. For an element with a shell, the first and second outermost electrons are equally available for electron redistribution. The non-linearity of the electron density distribution are different for elements which have an open shell. For these elements, the second outermost electron is more available for being attracted by an outer electron. The non-linearity of the electron density distribution is also different for a few elements like sulfur. Sulfur has a very large electron affinity. Therefore, the outermost electron is very strongly attracted by the outermost electron to form a covalent bond. This makes this element very reactive and highly reactive.
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