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Alternatively, the oxidation state of an element can be defined as the degree of an element’s ability to lose electrons from its valence shell in a chemical compound. This is also referred to as the degree of oxidation of the element in question. During the formation of their compounds, transition elements exhibit a wide range of oxidation states. Magnesium, for example, exhibits a wide range of oxidation states in its various compounds, ranging from +2 to +7 in a range of oxidation states. Some of the elements, on the other hand, have only a few oxidation states. Zinc and scandium are two elements that are found in only a few different oxidation states compared to other elements. The fact that any of the elements has so few oxidation states is due to the fact that they have so few electrons to lose from their valence shells. For example, scandium has an excessive number of d electrons and, as a result, has a limited number of orbitals in which to share electrons with others, resulting in a very high valence. The variable oxidation states of valence electrons are caused by the extremely small number of electrons that are filled in the d-orbital in such a way that their oxidation states differ from one another by a unitary amount of energy.
Stability of oxidation states :
Chromium, manganese, and cobalt exhibit extremely high levels of oxidation. Manganese does not exhibit a +7 oxidation state when present in halides, but the +7 oxidation state of manganese in the compound MnO3F is known. Due to the fact that the hydH of Cu2+ is greater than that of Cu+, which compensates for the second ionisation enthalpy of the metal, it is known that Cu2+ (aq) is more stable than Cu+ (aq). The oxidation state of manganese in Mn2O7 is +7, demonstrating that the oxidation state of manganese is higher in manganese oxides than in its oxides. The Mn oxide, Mn2O7, has a higher oxidation state than the Mn fluorides, MnF4, because oxygen has a tendency to form multiple bonds with metals, as opposed to the Mn fluorides, MnF4. This bridge is included in Mn2O7, which has each Mn surrounded by four O’s in a tetrahedral fashion. The other elements in the compound, such as Fe2O3 and V2O4, have oxidation states of +3 and +4 respectively, as do the other elements in the compound. Because of the inert pair effect in the p-block elements, the heavier elements prefer a low oxidation state, whereas the d-block elements prefer a high oxidation state, which is the polar opposite of the p-block elements. Similar to the findings in group 6, Mo (VI) is found to have greater stability when compared to Cr (VI).
Manganese :
When it comes to transition elements, manganese is no exception. Despite being a metal with a proclivity to lose electrons, manganese is capable of both, allowing it to lose electrons as well as gain electrons. In the presence of d-orbital, it has the ability to behave in a manner similar to both metals and non-metals, and for this reason it is referred to as the transition element. Mn is the chemical symbol for manganese, and the atomic number 25 represents the element’s atomic number. It is a silvery metal that is hard, brittle, and is frequently found in minerals in combination with iron. Manganese is a transition metal with a diverse range of industrial alloy applications, with the majority of these being in stainless steels. It increases the strength, workability, and wear resistance of the material. Manganese oxide is used as an oxidizing agent, as a rubber additive, and in the manufacture of glass, fertilizers, and ceramics, among other applications. Manganese sulfate can be used as a fungicide in certain situations.
Variability of oxidation state :
Because of the incomplete filling of d-orbitals in such a way that their oxidation states differ from each other by a factor of one, for example, Fe2+ and Fe3+, the variability in oxidation states of transition metals is caused by the presence of d-orbitals that are not completely filled. When using p-block elements, the oxidation states differ by two units of the element’s atomic number, for example, +3 and +5.
Dichromate :
Dichromate is an anion with the chemical formula Cr2O72-, and it is found in nature. When used as a strong oxidising agent in organic chemistry, it can also be used as a primary standard solution in volumetric analysis, among other things. In aqueous solution, the chromate ion and the dichromate ion can be converted into each other. There are numerous applications for dichromate compounds. They are used as oxidizing agents, as well as in the preparation of a variety of products such as waxes, paints, and glues, among other things. In contrast, potassium dichromate is carcinogenic and extremely toxic because it contains hexavalent chromium, which is a carcinogenic metal.
Conclusion :
Alternatively, the oxidation state of an element can be defined as the degree of an element’s ability to lose electrons from its valence shell in a chemical compound. This is also referred to as the degree of oxidation of the element in question. During the formation of their compounds, transition elements exhibit a wide range of oxidation states.When it comes to transition elements, manganese is no exception. Despite being a metal with a proclivity to lose electrons, manganese is capable of both, allowing it to lose electrons as well as gain electrons. In the presence of d-orbital, it has the ability to behave in a manner similar to both metals and non-metals, and for this reason it is referred to as the transition element.
