This is a table that shows each element's outermost electron shell configuration. For example: manganese shows all the oxidation states from +2 to +7 in its compounds. i know that-arises from the similar energies required for removal of 4s and 3d electrons. The valence electrons of these elements enter d-orbital. (ns) and (n -1) d electrons have … Transition elements are the elements which lie between 's' and 'p' block elements. Why do transition metals have variable oxidation states? • maximum oxidation state rises across the group to manganese • maximum falls as the energy required to remove more electrons becomes very high • all (except scandium) have an M2+ ion Except scandium, the most common oxidation state shown by the elements of first transition series is +2. This oxidation state arises from the loss of two 4s electrons. These elements show variable oxidation state because their valence electrons in two different sets of orbitals, that is (n-1)d and ns. Transition elements exhibit a wide variety of oxidation states in their compounds. Delhi 2014) Answer: The variability of oxidation state of transition elements is due to incompletely filled d-orbitals and presence of unpaired electrons, i.e. There is a great variety of oxidation states but patterns can be found. Properties All transition metals except Sc are capable of bivalency. Oxidation state of an element is defined as the degree of oxidation (loss of electron) of the element in achemical compound. Why do transition elements show variable oxidation states? Reason: Close similarity in energy of 4s and 3d electrons. The energy difference between these orbitals is very less, so both the energy levels can be used for bond formation. (i) Name the element showing maximum number of oxidation states among the first… Oxidation states, (aka oxidation numbers), are numbers that show how many electrons the element would lose or gain if it were to bond to other atoms. (Comptt. The transition elements have outer electrons that occupy a very large shell. The variable oxidation states shown by the transition elements are due to the participation of outer ns and inner (n–1)d-electrons in bonding. The 4s electrons are first used and then 3d electrons. These elements show variable oxidation state because their valence electrons in two different sets of orbitals, that is (n-1)d and ns. pH has an effect on the redox potential of the reduction of transition metal ions from higher to lower oxidation states. (i) Name the element showing maximum number of oxidation states among the first series of transition metals from Sc (Z = 21) to Zn (Z = 30). Manganate (VII) ions, MnO₄⁻, are strong oxidising agents in acidic solution but a weaker oxidising agent in alkaline solution. Solution for (a) Why do transition elements show variable oxidation states? Why do transition elements show variable oxidation states? (ii) Name the element which shows only +3 oxidation state. 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