Question

Which is the common lowest oxidation state exhibited by the transition elements?​

Answer 1

Answer:

+2

Explanation:

Transition Elements

Transition metals are defined as those elements which have partially filled d orbitals. Transition elements exhibit a variable number of oxidation states in their compounds.

Oxidation States

The oxidation state of an element is defined as the degree of capacity of an element in a chemical compound to lose electrons from its valence shell. It is also referred to as the degree of oxidation. Transition elements usually exhibits a wide range of oxidation states in their respective compounds.

Example: Magnesium shows a wide range of its oxidation states that starts from +2 and goes up to the +7 in its various compounds.

However, some of the elements also exhibits very few oxidation states. The elements that exhibits very few oxidation states are zinc and scandium.

+2 is the common lowest oxidation state exhibited by the transition elements.

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Answer 2

The common lowest oxidation state exhibited by the transition elements is +2

Explanation:

• Common lowest oxidation state is the number of  electrons present in the ns orbital.
• In transition metals most common oxidation state  found in the first-row transition elements is +2.
• Scandium is an exception in transition elements where the most common oxidation state found in the first-row transition elements is +2
• Here  loss of two 4s- electrons arises due to which the 3d block elements are more stable and are having lower in energy in th e4s orbitals.
• The transition elements have variable oxidation state because of its (n-1)d orbitals.
• The penultimate shell is the 3d orbitals.

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