MHTCET 14 May 2023 Shift 1 Solved Paper

The element from the options provided that commonly exhibits an oxidation state of +2 is Strontium (Sr). Let's elaborate on this answer.Strontium belongs to the group 2 elements of the periodic table, which are also known as the alkaline earth metals. Elements in this group typically lose two electrons to form ions with a +2 charge in order to achieve a noble gas configuration. This means that $\mathrm{Sr}^{2+}$ is the common ion formed by strontium when it reacts with nonmetals or in other chemical reactions where it is oxidized.Now, let's consider the other options:Rubidium (Rb) - This is an alkali metal that belongs to group 1 of the periodic table. Alkali metals typically have an oxidation state of +1 due to the loss of their single valence electron to form a cation $(\mathrm{Rb}^{+})$. Sodium $(\mathrm{Na})$ - Similar to rubidium, sodium is also an alkali metal and typically loses one electron to form an $\mathrm{Na}^{+}$ion with $a+1$ oxidation state.Lithium (Li) - Lithium is the lightest metal and the first element in the alkali metals group. Like the other group 1 elements, it exhibits an oxidation state of +1 when it forms a $\mathrm{Li}^{+}$ion.In summary, $\mathrm{Sr}$ most commonly exhibits the +2 oxidation state, making option $A(\mathrm{Sr})$ the correct answer to the question.