The general electronic configuration of $d$ - block elements is $(n-1) d^{1-10}, n s^{1-2}$. They show variable oxidation state because $d$ - electrons also take part in bond formation. They have degenerated orbitals. $s$ and $p$-block elements in general do not show variable oxidation states.
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Solution: To determine which type of elements exhibit variable oxidation states and degenerate orbitals, we need to understand the electronic configurations and characteristics of the s-block, p-block, and d-block elements. s-block elements: - Elements in the s-block have their outermost electrons in the s orbital. - They typically exhibit a limited number of oxidation states, usually corresponding to the loss of their valence s electrons (e.g., +1 for alkali metals and +2 for alkaline earth metals). - They do not have degenerate orbitals in the valence shell (only one s orbital). p-block elements: - Elements in the p-block have their outermost electrons in the p orbitals. - They can exhibit multiple oxidation states, but generally, this variability is less extensive compared to d-block elements. - The three p orbitals (px, py, pz) are degenerate. d-block elements: - Elements in the d-block have their outermost electrons in the d orbitals. - They are well known for exhibiting a wide range of oxidation states, often due to the involvement of both (n-1)d and ns electrons. - The five d orbitals (dxy, dxz, dyz, dx2-y2, dz2) are degenerate. Conclusion: - s-block elements do not typically show variable oxidation states or degenerate orbitals in the same context as p- and d-block elements. - p-block elements can exhibit variable oxidation states and have degenerate p orbitals. - d-block elements are renowned for their variable oxidation states and degenerate d orbitals. Thus, the correct answer is option :c :- d-block element
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Top Questions on Classification of elements & periodicity in properties
Classification of Elements & Periodicity in Properties
Since many elements were being discovered in the 19th century and the study of these elements individually was proving difficult, classification of elements was made necessary.
Classification by Johann Dobereiner - German chemist Johann Dobereiner classified certain elements on the basis of their similar properties in the groups of continuing - three elements each. These groups were called ‘triads’. In every triad, the atomic weight of the middle element was equal to the average of the atomic weights of the first and third elements.
Newlands Law of Octaves - The elements were arranged in increasing order of their atomic weights and found that every 8th element shows similarity with the 1st element.
Mendeleev’s Periodic Table - The arrangement of all 63 elements in rows or columns in order of their atomic weight was made by Mendeleev. He left some space for corresponding elements in his periodic table which were not even discovered till then. Although he predicted the properties of those elements through his periodic classification of elements.
Modern Periodic Law - The properties of the elements of the modern periodic law are periodic functions of their atomic numbers.
