Question

Which of the following represent a d-block element?
(A) $[Rn]6{d^{10}}7{s^2}7{p^2}$
(B) $[Xe]4{f^1}5{d^1}6{s^2}$
(C) $[Xe]4{f^{14}}5{d^1}6{s^2}$
(D) $[Xe]5{d^1}6{s^2}$

Answer 1

Hint In order to find which of the following will represent a d-block element, we must first know what a d-block element is. If we know about the general electronic configuration of the d-block element, it will be easy to answer the question.

Complete step by step solution:
The d-block elements are those elements which can be found in the third group to the twelfth group of the periodic table. The valence electrons of such elements will fall under the d-block. These elements will possess the metallic characteristics such as malleability and ductility. It will also have high thermal and electrical conductivity and also have good tensile strength. The d-block elements will have four series. These series are 3d, 4d, 5d and 6d. Each 3d, 4d and 5d will have 10 elements, while 6d is incomplete.
The d-block elements will be having a general electronic configuration of $(n - 1){d^{1 - 10}}n{s^2}$. they are placed between the s and the p block elements.
Let us now move to the given question. By using the general electronic configuration of the d-block element we can say that the d-block element present will be having the electronic configuration of $[Xe]5{d^1}6{s^2}$.

Therefore, the correct answer is option (D).

Note: We have to remember that the transition elements will occupy groups 4-11. Scandium and Yttrium present in the group 3 will have partially filled d subshells. Hence, they are considered as the transition elements. The elements like Zinc, Cadmium and Mercury will have completely filled d subshells and are not considered as the transition elements. Therefore, we can say that all transition elements can be d-block elements but all d-block elements are not transition elements.