An atom has electronic configuration $ 1s^2, 2s^2 \, 2p^6, \, 3s^2 \, 3p^6 \, 3d^3, \, 4s^2$, you will place it in which group : -
- fifth
- fifteenth
- second
- third
The Correct Option is A
Solution and Explanation
$ 1s^2, 2s^2 \, 2p^6, \, 3s^2 \, 3p^6 \, 3d^3, \, 4s^2$
It is a member of d-block element because the last
electron is filled in d-subshell as $3d^3$ and the
following electronic configuration is possible for
d-subshell as $(n - 1)d^{ 1 \, to \, 10 } $
Hence, it is member of fifth group.
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Concepts Used:
D and F Block Elements
The d-block elements are placed in groups 3-12 and F-block elements with 4f and 5f orbital filled progressively. The general electronic configuration of d block elements and f- block elements are (n-1) d 1-10 ns 1-2 and (n-2) f 1-14 (n-1) d1 ns2 respectively. They are commonly known as transition elements because they exhibit multiple oxidation states because of the d-d transition which is possible by the availability of vacant d orbitals in these elements.
They have variable Oxidation States as well as are good catalysts because they provide a large surface area for the absorption of reaction. They show variable oxidation states to form intermediate with reactants easily. They are mostly lanthanoids and show lanthanoid contraction. Since differentiating electrons enter in an anti-penultimate f subshell. Therefore, these elements are also called inner transition elements.
Read More: The d and f block elements