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(C) The general electronic configuration for the $d$-block elements is $(n - 1)d^{1-10} ns^{1-2}$.For the configuration $(n - 1)d^6 ns^2$,the lowest p

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fourth period

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(C) The general electronic configuration for the $d$-block elements is $(n - 1)d^{1-10} ns^{1-2}$.For the configuration $(n - 1)d^6 ns^2$,the lowest possible value for the principal quantum number $n$ is $4$,because the $d$-subshell starts from $n = 3$ (i.e.,$3d$ orbital).Substituting $n = 4$ into the configuration gives $3d^6 4s^2$,which corresponds to the element Iron ($Fe$,atomic number $26$).Since $n = 4$,the element is located in the fourth period of the periodic table.

The element with the lowest atomic number that has a ground state electronic configuration of $(n - 1)d^6 ns^2$ is located in the

Similar Questions

Which of the following statements is wrong?

In the periodic table,the element with atomic number $16$ will be placed in which group (in $^{th}$)?

Which among the following electronic configurations belong to main group elements?
$A. [Ne] 3s^1$
$B. [Ar] 3d^3 4s^2$
$C. [Kr] 4d^{10} 5s^2 5p^5$
$D. [Ar] 3d^{10} 4s^1$
$E. [Rn] 5f^0 6d^2 7s^2$
Choose the correct answer from the options given below:

What will be the $IUPAC$ symbol and name for the element with atomic number $123$?

If the $IUPAC$ name of an element is $Unununnium$,then the element belongs to the $n^{th}$ group of the periodic table. The value of $n$ is . . . . . .

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