Question

In what group of the periodic table of the element will found having electronic configuration $\left[ {Xe} \right]4{f^{14}}5{d^4}6{s^2}$?
A) 6
B) 5
C) 8
D) 10

Answer 1

Hint: We know
Aufbau’s principle:
Aufbau’s principle states that electrons are filled into atomic orbitals within the increasing order of orbital energy states. Consistent with the Aufbau principle the available atomic orbitals with rock bottom energy levels are occupied before those with higher energy levels.

Complete step by step answer:
Given,
The electronic configuration of the element is $\left[ {Xe} \right]4{f^{14}}5{d^4}6{s^2}$
We know that the electrons in the outermost shell are called valence electrons and the number of electrons it accepts or donates to form a bond is called the valency of an electron.
We know that the group of an element is equal to the number of valence electrons of an element. Thus the number of valence electrons is six (number of electrons in the d-orbital and number of electrons in s-orbital). Hence the element belongs to group-6.

Therefore, the option A is correct.

Note:
Pauli’s Exclusion principle states that the second electron can enter an orbital if the spin of that electron is in the opposite of the electron which is already present in the orbit.
The principal energy level of an electron refers to the orbital in which the electron is located relative to the atom’s nucleus.
The Azimuthal quantum number denotes the subshell (orbital) to which the electron belongs and also determines the shape of the orbital and the energy associated with the angular momentum of the electron.
The magnetic quantum number determines the preferred orientations of orbitals in space.
The spin quantum number’ is related to electron spin.