Answer :
We are tasked to find the element which has a noble gas electronic configuration [Xe] 6s2. First tasked is to find the molecular number and add 2 as the last orbital electron. Thus, we have an element that has a molecular number of 54+2= 56. Looking on the periodic table, find an element that has 56 as the molecular number. That element is Barium (Ba).
Answer : The element is, Barium.
Explanation :
Noble gas : It is the tendency of a chemical elements to gain or lose electrons to reach the electronic configuration of the noble gas.
As we know that if the element belongs to s-block , its group number = Number of valence electrons (or outermost shell electrons).
Period number = The number present before the outermost shell of an element
The given noble gas electronic configuration is, [tex][Xe]6s^2[/tex]
Form the electronic configuration we conclude that, the period number is, 6 and the group number is, 2 (because there are 2 valence electrons in outermost shell).
Thus, the element is barium that belongs to group 2 and period 6.