Question

In what group of the periodic table the element will found having electronic configuration : xe 4f14 5d4 6s2

Answer 1

Answer: Group 6

Explanation: Given configuration is :

$W:Xe4f^145d^46s^2$

Xenon is a noble gas with atomic number of 54 and thus there are 54 electrons in Xenon. The given element contains 74 electrons in total and thus has atomic no of 74. The element with atomic no of 74 is Tungsten which is represented by symbol W.

As the last electron enters the d orbital, it is a d block element. If the element belongs to d-block,

Group no. = no. of electrons in (n-1) d subshell + no. of electron/s in ns shell.

Thus group no for tungsten is = 4+2= 6.

Answer 2

Answer:

f-block, III B group

Explanation:

4f14 5d0 6fs2 belongs to f–block, III B group.