Answer : The condensed ground-state electron configuration for each is:
(a) [tex][Xe]6s^2[/tex]
(b) [tex][Ar]4s^23d^7[/tex]
(c) [tex][Kr]5s^14d^{10}[/tex]
Explanation :
Electronic configuration : It is defined as the representation of electrons around the nucleus of an atom.
Number of electrons in an atom are determined by the electronic configuration.
Noble-Gas notation : It is defined as the representation of electron configuration of an element by using the noble gas directly before the element on the periodic table.
(a) The given element is, Ba (Barium)
As we know that the barium element belongs to group 2 and the atomic number is, 56
The ground-state electron configuration of Ba is:
[tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^66s^2[/tex]
So, the condensed ground-state electron configuration of Ba in noble gas notation will be:
[tex][Xe]6s^2[/tex]
(b) The given element is, Co (Cobalt)
As we know that the cobalt element belongs to group 9 and the atomic number is, 27
The ground-state electron configuration of Co is:
[tex]1s^22s^22p^63s^23p^64s^23d^7[/tex]
So, the condensed ground-state electron configuration of Co in noble gas notation will be:
[tex][Ar]4s^23d^7[/tex]
(c) The given element is, Ag (Silver)
As we know that the silver element belongs to group 11 and the atomic number is, 47
The ground-state electron configuration of Ag is:
[tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^14d^{10}[/tex]
So, the condensed ground-state electron configuration of Ag in noble gas notation will be:
[tex][Kr]5s^14d^{10}[/tex]
