Question

Identify the element, having outer electronic configuration:

(n-1) d8

ns2

for n=4.​

Answer 1

Answer:

Answer

(i) For n=3, the period in which the element belongs is third. The electronic configuration is 3s

2

3p

4

and the element belongs to p block. The group number of the element is 10+ number of electrons in the valence shell.

=10+6=16

Thus, the element belongs to third period and sixteenth group.

(ii) For n=4, the period in which the element belongs is fourth. The electronic configuration is 3d

2

4s

2

and the element belongs to d block. The group number of the element is = number of electrons in the (n−1)d subshell + number of electrons in ns subshell=2+2=4

Thus, the element belongs to fourth period and fourth group.

(iii) For n=6, the period in which the element belongs is sixth. The electronic configuration is 4f

7

5d

1

6s

2

and the element belongs to f block. All f block elements belong to third group.

Thus, the element belongs to sixth period and third group.

Answer 2

Answer: I hope this helps .

Explanation: Please THANKS & kindly mark me as The Brainliest.