Question

1. Given the following full electron configuration, which is the noble gas electron configuration? → 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2
A. [Ar] 4s^2
B. [Mg] 3p^6 4s^2
C. [Ne] 3s^2 3p^6 4s^2
D. [Ne] 4s^2
(please help I am so lost)

Answer 1

The element identified in the original electron configuration is Calcium, Ca, so move backwards from there. The noble gas you reach first is Argon. For the noble gas configuration, you'd use Argon and then 4s^2 to acknowledge that it's still Calcium that the electron configuration is identifying.

The answer is A, [Ar] 4s^2.

Let me know if you need more of an explanation on electron configuration itself.

Answer 2

The electronic configuration of the given element in the term of noble gas will be $\rm \Bold [Ar]\;4s^2$.

The noble gas electronic configuration has been consisted of the electronic configuration of an element with the last noble gas found near to the element.

The given electronic configuration is $\rm 1s^2\;2s^2\;2p^6\;3s^2\;3p^6\;4s^2$.

The given element has been consisted of 20 electrons, giving the atomic number 20. Calcium in the periodic table has the atomic number 20. The nearest noble gas to the calcium atom is Argon.

The atomic number of Argon is 18. The electronic configuration will be: $\rm 1s^2\;2s^2\;2p^6\;3s^2\;3p^6$.

In the electronic configuration of Ca, at the place of $\rm 1s^2\;2s^2\;2p^6\;3s^2\;3p^6$, [Ar] can be written.

Thus the electronic configuration of the given element in the term of noble gas will be $\rm \Bold [Ar]\;4s^2$.

For more information about the electronic configuration, refer to the link:

https://brainly.com/question/14283892