Answered

Identify the noble gas that has atoms with the same electron configuration as the

positive ion represented in diagram 1, when both the atoms and the ion are in the

ground state.

Identify the noble gas that has atoms with the same electron configuration as the positive ion represented in diagram 1, when both the atoms and the ion are in class=

Verified Answer :

I think the noble gas that has the same electron configuration with the image on the diagram would be : Argon
Its configuration is : Ne 3s2 3p6

hope this helps

Explanation:

Cation represented in diagram 1 is potassium (K) and atomic number of K is 19.

Being a metal, potassium is able to lose an electron in order to gain stability. Therefore, when potassium loses one electron then it changes into \(K^{+}\) and then total number of electrons it has are 18.

Noble gases are group 18 elements that have completely filled shells.

Argon is the noble gas that has 18 electrons in its ground state that is similar to number of electrons present in a \(K^{+}\) ion.

Thus, we can conclude that argon is the noble gas that has atoms with the same electron configuration as the  positive ion represented in diagram 1.

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