Consider the following Lewis symbols for elements X and Y:
c. What ions would be formed by X and Y?

Question

Consider the following Lewis symbols for elements X and Y:

Lewis dot symbols for elements X and Y, illustrating their valence electrons for ion formation analysis.

c. What ions would be formed by X and Y?

Accepted Answer

Welcome back everyone. The Lewis dot symbols for M and N are given below, determine the ions formed by M and N. Let's begin by recalling that group number of an atom corresponds to its number of valence electrons. And based on the position of our atom on the periodic table will determine based on the column that's located the group number of that atom. Let's also recall that and Adam's charge is going to be connected to the number of electrons gained or lost for a stable configuration. And we should recall that a stable configuration would be noble gas like so recall that our noble gasses are located in group 8 a on the periodic table and have a total of eight valence electrons. So we'll note eight valence electrons. So in observation of our Lewis dot symbol of our atom M, we would count a total of seven surrounding valence electrons represented as lone pairs around Adam M. These seven valence electrons tell us that we have. So seven valence electrons tell us that we have an atom in group seven A. And in order to attain a noble gas like stability, we would want to gain one more electron to get a total of eight valence electrons like our atoms in group eight a our noble gas group. And so being in group seven a, any atom in this group will want to form a minus one charge for a noble gas like stability. And so our ion is going to be our M -1 anion. Since adding an electron two, our lewis dot symbol will give us a total of eight valence electrons which is one more or one extra than our atom M typically has being in group seven A with just seven original valence electrons. And that one extra electron we added in contributes to that minus one charge. So next observing our atom N, we count a total of two lone electrons surrounding our or within our Lewis dot symbol. And so we have two valence electrons for our atom N which will connect to the fact that our atom is in group two a of our periodic table. And in order to attain a noble gas like stability, our atom in group two A should want to lose two electrons. And so we would want to remove these two lone electrons from our Lewis dot symbol to attain a noble gas like stability. And so therefore, removing those two electrons would form a ion with a plus two charge, so we can say that our ion is going to be N two plus. So our two final answers are going to be that our ions formed by M and N are M one minus and N two plus based on our given Lewis dot Symbols. I hope that this made sense and let us know if you have any questions.

Consider the following Lewis symbols for elements X and Y:

c. What ions would be formed by X and Y?

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Key Concepts

Lewis Dot Structures

Ion Formation

Valence Electrons