Which of the following ions are likely to form? Explain.a. Li^2+b...

Question

Which of the following ions are likely to form? Explain.a. Li^2+b. K-c. Mn^3+d. Zn^4+e. Ne+

Accepted Answer

Welcome back, everyone. We need to identify the ions that are least likely to form. In choice. A, we have sodium plus one ion. In choice B we have the Oxonian plus one Calion. In choice C, we have the chlorine two plus ion. In choice D, we have the calcium C M three plus Calion. And in choice E it considers the oxonian chlorine and calcium Calion. And choice F considers the sodium oxonian and calcium Calion. We're going to need to recall the term ionization energy and recall its trend on our periodic tables which increases as we go towards the top right of the periodic table. Recall that ionization energy describes the amount of energy needed to remove an electron from an atom. So we can understand in terms of our prompt that the lower the ionization energy for a neutral atom, what correlate to a greater likelihood of the ion we say of the ion formation. So let's consider example A which considers sodium plus one cat. So we're going to need to think of now neutral sodium, which is just N A and we would consider its position on the periodic table which is down group one a and across period three of the periodic table, which is our third row. And based on its position, we would observe sodium being at about this position towards the far left of the periodic table. And with just a plus one counting on charge, we are considering its first ionization energy. So removing just one electron from sodium and in doing so because we should recall that sodium corresponds to atomic number 11. We can say Z for atomic number equals 11, that correlates to from neutral sodium, 11 electrons and protons. So removing one of the 11 electrons would now move to atomic number 10, which correlates to the very stable configuration of the noble gas neon across period Q and it located in group A a our noble gas group. So that would yield a stable configuration in the formation of sodium plus one ion. So based on its position, correlating to a low ionization energy and its first ionization energy forming a stable noble gas configuration for the sodium ion, we would say that therefore, the sodium ion is very likely to form. And we would rule out choice A moving on to choice B where we consider the Oxonian plus one cat, we're going to need to consider now neutral oxygen which on the periodic table is located down group six A and across period two, based on its position on the periodic table, we would find oxygen around here at, at this position in the periodic table group six A and period two. And that would be towards the far, right. So that correlates to a very high ionization energy. And considering it would be the first ionization energy, since we just have a plus one Ron for Oxon, we would only be removing one electron from oxygen. However, considering it's high ionization energy, it's going to be very difficult to pluck that electron off. And so therefore, we can say that the oxonian plus one ion is least likely to form. So let's put a check mark by choice. B now we've got choice C to consider which considers the chlorine plus two ion. We're going to consider neutral chlorine. And we're going to recall that it is located down group seven a hour halogen group and across period three to the third row of the periodic table. And based on chlorine's position, it would be located also towards the far right of the periodic table. And that would correspond to a high ionization energy or large amount of energy required to remove two electrons this time because it has that plus two count on charge. So we are considering not only its first ionization energy but its second ionization energy. And based on neutral chlorine's very high ionization energy, it's going to be difficult to remove those two electrons. So therefore, we would say that the chlorine plus two Calion is going to be less likely to form. And let's place a check mark by choice C then we consider choice D which lists calcium three plus Calion. So we're going to consider neutral calcium and recall that it is located down group two, a, the second column of the periodic table in a cross period four. And based on its position on the periodic table, it would be towards the far left of the periodic table which correlates to a low ionization energy. However, we are considering its 1st, 2nd and 3rd ionization energy because we have the plus three caton formation, meaning we would remove three electrons. And considering that has an atomic number equal to 20 removing three electrons from neutral calcium would correlate to an atomic number of 17 corresponding to only electrons from the original 20. And so, although neutral calcium has a low ionization energy and a lower second ionization of energy once direction a higher ionization energy. And that is because we would be removing an electron from a positively charged ion. Once we get to the third ionization energy, we would be removing an electron from an even higher magnitude of a charge plus two. And that would remove the noble gas configuration of calcium. So let's note down that for calcium, for calcium's second ionization energy that would correlate to 18 electrons total, which corresponds to the noble gas configuration being argo. And recall that our noble gasses are very stable with a filled three P subs shell. And due to that stability, it's going to be unfavorable to remove a third electron for the third ionization energy and ultimately remove this noble gas configuration for the calcium plus two ion. And so we would say that therefore, the third ionization energy is a high amount of energy and removes be stable noble gas configuration. So ultimately, the calcium three plus ion is less likely to form because we would like to keep that stable configuration, that stable noble gas configuration of calcium two plus. So we would rule out or rather place a checkmark by choice D because we want the ions least likely to form. And we determine that calcium plus three is least likely to form. So now, moving on to choice E which considers choices BC and D that actually checks out and we can then confirm that choice. E would be the final answer choice because in choice F it includes the sodium plus one ion as being less likely to form. And we agreed that due to its low ionization energy, the first ionization energy for sodium plus one to form would occur easily. And so we would rule out choice F since sodium plus one should not be considered least likely to form. And that leaves us with choice E as our final answer being the Oxonian plus one CAD on chlorine plus two CAD and calcium plus three caton as the ions least likely to form. I hope this made sense. And let us know if you have any questions.

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Which of the following ions are likely to form? Explain.a. Li^2+b. K-c. Mn^3+d. Zn^4+e. Ne+

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