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The Periodic Table, Molecules and
Chapter , Problem 57E(choose chapter or problem)
Each of the following elements is capable of forming an ion in chemical reactions. By referring to the periodic table, predict the charge of the most stable ion of each:
(a) Mg,
(b) Al,
(c) K,
(d) S,
(e) F.
Questions & Answers
QUESTION:
Each of the following elements is capable of forming an ion in chemical reactions. By referring to the periodic table, predict the charge of the most stable ion of each:
(a) Mg,
(b) Al,
(c) K,
(d) S,
(e) F.
ANSWER:
Step 1 of 5
Here, we are going to predict the most stable ions for each of the element.
The electronic configuration of Mg is (atomic number Z =12) \([\mathrm{Ne}] 3 \mathrm{~s}^{2}\)
Thus, by removing of two electrons from 3s orbital, Mg can attain the stable noble gas configuration of Neon (Ne).
Therefore, \(M g(s) \rightarrow M g^{2+}+2 e^{-}\)
\([\mathrm{Ne}] 3 s^{2} \rightarrow[\mathrm{Ne}]\)
Hence, (a) Mg atom has 2+ charge to form the most stable ion \(\mathrm{Mg}^{2+}\).