Consider the Mg2+, Cl-, K+, and Se2- ions.The four spheres below represent these four ions, scaled according to ionic size. A) Match each ion to its appropriate sphere. B) In terms of size, between which of the spheres would yo find the (i) Ca2+ and (ii) S2- ions?

Remember that, cations are smaller in size than the corresponding atom atom because the formation of a cation often involves the removal of an entire shell. Anions are larger in size than the corresponding atom because an electron is added thereby expanding the electron cloud and size of the anion.

From left to right let us designate the spheres as ABCD.

A is Mg^2+

B is K^+

C is Se^2-

D is Cl^-

Ca^2+ lies between Mg^2+ and K^+

S^2- lies between K^+ and Se^2-

annyksl annyksl · Answer 2 · 2021-11-23T01:54:56+01:00

The size of the spheres, going from smallest to largest, would be: [tex]Mg^2^+[/tex], [tex]K^+[/tex], [tex]Ca^2^+[/tex], [tex]Cl^-[/tex], [tex]S^2^-[/tex], [tex]Se^2^+[/tex].

We can arrive at this answer because:

To know the size of the spheres of an ion, we must know if they are a cation or an anion and the number of electrons in each valence layer that is gained or donated.
Cations are the ions that donate electrons. They are represented by the + symbol and get smaller and smaller as they donate electrons.
Therefore, we can state that the cations [tex]Mg^2^+[/tex], [tex]K^+[/tex], [tex]Ca^2^+[/tex] have the smallest spheres.
On the other hand, anions, represented by the - symbol , have the largest spheres because they receive electrons.
In this case, the [tex]Cl^-[/tex], [tex]S^2^-[/tex], [tex]Se^2^-[/tex] anions have the largest spheres.

This is because when donating electrons, the cations get the largest number of protons. This makes the cation nucleus attract the electronic layers, decreasing their extension. In anion, the opposite happens and the increase of electrons increases the extension of the electronic layers.

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