What is inert pair effect?
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The inert pair effect is defined as the tendency of electrons in the outermost atomic s orbital to remain unionized or unshared in compounds of post-transition metals. For simplicity, let’s summarize it as the tendency of heavier atoms to form ions with a difference in charge of two. When we say that electrons are inert, we essentially mean that they are spin paired. An example is in helium, with two electrons. Its orbital diagram looks like this:
This can be seen in other noble gases as well, where the generic configuration involves ns^2, np^6. All electrons are paired, and inert.
Let's take a look at antimony. Its electron configuration is
For the ionization of antimony, we would begin by removing the valence electrons in the outermost shell, 5p, because it has the highest energy. We remove 3 electrons, thus giving us Sb3+
For the second cation of antimony, we remove valence electrons from the s orbital by convention. We remove two additional electrons, thus giving us Sb 5+
As you can see, there is a difference of 2 between the two ions of antimony, +3 and +5.
I'll use lead as a second example. Its electron configuration is
We begin, as before, by removing the electrons from the outermost shell, 6p. We remove 2 electrons, thus giving us Pb2+
Again, for the second ionization, we will remove electrons from the 6s orbital. We remove 2 additional electrons, thus giving us Pb4+
We can see that there is a difference of 2 in the charges between Pb2+ and Pb4+
No electrons are left unpaired, no orbital diagrams incomplete
This can be seen in other noble gases as well, where the generic configuration involves ns^2, np^6. All electrons are paired, and inert.
Let's take a look at antimony. Its electron configuration is
For the ionization of antimony, we would begin by removing the valence electrons in the outermost shell, 5p, because it has the highest energy. We remove 3 electrons, thus giving us Sb3+
For the second cation of antimony, we remove valence electrons from the s orbital by convention. We remove two additional electrons, thus giving us Sb 5+
As you can see, there is a difference of 2 between the two ions of antimony, +3 and +5.
I'll use lead as a second example. Its electron configuration is
We begin, as before, by removing the electrons from the outermost shell, 6p. We remove 2 electrons, thus giving us Pb2+
Again, for the second ionization, we will remove electrons from the 6s orbital. We remove 2 additional electrons, thus giving us Pb4+
We can see that there is a difference of 2 in the charges between Pb2+ and Pb4+
No electrons are left unpaired, no orbital diagrams incomplete
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The outer sell of S electron (nS2) penetrate to (n-1) d electron and thus become closer to nucleus and more effective pulled towards nucleus. therefore less availability of ns2 electron pair for bonding or ns2 electron pair become inert.
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