Answered

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Identify the element of Period 2 which has the following successive ionization energies in kJ mol:

IE1,1314 IE2,3389 IE3,5398 IE4, 7471
IE5, 100992 IE6,13329 IE,71345 IE8,84087

a. Li
b. B
c.O
d. Ne
e. None of these

Sagot :

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Answer:

c.O

Explanation:

From the periodic table:

Ionization energy tends to increase from IE6 → IE7 drastically at 13329 to 71345. Hence, from this process, we can infer that the removal of electrons takes place from the inner shell which in turn has a higher affinity for the nucleus. This must be oxygen because oxygen contains 6 valence electrons. The removal of this valence electron after the sixth ionization results in the achievement of a stable nearest Noble gas configuration. Hence, the rapid change in the ionization is obvious from IE6 to IE7.

Thus, the element that relates to the IE trend is oxygen.

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