Question

27. The first five ionization energies of an element, X, are shown in the table. Ionization energy 1st 2nd 3rd 4th 5th Value / kJ mol-1 631 1235 2389 7089 8844 What is the mostly likely formula of the oxide that forms when X burns in oxygen A. X20 O B. XO I C. X203 D. XO2​

Answer 1

The correct formula of the oxide that forms when X burns in oxygen is X2O3.

Ionization energy is defined as the energy required to remove an electron from an atom. There are as many ionization energies present in an atom as there are electrons in that atom.

However, we can know the ionization energy values that belong to electrons in the outermost shell because they lie close together. If we go further into the inner shells, there is a sudden quantum jump in ionization energy values.

The element X must have three valence electrons because  631 ,1235, 2389 all refer to ionization energies of electrons in the valence shell. As we get into a core shell, there is a sudden jump hence the fourth and fifth ionization energies are 7089 and 8844 respectively.

The correct formula of the  oxide that forms when X burns in oxygen is X2O3.

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