There are some exceptions to the trends of first and successive ionization energies. For each of the following pairs, explain which ionization energy would be higher:
(a) IE₁ of Ga or IE₁ of Ge
(b) IE₂ of Ga or IE₂ of Ge
(c) IE₃ of Ga or IE₃ of Ge
(d) IE₄ of Ga or IE₄ of Ge

2 nd ionisation requires higher amount of ionisation energy. In case of Ge , there are 2 electrons in outermost orbital so it becomes stable after ionisation of 2 electrons.

Manetho Manetho · Answer 2 · 2020-02-05T17:01:37+01:00

Explanation:

a) IE1 of Germenium. ionization energy decreases down the group.

b) Here IE2 of Ga is higher because second valence electron of gallium is in s orbital whereas second valence electron of germenium is in p orbital.

c) IE3 of Ge is higher as this follows the trend.

d)IE4 of Ga is higher because the 4th valence electron of Ga is a core electron and the for Ge it is in s orbital and it takes higher energy to break a core electron than the orbital ones.

There are some exceptions to the trends of first and successive ionization energies. For each of the following pairs, explain which ionization energy would be higher: (a) IE₁ of Ga or IE₁ of Ge (b) IE₂ of Ga or IE₂ of Ge (c) IE₃ of Ga or IE₃ of Ge (d) IE₄ of Ga or IE₄ of Ge

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There are some exceptions to the trends of first and successive ionization energies. For each of the following pairs, explain which ionization energy would be higher:
(a) IE₁ of Ga or IE₁ of Ge
(b) IE₂ of Ga or IE₂ of Ge
(c) IE₃ of Ga or IE₃ of Ge
(d) IE₄ of Ga or IE₄ of Ge