Which element in each of the following sets would you ex-pect to have the highest IE₂?(a) Na, Mg, Al(b) Na, K, Fe(c) Sc, Be, Mg
(a)
The first ionization energy is determined by the removal of an electron from the neutral parent atom. The value of the second ionization for all the elements will be higher than that of IE1 because the second electron is to be removed from the cation which is very difficult.
After the removal of an electron, Na will be converted into Na+ and its electronic configuration is 1s22s22p6 which represents the stable configuration of Ne.
For the second ionization energy, Na+ will have to lose an electron from its stable noble gas configuration of Ne, which is quite difficult so the value of IE2 will be the highest.
The atomic number of Mg is 12 so it's ground state electronic configuration is 1s22s22p63s2. After the removal of an electron, Mg will be converted into Mg+ and its electronic configuration is 1s22s22p63s1
For the second ionization energy, Mg+ will have to lose an electron and get converted into the stable noble gas configuration of Ne so the value of IE2 will be low.
The atomic number of Al is 13 so it's ground state electronic configuration is 1s22s22p63s23p1.
For the first ionization energy, the change in electronic configuration is as follows:
For the second ionization energy, the change in electronic configuration is as follows,
The first ionization energy is determined by the removal of an electron from the neutral parent atom. The value of the second ionization for all the elements will be higher than that of IE1 because the second electron is to be removed from the cation which is very difficult.
Answer: Na will have the highest value of IE2 among the given elements.
(b)
After the removal of an electron, Na will be converted into Na+ and its electronic configuration is 1s22s22p6 which represents the stable configuration of Ne.
For the second ionization energy, Na+ will have to lose an electron from its stable noble gas configuration of Ne, which is quite difficult so the value of IE2 will be the highest.
The atomic number of K is 19 so it's ground state electronic configuration is 1s22s22p63s23p64s1
For the first ionization energy, the change in electronic configuration is as follows:
For the second ionization energy, the change in electronic configuration is as follows,
For both sodium and potassium the second electron is removed from a stable noble gas configuration but because the size of sodium is smaller than potassium the second ionization energy of sodium will be greater than potassium.
The atomic number of Fe is 26 so it's ground state electronic configuration is 1s22s22p63s23p64s23d6
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