Question

Which one of the following statements is incorrect in relation to the ionization enthalpy?
A. Ionization enthalpy increases for each successive valence shell electron.
B. The greatest increase in ionization enthalpy is experienced on removal of electrons from the core of noble gas configuration.
C. End of valence electrons is marked by a big jump in ionization enthalpy.
D. Removal of electrons from orbitals bearing lower n value is easier than from an orbital having higher n-value.

Answer 1

Remember the ionization enthalpy of ionization potential of an atom or an element is the amount of energy that is required to remove one electron from the atom or an element. And deeper the electron is placed; more will be its ionization enthalpy.

Complete step by step answer:
So, to solve such a problem, we will first check all the statements to find whether it is wrong or not, but before that let’s see what is meant by ionization enthalpy.
Ionization enthalpy of an element can be referred to as the amount of energy which will be required to remove one electron from an isolated gaseous atom in its gaseous state. Remember, closer the electrons present, more will be the requirement of energy to remove from its orbital. The electrons which are present below the valence shell are known as core electrons.
So, going through each option we see that,
Ionization enthalpy increases for each successive valence shell electron (means the first ionization enthalpy will be less than the second ionization enthalpy) stating a correct statement.
As explained above, the noble gas configuration (stable in nature) will have higher ionization energy. So, this is also correct. Further, in option C the end of the valence electron will mark a big jump in the ionization energy as the first energy required will be less than the second ionization enthalpy.
Further coming to option D, the orbitals having lower n value will be closer to the nucleus and thus the electrons will experience greater attraction from the nucleus and thus will require more energy for the removal of the electrons. Thus, this statement given is incorrect.
So, the correct answer is “Option D”.

Note: Ionization energy of an element usually depends on the force of attraction between the negatively charged electrons and the positively charged nuclei. In a periodic table, when we move from the left to right ionization enthalpy increases while moving from top to bottom, it decreases.