Question

The amount of energy required to remove an electron from an isolated atom or molecule is the ionization potential. There is an ionization energy for each successive electron removed.
A. True
B. False

Answer 1

Hint: The electrons are bound with the help of electrostatic force created by the nucleus and more the closer the electron is to the nucleus, there will be more energy required to remove the electron from that particular shell. That’s why there are core electrons and valence electrons and only valence electrons take part in the process of the formation of a bond.

Complete step by step process:
The amount of energy required to remove an electron from an isolated atom or molecule is called ionization potential resulting in a cation. This energy is measured in KJ/mol.
$H(g)\to {{H}^{+}}(g)+{{e}^{-}}$
There is an ionization energy for each successive electron removed as the electron which is removed first will take less energy than the second one and second one will require less energy than the third one. Therefore, there is a particular ionization energy for each successive electron removed.
There is a difficulty in removing the second electron as compared to the first because once an electron is removed then the whole atom acquires a positive charge and the electrons are more attracted to this newly formed positive charge. Therefore, as stated above ionization energy is a function of atomic radius, the farther the electron is from the nucleus, the easier it is to get removed.
But the second statement is incorrect because generally, ionization energy of the electron which is removed first is used. Therefore, the answer to this question is false.

Note: Some formulas are given in various books which are derived from the Bohr’s model of atom and usually determined for the Hydrogen atom, but it is good for students if they try the question related to ionization energy with the help of basic concepts.