Define IE and write factors affecting it
Answers
Answer:
Size of atom (distance of outermost electron from the nucleus) As atomic size increases, the attraction of the positive nucleus for the negative electron decreases and less energy is required to remove an electron. This means that the ionisation energy decreases.
Explanation:
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Answer:
IE is the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom or molecule.
Factors
(i) Size of the atom
As the distance between the electron and the nucleus increases, i.e., as the size of the atom increases, the outermost electrons are less tightly held by the nucleus. Thus, it becomes easier to remove an outermost electron. Thus ionization enthalpy decreases with increases in atomic size.
(ii) Charge on the nucleus
Ionization enthalpy increases with
increase in nuclear charge because of the increase in the attractive force between the nucleus and the electron.
(iii) Screening effect of inner electrons
Ionization enthalpy decreases when the shielding effect of inner electrons increases. This is because when the inner electron shells increases, the attraction between the nucleus and the outermost electron decreases