How would you explain the fact that the second ionisation potential is always higher than the first ionisation potential?

संक्षेप में उत्तर

Second ionization potential is always higher than the first ionization potential.
Removal of one electron from the valence orbit of a neutral gaseous atom is easy so first ionization energy is less. But from a uni positive ion, removal of one more electron becomes difficult due to the more forces of attraction between the excess of protons and less number of electrons.
Due to greater nuclear attraction, second ionization energy is higher than first ionization energy.

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अध्याय 3: Periodic Classification Of Elements - Evaluation [पृष्ठ ९६]

अध्याय 3 Periodic Classification Of Elements
Evaluation | Q II. 7. | पृष्ठ ९६

Various successive ionisation enthalpies (in kJ mol^-1) of an element are given below.

IE₁	IE₂	IE₃	IE₄	IE₅
577.5	1,810	2,750	11,580	14,820

The element is

In the third period the first ionization potential is of the order.

The element with positive electron gain enthalpy is

The correct order of decreasing electronegativity values among the elements X, Y, Z and A with atomic numbers 4, 8, 7 and 12 respectively

Assertion: Helium has the highest value of ionisation energy among all the elements known

Reason: Helium has the highest value of electron affinity among all the elements known

The electronic configuration of the atom having maximum difference in first and second ionisation energies is

How does electron affinity change when we move from left to right in a period in the periodic table?

What are isoelectronic ions? Give examples.

Magnesium loses electrons successively to form Mg⁺, Mg²⁺and Mg³⁺ ions. Which step will have the highest ionisation energy and why?

Define electronegativity.