The first ionization potential of Na, Mg, Al, and Si are in the order: (1) Na < Mg > Al < Si (2) Na >Mg>Si>Al (3) Mg > Na > Al > Si (4) Na > Al > Mg > Si.

By Ritesh|Updated : November 8th, 2022

The first ionization potential of Na, Mg, Al, and Si are in the order Na < Mg > Al < Si. The period II elements include Na, Mg, Al, and Si. From left to right, the ionisation potential rises over time. Al has a lower ionisation potential than Mg because Mg's highest energy orbital (3s) has paired electrons, whereas Al's highest energy orbital (3p) has an unpaired electron. Since it is energetically advantageous for all the electrons in an orbital to be paired, it would take more energy to break up this pair.

Ionization potential is the potential difference that corresponds to the amount of energy, measured in electron volts, required to completely remove an electron from an atom or ionize a gas molecule. Ionization energy, which is expressed in electron volts, is the energy that corresponds to ionisation potential.

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Factors affecting Ionization Energy

The electrons are attracted to the nucleus strongly if it has a positive charge.
The attraction will be stronger if an electron is nearby or close to the nucleus than if it is farther away.
The attraction forces are weaker if there are more electrons between the outer level and the nucleus.
Two electrons in the same orbital are subject to some sort of repulsion when they are there. Consequently, the nucleus's attraction is disturbed. In essence, paired electrons will exhibit lower ionisation energy due to their ease of removal.

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