Ionization energy is the energy required to remove an electron from an atom or a positive ion. Generally, ionization energy tends to increase across a period (from left to right) and decrease down a group (from top to bottom) in the periodic table.
Helium typically has the highest ionization energy among the elements. This is because helium, with its electron configuration 1s², has a fully filled electron shell, making it more stable. Removing an electron from a stable, fully-filled shell requires more energy compared to other elements.
In general, noble gases (helium, neon, argon, etc.) have high ionization energies due to their stable electron configurations. The trend of increasing ionization energy across a period is also observed for nonmetals, while alkali metals (such as cesium and francium) at the bottom of Group 1 have relatively low ionization energies.
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The elements with the highest ionization energy is Helium (He).
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Ionization energy is the energy required to remove an electron from an atom or a positive ion. Generally, ionization energy tends to increase across a period (from left to right) and decrease down a group (from top to bottom) in the periodic table.
Helium typically has the highest ionization energy among the elements. This is because helium, with its electron configuration 1s², has a fully filled electron shell, making it more stable. Removing an electron from a stable, fully-filled shell requires more energy compared to other elements.
In general, noble gases (helium, neon, argon, etc.) have high ionization energies due to their stable electron configurations. The trend of increasing ionization energy across a period is also observed for nonmetals, while alkali metals (such as cesium and francium) at the bottom of Group 1 have relatively low ionization energies.