Helium has the highest first ionization energy and francium has the lowest first ionization energy.
The order from highest to lowest ionization energy is Cl > Al > Si > Na > S. This is because ionization energy generally increases from left to right and from bottom to top in the periodic table.
The lowest first ionization energy is found in francium, the element with the highest atomic number. Francium has the lowest ionization energy because the outermost electron is held the weakest due to the large atomic size and shielding effects.
Elements in the alkali metal group (Group 1) have the lowest first ionization energy within any periodic table. This is because they have a single electron in their outermost shell, which is easier to remove compared to other elements. Sodium and potassium are examples of alkali metals.
Sodium (Na) has the lowest first ionization energy in period 3.
Group 1 because across group 1 to 8 nuclear force of attraction increases to a significant extent and as a result greater amount of energy is needed to remove an electron. More specifically Fr has the lowest IE and He has the highest
The energy required for an element to ionize and helium has the lowest.
Ne (Highest First Ionization Energy) C Be Mg Sr (Lowest First Ionization Energy)
Among the given elements, neon has the lowest ionization energy. It is in Group 18 (Noble Gases) of the periodic table, and noble gases have the highest ionization energies due to their stable electron configurations.
There is no relation ship. They have the lowest ionization energies.
strontium
The order from highest to lowest ionization energy is Cl > Al > Si > Na > S. This is because ionization energy generally increases from left to right and from bottom to top in the periodic table.
The lowest first ionization energy is found in francium, the element with the highest atomic number. Francium has the lowest ionization energy because the outermost electron is held the weakest due to the large atomic size and shielding effects.
All of the elements on the top half of the periodic table belong in upperionizationenergy because the trend is top to bottom. Top being lowest and getting bigger as it goes down.------------------------------------------------------* In a group: the ionization energy decrease from the lighter elements to heavier elements.* In a period: the ionization energy increase from the left elements to the elements of the right.* When the atomic radius decrease the ionization energy increase.
Elements in the alkali metal group (Group 1) have the lowest first ionization energy within any periodic table. This is because they have a single electron in their outermost shell, which is easier to remove compared to other elements. Sodium and potassium are examples of alkali metals.
Sodium (Na) has the lowest first ionization energy in period 3.
the lowest ionization energy in IA :hydrogen ,lithiun ,sodium and potassium
The elements that typically give up electrons are the ones which have the lowest ionization energy. The valence electron which holds on loosely will be the one to be given out easily.