Cl -apex.
The element with the highest first ionization energy in group 14 is carbon.
Fluorine has the largest first ionization energy among the halogens.
Potassium has the smallest first ionization energy among those elements listed. This is because potassium has the largest atomic size and the weakest attraction between its nucleus and outermost electron, making it easier to remove that electron.
Noble gases have the highest first ionization energies because they have a full valence shell, making it difficult to remove an electron. Within a period, ionization energy generally increases from left to right due to increasing nuclear charge.
Carbon (C) has a higher first ionization energy than silicon (Si). This is because as you move across a period in the periodic table, the first ionization energy generally increases due to increasing nuclear charge pulling electrons closer. Silicon is positioned to the right of carbon in the same period, resulting in a lower first ionization energy compared to carbon.
Fluorine has the largest first ionization energy among the halogens.
The element with the largest first ionization energy is (a) Sb (antimony). It has the highest first ionization energy among the elements listed.
Helium has the highest ionization energy.
No, helium does not have the largest first ionization energy of all the elements. Helium actually has the highest first ionization energy of any element, due to its small atomic size and stable electron configuration.
The element with the highest first ionization energy in group 14 is carbon.
Fluorine has the largest first ionization energy among the halogens.
boron
Helium has the highest ionization energy.
Helium has the highest ionization energy.
Potassium has the smallest first ionization energy among those elements listed. This is because potassium has the largest atomic size and the weakest attraction between its nucleus and outermost electron, making it easier to remove that electron.
Beryllium will have the highest. Down a group ionization energy decreases.
Noble gases have the highest first ionization energies because they have a full valence shell, making it difficult to remove an electron. Within a period, ionization energy generally increases from left to right due to increasing nuclear charge.