Neon had a higher proton charge than Fluorine (first I.E increase)
Neon the same radius, due to the same amount of shells, but it is slightly smaller than fluorine due to a higher number of protons in the nucleus attracting the electrons in the outer shells close (Doesn't really affect first I.E.)
Neon also has the same amount of shielding electrons, due to having the same number of sub-shells, therefore this doesn't really affect I.E. either
However the largest factor is that the 2p sub shell in neon is full, whereas in fluorine it is not, a full sub shell means that the atom is more stable therefore ionization energy significantly rises.
Therefore Neon, overall has a larger first ionization energy.
Neon- First I.E.=2080.7
Fluorine-First I.E. =1681.0
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.
Helium and neon are noble gases, which have full valence shells of electrons and are highly stable. They do not readily form compounds with other elements, including fluorine, because they have little tendency to gain or lose electrons to form chemical bonds. This makes them unreactive and inert.
In the periodic table of elements, fluorine and iodine are in the same column, but fluorine is in the second, iodine in the fifth row. That means fluorine has only nine electrons flying around in orbitals while iodine has 53 of them. Ionization is the called a process during which a single electron is abstracted - we're now talking about the 1st ionization energy, which is much higher for fluorine. Well, as it only has nine electrons scattered in the orbitals (but according laws, of course), they do not really influence the repelling - attracting actions between the positive center and the other electrons beside them. For iodine with 53 electrons, they really do interfere with the attraction of other electrons AND as the outmost electrons (which are the ones taken away by ionization) are in those orbitals which are at the biggest distance to the center - for 53 electrons the outmost orbitals is at a much bigger distance... both results in a smaller attraction of the electrions at max distance from the center... so for iodine you need less energy to perform ionization.
When fluorine forms an ionic bond to achieve the electron configuration of neon, it gains one electron to become a fluoride anion. By gaining an electron, fluorine's outer electron shell is filled with eight electrons, similar to neon's stable electron configuration. This allows the fluorine atom to achieve greater stability.
Neon does not form compounds with fluorine because neon is a noble gas with a full outer electron shell, making it very stable and unreactive. Fluorine is a highly reactive non-metal that tends to react with other elements to fulfill its electron configuration.
Fluorine has a higher ionization energy than neon because fluorine has one less electron shell than neon, resulting in a stronger attractive force between the nucleus and the outermost electron. Additionally, fluorine's smaller atomic size leads to greater electron-electron repulsions, making it more difficult to remove an electron from fluorine compared to neon.
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.
Neon's ionization energy is 20.1397
Cl
The first ionization energy of neon is higher: 2 080,7 kJ/mol.
Neon is a much smaller atom than selenium because neon has fewer occupied energy levels so it has a considerably smaller atomic radius. For that reason, it will be more difficult to remove an electron from Ne than Se, so Ne has the greater ionization energy.
Helium and neon are noble gases, which have full valence shells of electrons and are highly stable. They do not readily form compounds with other elements, including fluorine, because they have little tendency to gain or lose electrons to form chemical bonds. This makes them unreactive and inert.
Neon
In the periodic table of elements, fluorine and iodine are in the same column, but fluorine is in the second, iodine in the fifth row. That means fluorine has only nine electrons flying around in orbitals while iodine has 53 of them. Ionization is the called a process during which a single electron is abstracted - we're now talking about the 1st ionization energy, which is much higher for fluorine. Well, as it only has nine electrons scattered in the orbitals (but according laws, of course), they do not really influence the repelling - attracting actions between the positive center and the other electrons beside them. For iodine with 53 electrons, they really do interfere with the attraction of other electrons AND as the outmost electrons (which are the ones taken away by ionization) are in those orbitals which are at the biggest distance to the center - for 53 electrons the outmost orbitals is at a much bigger distance... both results in a smaller attraction of the electrions at max distance from the center... so for iodine you need less energy to perform ionization.
The noble gases such as helium, neon, argon, and xenon typically have the highest ionization energies on the periodic table. This is because they have a full valence shell of electrons which makes it difficult to remove an electron.
Elements in the top right corner of the periodic table tend to have the largest first ionization energies. This includes elements such as helium, neon, and fluorine. They have a strong attraction for their valence electrons due to their small atomic size and high effective nuclear charge.
The closest noble gas to fluorine is neon. Neon is located directly above fluorine on the periodic table.