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
The definition of a noble gas is an atom in Group 0 of the Periodic Table and hence has all it electron p-shells filled, which is true for Argon (aswell as Helium, Neon, Krypton, Xenon and Radon).
neon has ten electrons. 8 electrons in the outer most orbit therefore it is more stable than sodium which has 11 electrons with electronic configuration 2, 8, 1. you require higher energy to remove one electron from Ne atom. so 1st IE of Ne is higher than that of Na.
Chlorine atom forms diatomis molecules. The two chlorine atoms in a chlorine molecule are held together by a strong covalent bond. Therefore,its covalent radius,which is one half of the distance between the nuclei of two chlorine atoms,is small. On the other hand, Argon is monoatomic. The atoms Are held together by weak forces(known as Van der waal's forces). So its radius (one half of the internuclear distance between two near argon atoms)is large.
argon is a noble gas, it is therefore monoatomic and the forces holding the atoms in the solid together are weak London dispersion forces. Sulfur is found as S8 molecular weight 256.5 the forces holding the molecules together are again weak London dispersion forces but it is considerably heavier than argon, (atomic weight of argon approx. 40)
The answer is in the electron configuration:
F: 1s2, 2s2, 2p5.
Ne: 1s2, 2s2, 2p6.
As you know, teh maximum capacity of the P subshell is 6. Because Neon has a full 2P subshell, and all electrons seek to fill in their shells - this way they are more stable, Neon does not want an electron to be taken, so it will "hold" on to it's elecrons tighter so the Ionization Energy (energy you need to put into the system to remove the electron) will be higher than Fluorine, who does not have a full 2P shell.
The actual IE values, by the way, are:
Fluorine 1.68
Neon 2.08
It requires more energy to heat more electrons and protons than less...so has higher boiling point
Helium is a very light atom, and it is difficult for it to hold a charge. You will find a periodic trend down the periodic table of lower and lower first ionization energies.
Higher surface area (larger atoms), larger van der waals forces.
The external shell of electrons is completely filled.
The first Ionization energy of fluorine is less than that of the helium and neon.
lithium
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.
No because neon is a noble gas so it only forms with helium,Argon and Hydrogen and that doesnt make Fluorine
Only Fluorine belongs in the halogen family.
The first Ionization energy of fluorine is less than that of the helium and neon.
lithium
because neon is a noble gas which has stable electronic configuration ,but this is not the same in case of fluorine.This means we have to give high energy to gaseous neon atom to ionise it.
Neon's ionization energy is 20.1397
The first ionization energy of neon is higher: 2 080,7 kJ/mol.
Cl
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.
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.
Helium (He) has the highest ionization energy, then Neon (Ne) Ionization energy increases as you go across a period from left to right. Ionization energy decreases as you go down a group. Therefore, elements in the upper right of the periodic table have the highest ionization energy.
If you think to neon this energy is 2 080 kJ/mol.
No- fluorine is a halogen and Neon is an inert or noble gas. Fluorine is one of the most reactive elements of all and Neon is the 2nd most unreactive after Helium. You can not get more different.