Why is the ionization energy for Neon greater than Fluorine?

Answer 1

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

Answer 2

The ionization energy of Neon is greater than Fluorine because Neon has a full outer electron shell (valence shell), making it very stable and less likely to lose an electron compared to Fluorine, which only needs to lose one electron to achieve a stable electron configuration. Therefore, it requires more energy to remove an electron from Neon than from Fluorine.

Answer 3

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).

Answer 4

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.

Answer 5

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.

Answer 6

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)

Answer 7

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

Answer 8

It requires more energy to heat more electrons and protons than less...so has higher boiling point

Answer 9

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.

Answer 10

Higher surface area (larger atoms), larger van der waals forces.