Why does fluorine have higher ionization energy than chlorine?

Since the most loosely held electron in fluorine is closer to the nucleus than chlorine, it takes more energy to remove the electron from fluorine than in chlorine. As a result, their energies are equal in magnitude but opposite in sign.

Why is the ionization energy for chlorine less than fluorine?

Now we can conclude that the ionization energy for chlorine should be lower than that of fluorine because the electron would be easier to pull off when it is further away from the nucleus.

Why does fluorine have a higher ionization energy?

Fluorine has higher ionization energy than iodine because the size of fluorine is smaller than the iodine. This means that the shielding effect is less for fluorine. Therefore, the nucleus attracts more valence electrons in fluorine than in iodine.

Why electron affinity of chlorine is more than fluorine all the electron affinity decreases down the group?

Fluorine, which is higher up the group then chlorine, has a lower electron affinity. This is because the electrons in the outermost shell of a fluorine atom are closer together. Energy is required to keep the gained electron in the shell, causing fluorine to have a smaller electron affinity than chlorine.

Why would fluorine have a smaller atomic radius than chlorine?

Fluorine has a smaller atomic radius than oxygen because fluorine has a larger nuclear charge. Fluorine has a smaller radius than chlorine because it has eight fewer electrons.

Why does fluorine have a higher electron affinity than bromine?

As the atomic size increases the nuclear charge towards the valence electron decreases. So affinity for electron also decreases. Hence fluorine has more affinity for electron than bromine.

Why does fluorine have a smaller atomic radius than chlorine?

Does fluorine have high electron affinity?

Electron affinity follows the trend of electronegativity: fluorine (F) has a higher electron affinity than oxygen (O), and so on. The trends noted here are very similar to those in ionization energy and change for similar (though opposing) reasons.

Why does the electron affinity of fluorine have a negative value?

Electron affinity is the energy released when 1 mole of gaseous atoms each acquire an electron to form 1 mole of gaseous 1- ions. Fluorine has a negative value as energy is released when the electron is gained. This is because there is an attraction between the protons in the nucleus and the added electrons.

Why does fluorine have a bigger atomic radius?

So fluorine has more protons in its nucleus. Since outermost electrons are located on the same energy level in both the lithium and the fluorine atoms, it follows that the nucleus that has more protons will attract these electrons more – this is known as effective nuclear charge.

Why electron affinity of fluorine is less than that of chlorine?

This is because the size of fluorine atom is very small as compared to chlorine atom and due to its small size there are strong inner repulsions among valence electrons and so the outer electron doesnot feel the attraction from the nucleus. So electron affinity of fluorine is less than that of chlorine.

Why is the ETA of fluorine less than that of chlorine?

E.A of fluorine is less than that of chlorine due to two reasons: (1) Small size fluorine atom makes the 2p subshell more compact. This results in repulsion among electrons of the valence shell and also with electron to be added. Due to this F atom has less tendency to accept electron.

Why does fluorine have a low effective nuclear charge?

Due to this F atom has less tendency to accept electron. (2) Because of small size of fluorine, there will be high electron density around the nucleus. This high electron density screens the nucleus. Because of this, effective nuclear charge gets decreased.

Why does Cl have a higher ionization energy than FL?

So lesser energy must be provided to remove the outermost electron in Cl when compared to that with Fl. Therefore Fl has a higher ionization energy than Cl. Because chlorine is a larger atom and has a lower effective nuclear charge.