Even though Fluorine has the highest electronegativity among all the elements and it should have the highest electron gain enthalpy among all the halogens but
this is an exception and chlorine has higher electron gain enthalpy than Fluorine.
The reason for this is that the size of Fluorine atom is very small and hence there is very high inter-electronic repulsion among the electrons of fluorine.
This makes incoming of another electron not very favourable.
Even though fluorine has large negative electron gain enthalpy but for chlorine its even more negative.
Many similarities exist between fluorine and chlorine.
no
Chlorine is extremely electronegative and will steal electrons from the valence shell of sodium. When chlorine steals the electron, both sodium and chlorine have full valence shells.
Chlorine has one more electron then sulfur, so it has 1 more electron in the outer shell, 1 more valence electron. Chlorine has 5 electrons in the outermost shell and sulfur has 4.
A chlorine ion has one less electron, giving it a +1 charge.
electron affinity is the negative of electron gain enthalpy. for example, the electron gain enthalpy of fluorine is -328, and electron affinity is 328 which is -(-328)
Generally electron affinity goes up as you go from left to right across the periodic table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine (note that the most electronegative element is fluorine however).The reason that the electron affinity is not as high as might otherwise be predicted for fluorine is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).Note that there are a number of other exceptions to the general rule of electron affinity increasing towards the upper right corner -- see the Related Questions links to the left for an explanation of some of those other exceptions.See also the Web Links to the left for more information about electron affinities and the fluorine-chlorine exception.
Generally electron affinity goes up as you go from left to right across the Periodic Table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine (note that the most electronegative element is fluorine however).The reason that the electron affinity is not as high as might otherwise be predicted for fluorine is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).Note that there are a number of other exceptions to the general rule of electron affinity increasing towards the upper right corner -- see the Related Questions links to the left for an explanation of some of those other exceptions.See also the Web Links to the left for more information about electron affinities and the fluorine-chlorine exception.
This element is fluorine.
Generally electron affinity goes up as you go from left to right across the periodic table, and decreases as you go down a column. However, fluorine is an exception -- and the element with the highest electron affinity is chlorine.(Note that the most electronegative element is fluorine however; 'electronegativity' is not exactly the same as 'electron affinity'.)Electronegativity is the ability of an atom in a molecule to draw bonding electrons to itselfElectron affinity is a measure of the energy change when an electron is added to a neutral atom to form a negative ion.The reason that the electron affinity is not as high as might otherwise be predicted for fluorine, is that it is an extremely small atom, and so it's electron density is very high. Adding an additional electron is therefore not quite as favorable as for an element like chlorine where the electron density is slightly lower (due to electron-electron repulsion between the added electron and the other electrons in the electron cloud).
Fluorine's electron configuration is 1s2 2s2 2p5, and since fluoride is just fluorine with an extra electron, or F-1, its electron configuration is 1s2 2s2 2p6.
Many similarities exist between fluorine and chlorine.
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no
Only one, from sodium to chlorine.
in sodium chloride chlorine gains an electron and the bond formed between then is ionic.
AnswerElectron affinity is the energy released when we add an electron to the outermost orbit of the atom. Halogens are the higher in electron affinity, and chlorine has the higher electron affinity than rest of the halogens. The irregularity in the electron affinity trend between Cl and F is due to the small size of the F atom. Although F definitely has a higher attraction for an electron than Cl (as evidenced by its high electro negativity value), the small size of the F atom means that adding an electron creates significant repulsion. Since electron affinity is an energy measurement, the total energy associated with electron affinity winds up being the energy that is released by the electron binding to the nucleus, minus the energy involved in overcoming the electrical repulsion in the outer shell.This makes the fluoride anion so formed unstable due to a very high charge/mass ratio. Also, fluorine has no d electrons which limits its atomic size. As a result, fluorine has an electron affinity less than that of chlorine.