Electronegativity -

Electronegativity is the tendency of atoms in covalent bonds to attract electrons closer to themselves (I'll admit I realised ions do not form covalent bonds only after I finished writing).

Electronegativity depends on a variety of factors including the number of protons, the number of electrons in the outer shell and the ionic radii. In general it depends on the effective nuclear charge (or the pull)

Generally Atoms towards the left end of the Periodic Table are more electropositive (groups 1,2,3...) while those at the right end of the Periodic Table are more electronegative (group 17,16...). So $Cl$ should be more electronegative than $Na$.

Now coming to ions, it should be noted that in Chlorine the outermost shell is completely filled so its nearly impossible for Chlorine to continue attracting due to electron repulsions, So its EN must have reduced

On the other hand, Na+ is positively charged and so it should be attracting more electrons but isn't its octet already filled so should it be still attracting electron?

Is it incorrect to compare qualitatively the electronegativities of ions? I wasn't able to find much on the google about it.

Electronegativity is the tendency of atoms in covalent bonds to attract electrons closer to themselves (I'll admit I realised ions do not form covalent bonds only after I finished writing).

Electronegativity depends on a variety of factors including the number of protons, the number of electrons in the outer shell and the ionic radii. In general it depends on the effective nuclear charge (or the pull)

Generally Atoms towards the left end of the Periodic Table are more electropositive (groups 1,2,3...) while those at the right end of the Periodic Table are more electronegative (group 17,16...). So $\ce{Cl}$ should be more electronegative than $\ce{Na}$.

Now coming to ions, it should be noted that in Chlorine the outermost shell is completely filled so its nearly impossible for Chlorine to continue attracting due to electron repulsion, so its EN must have reduced.

On the other hand, $\ce{Na+}$ is positively charged and so it should be attracting more electrons but isn't its octet already filled so should it be still attracting electron?

Is it incorrect to compare qualitatively the electronegativities of ions? I wasn't able to find much on the google about it.

Electronegativity is the tendency of atoms in covalent bonds to attract electrons closer to themselves (ill admit I realised ions do not form covalent bonds only after I finished writing).

Electronegativity depends on a variety of factors including the number of protons, the number of electrons in the outer shell and the ionic radii. In general it depends on the effective nuclear charge (or the pull)

Generally Atoms towards the left end is more electropositive (groups 1,2,3...) while those at the left is more electronegative (group 17,16...). So Cl should be more electronegative than Na

Now coming to ions, it should be noted that in Chlorine the outermost shell is completely filled so its nearly impossible for Chlorine to continue attracting due to electron repulsions, So its EN must have reduced

On the other hand, Na+ is positively charged and so it should be attracting more electrons (but wait, isn't its octet already filled so should it be still attracting electron?)

Coming back to my first line, is it incorrect to compare qualitatively the electronegativities of ions. I wasn't able to find much on the google about it.

Electronegativity -

Electronegativity is the tendency of atoms in covalent bonds to attract electrons closer to themselves (I'll admit I realised ions do not form covalent bonds only after I finished writing).

Electronegativity depends on a variety of factors including the number of protons, the number of electrons in the outer shell and the ionic radii. In general it depends on the effective nuclear charge (or the pull)

Generally Atoms towards the left end of the Periodic Table are more electropositive (groups 1,2,3...) while those at the right end of the Periodic Table are more electronegative (group 17,16...). So $Cl$ should be more electronegative than $Na$.

Now coming to ions, it should be noted that in Chlorine the outermost shell is completely filled so its nearly impossible for Chlorine to continue attracting due to electron repulsions, So its EN must have reduced

On the other hand, Na+ is positively charged and so it should be attracting more electrons but isn't its octet already filled so should it be still attracting electron?

Is it incorrect to compare qualitatively the electronegativities of ions? I wasn't able to find much on the google about it.