Is the sodium ion larger than the fluoride ion?

Answer 1

Sodium ion is smaller than fluoride ion. Sodium ion and fluoride ion are isoelectronic.They have the same number of electrons. For example, Na+ and F- has 10 electrons.In any isoelectronic series we can list the members in order of increasing atomic number; therefore, nuclear charge increases as we move trhrough the series. Because the number of electrons remains constant, ionic radius decreases with increasing nuclear charge as the electrons are more strongly attracted to the nucleus.

Answer 2

Because the fluorine ion has an extra electron which is not held as tightly as the other 7 valence electrons. The effective nuclear charge of fluorine is +7, so its' 7 valence electrons are held tightly, but that Zeff is not powerful enough to maintain the small size of fluorine once an electron is added.

Answer 3

Although fluorine has a larger mass, the general rule for the Periodic Table is, as you move across a period (from left to right) - the size of elements decreases. This is because - elements of the same period have the same number of shells (ie lithium and fluorine both have 2 energy shells). The difference is - as fluorine has more protons - its nucleus has a strong force of attraction and thus - it holds the energy shells more 'tightly' then lithium resulting in a more 'compact' atom (which is smaller).

Answer 4

No, the fluoride ion is larger than the sodium ion. This is because the sodium ion has lost an electron, resulting in a smaller size due to increased nuclear charge pulling the remaining electrons closer. The fluoride ion, on the other hand, has gained an electron, leading to an increase in electron-electron repulsions and thus a larger size.

Answer 5

Yes! A Fluorine ion has two full shells of electrons while Lithium only has one full shell!

Answer 6

Fluorine