Define IE, and explain why Na has a smaller value than Cl in terms of ion stability (Na+1 versus Cl+1).
Would it be Na? But I can't explain why?
IE stands for ionization energy. It refers to the energy required to remove an electron from an atom or ion in its gaseous state. The ionization energy can help explain why Na has a smaller value than Cl in terms of ion stability.
When an atom or ion loses an electron, it forms a positive ion or cation. In the case of Na, it loses one electron to form Na+1, while Cl gains one electron to form Cl-1.
The ionization energy of an element is influenced by two main factors: the size of the atom/ion and the effective nuclear charge.
In terms of size, Na has a larger atomic radius compared to Cl. This means that the outermost electron in Na is further away from the nucleus and is less attracted to it than the outermost electron in Cl. As a result, it is easier to remove the electron from Na, requiring less energy.
Regarding the effective nuclear charge, it refers to the net positive charge experienced by the outermost electrons in an atom/ion. In Na, the effective nuclear charge is lower compared to Cl because Na has fewer protons in its nucleus. Therefore, the attractive force between the nucleus and the outermost electron is weaker in Na, making it easier to remove the electron.
In summary, both the larger atomic radius and lower effective nuclear charge contribute to Na having a smaller ionization energy compared to Cl. This lower ionization energy makes it easier for Na to lose an electron and form a stable Na+1 ion, while it is harder for Cl to lose an electron and form a Cl+1 ion.