Explain the thinking that goes into the concept of the effective nuclear charge. Why do the outer electrons of fluorine behave as if the charge on the nucleus is 4 when it is actually 9?

a) Due to shielding effects, inner electrons partially cancel out the positive charge of the nucleus, resulting in a reduced effective nuclear charge.
b) Fluorine has a high electronegativity, causing its outer electrons to be more attracted to the nucleus.
c) The outer electrons of fluorine are located farther from the nucleus, experiencing less attraction to the positive charge.
d) Fluorine has a smaller atomic size compared to other elements, leading to stronger nuclear attraction on its outer electrons.