What is the identity of an element when the effective nuclear charge of its valence electrons is 18 while its shielding constant is 5?

(c) Detailed calculations indicate that the effective nuclear charge is 5.6+ for the 3s electrons and 4.9+ for the 3p electrons. Why are the values for the 3s and 3p electrons different?

(b) Would you expect it to require more or less energy to remove a 3s electron from the chlorine atom, as compared with a 2p electron?

In which orbital does an electron in a sulfur atom experience the greatest shielding?

Using Slater's Rules calculate the effective nuclear charge of the 4d orbital electron in iodine.