The size of ions as measured by ionic radii varies in a systematic manner. The size of the ion can be explained in part by effective nuclear charge, Z eff, which is the net nuclear charge felt by an electron. The effective nuclear charge takes into account the actual nuclear charge and the shielding of this charge by inner electrons. When an atom loses electrons, the resulting cation is smaller both because the remaining electrons experience a larger Z eff and because these electrons are usually in orbitals closer to the nucleus than the electrons that were lost. The more electrons that are lost, the smaller the ion becomes.
Similarly, when an atom gains electrons, the resulting anion is larger owing to both increased electron-electron repulsions and a reduction in Z eff. The more electrons that are gained, the larger the ion becomes.
1.) Rank the following ions in order of decreasing radius: F− , Cl− , Br− , I− , and At− .
2.) Rank the following items in order of decreasing radius: Ca , Ca2+ , and Ca2− .
3.) Rank the following in order of decreasing ionic radii. K+, S^2-, Ca^2+, Sc^3+, Cl^-, P^3-
Posted on October 16, 2013, in Question and tagged Chemistry, effective nuclear charge, electrons, Ionic Radii, nuclear charge, question, science, The size of ions as measured by ionic radii. Bookmark the permalink. Leave a comment.