![]() I would put it between #"Al"# and #"Ag"#. When you add two electrons, the electron repulsion is so great that the ion swells to the size of atoms in the next row of the Periodic Table. The general trend is that atomic sizes increase as one moves downwards in the Periodic Table of the Elements, as electrons fill outer electron shells. #"Period": color(white)(m)2color(white)(mm)3color(white)(mmm) 3color(white)(mml)3color(white)(mml)5color(white)(mml)5color(white)(mmll)6# I would move it to the other side of #"Si"#: When #"Al"# loses its three #(n = 3)# electrons to form #"Al"^"3+"#, the outer electron shell becomes the #(n = 2)# level, so the cation is smaller than the atom. ![]() #"Period": color(white)(m)2color(white)(mm)3color(white)(mm) 3color(white)(mml)5color(white)(mml)5color(white)(mmll)6# The smallest atoms are at the top right and the largest atoms are at the lower left of the Periodic Table. We know that atomic size increases from right to left and from top to bottom in the Periodic Table. It is fairly easy to arrange the atoms according to atomic size. Note the trends indicated above apply only to Covalent Radii and not to van der Waals Radii. There is a list of atomic (covalent) radii here: The rest line up according to the periodic table as mentioned above. As a result, the #3Al^(3+)# ion will be smaller than the #Si# element, which has #14# protons attracting #14# electrons. Arrange the members of each of the following sets of elements in order of increasing first ionization energies: (a) the alkali metals. In this case, we have 13 protons attracting ten electrons. The aluminum ion is much smaller than the elementary aluminum with the loss of three electrons. It has grown in radius to 140nm, to position its size into the next period. The oxygen ion you have with #8# protons attracting #10# electrons is larger, with it's two extra electrons, than the oxygen in the elementary form. ![]() Outer electrons can move further away from the nucleus. This effectively pulls the electrons closer to the nucleus.Ītomic size increases moving top to bottom because of the addition of another ring of electrons to each element as we move from top to bottom. Atomic size decreases left to right on the periodic table because the attractive force of the protons on the same number of rings of electrons increases for each element as we move left to right.
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