![]() ![]() alkali, and alkaline-earth metals, tend to be good reducing agents, as their valence electrons, whose radial orbit DEFINES the atomic radius, tend to be readily oxidized. On the other hand, the larger elements, i.e. Because of these two trends, the largest atoms are found in the lower left corner of the periodic table, and the smallest are found in the upper right corner (Figure 7.6. nitrogen, fluorine, oxygen, TEND to be very powerful oxidants, and this is also manifested by their small atomic size. In the periodic table, atomic radii decrease from left to right across a row and increase from top to bottom down a column. Excluding the Noble Gases, the smaller atoms from the right hand side, i.e. It follows that the SMALLEST atoms derive the right of the Table as we face it. Of course, the diagram shows NO data (it should do so), but the relative size of the atoms across the Period, and down the Group is clear. And the best metric that illustrates this trend is the well-known diminution of atomic radii across the Period from left to right? And of course, we should look at some data. In that case, the ionization energy decreases as atomic size increases due to adding a valence shell, thereby diminishing the nucleuss attraction to electrons. Now it is a fact that the nuclear charge is SHIELDED very poorly by incomplete electronic shells. The chemistry and atomic structure of the elements is a contest between (i) nuclear charge, conveniently represented by #Z_"the atomic number"#, and (ii) shielding by other electrons. The arrow indicates the direction of the increase. The Periodic Table below shows the trend of atomic size for groups. #"Increase in atomic radii down a Group, a column of the Periodic"#"Table."# Therefore, the trend within a group or family on the periodic table is that the atomic size increases with increased number of energy levels. ![]()
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