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. The atomic radius is the radius of an atom that is measured from the nucleus to the outermost cloud of electrons.2 Group Period Atomic Radius Trend Atomic radius tends to increase as we go down the periodic table Atomic radius tends to decrease as we go across a period.
On the other hand, the larger elements, i.e. nitrogen, fluorine, oxygen, TEND to be very powerful oxidants, and this is also manifested by their small atomic size. Sn - Sb (stays the same) Sb - Te (increases) Pb- Bi (increases) Bi-Po (increases) At - Rn (tays the same) What accounts for the trend in atomic radii within a period Each successive. Cite any exceptions to the vernalization you stated in your answer to the question above. Do you notice a general trend (don’t worry about a few outlierslook for the overall trend) in the atomic radius across the period Describe the trend. As atomic increases, with in a period, the atomic radii decreases. So the atomic number is the independent variable that is placed on the x-axis by convention. Excluding the Noble Gases, the smaller atoms from the right hand side, i.e. The atomic radius is dependent on the number of protons found in an element. It follows that the SMALLEST atoms derive the right of the Table as we face it. Vocabulary: atomic radius, electron affinity, electron cloud, energy level, group, ion, ionization energy, metal, nonmetal, nucleus, period, periodic trends, picometer, valence electron Prior Knowledge Questions (Do these BEFORE using the Gizmo. 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. 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.
#"Increase in atomic radii down a Group, a column of the Periodic"#"Table."#
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