![]() 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. ![]() ![]() nitrogen, fluorine, oxygen, TEND to be very powerful oxidants, and this is also manifested by their small atomic size. 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. EA also follows this trend, because electrons will me more attracted to an atom. (b) Covalent radii of the elements are shown to scale. We can use these periodic trends to predict relative atomic size, reactivity. The atomic radius for the halogens increases down the group as n increases. 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. 1: (a) The radius of an atom is defined as one-half the distance between the nuclei in a molecule consisting of two identical atoms joined by a covalent bond. 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."#
0 Comments
Leave a Reply. |
Details
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |