![]() ![]() However, the general trend going across the periodic table should be obvious. The trend isn’t absolute, especially considering the large positive EA values for the second column. ![]() Figure 8.21 “Electron Affinity on the Periodic Table” shows EA values versus position on the periodic table for the s– and p-block elements. There is not a definitive trend as you go down the periodic table sometimes EA increases, sometimes it decreases. This is because the valence electron shell is getting a larger and there is a larger principal quantum number, so the valence shell lies physically farther away from the nucleus. Such radii can be estimated from various experimental techniques, such as the x-ray crystallography of crystals.Īs you go down a column of the periodic table, the atomic radii increase. Although the concept of a definite radius of an atom is a bit fuzzy, atoms behave as if they have a certain radius. The atomic radius is an indication of the size of an atom. The first periodic trend we will consider atomic radius. There may be a few points where an opposite trend is seen, but there is an overall trend when considered across a whole row or down a whole column of the periodic table. There is no other tool in science that allows us to judge relative properties of a class of objects like this, which makes the periodic table a very useful tool. The variation of properties versus position on the periodic table is called periodic trends. One of the reasons the periodic table is so useful is because its structure allows us to qualitatively determine how some properties of the elements vary versus their position on the periodic table. Be able to state how certain properties of atoms vary based on their relative position on the periodic table. ![]()
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