We can calculate the number of unpaired electrons based on the increase in weight. When we compare the weight of a sample to the weight measured in a magnetic field ( Figure 1), paramagnetic samples that are attracted to the magnet will appear heavier because of the force exerted by the magnetic field. Magnetic susceptibility measures the force experienced by a substance in a magnetic field. And yet, the Lewis structure of O 2 indicates that all electrons are paired. Such attraction to a magnetic field is called paramagnetism, and it arises in molecules that have unpaired electrons. Thus, when we pour liquid oxygen past a strong magnet, it collects between the poles of the magnet and defies gravity, as in Figure 1 in Chapter 8 Introduction. By itself, O 2 is not magnetic, but it is attracted to magnetic fields. However, this picture is at odds with the magnetic behavior of oxygen. There is an O=O double bond, and each oxygen atom has eight electrons around it. This electronic structure adheres to all the rules governing Lewis theory. We would write the following Lewis structure for O 2: However, one of the most important molecules we know, the oxygen molecule O 2, presents a problem with respect to its Lewis structure. Relate these electron configurations to the molecules’ stabilities and magnetic propertiesįor almost every covalent molecule that exists, we can now draw the Lewis structure, predict the electron-pair geometry, predict the molecular geometry, and come close to predicting bond angles.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |