The purpose of this lab was to explore how electron configurations vary around the periodic table. The lab also helped us examine the relationships between electron configurations and reactions. Analysis
The first pattern we discovered was that the sum of the superscripts equaled the number of electrons in the atom. Then, we learned that as you travel across the periodic table (starting from hydrogen up to the element of interest) the superscript increases by one. After finally writing out the electron configurations for all the elements, the results revealed that the location of the element (block s, d, p, or f) states its highest energy sublevel. Using these patterns you can determine the electron configuration of any element by simply by looking at the periodic table. Let’s use Carbon(C) for example. The periodic table tells us that Carbon has a total of six electrons. Its location in the table is in block “p”, specifically the second period which means 2p. Now that you know where the electron configuration ends you simply fill in the preceding sublevels until you reach 2p. Just make sure the superscripts add up to six, the number of electrons in Carbon.
Historically, elements are grouped together because of the similar characteristics that they share. For example, all elements in group 18 are noble gases. Well there can be a connection made by the historical reason for grouping elements in families and the electron configurations of the elements. Group 18 only contains noble gases. If you take a look at the electron configurations of each element all end in p⁶ (with an exception of Helium which is only s²). Neon’s electron configuration ends in 2p⁶. The two represents the period it is in and the six tells us that it is in the sixth column of block “p”. While noble gases are grouped for being such, their electron configuration also justify their reason for being organized together.
The shape of the periodic table,...