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.
The Essay on Aluminum: The 13th Element on the Periodic Table
One of the many elements on the periodic table is Aluminum. Aluminum is the 13th element, and it is located in period two and group thirteen. Aluminums symbol is Al and it has an electron configuration of [Ne] 3s2 3p1. Aluminum also has an atomic mass of 26.982 and its atomic number is 13. This element was discovered by Hans Christian Oersted in the year of 1825, and was named by the English ...
Group 18 only contains noble gases. If you take a look at the electron configurations of each element all end in p? (with an exception of Helium which is only s? ).
Neon’s electron configuration ends in 2p?. 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, after the lab, can be easily explained.
As you know, that as you go across the periodic table the number of electrons in each element increases by one. So when you are doing electron configurations you can see that the different subshells have different letters which correspond to the different blocks of the periodic table. This is useful in writing electron configurations because the number of elements across from the first one in a period also matches the number next to the letter or block of a periodic table.
This very close relationship makes it seem as if the periodic table was based off of electron configuration. The most stable configuration are those that do not react, gain, or lose an electron. The elements that have the most stable configurations are noble gases. They are the most stable due to having the maximum number of electrons in their outer shell. As a result, they rarely react with other elements since they are already stable. Other characteristics of the noble gases are that they all conduct electricity, fluoresce, odorless and are colorless
