6 posts • Page 1 of 1
How do trends in the periodic table affect electron configurations? Is there a relationship between the two concepts?
Trends and electron configuration are related in that you can see the reasoning behind the trends when writing out the electron configurations of elements. For example, a full valence shell is the most stable electron configuration.
There is definitely a relationship between trends and electron configurations. For example, as the period goes from left to right, the electron configuration changes so that more electrons are added to the levels. This reflects the increase in Ionization Energy, since IE increases going left to right because of the increase in pull of electrons towards the nucleus.
You can also clearly see the trends in the periodic table as you write out the electron configuration for any given element. Because you write an element's configuration based on their physical position on the periodic table, the organization of the periodic table according to their chemical characteristics and trends becomes more apparent.
The electron configurations go in order from left to right on the periodic table. Beginning in row 1, group 1, with hydrogen, it is 1s2, as you move left one it is 2s2, and so on and so forth. You can look to the periodic table to figure out electron configurations quite easily, just remember the two exceptions.
understanding the trends of the periodic table make it easier to understand the nature of the atoms and what way they'll react in order to reach a stable valence shell. for example, something like sodium is more likely to lose 1 electron in order to create a full outer shell rather than gain 7 electrons to react the next shell.
Who is online
Users browsing this forum: No registered users and 2 guests