1. Principal energy level: How far away from the nucleus an electron is (n).
2. Sublevel: There are four different sublevels called s, p, d, and f. They are shown here:
Source of above picture
3. Orbitals: The s sublevel has one spherical orbital. The p sublevel has three dumb-bell shaped orbitals. The d and f sublevels have five and seven orbitals, respectively, and are complexly shaped.
4. Spin: Each orbital can hold two electrons of opposite spin, one upward and the other downward.
There are rules for placing electrons:
1. Aufbau Principle: Electrons enter the lower energy orbitals first.
2. Pauli Exclusion Principle: An orbital can only have two opposite spinning electrons.
3. Hund's Rule: In a sublevel, electrons must enter singly and then pair up.
Here is a website that explains these rules more in-depth: Electron Placing Rules
Carly, your post was very detailed and educational! I like how you explained everything with definitions, allowing people new to the subject to be able to understand what you are talking about. In addition, I like how you stated the three rules for placing electrons, showing the restrictions of electronic configuration. Lastly, your link was very helpful and interesting! I like how it further explained each of the principles you mentioned with examples to show how they are different.
ReplyDeleteCarly, this post is so helpful! You condensed the lecture down and highlighted all of the crucial info needed for the quiz and test. I could totally come back and reference this as a quick way to review this part of the unit. Your periodic table image is also extremely helpful. Great job!
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