You all know that we didn't have a quiz last Friday due to the field trip on Wendesday and the assembly Friday afternoon. Don't get used to that! Another one is coming up this Friday.
Anyway, this week we will be talking about quantum numbers and orbitals (and what that means for us chemists). Quantum numbers are used to identify the energy states and orbitals (paths around the nucleus) available to electrons. There are three principle quantum numbers. The first is called the principal quantum number and its symbol is n. The principle quantum number can have any whole number value from 1 to infinity. It is the primary factor in determining the energy of an orbital and it defines the size of the orbital. If more than one electron in an atom has the same (n) number, they are said to be in the same shell. Shells can be broken down into subshells as well. The second quantum number is called the azimuthal quantum number and its symbol is l. This quantum number determines the actual shape of the orbital and it can have any whole number value from 0 to n-1.
If l = 0, you have an s orbital.
If l = 1, you have a p orbital.
If l = 2, you have a d orbital
And finally, if l = 3, you have an f orbital.
Our last quantum number is called the magnetic quantum number and it has the symbol m. This number refers to the orientation in space of the orbitals within a subshell. You can see from the above pictures that an s orbital can be oriented in just one way. P orbitals can be oriented in 3 ways, d orbitals in 5 ways and f orbitals in 7 ways. The magnetic quantum number can have the value of -l to l.
So now you can visualize exactly where the electrons have a good probability of being located around the nucleus.
For Parents:
Grades are looking very good so far this semester. If you or your child have any questions don't hesitate to ask. You can post on this blog, write me an email or see me after class everyday until 4:30pm. Thanks again!
No comments:
Post a Comment