Electron configuration important concepts

Question 1

What is electron configuration?

Answer 1

• This is a branch of chemistry that helps us locate the location of the electrons.

Question 2

Where are the electrons located?

Answer 2

1. Shells: represent energies levels and represent circles that surrounds the nucleus. These are the location where most electrons are located
   
   1. The higher the shell the farther away the electron is from the nucleus. (y-axis of the periodic table)
2. Subshell: each shell is equiped with a subshell SPDF, if of those subshell can house electrons.
3. Orbitals: part of the subshell, a 3D path where you can find the electrons.
   
   1. S-subshell: houses 1 orbitals= 2 electrons
   2. P-subshell: houses 3 orbitals = 6 electrons
   3. d-subshell: houses 5 orbitals = 10 electrons ( on periodic table start a lack behind)
   4. f -subshell: houses 7 orbitals = 14 electrons (on periodic start at 4)

Question 3

What is the excited vs. grounded states?

Answer 3

1. Excited when an electron filled a higher shell before filling the low shell.
2. Ground state: normal electrons configurations
   
   1. in this process you fill out the smaller orbitals fully before you move to the next one
   2. if the electrons have jump orbitals they become excited.

Question 4

How to assign Quantum numbers to electrons?

Answer 4

1. a ways to explain the exact location of an electron
   
   1. Pauli’s exclusion principle: no two electrons can have the same position at the same time so when you draw one you make sure the other one is upside down.
   2. All electrons have to fill each orbitals first or else they are considered excited.
      
      1. n= shell the electron is in
      2. l = the orbital it is in
      3. ml: the energy subshell: -l to l
      4. ms : how the electron spin +1/2 up or - 1/2 down.