Electron Configuration Lab
Chemistry
Name: ______Score: ____/10
Put the correct number of electrons (symbolized by the chips) into the subshells (cups). Each cup can hold up to 2 electrons. Remember that the electrons will fill in an orbital which has more then one subshell individually before they will pair.
Important Information to remember:
EVERY subshell can hold up to ______electrons.
The s (lowercase) orbital can hold up to ______electrons.
The p (lowercase) orbital can hold up to ______electrons.
The d (lowercase) orbital can hold up to ______electrons.
The f (lowercase orbital can hold up to ______electrons.
The ______(pronounced OFF-ba) diagram tells how the electrons fill the orbitals. Draw this diagram below. Be sure to add the arrows!
Hund’s rule states that electrons will fill a subshell ______until it cannot occupy a subshell ______and has to ______.
According to the ______Exclusion Principle, states that when two
electrons must occupy the same subshell they will have ______spin. One will be symbolized by an ______arrow and the other by a ______arrow in a box. Such as this example
Fill in the chart below by writing in the electron configuration of each element. Use the cups and chips to figure it out. Leave your chips in the cups until your teacher has approved your configuration. You will do TWO configurations at each station. Be sure to get approval after each configuration—don’t wait until you have both done. (Electron configuration for neon looks like this: 1s2 2 s2 2 p6. Take special notice to write the energy levels in large numbers, the orbital in lowercase letters, and the number of electrons in superscript above the letter. )
Station # Element / Electron Configuration / Teacher’s initials1. K
1. F
2. Sn
2. Ra
3. Ba
3. Mn
4. Fe
4. Dy
5. Ti
5. As
6. Kr
6. Co
7. S
7. Ni
8. Si
8. Eu
Your choice
Your choice
Your choice