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
_______ arrow in a box. Such as this example
the other by a
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
1. K
1. F
2. Sn
2. Ra
3. Ba
3. Mn
4. Fe
4. Dy
Electron Configuration
Teacher’s
initials
5. Ti
5. As
6. Kr
6. Co
7. S
7. Ni
8. Si
8. Eu
Your choice
Your choice
Your choice