Title: Electron configurations of selected Elements
Purpose: The purpose of this lab is to determine the electron configuration of selected elements.
Materials: Pen, pencil, paper, and the Periodic Table
Procedure: Select one (1) element from Period 1 and 7, select three (3) elements from 2-6 and do an electron
configuration for each. At least five of these must be a pictorial representation, and five the Noble Gas method.
Clearly label each sublevel. Use arrows to indicate electrons. Please follow the rules given in class for filling
sublevels and electron spins.
Period 1
Name
e- config
Period 7
Name
e- config
Period 2
Name
e- config
Period 3
Name
e- config
Period 4
Name
e- config
Period 5
Name
e- config
Period 6
Name
e- config
Questions:
1.Why does the 5-s fill before the 4-d sublevel?
2.Why would three electrons fill separate p-orbitals rather than two of them doubling up in an orbital?
3. Why do electrons in the same orbital have opposite spins?
4. Be specific and state what sublevels are being filled in groups 1-2, 3-12, 13-18. Lanthanides, and Actinides?
5. If all of the sublevels are filled through the 5-p sublevel how many electrons will that element contain?
6. Name the following:
a.
1s22s22p63s23p4
b.
1s22s22p63s23p64s23d5
c.
1s22s22p63s23p64s23d104p3
d.
[Kr]-5s24d4