Name:_____________________________ Date:___________________ Per:_______
Electron Configuration and Quantum Theory Worksheet
Element
Complete the following:
Electron
configuration
Orbital Notation
Noble Gas Notation
Lewis Electron Dot
Notation
1.Chromium
2. Tin
Not needed
Not Needed
Not Needed
Not Needed
3. Aluminum
4. Helium
5. Gold
5.
What are the elements that have the following electron configurations?
a) 1s22s22p63s23p64s23d104p65s24d105p66s25d14f4 __________________________
b) 1s22s22p4 ____________________________________
c) 1s22s22p63s23p64s23d7 ___________________________________
d) 1s22s22p63s23p64s23d104p65s24d105p6 _________________________________
6.
How many orbitals does each of the following subshells have?
a) s ________
7.
c) f _________
d) p________
How many electrons does each of the following subshells have?
a) s________
8.
b) d _________
b) d_________
c) f_________
d) p________
How many electrons can occupy each of the following energy levels?
a) 1________
b) 6________
c) 3_________
d) 4________
9. Describe the property of the electron that each of the four Quantum Numbers
exhibit.
n - Principal Quantum Number
l- Angular Momentum Quantum Number
ml - Magnetic Quantum Number
Name:_____________________________ Date:___________________ Per:_______
Electron Configuration and Quantum Theory Worksheet
ms – Spin Quantum Number
10. Which of the following sets of quantum numbers is NOT permissible? (answer yes or no)
a. n = 1, l = 0, ml = 0, ms = + 1/2 _________________________
b. n = 4, l = 0, ml = 0, ms = + 1/2 _________________________
c. n = 3, l = 3, ml = -3, ms = - 1/2 _________________________
d. n = 2, l = 1, ml = 1, ms = - 1/2 __________________________
e. n = 2, l = 1, ml = 2, ms = + 1/2 __________________________
11. Indicate whether the following statements are true or false.
a. The n=3 energy level has no f orbitals._____________________________
b. The 2p orbitals can have a maximum of 6 electrons.________________________
c. The s orbital has a spherical shape.______________________________
d. The n=4 energy level has three sublevels.___________________________
12. Circle the orbital designations shown below that does NOT make sense?
2s1
3d10
4p7
4f7
1s2
13. a. What is the value of l for a 4f electron? ________________________________
b. What is the orbital designation for an electron in the 3rd shell and p sublevel? _________
c. What are the possible values of ml for a 5d electron?______________________________
d. What is the maximum number of electrons in the 3rd energy level?___________________
14. Which is the first element that can have an electron with the following set of quantum
numbers:
a) (3, 2, 1, ½ ) ________________________________________
b) (2, 1, -1, - ½ ) ______________________________________
c) (3, 0, 0, - ½ )________________________________________
d) ( 2, 1, -1, ½ )________________________________________
15. The following deals with the element sulfur:
a. Write out the noble gas notation for sulfur. ________________________________
b. Draw the orbital notation for sulfur. _______________________________________
c. What’s the set of quantum numbers possible for the last electron place. ___________