NAME:
PERIOD:
REPRESENTING ELECTRON CONFIGURATIONS
We’ve seen that electron configurations may be shown using an energy level diagram (orbital filling
diagrams), electron configuration notation or noble gas configuration, or electron dot notation. This
worksheet will allow you to practice these various methods for atoms and ions.
ELEMENT: Ca
1. Write the full electron configuration. ______________________________________
2. How many valance electrons does Ca have?
3. Write the electron dot notation to show the valence electrons.
4. Write the noble gas configuration. ______________________________________
5. Ca loses 2 electrons when it becomes an ion (Ca+2), which electrons are lost?
6. When calcium loses 2 electrons, it will have the same configuration as the noble gas
____________. This means that Ca will have a full octet and will be more stable than the ion.
ELEMENT: Mn
1. Write the full electron configuration. ______________________________________________
2. How many valence electrons does Mn have? Remember to count only those that are in the
outermost energy level.
3. Write the electron dot notation to show the valence electrons.
4. Write the noble gas configuration.________________________________________
5. Mn can have a charge of +2,+3,+4,+6, and +7, which electrons are lost when Mn becomes +2,
+7?
Complete the following table of atoms:
Configuration
Element
identity/number of
electrons
[Ne] 3s233
1s22s22p63s23p64s1
Sn / 50
[Kr] 5s24d5
Number of valence
electrons
Electron dot notation
ELECTRON CONFIGURATION, NOBLE GAS CONFIGURATION, and THE PERIODIC TABLE
PRACTICE SHEET
Please complete the following worksheet to help review for the upcoming exam. Use your color coded
periodic tables.
PART I:
Write the full electron configuration for the following elements
Example: Silicon 1s22s22p63s23p2
1. Oxygen
2. Sodium
PART II: write the noble gas configuration for the following:
Example : Silicon [Ne] 3s23p2
1.
2.
3.
4.
5.
6.
7.
Cobalt
Rubidium
Xenon
Uranium
Radium
Lead
Molybdenum
PART III: List the region of the periodic table where each of the following elements is found. Determine
the region using s block, p block, d block, or f block as well as using family names/ series names.
Example: Silicon d-block, transition metal
1.
2.
3.
4.
5.
6.
7.
8.
9.
Oxygen
Sodium
Cobalt
Rubidium
Xenon
Uranium
Radium
Lead
Molybdenum
PART IV: Identify the following elements based on the clues given.
1. _____________ it’s noble gas configuration is [Kr]5s24d10
2. ______________ When this element from a +2 ion, it (gains/loses) 2 electrons and ahs the
same electron configuration as Ar
3. ______________ When this element forms a -1 ion, it (gains/loses) 1 electron and has the
same configuration as Ne.
4. ______________ When this element forms a +1 ion, it (gains/loses) 1 electron and has the
same electron configuration as Rn.
5. ______________ This element’s noble gas configuration is [Xe]6s24f105d4
1. What is the maximum number of electrons that can be in the:
a. Second energy level? __________________________
b. Third energy level? ____________________________
c. fourth energy level? ____________________________
2. Which quantum number signifies the size of the electron cloud?
3. The sublevel or shape of the electron cloud is designated by which quantum number?
4. The orbital describes the direction in space of the electron cloud. Which quantum number is
used to represent the orbital?
5. The s quantum number is used to describe the clockwise and counterclockwise rotation of the
electrons in the orbital. What tow numerical values can s have?
6. When n has the numerical value of 4, what values can l have?
7. When l=3, what value can m have?
8. How many orbitals are contained in the p sublevel?
9. How many orbitals are contained in the d sublevel?
10. How many electrons can be in one orbital?
11. What is the maximum number of electrons that can be in the p sublevel?
12. What is the maximum number of electrons that can be in the f sublevel?
13. What is the maximum number of electrons that can be in a d sublevel?
14. What names are used for the three p orbital?
15. What is the name of the scientist who stated that no two electrons in the same atom can have
the same set of quantum numbers?
16. What is the name of the scientist who pointed out that it is impossible to know both the exact
position and the exact momentum of the electron?
17. What is the name of the scientist who treated the electron mathematically as a wave?
18. Mechanics is a word used to describe a system of mathematical equations. Which system of
mathematical equations is used to describe the behavior of extremely small particles travelling
at velocities near the speed of light?
Chapter 4 Review
Please highlight the following scientists major contributions to modern atomic theory.




Bohr
Schrodinger
Heisenberg
DeBroglie
Energy level diagrams and quantum numbers
1. Write and fill an energy level diagram for sulfur
2. Fill the diagram using the three rules. Write a short definition for each.
 Pauli Exclusion Principle
 Hund’s Rule
 Aufbau Principle
3. Write sulfur’s full electron configuration
4. Write sulfur’s noble gas configuration
5. What is the quantum set for sulfur’s last electron?
n
l
ml
ms
6. What is the shape of the orbital where sulfur’s outermost electrons exist?
7. When forming compound, sulfur will generally gain two electrons and will have a charge of
_________. When this happens, sulfur has the same electron configuration of __________, the
closest noble gas. It now has 8 ________ electrons, which is known as an octet.
8. Write the full electron configuration for fluorine.
a. How many valence electrons does it have?
b. Show an electron dot diagram.
9. Write the noble gas configuration for osmium
a. How many valence electrons does it have?
b. Show an electron dot diagram.
10. Given the configuration [Kr] 5s24d105s7 what is the element’s identity?
a. How many valence electrons does the atom have?
b. Show the electron dot diagram for this atom
c. What is the name of the group to which this atom belongs?
d. What charge would the atom in this problem have in a compound? Why does it have
that charge?