Electron Configurations Worksheet

Electron Configurations Worksheet

Write the complete ground state electron configurations and orbital notations for the following:

# of e- Element (atom) e- configuration Orbital Notations/ diagrams

1)_____lithium ______

2)_____ oxygen ______

3)_____calcium ______

4)_____nitrogen ______

5)_____potassium ______

6)_____chlorine ______

7)_____hydrogen ______

8) _____copper ______

9) _____ neon ______

10) _____ phosphorous ______

Write the abbreviated ground state electron configurations for the following:

# of electrons Element

11)______helium ______

12)______nitrogen ______

13)______chlorine ______

14)______iron ______

15)______zinc ______

16)______barium ______

17)______bromine ______

18) ______magnesium ______

19) ______fluorine ______

20) ______aluminum ______

Electron Configuration Elements (atoms) and Ions

Write the electron configuration and orbital notations for the following Atoms and ions:

Electron Configuration Practice

Directions: Write and draw the electron configurations of each of the following atoms.

Example:

Co : 27 e- 1s2 2s2 2p6 3s2 3p6 4s2 3d7

1. Scandium:

2. Gallium:

3. Silver:

4. Argon:

5. Nitrogen:

6. Lithium:

7. Sulfur:

Name:______Date:______Period:______

Electron Position and Configuration

Chemistry 513/543

Position: Draw the Electron Position of each of the following atoms.

Example:

He:

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1. Li

2. C

3. O

4. Ar

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Directions: Draw the electron configurations of each of the following atoms.

Example:

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1. Chlorine:

2. Nitrogen:

3. Aluminum:

4. Oxygen:

5. Sodium:

6. Potassium:

7. Sulfur:

8. Calcium

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Name:______Date______Per:______

Electron Configuration Practice - Homework

In the space below, write the expanded electron configurations (ex. = 1s22s1) of the following elements:

1)Sodium______

2)potassium ______

3)chlorine ______

4)bromine ______

5)oxygen ______

In the space below, write the abbreviated electron configurations (ex. Li= [He]2s1) of the following elements:

6)manganese______

7)silver______

8)nitrogen______

9)sulfur______

10)argon______

In the space below, write the orbital notation (arrows) of the following elements:

11)manganese______

12)silver______

13)nitrogen______

14)sulfur ______

15)argon ______

Determine what elements are denoted by the following electron configurations:

16) 1s22s22p63s23p4 ______

17) 1s22s22p63s23p64s23d104p65s1 ______

18) [Kr] 5s24d105p3 ______

19) [Xe] 6s24f145d6 ______

20) [Rn] 7s25f11 ______

Determine which of the following electron configurations are not valid:

21) 1s22s22p63s23p64s24d104p5 ______22) 1s22s22p63s33d5 ______

23) [Ra] 7s25f8 ______24) [Kr] 5s24d105p5 ______

25) [Xe] ______

Law of Conservation of Matter and Electron Configuration Review

1. a. Define the term valence shell.

b. Why is the valence shell so important in studying chemical reactions?

1. Given an element with atomic number 11, provide the following information:

1. How many electrons will fill each of the following shells:

1st shell:

2nd shell:

3rd shell:

1. Is this element likely to form a cation or anion?
2. What charge will the ion formed by this element have?

1. Roman numerals are needed when naming many of the transition metals because ______

1. a. A molecule with an overall positive or negative charge is called a ______.

b. An example of one is ______

1. Explain, based on electron configuration, why the noble gases are so unreactive. Use helium and neon as examples to illustrate your explanation.

1. Each of the following chemical formulas and names are written incorrectly. Rewrite them correctly.

1. Cl2Mg
2. NaP
3. Iron Sulfur
4. NH4Cl3
5. Cesium (I) bromide

1. a. What does the Law of Conservation of Matter state?

______

b. Explain the reason for balancing equations based on this law.

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