1. Atomic Orbitals Drawing 2. Electron Configurations

3. Designing Your own Periodic Table 4. Modeling Atoms and Ions

5. Lewis Structures 6. Molecular Geometry

 

                                                                   

 

 

 

 

   

I. Title: Designing Your Own Periodic Table

II. Purpose: to design your own periodic table using information similar to that available to Mendeleev

III. Materials: 1. Periodic table, 2. Index cards

IV. Procedure:

1. Write down info available for each element on separate index cards. Choose 15-20 elements from s and p blocks only.

2. Appropriate information includes: a. Atomic mass b. States of matter c. Density d. Other readily observable properties

3. Do not write the name of any element on card but keep a separate key.

V. Data: Part A: Index Cards and Key Part B: Initial Attempt at Organizing Elements

1 2 13 14 15 16 17 18 1 2 G L C E 3 A 4 M N 5 D P R O I J 6 H K 7 F B Q

Part C: Actual Order of Elements

1 2 13 14 15 16 17 18 1 2 G L C E 3 A M D N I J 4 H K P 5 R O F 6 B Q 7

VI. Analyze and Conclude: 1. Keeping in mind that the information you have is similar to that available to

Mendeleev in 1869, answer the following questions. a. Why are atomic masses given instead of atomic numbers? b. Can you identify each element by name?

2. How many groups of elements or families, are in your periodic table? How many periods, or series are in the table?

3. Predict the characteristics of any missing elements. When you have finished, check your work using your separate list of elements and a periodic table.

VII. Answers: 1. So that elements with similar properties fall in the same column or group. Sort of. 2. There are 8 groups and 7 periods.

 

   

 

 

 

 

 

 

 

 

Additional Problems:

1. Model and diagonal a neutral Na atom and Na ion. How do the radii compare?

2. Model and diagram an oxygen ion. What charge does it have? Explain.

3. Model and diagram a Mg ion. What charge does it have? Explain.

4. Model and diagram the second ionization energy of a Li atom. Explain why it is much higher than the first.

5. Model and diagram the atom with the highest electro negativity. Explain why it is so high.

6. Model and diagram and explain how an atom’s radius increases down a group (1st group: (H-Na)

7. Model and diagram a neutral Cl atom and a Cl ion. How do the radii compare?