Interactive Periodic Trends Activity



Name:__________________________________________Date:________________Period:__

Interactive Periodic Trends Activity

Honors Chemistry

Instructions:

-Enter the domain for the excel sheet into your web browser to download the interactive file. If it asks you a question, click “ok”.

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- As you explain why these properties change predictably, use the following key ideas in your explanations:

✓ The number of protons in the atom’s nucleus aka the “nuclear charge”

✓ The number of electrons in the atom

✓ Where the electrons are located among the energy levels

(valence vs. “core” electrons)

✓ How the nucleus can be “shielded” by core electrons

-Click on the bottom tab that says “atom properties” to begin the activity.

Part I: Atomic Radius

1. Along the side of the graph area are a series of trends that you can select to display on the graph with respect to atomic number. Click on Atomic Radius if it is not already selected.

a. Atomic radius is the distance from the center of the nucleus to the outermost occupied energy level. What units are used to measure atomic radius?

b. Look at the big picture. In general, what happens to atomic radius as the atomic number increases?

2. At the bottom of the page is a pull down menu that allows you to select the period of the periodic table that you want to see alone. Select period 3.

a. Is there a trend within this period for atomic radius? What is it?

b. Is it what you expected? Why or why not?

3. Now select period 4. Is the pattern the same? What might account for any differences?

4. Fill in the blanks about atomic radius:

Atomic radius increases as you move ________________ a family,

and __________________ across a period

5. Explanation time! Since different patterns exist across and down on the PT, there must be atomic properties that experience different changes, going across versus going down. Explain how electrons and protons are affecting the property of atomic radius, both down a group and across a period in the PT.

Part II: Ionization Energy

6. Reset the pull down menu to graph all the elements. Now click on the side option called “first ionization energy.” This will graph the amount of energy required to remove the outermost electron from the atom.

a. Look at the big picture. Is there a trend you see as atomic number increases?

b. How does this trend compare to that of atomic radius? Does the relationship make sense? Why or why not?

7. Use the pull down menu to select period 3 again. What do you notice about the pattern of ionization energy within a period? Is it what you expected? Why or why not?

8. Explanation time! Since different patterns exist across and down on the PT, there must be atomic properties that experience different changes, going across versus going down. Explain how electrons and protons are affecting the property of ionization energy, both down a group and across a period in the PT.

Part III: Electronegativity

9. Reset the pull down menu to graph all the elements. Now click on the side option called “Electronegativity, Pauling Scale.”

a. Look at the big picture. Is there a trend you see as atomic number increases?

b. How does this trend compare to that of atomic radius? Does the relationship make sense? Why or why not?

c. How does this trend compare to that of first ionization energy? Does the relationship make sense? Why or why not?

10. Explanation time! Since different patterns exist across and down on the PT, there must be atomic properties that experience different changes, going across versus going down. Explain how electrons and protons are affecting the property of electronegativity, both down a group and across a period in the PT.

Part IV: Ionic Size

11. Now click on the tab on the bottom of the screen called “ion properties.” The graph shows the size of the Period 3 elements. In the top right corner, click the box that says add cations.

a. What type of charge do cations carry?

b. How does the size of the cation relate to the size of the original atom? Why?

12. Add the anions by clicking on the box in the upper right corner of the screen.

a. What type of charge do anions carry?

b. How does the size of the anion relate to the size of the original atom? Why?

ATOMIC RADIUS

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IONIZATION ENERGY

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ELECTRONEGATIVITY

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IONIC SIZE – CATIONS (IN RED)

[pic]

IONIC SIZE – ANIONS (IN GREEN)

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Refer back to these ideas, every time you have to explain why a property changes!

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