Reference no: EM13863209

I - Collect and graph data:

The number of protons and electrons in an atom can be set using the widgets on the left. The extent to which the outermost electron (last one added) is shielded from the positive charge of the nucleus is calculated by the spreadsheet and subtracted from the actual nuclear charge (Z, atomic number) to get the effective nuclear charge, Zeffective, that is felt by the outermost valence electron. Use the simulation to determine the Zeffective for the elements sodium through calcium. Create a graph of both Z and Zeffective on the y-axis plotted vs. the number of protons (Z) on the x-axis. Use the Scatter Plot graphing option for this. Your graph will have two sets of data on the same graph, one of which will be a straight diagonal line. Be sure to label your graph appropriately and print a copy to turn in with this exercise.

II - Use your graph and the simulation to answer the following questions:

1) For the elements across the 3rd row of the Periodic Table (Na through Ar), how does the change in effective nuclear charge, Zeff, compare with the change in actual nuclear charge, Z? {Be sure the number of electrons is the same as the number of protons for each element so that you are comparing neutral atoms!} Which element in the row exerts the greatest attraction on its valence electron(s), and which element exerts the least attraction on its valence electron(s)?

2) How does the Zeff for potassium compare with the Zeff for argon? Explain why the trend in Zeff suddenly reverses when another proton and electron are added to Ar to create a potassium atom.

3) Create a potassium cation, K+, by removing one electron from the potassium atom to leave it with a positive charge. How does the Zeff for K+ compare with the Zeff for a neutral atom of argon? Try to explain what you observed.

4) If atoms exert a stronger attractive force on the valence electrons, it is more difficult to remove an electron to create a cation. The energy required to remove an electron from a neutral atom is called the First Ionization Energy. Based on the data you graphed, which of the 10 elements would be expected to have the largest First Ionization Energy? Which would have the lowest? Do your predictions agree with the data in Figure 4.19 on p. 129 of the textbook?