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Summary
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(Reopen the Periodic Table by clicking on the image, if you have closed it.)
The patterns
Revisit the table by viewing atoms in the second and third period.
What does it all mean?
It is known that negatively charged electrons are attracted to the positively charged nucleus. It is also known that the attractive force diminishes with distance.
Consider what might happen when a small atom like fluorine (Fl) (( Protons) comes close to a larger atom like potassium (K). Look at both atoms in the periodic table. Imagine them coming close together.
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<font size=4 face=Verdana>Can you make a generalization about the size of the atoms as one goes horizontally from left to right across the table?
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<font size=4 face=Verdana>Can you make a generalization about the size of atoms in a column in the table?<BR>
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<font size=4 face=Verdana>Where are the smallest atoms in the periodic table? Are they located on the left or the right side of the table?
Explain why this is.
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<font size=4 face=Verdana>What do you predict will happen to the outer electron in the potassium when it comes close to the fluorine atom?
Give reasons for your answer.
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<font size=4 face=Verdana>Imagine Cl (Chlorine)(17 Protons) and Na (Sodium) coming close together. Predict what might happen to the outer electron of the sodium atom when it is near the chlorine atom.
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<font size=4 face=Verdana>Can you make a generalization about which atoms have the strongest attraction for the outer electrons of other atoms?
Please give reasons for your generalization.
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