Name: _____________________
Chemical Bonding Webquest
A. http://www.visionlearning.com/library/science/chemistry-1/CHE1.7-bonding.htm
1. Approximately how many elements are represented on the periodic table? __________
2. What accounts for the fact that there are far more substances than listed on the periodic table?
3. What is the definition of a compound?
4. How is it different from its parent atoms?
5. What compound forms during the reaction between elemental sodium and elemental chlorine?
Name _____________________________ Formula ____________________
6. List 5 facts related to G.N. Lewis.
1.
2.
3.
4.
5.
7. Read Ionic Bonding. Explain in your own words the nature of an ionic bond.
8. In the process of either ____________ or ____________ negatively charged _____________, the
reacting atoms form ____________
9. In the reaction between sodium and chlorine, which atom loses an electron? Which atom gains the
electron?
10. What do they mean by valence electron?
11. After transferring the electron, which ion is negatively charged? Why is the ion negatively charged?
Write the symbol for the negative ion: ________________
12. After transferring the electron, which ion is positively charged? Why is the ion positively charged?
Write the symbol for the positive ion: _____________________
13. Click on the Simulation of the reaction of NaCl. There are three pages. Click on the prompt at the
bottom right to go to page 2 and 3. Explain what you see.
14. How does the sodium atom contrast to the sodium ion? (charge, size)
15. How does the chlorine atom contrast to the chlorine ion? (charge, size)
16. What are the 5 common features of ionic compounds?





17. Summarize the explanation for the reason why ionic compounds are solids.
18. What physical property results from ionic compounds forming crystals?
19. Read Covalent Bonding. Click on the covalent bonding simulation and explain what you see.
20. Continue reading Covalent Bonding. What is a covalent bond?
21. What causes covalent bonding to occur rather than ionic bonding?
22. What types of atoms have a tendency to bond in this way?
23. Which type of bonding is greater: ionic or covalent? Why?
24. How many electrons are necessary to form a single bond? ______________
25. How many electrons are present in a double bond? ___________ Triple bond? __________
26. Why does Hydrogen commonly exist as H2?
27. Read Multiple Bonds And Lewis Dot Structures. Why do multiple bonds form?
28. Draw the Lewis dot structure of 3 molecular compounds- One with single bond(s), One with double
bond(s) and one with triple bond(s).
1.
2.
3.
29. Read Polar and Nonpolar Covalent Bonding. Define each.
Polar Covalent Bond-
Nonpolar Covalent Bond30. List 2 examples of non-polar covalent bonds. Draw the Lewis structure.
31. List two examples of polar covalent bonds. Draw the Lewis structure.
32. Click on the simulation of the water molecule. Explain what you see.
33. Read Dipole. Explain the nature of a dipole. Go back to the previous simulation and explain why water
is a dipole.
34. In a polar covalent molecule, the region containing more electrons has a partial _______ charge.
However, the other pole of the molecule, which has fewer electrons, has a partial __________ charge.
35. Click on the ‘Chemical Bonding Quiz.”
1. Take the quiz.
2. Record your score here. __________________