INTRODUCTION TO CHEMICAL BONDING
NAME: _____________________
Section 6.1
1. What is a chemical bond?
2. In which of the two situations are atoms most stable, existing by themselves or bonded?
3. Contrast ionic and covalent bonding.
4. Again… what is electronegativity?
5. Distinguish between a nonpolar-covalent bond and a polar-covalent bond.
6. See Fig. 6-2. Create a similar chart or a number line that will help you to remember how you
will use electronegativity to determine the type of bond between atoms.
7. See Fig 6-3. What do the funny looking symbols that have “+” and “-“ on them mean?
Sample pb: Review Sample Problem 6-1.; Answer Section Review # 3. Make sure you list the
more negative atom.
Section 6-2
1. A molecule is…?
2. What does a molecular formula show?
3. List 3 examples of molecules. See Fig 6-4.
4. What are diatomic molecules?
5. The potential energy of a hydrogen molecule is at a minimum when the ______________ of
the like charges equals the ________________ of the opposite charges.
6. Define bond length.
7. Define bond energy.
8. Define octet rule.
9. What is an Electron-dot notation?
10. Write the electron-dot notation for fluorine.
11. Write the Lewis Structure of two fluorine atoms bonded together and label the “parts”
using the description of Lewis Structures.
12. Write a structural formula for two fluorine atoms bonded together.
13. Distinguish between double and triple covalent bonds.
Section 6-3
14. Define ionic compound.
15. What is the formula unit for sodium chloride?
16. As you look at the formation of a bond between a sodium atom and a chlorine atom, which
atom loses a valence electron? What sort of charge does it acquire? What name is given to the
atom now that it has a charge?
17. Referring to question 16, which atom accepts an electron? What sort of charge does it
acquire? What name is given to the atom now that it has a charge?
18. What name is given to the orderly arrangement that ions take on as they form a crystal?
19. As a lattice forms, is energy gained or released? Reflecting on earlier statements, does this
agree with the idea that atoms in a bond have less potential energy than atoms that exist
individually?
20. Which type of bond experiences the greater force of attraction… ionic or covalent?
21. Compare the melting temperatures of molecular compounds to that of ionic compounds.
22. Explain why ionic compounds are brittle.
23. Why can’t ionic compounds conduct electricity in their solid state?
24. Explain how ionic compounds conduct electricity in their molten state.
25. Explain how ionic compounds conduct electricity when they are dissolved in water.
26. What is a polyatomic ion?
Section 6-4
27. Can elements with metallic bonds conduct electricity in their solid state? If so, why?
28. Define metallic bonding.
29. Why are metals shiny? (Dig a little bit. The statement that says something about deexcitation won’t cut it!)
30. If elements are malleable they can be…. (finish the statement).
31. If elements are ductile they can be … (finish the statement).
32. What periodic trend do you see in the heat of vaporization values in table 6-4? What does
this imply about the strength of metallic bonds for elements as you move across the period
from left to right? (Will this trend extend into the nonmetals??? NOPE.. NONmetals don’t
experience metallic bonding)
Section 6-5
33. Translate the term “molecular polarity”.
34. Just out of curiosity, what does VSEPR stand for?
35. More importantly, what does the VSEPR theory state?
36. To the best of your abilities, draw stick figures to represent the following molecular
arrangements: (See fig 6-21 for help)
a. linear
b. trigonal planar
c. tetrahedral
37. To the best of your abilities, draw the molecular orbitals that represent methane, NH3.
Then draw the ball and stick version of the molecule. Notice that only the atoms themselves
are used in the ball and stick models, but the unshared pair affects the shape. Turn the page..
find the name of the shape from Table 6-5.
38. Repeat all directions from 37, but do water, H2O, instead.
39. What are hybrid orbitals?
40. What are intermolecular forces??? How are these different from intramolecular forces?
Use your “noggin” here.
41. How is a dipole created?
42. What name is given to the force that results when the negative region of one polar
molecule attracts the positive end of a nearby polar molecule?
43. Define hydrogen bonding.
44. Define London dispersion forces.