Define:
1. chemical bond
12. nonpolar covalent bond
2. bond energy
13. delta
3. endothermic
14. electronegativity
4. exothermic
15. octet rule
5. electrostatic attraction
16. double bond
6. ionic bond
17. triple bond
7. crystal lattice
18. structural formula
8. electron dot symbols
19. lone pair
9. covalent bond
20. resonance
10. bond length
21. VSEPR theory
11. polar covalent bond
22. dipole moment
Questions:
1. What do compounds have in common?
2. Why is the shape of a molecule important?
3. Describe how an ionic bond is formed.
4. Can you have one molecule of NaCl? Explain.
5. How are covalent bonds formed?
6. Give an example of a polar and nonpolar bond.
7. Compare electronegativity values between metals and nonmetals.
8. Compare the values of electronegativity differences for ionic compounds,
polar covalent and nonpolar covalent compounds.
9. When are compounds stable?
10. Why is hydrogen an exception to the octet rule?
11. What four things do you need to know in order to write Lewis structures
for a molecule?
12. Compare bond strength of a single bond and of a multiple bond.
13. What changes must you consider when writing electron dot structures
for ions?
14. List three examples of compounds that do not follow the octet rule.
15. What is the main theory behind the VSEPR theory?
16. List the different shapes of molecules and the criteria used to
determine their shape. (i.e., # bonds, # lone pairs)
17. Give an example of a nonpolar molecule that has polar bonds.
Problems:
p.435 # 1,2,3 p. 436
# 4,5 p. 442 # 6,7,8,11,14,15,16
p. 445 #18,19 p. 447 #20,21
p. 448 # 22,23 p. 450 # 26,27 p. 456 # 33,34
p. 461 # 35,36,37 Review # 10,11,13,17,18,22,23,24,25,26,31,32,39,43,44,45
