Lesson 7: Wrap Up
Now that you have worked your way through this lesson you should be able to figure out what type of bonding will hold together any collection of atoms. This lesson particularly focused on ionic bonding. You should be able to predict the ion charges of representative elements - metals and nonmetals - based on their location on the periodic table. You also have memorized eight common polyatomic ions (their formulas - including their charges - and names), and a few transition metal ions (both common ions of copper and iron, and the simple ions of silver and zinc). You can determine the formulas of ionic compounds and name them. Throughout all of this you should be able to explain what happens to the electrons of individual, isolated atoms when they come in contact with and fall under the influence of other atoms because that is what bonding is all about. In the next lesson, Lesson 8, we will continue our study of bonding with the other two kinds of atomic bonding, metallic bonding and covalent bonding.
Your lab work this week is to practice with the names and formulas of ionic compounds. There is a practice program on the lab computers called Ionic Bonding, similar to the Balancing Equations practice you completed in Lesson 3. You need to complete enough practice problems to have 30 correct to earn full credit for this lab. There is no penalty for incorrect answers - just be sure to keep going until you have at least 30 correct. (Of course, you can do more than 30 practice problems - the more you practice, the easier it gets!) Don't forget to print out your score sheet so that you can hand it in to get credit for completing the lab work.
You should finish up the lesson by reviewing the Objectives and trying the Self Quiz.
Self Quiz | Answers to Self Quiz
Self Quiz
1. Ionic bonding involves:
a. atoms which have gained electrons being attracted to the opposite charge of atoms which have lost electrons
b. atoms sharing tightly held electrons between them
c. atoms sharing very loosely held electrons
2. What is the name and formula of the compound formed by sodium and oxygen?
3. What is the name and formula of the compound you would expect to form between silver and chlorine?
4. Predict the charge(s) on the ions formed by the following elements:
K Br O Cu Zn
5. What is the formula (including the charge) for nitrate?
6. What is the name of CO32-?
7. What is the name of Fe(OH)3?
8. What is the name of (NH4)3PO4?
9. What is the name and formula of the compound formed between nitrogen and calcium?
10. Why are ionic compounds network materials?
Answers to Self Quiz
1. a
2. Na2O; sodium oxide
3. AgCl; silver chloride
4. K+; Br-; O2-; Cu+ and Cu2+; Zn2+
5. NO3-
6. carbonate ion
7. iron(III) hydroxide or ferric hydroxide
8. ammonium phosphate
9. Ca3N2; calcium nitride
10. The ions in the crystal structure are attracted to all the ions that surround them. Since the attraction is spread out through the entire structure, the ionic compound is a network. (You cannot point to just two ions, or three ions, or even a small cluster of ions and say that they are only attracted to each other and not attracted to any of the other surrounding ions.)