1. Pretest 1. Describe the structure of atoms.
Chapter 6
1. Describe the structure of atoms.
2. True or False: Objects with opposite charges attract one another.
3. What are valence electrons?

2. Pretest (continued)
Chapter 6
4. Which group in the periodic table contains elements that hardly react at all?
5. Where on the periodic table are nonmetals generally found?
6. How do the compositions of mixtures differ from those of substances?

3. Pretest (continued)
Chapter 6
7. What property is being described when someone says that a solid is easily hammered into sheets?
a. conductivity b. malleability c. melting point d. density

4. Observing Charged Objects
Interest Grabber
Section 6.1
Observing Charged Objects
Record your observations as your teacher does the following demonstration. Cut two pieces of string about 3 feet in length (or long enough to extend from your teacher’s head to the ceiling). Tie the ends of the strings together and use a thumbtack to hang them from the ceiling. Tie a balloon to the end of each string. Stand under and between the balloons and rub both them on your hair. Let go of the balloons and walk away from them.
1. What happens to the balloons?
2. Offer an explanation for the behavior of the balloons.
3. Predict which subatomic particle is most likely to be transferred during the rubbing. Give a reason for your choice.

5. Reading Strategy Sequencing a. form a cation b. form an anion
Section 6.1
Sequencing
a. form a cation
b. form an anion

6. Electron Dot Diagrams for Some Group A Elements
Figure 2

7. Interest Grabber Ionic Compounds
Section 6.2
Ionic Compounds
Study the samples provided by your teacher. Use the list of properties of ionic compounds to determine which if any of the samples are ionic compounds.
Some properties of ionic compounds:
1. solid at room temperature
2. relatively high melting point
3. crystalline
4. brittle

8. Relating Text and Visuals
Reading Strategy
Section 6.2
Relating Text and Visuals
a. Dots represent valence electrons.
b. A line represents a pair of shared valence electrons.
c. Three-dimensional spheres represent atoms.
d. Electron clouds represent atoms.

9. Molecular Models of Hydrogen
Figure 9
Molecular Models of Hydrogen

10. Molecular Models of Hydrogen
Figure 9
Molecular Models of Hydrogen

11. Molecular Models of Hydrogen
Figure 9
Molecular Models of Hydrogen

12. Molecular Models of Hydrogen
Figure 9
Molecular Models of Hydrogen

13. Molecular Models of Hydrogen
Figure 9
Molecular Models of Hydrogen

14. Interest Grabber Writing Formulas
Section 6.3
Writing Formulas
The names of some compounds contain clues about their chemical formulas. Look at the names of the compounds below. Try to write a formula for each compound based on what you can derive from its name and what you know about the elements the compound contains. Explain how you determined each formula.
1. sulfur trioxide
2. magnesium bromide
3. iron(II) chloride

15. Reading Strategy Predicting
Section 6.3
Predicting
a. and b. Students should assume that any particle described as an ion has a charge. If they know the meaning of poly-, they may predict that the ion contains two or more atoms.

16. Common Anions
Figure 16

17. Some Metal Cations
Figure 17

18. Some Polyatomic Ions
Figure 19

19. Using Scientific Notation
Section 6.3
Using Scientific Notation

20. Using Scientific Notation
Section 6.3
Using Scientific Notation

21. Using Scientific Notation
Section 6.3
Using Scientific Notation

22. Using Scientific Notation
Section 6.3
Using Scientific Notation

23. Comparing Melting Points
Interest Grabber
Section 6.4
Comparing Melting Points
The table below compares the melting points of some metal elements, nonmetal elements, and ionic compounds. Study the table and answer the question.
Is bonding in metals more like bonding between nonmetals or bonding in ionic compounds? Give a reason for your answer.
1330°C
Calcite (CaCO3)
Ionic Compounds
2825°C
Magnesium Oxide (MgO)
114°C
Iodine (I2)
115°C
Sulfur (S8)
Nonmetals
1668°C
Titanium (Ti)
1907°C
Chromium (Cr)
Metals
Melting Point
Name

24. Relating Cause and Effect
Reading Strategy
Section 6.4
Relating Cause and Effect
a. and b. conductivity or malleability

25. Bonding and Malleability of a Metal
Figure 22
Bonding and Malleability of a Metal

26. Bonding and Malleability of a Metal
Figure 22
Bonding and Malleability of a Metal

27. Pretest Answers 1. Describe the structure of atoms.
Chapter 6
1. Describe the structure of atoms.
2. True or False: Objects with opposite charges attract one another.
3. What are valence electrons?
An atom consists of a dense, positively charged nucleus containing protons and neutrons, surrounded by space in which negatively charged electrons move.
electrons in the highest occupied energy level of an atom
Click the mouse button to display the answers.

28. Pretest Answers (continued)
Chapter 6
4. Which group in the periodic table contains elements that hardly react at all?
5. Where on the periodic table are nonmetals generally found?
6. How do the compositions of mixtures differ from those of substances?
the noble gases
the right side
The composition of a mixture can vary. The composition of a substance is fixed.
Click the mouse button to display the answers.

29. Pretest Answers (continued)
Chapter 6
7. What property is being described when someone says that a solid is easily hammered into sheets?
a. conductivity b. malleability c. melting point d. density
Click the mouse button to display the answers.

30. Interest Grabber Answers
Section 6.1
1. What happens to the balloons?
Answers will vary. The balloons move apart, or repel each other.
2. Offer an explanation for the behavior of the balloons.
Rubbing caused the balloons to gain a similar charge.
3. Predict which subatomic particle is most likely to be transferred during the rubbing. Give a reason for your choice.
Electrons are most likely to be transferred based on their location in atoms and their motion.

31. Interest Grabber Answers
Section 6.2
Study the samples provided by your teacher. Use the list of properties of ionic compounds to determine which if any of the samples are ionic compounds.
Some properties of ionic compounds:
1. solid at room temperature
2. relatively high melting point
3. crystalline
4. brittle
You should conclude that the samples provided are not or do not contain ionic compounds. (Possible samples include paraffin wax, rubber, vegetable oil, and ice.)

32. Interest Grabber Answers
Section 6.3
1. sulfur trioxide
SO3, because tri means three.
2. magnesium bromide
MgBr2, because Mg (Group 2A) has ions with a 2+ charge and Br (Group 7A) has ions with a 1– charge.
3. iron(II) chloride
FeCl2 (or Fe2Cl, depending on what you think the Roman numeral II indicates).

33. Interest Grabber Answers
Section 6.4
Is bonding in metals more like bonding between nonmetals or bonding in ionic compounds? Give a reason for your answer.
Bonding in metals is more like the bonding in ionic compounds because the melting points of metals and ionic compounds are higher than those of nonmetals.

34. Go Online Self-grading assessment Articles on metals
Chapter 6
Self-grading assessment
Articles on metals
For links on ionic bonds, go to and enter the Web Code as follows: ccn-1061.
For links on covalent bonding, go to and enter the Web Code as follows: ccn-1062.
For links on chemical formulas, go to and enter the Web Code as follows: ccn-1063.