1. Chapter #2 Section Assessment
#1 - 34

2. 2.1 section assessment
Name two categories used to classify properties of matter.
Intensive and extensive properties

3. 2.1 section assessment
2.Explain why all samples of a given substance have the same intensive properties.
Every sample of a given substance has the same chemical composition.

4. 2.1 section assessment 3. Name three states of matter.
Solid, Liquid, Gas.

5. 2.1 section assessment
4. Describe the two categories used to classify physical changes.
Physical changes are either reversible or irreversible. Reversible changes can be “undone,” or reversed. Irreversible changes can not be undone.

6. 2.1 section assessment
5. Which property in Table 2.1 can most easily distinguish sodium chloride from the other solids?
Color; sodium chloride is the only white solid listed.

7. 2.1 section assessment
6. In what way are liquids and gases alike? In what way are liquids and solids different?
Liquids and gases have an indefinite shape. The shape of a solid is definite; the shape of a liquid is indefinite.

8. 2.1 section assessment
7. Is the freezing of mercury a reversible or irreversible physical change? Explain your answer.
The freezing of mercury is reversible because solid mercury can be melted.

9. 2.1 section assessment
8.Explain why samples of gold and copper can have the same extensive properties, but not the same intensive properties.
Samples of gold and copper can have the same mass and volume (extensive properties). They can not have the same set of intensive properties because they have different chemical compositions.

10. 2.2 section assessment 11. How are mixtures classified?
As heterogeneous or homogeneous.

11. 2.2 section assessment
12.What type of properties can be used to separate mixtures?
Differences in physical properties.

12. 2.2 section assessment
13. Explain the term phase as it relates to homogeneous and heterogeneous mixtures.
A phase is any part of a sample with uniform composition. There is one phase in a homogeneous mixture and two or more phases in a phases in a heterogeneous mixture.

13. 2.2 section assessment
14. Classify each of the following as a homogeneous or a heterogeneous mixture.
a. food coloring
b. Ice cubes in liquid water
c. Mouthwash
d. Mashed, unpeeled potatoes
Homogeneous
Heterogeneous

14. 2.2 section assessment
15. How are a substance and a solution similar? How are they different?
Both have a uniform composition throughout. A substance has a definite composition; a solution has a variable composition.

15. 2.2 section assessment
16. In general, when would you use filtration to separate a mixture? When would you use distillation to separate a mixture?
Filtration separates solids from a liquid in a heterogeneous mixture. Distillation can separate a liquid from substances dissolved in a liquid.

16. 2.2 section assessment
17. Describe a procedure that could be used to separate a mixture of sand and table salt.
Add water to dissolve the salt. Pour the resulting mixture onto a piece of closely woven cloth. The sand will remain on the cloth, and the salt solution will pass through. Use evaporation to remove the water from the salt solution, leaving solid salt behind.

17. 2.3 section assessment
20. How is a compound different from an element?
Compounds can be broken down into simpler substances by chemicals means, but elements cannot.

18. 2.3 section assessment
21.How can you distinguish a substance from a mixture?
A substance has a fixed composition. The composition of a mixture may vary.

19. 2.3 section assessment
22.What are chemical symbols and chemical formulas used for?
Chemical symbols are used to represent elements. Chemical formulas are used to represent compounds.

20. 2.3 section assessment
23. Name two methods that can be used to break down compounds into simpler substances.
Heating or an electric current.

21. 2.3 section assessment
24. Classify each of these samples of matter as an element, a compound, or a mixture.
A. table sugar B. tap water
C. cough syrup D. nitrogen
A. compound B. mixture
C. mixture D. element

22. 2.3 section assessment 25. Write the chemical symbol for each element.
A. lead B. oxygen
C. silver D. sodium
E. hydrogen F. Aluminum
A. Pb B. O
C. Ag D. Na
E. H F. Al

23. 2.3 section assessment
26. Name the chemical elements represented by the following symbols.
a. C b. Ca c. K d. Au e. Fe f. Cu
a. Carbon
b. Calcium
c. Potassium
d. Gold
e. Iron
f. Copper

24. 2.3 section assessment
27. What elements make up the element acetaminophen, chemical formula C8H9O2N? Which element is present in the greatest proportion by number of particles?
Carbon, hydrogen, oxygen, and nitrogen; hydrogen is present in the greatest proportion by number of atoms.

25. 2.4 section assessment
28. How does a chemical change affect the composition of matter?
The composition of matter always changes during a chemical change.

26. 2.4 section assessment
29. Name four possible clues that a chemical change has taken place.
A transfer of energy, a change in color, the production of a gas, the formation of a precipitate.

27. 2.4 section assessment
30. In a chemical reaction, how does the mass of the reactants compare with the mass of the products?
The mass of the products is always equal to the mass of the reactants.

28. 2.4 section assessment
31. What is the main difference between physical changes and chemical changes?
In a physical change, the chemical composition of a substance does not change. In a chemical change, the chemical composition of the reactants changes as one or more products form.

29. 2.4 section assessment
32. Classify the following changes as physical or chemical changes.
a. Water boils b. Salt dissolves in water
c. Milk turns sour c. A metal rusts
a. physical b. physical
c. chemical c. chemical

30. 2.4 section assessment
33. According to the law of conservation of mass, when is mass conserved?
Mass is conserved in every physical change or chemical reaction.

31. 2.4 section assessment
34. Hydrogen and oxygen chemically react to form water. How much water would form if 4.8 grams of hydrogen reacted with 38.4 grams of oxygen?
43.2 g