1. Chapter 1
Matter
and
Change

2. What is Chemistry?
Chemistry is the study of matter and its interactions.
We will study the following properties of matter:
composition
properties
interactions
changes
How will matter be studied?
Using the scientific method.

3. What is the Scientific Method?
Logical approach to exploring a problem or question that has been raised through observation.
Designed to produce a solution or answer that can be tested, retested, and supported by experimentation.

4. Problem: You turn on the switch to a flashlight lamp, but the light does not turn on.
Determine why the flashlight will not turn on.

5. What are the steps of the
Scientific Method?
State the problem.
Gather information about the problem.
Form a hypothesis.
Test hypothesis.
- variables
- controlled experiments
Gather and organize data and observations.
Interpret data.
Form a conclusion.
Replication.

6. What happens to a hypothesis?
Model: An explanation of how phenomena occur and how data or events are related.
Theory: A broad generalization that explains a body of facts or phenomena.
Scientific Law: Statement or mathematical expression about behavior of the natural world.

7. Use the following terms to organize a Concept Map for matter.
Can it be separated?
Is composition uniform?
Can it be decomposed by ordinary chemical means?
Elements
Compounds
Mixtures
Pure Substance
Heterogeneous mixture
Homogeneous mixture
Air
Stainless steel
Blood
Wood
Water
Sodium chloride
Gold
Oxygen

8. Matter How is matter classified?
Matter – anything that has mass and volume.
How is matter classified?
Matter is broken down into two major categories
- Pure Substance
- Mixture

9. Pure Substance Elements - Have unique properties
- Cannot be separated by physical means
- There are two categories of pure substances:
Elements and Compounds
Elements
- simplest pure substances
- contain only one kind of atom
- cannot be broken down by physical or chemical
means
- unique physical and chemical properties

10. Compounds are chemically combined
- substance composed of 2 or more elements that
are chemically combined
- have unique chemical and physical properties
- can be broken down chemically (not physically)
- properties of elements that compounds are broken down into do not resemble properties of original
compound
- always break down to the same proportion by
mass

11. Mixtures Collection of 2 or more pure substances
physically mixed together. (No chemical formula)
- Properties vary depending on what is in the
mixture
Composition can vary (no definite proportion)
There are 2 types of mixtures:
Heterogeneous
Homogeneous

12. Heterogeneous Mixture
Homogeneous Mixture
- Substances are distributed evenly throughout the
mixture
- All regions are identical in their composition and
properties
Heterogeneous Mixture
- Substances are not evenly distributed throughout
the mixture
- Some regions have different properties than
others

13. Classification of Matter

14. Matter is described by its properties
Extensive Properties
- Depend on how much of a substance there is
- Not useful in identifying the substance.
Intensive Properties
- Properties that do not depend on size.
- Can be useful in identifying the substance.

15. Comparing Extensive and Intensive Properties

16. Physical Properties Physical Change
- Characteristics that can be observed without changing the substance.
- Melting point and boiling point are examples
Physical Change
- Change in a substance that does not involve a change in the identity of the substance.
- Phase changes are examples:
solid to liquid - melting
liquid to solid - freezing
liquid to gas - vaporization
gas to liquid - condensation
solid to gas - sublimation
gas to solid - deposition

17. Phase Changes are also called changes in state. Plasma
There are 4 states of matter: Solid
Liquid
Gas

18. Phase Diagrams
A phase diagram is a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist.
The triple point of a substance indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium.
The critical point of a substance indicates the critical temperature and critical pressure.

19. Phase Diagram

20. Phase Diagram

21. Phase Diagram for CO2

22. Changes of State - Summary

23. Water in Three States

24. Heating Curve for Water

25. Heat of Fusion: The amount of energy as heat required to melt a solid at the solid’s melting point
Heat of Vaporization: The amount of energy as heat that is needed to vaporize a liquid at the liquid’s boiling point at constant pressure

26. Chemical Properties Chemical Change
- characteristics that describe how a
substance interacts (or fails to interact) with
other substances.
Chemical Change
- also called a chemical reaction
- change that results in production of 1 or more substances that differ in chemical properties and composition from the original substance

27. Chemical Reaction

28. Evidence of a Chemical Change

29. Comparison of Physical and Chemical Properties

30. Comparing Physical and Chemical Properties

31. Comparing Chemical and Physical Changes

32. Periodic Table of the Elements

33. Review Questions
1. Matter that has a definite shape and a definite volume is?
2. Why is air considered a mixture and not a compound?
3. How do compounds differ from mixtures?
4. Is each of the following a chemical or physical property?
A. Its mass is g.
B. It is a shiny solid at room temperature.
C. It is easily etched by nitric acid.
D. It melts when heated to 670°C.
E. It is 31.7 centimeters long.
F. It is a good heat conductor.
G. It burns in air.
H. It is a good conductor of electrical energy
5. Describe the difference between a chemical change and a physical change. Give one example of each kind of change.