1. Matter and Its Properties

2. What is matter? All matter has volume. All matter has mass.
Mass = “a measure of the amount of matter” (Davis, Frey, Sarquis, and Sarquis 6)
Matter = “anything that has mass and takes up space” (Davis et al. 6)
Example: a rock
Not an Example: thoughts

3. Atoms and Compounds
Atom = “the smallest unit of an element that maintains the chemical identity of that element” (Davis et al. 6)
Sodium (Na)
Helium (He)
Potassium (K)
Element = “a pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom” (Davis et al. 6)

4. Atoms
Helium (He)

5. Compounds
Compound = “a substance that can be broken down into simple stable substances. Each compound is made from the atoms of two or more elements that are chemically bonded” (Davis et al. 7)
Water – made up of an oxygen atom and two hydrogen atoms chemically bonded.

6. Compounds
molecule – for now, think of it as “the smallest unit of an element or compound that retains all of the properties of that element or compound” (Davis et al. 7).

7. What do we do with all of this matter?
We can classify it according to its properties
Extensive properties – “depend on the amount of matter present” (Davis et al. 7)
Mass
Volume
Intensive properties – “do not depend on the amount of matter present” (Davis et al. 7)
Melting point
Boiling point
density

8. Physical Properties
Physical property – “a characteristic that can be observed or measured without changing the identity of the substance” (Davis et al. 7)
Color
Smell
Mass
Boiling point
Melting point

9. Chemical Properties
Chemical property – “relates to a substance’s ability to undergo changes that transform it into different substances” (Davis et al. 8)
Hydrogen gas reacts violently with oxygen
Acids react with bases to form water

10. Physical Change
Physical change – “[a] change in a substance that does not involve a change in the identity of the substance” (Davis et al. 7)
Ice melting
Water boiling
Paper crumpling
Molding clay

11. Changes of State A physical change is an example of a change of state
Change of state = “a physical change of a substance from one state to another” (Davis et al. 8)
States of Matter
Solids
Liquids
Gases
Plasma

12. Solids (Davis et al. 8) “has definite volume and definite shape”
particles “are packed together in relatively fixed positions”
There are strong attractive forces between the particles
The particles move only slightly. They vibrate about a fixed position.

13. Liquids (Davis et al. 8) “definite volume but an indefinite shape”
Particles are close to each other but not as close as solid particles are to each other
The particles can also move past each other more easily
The particles move more rapidly in a liquid than a solid

14. Gases (Davis et al. 8) No definite shape and no definite volume
Particles are moving rapidly
They are spaced far from each other and therefore can move easily past each other

15. Plasma (Davis et al. 8)
“high temperature physical state of matter in which atoms lose most of their electrons”
Fluorescent bulbs

16. Change of State Solid  liquid = melting Liquid  gas = boiling
Liquid  solid = freezing
These are all examples of physical changes!

17. Chemical Change
“A change in which one or more substances are converted into different substances” (Davis et al. 9)
Also known as a chemical reaction
Reactants  Products
Reactants = “[t]he substances that react in a chemical change” (Davis et al. 9)
Products = “[t]he substances that are formed by the chemical change” (Davis et al. 9)

18. Chemical Change
Sodium metal + oxygen gas  sodium oxide “sodium metal plus oxygen gas yields sodium oxide” Even though a new chemical, sodium oxide, is formed, the total mass of the reactants will equal the total mass of the product.

19. Indications of a Chemical Change (“Chemical Reactions”)
Color change
Formation of a gas or odor
Formation of a precipitate (a solid)
Temperature change

20. Law of Conservation of Energy
The amount of energy during a physical or chemical change remains the same.

21. Elements, Compounds, and Mixtures
Think back to the POGIL activity. Do you remember the definitions of elements, compounds, pure substances, and mixtures?

22. Mixtures
“a blend of two or more kinds of matter, each of which retains its own identity and properties” (Davis et al )
Each substance retains its identity!
The substances can usually be separated from each other (Davis et al. 12)

23. Mixtures Mixtures can either be homogeneous or heterogeneous
Homogeneous (also called “solutions”) – “uniform in composition” (Davis et al. 12)
sugar water
Heterogeneous – “not uniform throughout” (Davis et al. 12)
Italian salad dressing

24. Homogeneous Mixtures Soft drinks Gatorade Bleach Vinegar
Air (no clouds though)
Brass

25. Heterogeneous Mixtures
Ocean water
Muddy water
Cake
Salad
Omelets

26. Separation Techniques
Mixtures typically can be separated into their individual substances
Filtration
Centrifuge
Chromatography

27. Pure Substances
“A pure substance has a fixed composition and differs from a mixture in the following ways:
Every sample of a given pure substance has exactly the same characteristic properties . . .
Every sample of a given pure substance has exactly the same composition” (Davis et al. 13)
They can be either elements or compounds.
Remember that elements cannot be broken down into simpler substances but compounds can!

28. Matter Pure Substance Mixture Element Compound Homogeneous
Heterogeneous

29. Works Cited
“Chemical Reactions.” Virtual Chemistry Lab. Harper College, ps/chm/100/dgodambe/thedisk/chemrxn/chem rxn.htm. 14 September Davis, Raymond E., Regina Frey, Mickey Sarquis, and Jerry Sarquis. Modern Chemistry. Austin: Holt, Rinehart, and Winston, Print.