1. Chapter 2 - Matter Section 1 – Classifying Matter
Section 2 – Properties of Matter
Section 3 – Changes of Matter

2. Section 1 – Classifying Matter
Previously, we watched a 30 minute video on “Properties of matter”
Key Questions
1] How can matter be classified?
2] Why are carbon and copper classified as elements?
3] How are elements related to compounds?
4] What is the difference between a pure substance and a mixture?

3. TN Standards
CLE – Evaluate pure substances and mixtures

4. Matter
Bellwork A – Which of the following is not an example of matter :
( sunglasses, beach towel, sunlight, water )
Bellwork B – Elements, Compounds, and Mixtures are all ____________ ?

5. Matter Matter – Anything that has mass and takes up space
Matter is either an element, compound, molecule, or mixture
Element – a substance that cannot be broken down into simpler substances by chemical means
Compounds – substance made of atoms from different elements BONDED TOGETHER

6. More on Matter
Molecule – smallest unit of a substance that behaves like the substance
Not always the same as a compound!!
Atoms combined but can be same element
Compounds are molecules; molecules not always compounds
Examples of substances that exist in molecule form, BUT ARE NOT COMPOUNDS:
Oxygen and Nitrogen gas in Air
Hydrogen and Chlorine gas
Phosphorus
If a compound: each molecule of that compound will have two or more chemically combined ( BONDED ) elements

7. More on Matter Compounds have unique properties
Table salt, water, sugar, gasoline
Molecules have their own chemical formulas
H2O, CO2, H2, HF

8. Atoms What about Atoms – are ( DO ) they matter? Yes!
Atoms – smallest unit of an element that maintains the chemical properties of that element
Atoms that make up a molecule act as a unit
Again, this can be a compound or only a molecule

9. Pure Substances & Mixtures
Pure Substance – matter with definite composition ( or concentration of the components )
Elements, compounds, and molecules
Mixtures – combination of substances NOT chemically combined
Heterogenous and Homogeneous

10. Pure Substances and Mixtures
What is the difference?
Chemical bonds ( mixtures are not chemically bonded )
Example of pure substance?
Water, carbon dioxide
Example of homogeneous mixture?
Salt or sugar water ( dissolved ), vinegar
Example of heterogenous mixture?
Pulpy orange juice, skittles, salad

11. Mixtures - Defined Homogeneous – looks the same throughout
Heterogenous – does not look the same throughout

12. Concept Map
Word List:
Matter, Pure Substances, Atoms?, Elements, Compounds, Mixtures, Homogeneous, Heterogeneous,

13. Bellwork
What are the two different types of mixtures?

14. Bellwork What are the two different types of mixtures?
Homogeneous and Heterogeneous

15. Section 2/3 – Properties & Changes of Matter
Key Questions
1] Why are color, volume, and density classified as physical properties?
2] Why are flammability and reactivity classified as chemical properties?
3] Why is getting a haircut an example of a physical change?
4] Why is baking bread an example of a chemical change?
5] How can mixtures and compounds be broken down?

16. TN Standards
CLE – Explore matter in terms of its physical and chemical properties
CLE – Investigate chemical and physical changes

17. Physical Properties
Physical properties are characteristics observed without changing the identity of the substance
Examples: color, texture, density, melting temperature, boiling temperature
Physical properties help determine many uses

18. Chemical Properties
Chemical properties are characteristics observed only by changing the identity of the substance
Examples: flammability, reactivity

19. Changes Physical changes do not change the identity of the substance
Cutting hair, Cutting paper
Can be reversed
Chemical changes do
Burning, Rusting, Color, Smell
Can’t be reversed