1. Unit 1 Matter/Change Classification of Matter

2. Physical Property Extensive Extensive –Depends on amount of matter present Mass Mass Volume Volume Intensive Intensive –Does not depend on the amount of matter present Color Color Phase Phase Density (mass/volume) Density (mass/volume)

3. Chemical Property Only observed when there is a change in the composition of the substance Ability of a substance to react with other substances or to decompose.

4. What is matter? Has a mass Has a mass Takes up space Takes up space

5. States of Matter Solid Solid –Has a rigid, definite shape –The atoms, ions, or molecules that make up a solid are fixed in place

6. States of Matter Liquid Liquid –Has an indefinite shape –Is flowing matter with definite volume –Takes the shape of its container –Particles of a liquid can move and easily glide over each other

7. States of Matter Gas Gas –Has no definite shape –Has no definite volume –Is compressible matter –Particles of gas are much farther apart and are easily pushed together

8. Matter Pure Substance Mixtures Uniform/Definite composition One Chemical Formula 2 or more substances physically combined Element Compound One type of atom Found on Period Table 2 or more elements chemically combined HomogeneousHeterogeneous Solutions Uniform throughout Not uniform through out.

9. Matter/Change Physical/Chemical Changes

10. Physical Property Characteristics that a sample of matter exhibits WITHOUT any change to its identity.

11. Physical Change A change that does not produce a new substance! A change that does not produce a new substance! New Substance

12. Examples: Solubility Solubility Melting/Boiling Point Melting/Boiling Point Phase Change Phase Change Size/Shape Change Size/Shape Change It’s Color (not change in) It’s Color (not change in) Density Density Electrical Conductivity Electrical Conductivity Physical State (solid, Liquid, or gas) Physical State (solid, Liquid, or gas)

13. Chemical Change A change that does produce a new substance (chemical reaction) A change that does produce a new substance (chemical reaction)

14. “Can the change be reversed?” “Can the change be reversed?” –If yes: probably physical. –If no, probably chemical. Example: Milk goes sour. Example: Milk goes sour. – Can the change be reversed? NO. – You cannot get the milk to taste good again. So it is a chemical change. Note that a new substance (lactic acid) has been produced. This acid is formed when bacteria break down the lactose in the milk. Example: An ice cube melts. Example: An ice cube melts. – Can the change be reversed? YES. –Just put the water back in the freezer. Note that no new substance is produced. Phase changes (changes between states of matter— solid, liquid, gas) are NOT chemical changes! This rule is not perfect; it is just meant as a guide. Physical vs. Chemical Changes

15. Chemical Change-Look for: Formation of a gas (odor) Formation of a gas (odor) Light produced Light produced Formation of precipitate Formation of precipitate Change in temperature Change in temperature – –(gets hot—exothermic* or cold— endothermic**) Permanent Change in color Permanent Change in color

16. Matter/Change Energy Law of Conservation of Matter

17. Law of Conservation of Mass (Matter) Matter can be neither created nor destroyed. Matter can be neither created nor destroyed. –Original atoms in reactants may move around, but will be found on the product side.

18.  How many atoms of carbon are on the reactant side?  On the product side?  How many H on the reactant side?  On the product side?  How many O on the reactant side?  On the product side? 6 6 12 18 Don’t need to write!

19. The mass of the reactants must equal the mass of the products!! Reactants = Products 372g = 372g

20. Exothermic Exothermic The chemical reaction releases heat energy to the surroundings. The chemical reaction releases heat energy to the surroundings.

21. Endothermic  The chemical reaction absorbs heat energy from the surroundings.

22. Energy Changes What is energy? What is energy? –The capacity to do work.

23. Two Types of Energy Potential Potential –Energy of position. –Stored energy in bonds of molecules.

24. Example Gasoline stored at a gas station Gasoline stored at a gas station

25. Two types of energy Kinetic Kinetic –Energy in motion

26. Example Moving cars as they go down the road. As the gasoline is burned, energy is released from the bonds and is used to power the car’s engine. Moving cars as they go down the road. As the gasoline is burned, energy is released from the bonds and is used to power the car’s engine.

27. Energy Conversions Law of Conservation of Energy Law of Conservation of Energy –Energy can be converted from one form to another, but it is not created or destroyed.

28. Metals Nonmetals Metalloids

29. Metals Nonmetals Metalloids

30. Properties of Metals Metals are good conductors of heat and electricity. Metals are good conductors of heat and electricity. Metals are shiny. Metals are shiny. Metals are ductile (can be stretched into thin wires). Metals are ductile (can be stretched into thin wires). Metals are malleable (can be pounded into thin sheets). Metals are malleable (can be pounded into thin sheets). A chemical property of metal is its reaction with water which results in corrosion. A chemical property of metal is its reaction with water which results in corrosion.

31. Properties of Non-Metals Non-metals are poor conductors of heat and electricity. Non-metals are poor conductors of heat and electricity. Non-metals are not ductile or malleable. Non-metals are not ductile or malleable. Solid non-metals are brittle and break easily. Solid non-metals are brittle and break easily. They are dull. They are dull. Many non-metals are gases. Many non-metals are gases. Sulfur

32. Properties of Metalloids Metalloids (metal-like) have properties of both metals and non-metals. Metalloids (metal-like) have properties of both metals and non-metals. They are solids that can be shiny or dull. They are solids that can be shiny or dull. They conduct heat and electricity better than non-metals but not as well as metals. They conduct heat and electricity better than non-metals but not as well as metals. They are ductile and malleable. They are ductile and malleable. Silicon

33. Columns of elements are called groups or families. Columns of elements are called groups or families. Elements in each family have similar but not identical properties. Elements in each family have similar but not identical properties. For example, lithium (Li), sodium (Na), potassium (K), and other members of family 1 are all soft, white, shiny metals. For example, lithium (Li), sodium (Na), potassium (K), and other members of family 1 are all soft, white, shiny metals. All elements in a family have the same number of valence electrons. All elements in a family have the same number of valence electrons.

34. Each horizontal row of elements is called a period. Each horizontal row of elements is called a period. The elements in a period are not alike in properties. The elements in a period are not alike in properties. In fact, the properties change greatly across even given row. In fact, the properties change greatly across even given row. The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas. The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.