1. Chapter 2: Matter and Change

2. Matter
Anything that has mass and takes up space

3. Mass The amount of matter an object has Units: Grams
Measuring tools: Triple Beam Balance, Electronic scale, Analytical Scale

4. Pure Substance Contain only one kind of matter
Have identical physical properties

5. Physical Properties
A quality or condition that can be observed or measured without changing the substances composition
Color, solubility, odor, hardness, density, melting point, boiling point

6. States of Matter

7. Solid Definite shape AND volume Incompressible
Particles are packed tightly together

8. Liquid Definite volume Takes the shape of its container
Almost incompressible-particles not rigidly packed

9. Gas Takes the volume and the shape of its container
Particles in a gas are spaced far apart
Easily compressed

10. Vapor
The gaseous state of a substance that is generally a solid or a liquid at room temperature

11. Physical Change Changes the material without changing the composition
Boiling, freezing, dissolving, melting, condensing, breaking, splitting, cracking, cutting, crushing, bending………
Usually reversible

12. Mixture
A physical blend of 2 substances
Compositions may vary

13. 2 Types of Mixtures
Heterogeneous Mixtures
Homogeneous Mixtures

14. Heterogeneous Mixture
One that is NOT uniform in composition

15. Homogeneous Mixture
The same throughout

16. Solution A homogeneous mixture
Solutions may be solids, liquids, or gases
Same composition throughout

17. Phase Any part of a system with uniform composition and properties

18. Separation of Mixtures
Distillation

19. Separation of Mixtures
Centrifuge

20. Separation of Mixtures

21. Elements
The simplest forms of matter that can exist under laboratory condition
Can not be separated into simpler substances by chemical means
The building blocks for all other substances

22. Chemical Symbol One or 2 letters
The first letter is always capitalized

23. + = Compounds Sodium Metal Sodium Chloride Chlorine Gas
2 or more elements chemically combined
Can be separated into simpler substances by chemical means + =
Sodium Metal
Sodium Chloride
Chlorine Gas

24. Compounds
The subscript numbers in chemical formulas represent the proportions of elements that make up the compounds
Pb2(SO4)3
Pb (lead)  2
S(Sulfur) 3
Oxygen  12

26. Chemical Reaction One or more substances change into new substances
2 H2 (g) + O2 (g)  2 H2O (g)
Reactants
Products

27. Chemical Property
The ability of a substance to undergo a chemical reaction to form a new substance
I.e. flammability, alkalinity, acidity, rusting
Chemical properties are only observed when a substance undergoes a chemical change

28. Chemical Reactions (rust-oxidation)

29. Chemical Reactions (combustion)

30. Chemical Reactions (acid/base)

31. Indicators of a Chemical Reaction
Energy is absorbed or given off (change in temperature)
Change in color
Change in odor
Formation of a solid (precipitation)
Formation of a gas

32. Law of Conservation of Mass
Mass is neither created nor destroyed  mass of reactants = mass of products