1. Matter and Change

2. Properties of Matter What is mass?
1.) The force of gravity on an object.
2.) The amount of matter an object contains.
3.) The measure of space occupied by an object.

3. Mass and Volume Mass – the amount of matter an object contains (grams)
Volume – measure of space occupied by an object (cm3, mL, L)

4. Extensive vs. Intensive Properties
Extensive Properties – depends on amount of matter
Example: mass and volume
Intensive Properties – depends on type of matter, not amount
Example: color and density

5. Identifying Substances
Substance – matter with uniform and definite composition
- sample of given substance has same intensive properties

6. Physical Properties
Physical Properties – quality or condition of substance that can be observed or measured without changing composition
Physical states of matter
- Solid
- Liquid
- Gas

7. States of Matter Solid – matter with definite shape and volume
- particles packed tightly together
- not easily compressed

8. States of Matter Liquid- Indefinite shape, flows, definite volume
- flowing/loosely packed molecules
- not easily compressed

9. States of Matter Gas – indefinite shape and volume
- molecules spaced out
- easily compressed
Vapor- gaseous state of substance that was generally a liquid or solid at room temp

10. Physical Changes
Physical Change – when properties change but composition does not
- Example:
ice water

11. Mixtures Mixtures – physical blend of 2 or more components
Example: salad (tomatoes, lettuce, onions, etc.)

12. Heterogeneous Mixtures
Heterogeneous Mixtures – composition not uniform
- Example: Chicken noodle soup (more chicken in one spoonful than another)

13. Homogeneous Mixtures
Homogeneous Mixtures – composition uniform throughout
Example: salt water
Solution- homogeneous mixture (mostly liquids/some gases)

14. Phase
Phase – any part of sample with uniform composition and properties
-Homogeneous = 1 phase
-Heterogeneous = 2 phases or more
1 phase
1 phase

15. Separating Mixtures
Differences in physical properties can be used to separate mixtures.
Filtration – separate solid from liquid in heterogeneous mixtures

16. Separating Mixtures
Distillation – process used to separate dissolved solids from liquid
- liquid boiled to produce vapor and condensed into liquids

17. Elements and Compounds
Element – simplest form of matter
- has unique set of properties
- can not be broken into simpler substances
- Example: Oxygen and Hydrogen

18. Compound Compound – substance contains 2 or more elements
- chemically combined in fixed proportion
- can be broken down
into simpler substances
- Example: Carbon Dioxide (CO2)

19. Breaking Down Compounds
Chemical Change- produces matter with different composition
Example:
Water Hydrogen + Oxygen
electricity

20. Properties of Compounds
Properties of compounds different from component elements.
Example:
Hydrogen = explosive/flammable
Oxygen = flammable
Water (H2O) = puts fires out

21. Substances vs. Mixtures
Composition fixed = substance
Example: Carbon Monoxide (1Carbon:1Oxygen)
Composition varies = mixture
Example: chicken soup

22. Symbols and Formulas
Chemical Symbol – each element represented by 1 or 2 letter symbol
- first letter capitalized
- second is lowercase

23. Symbols and Formulas Chemical formulas represent compounds
Example: Sucrose (table sugar) = C12H22O11

24. Chemical Changes
Chemical Property – ability of substance to undergo chemical change
- during chemical change composition of matter always changes
- Example: burn, rot, rust, decompose, ferment, explode, corrode

25. Chemical Changes
Chemical Reaction – one or more substances change into one or more new substances
- Reactant – substance at beginning of reaction
- Product – substance produced in reaction
Example: HCl + NaOH NaCl + H2O

26. Recognizing Chemical Change
Clues to chemical change include:
- transfer of energy
- change in color
- production of gas
- formation of precipitate
- precipitate – solid that forms and settles out of liquid mixture

27. Conservation of Mass
Law of Conservation of Mass- in any physical change or chemical reaction mass is conserved
- mass of products = mass of reactants