1. Matter and Change

2. Matter Anything that has mass and takes up space. Everything is made up of matter.

3. Mass - amount of matter the object contains - measured in grams. Substance - matter that has uniform and definite composition (pure substances) - contain only one kind of matter.

4. Physical Properties Quality or condition of a substance that can be observed or measured without changing the substance’s composition. Color odor hardness density melting & boiling points solubility

5. Physical properties help chemists identify substances. Refer to page 29, Table 2.1

6. States of Matter Solid - definite shape and volume. –Particles are packed tightly together. –Almost incompressible. –Expand only slightly when heated.

7. Liquid - indefinite shape and definite volume. –In close contact with one another. –Liquids can flow. –Almost incompressible. –Tend to expand when heated.

8. Gas - indefinite shape and volume. –Gas particles are far apart. –Easily compressed. –Expand without limit to fill any space. –Vapor - describes the gaseous state of a substance that is generally a liquid or solid at room temperature (different than a gas).

9. Physical Change Matter can be changed in many ways without changing the chemical composition of the material. Cutting Dissolving Crack Grinding Melting Boiling Bending Freezing Crush Tearing Condensing Break

10. Melting or Freezing of Water Melting ice into liquid is a physical change, along with changing liquid to steam and steam to condensation. There is no alteration to the chemical composition of water, only a change of state.

11. Classifying Mixtures Physical blend of two more more substances. Compositions may vary.

12. Heterogeneous Mixture Not uniform in composition. If you were to separate the mixture into portions, each portion would be different from the other.

13. Homogeneous Mixture Completely uniform throughout. Components are evenly distributed throughout. Separate the mixture into portions and the portions would be the same. Also called solutions - may be gases, liquids, or solids.

14. Separating Mixtures Distillation - boil a liquid to produce a vapor that is then condensed back into a liquid. (see page 34 diagram) Evaporation - heterogeneous mixture of a solid and a liquid - heat the mixture to evaporate the liquid. Magnets - separate a metal from other solids.

15. Elements and Compounds

16. Elements Simplest forms of matter that can exist under normal laboratory conditions. Cannot be separated into simpler substances by chemical means. Building blocks of other substances.

17. Compounds Two or more elements combined together. Can be separated into simpler substances only by chemical means.

18. Chemical Symbols Shorthand representation of an element. The symbol may be the first or the first two letters of the name of the element. Some symbols are representative of the Latin or Greek names for the element. Represented by one, two, or, less often, three letters. –First letter is always capitalized. –Second or third letter is always lower case.

19. Chemical Symbols Elements you must know: –Hydrogen- Chromium- Zinc –Lithium- Manganese- Mercury –Sodium- Iron- Boron –Potassium- Cobalt- Aluminum –Magnesium- Nickel- Gallium –Calcium- Copper- Carbon –Strontium- Silver- Tin –Barium- Gold- Lead –Nitrogen- Oxygen- Sulfur –Phosphorus- Arsenic- Fluorine –Chlorine- Bromine- Iodine –Helium- Neon

20. Chemical Formulas Shorthand representation of a compound. The subscript of a formula represents the proportions of the various elements in the compound - the proportions are always the same for any one compound. H 2 O = water CO 2 = carbon dioxide CO = carbon monoxide

21. Chemical Reactions One or more substances changing into new substances. Starting substances are the reactants. Arrow dividing the two indicate “to form” or “yields”. Ending substances are the products. Reactants  Products

22. Chemical Property The ability of a substance to undergo a chemical reaction and to form new substances. Chemical properties are only observed when a substance undergoes a chemical change. A chemical change always results in a change in the chemical composition of the substances involved.

23. Burning Decompose Rust Explode Corrode Rot

24. Conservation of Mass Law of Conservation of Mass –In any physical change or chemical reaction, mass is neither created nor destroyed; it is conserved. –The mass of the reactants equals the mass of the products.