2. The term matter describes all of the physical substances around us: your table, your body, a pencil, water, and so forth.

3. If the formula of water were to change, that would be a chemical change. If you added another oxygen atom, you would make hydrogen peroxide (H 2 O 2 ). Its molecules would not be water anymore. Changing states of matter is about changing densities, pressures, temperatures, and other physical properties. The basic chemical structure does not change.

4.  Building blocks of all substances

5. a. Protons—positively-charged particles; located in the nucleus

6. b. Neutrons—neutral (no charge) particles located in the nucleus

7. c. Electrons—negatively-charged particles; orbit the nucleus

8. Atomic Number —number of protons in the nucleus (hint: if you know how many protons there are, then you know how many electrons there are [positive =negative] Atomic Mass —protons + neutrons (mass of the nucleus)

9. To find protons: atomic number To find electrons: same as protons To find neutrons= atomic mass-atomic number

11.  A molecule is the combination of two or more atoms. › Some molecules are made of atoms that are all alike, as in Oxygen (O 2 ) that you breathe!

12.  A substance that cannot be broken down into any other substance by chemical or physical means.  All matter is composed of one element or a combinations of two or more elements.

13.  Combination of two or more substances that are not chemically combined. › No new substance formed. › Do not exist in fixed proportions to each other. › They just mix. › Most natural substances are mixtures. › Can be physically separated into pure compounds or elements. › Can be separated by mechanical means › Physical properties can change. › Any combination of solid, liquid or gas can be a simple mixture.

14.  Two or more elements chemically combined in a specific ratio, or proportion.  A pure compound has the same elements and the same amount of elements all of the time. › Elements are chemically combined. › Compound properties are different from the properties of the elements. › They cannot be separated physically. › When naming a compound, metals are named first.

15.  Small number after the element.  Only affects the element it follows! › Example O 2, H 2 O

16.  BIG number.  Effects every element that follows it. › Example: 2Na 2 CO 3 C 3 H 8 O

17.  Also note: › Chemical formulas and symbols must be written a certain way! › Al - Aluminum  NOT AL or al  Must always be Capital Letter then small letter(s) if applicable.  CO is one Carbon, one Oxygen (Two capital letters mean two different elements)  Co is Cobalt

18.  C 12 H 22 O 11 (sugar)C=H=O=   6NaCl (table salt)Na=Cl=   2Na 2 CO 3 (sodium carb.) Na=C=O=   3CaCl 2 (calcium chloride) Ca=Cl=   2C 6 H 8 O 7 (citric acid)C= H= O=

19.  Create the foldable.  Tabs – Atoms/Molecules, Elements, Compounds, Mixtures.  Behind each tab state at least two facts about each and give an example. At least one illustration on inside of tab.