4. http://en.wikipedia.org/wiki/Chemical_reaction http://facstaff.gpc.edu/~pgore/PhysicalScience/at om-with-electrons.gif

5. http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm Reactants: Also known as substrates, are the starting materials for a chemical reaction. Product: The result of the reaction between the reactants. http://www.marietta.edu/~spilatrs/biol103/photolab/reaction.html http://www.liquidsculpture.com/images/water/water-drop-a.jpg

6. http://en.wikipedia.org/wiki/Law_of_Conservation_of_Mass http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm

8.  In every chemical reaction there is energy  This energy is needed to either break bonds in the reaction or create them  As the bonds break energy is released, but when bonds are made energy is absorbed  Chemical reactions are classified as exothermic or endothermic http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm

9. http://en.wikipedia.org/wiki/Potential_energy

10. Exothermic reactions are reactions in which energy is released. The energy that is released is chemical potential energy. This energy is the energy stored in the bonds between atoms. It is called potential energy because it has the potential to be converted to other forms of energy. Some of the time this energy is turned into heat which causes the product to feel hot. This would be called combustion (a.k.a. burning) and is always a exothermic reaction. http://en.wikipedia.org/wiki/Potential_energy http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm Endothermic reactions are reactions in which energy is absorbed. This energy is needed for the reaction to occur. Mostly this energy is either heat of electrical energy. When you add electrical energy to metal oxides, it can separate them into just metal and oxygen. If you add electrical energy to sodium chloride it may cause the table salt to break into sodium and chlorine. http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm http://www.geocities.com/newideasfromtelewise/endo_exothermic.gif

11. 1. The formation of a precipitate, a precipitate is formed in a chemical reaction and is a solid that is different from the reactants. 2.A change in the color of the reactants 3.A formation of gases, usually in the form of bubbles or foam 4.A change in temperature 1.2. 3. 4. http://www.harpercollege.edu/tm-ps/chm/100/dgodambe/thedisk/chemrxn/signs.htm

12. Barium hydroxide and an ammonium salt. When the two solids are mixed and then combined with water. When mixed, the temperature of the solution drops below the freezing point of water. In the first picture a heated metal rod in placed into a mixture of iron powder and sulfur (iron sulfide). This heated metal rod starts a exothermic reaction. Then as you can see in the second picture the product of the reaction is that the iron sulfite is fused to the metal rod. http://jchemed.chem.wisc.edu/jcesoft/CCA/CCA3/MAIN/FEZNSUL/PAGE1.HTM http://genchem.chem.wisc.edu/demonstrations/Gen_Chem_Pages/06thermopage/endothermic_reactions_of_b.htm

13. Activation Energy is the least amount of energy needed for a chemical reaction to start. Some elements and compounds react to each other by just being near each other. This makes their activation energy zero. Most other elements and compounds will only react to each other if a certain amount of energy is added to both of them. For example: when you slide a match on the side of a matchbox, the friction provides activation energy (in the heat form) for the match to light. Activation energy is measured in the number of joules per mole of reactants. http://www.thefreedictionary.com/activation+energy http://upload.wikimedia.org/wikipedia/common s/thumb/c/c1/Streichholz.jpg/250px- Streichholz.jpg

15. A synthesis reaction occurs when two or more simple substances (reactants) combine to form a bigger, more complex substance (product). In a chemical formula: if two or more reactants produce one product, it is a synthesis reaction. http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm In this example, hydrogen and oxygen bond together in a synthesis reaction to produce water. This reaction is easy to perform. Just mix hydrogen and oxygen and the reaction does the rest. http://web1.caryacademy.org/chemistry/rushin/StudentProjects/ ElementWebSites/hydrogen/Hindenberg.jpg The Hindenburg balloon blowing up after the HYDROGEN gas inside was ignited http://periodictable.com/Samples/008.10/s13.JPG Liquid OXYGEN in a bowl http://www.idswater.com/Common/header/Img-water.jpg WATER droplet General Form: A + B ---> AB http://misterguch.brinkster.net/6typesofche micalrxn.html

16. A decomposition reaction occurs when a complex substance containing more than one simple substance breaks down into its original elements. Basically in a chemical formula a reactant makes two or more products as in the example below. Yes, synthesis and decomposition reactions are exact opposites. In this example, water breaks down into hydrogen and oxygen as separate substances. This reaction is not as easy as bonding hydrogen and oxygen. It takes a more complex procedure. http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm http://www.backactive.ca/Portals/backactive/wat er_glass.jpg The reaction of calcium metal and water. The bubbles you see is a HYDROGEN gas A glass of WATER http://www.uncp.edu/home/mcclurem/ptable/ca_2.jpg A tank of compressed OXYGEN gas http://www- personal.umich.edu/~lpt/oxlabe l_files/oxlabel.gif General Form AB ---> A + B http://misterguch.brinkster.net/6typesofche micalrxn.html

17. Combustion (also know as burning) is a sequence of exothermic reactions. These reactions include a fuel and an oxidant. When this reaction takes place, heat is produced. This heat is shown as just a rise in temperature or by a rise in temperature and the production of light. The light is either shown in the form of flames (fire) or a glow. http://en.wikipedia.org/wiki/Combustion A combustion reaction is when oxygen combines with another compound to form water and carbon dioxide. This means the chemical formula must have a CO 2 and a H 2 O in the product as seen above in the formula for the burning of naphthalene. C 10 H 8 + 12 O 2 ---> 10 CO 2 + 4 H 2 O http://misterguch.brinkster.net/6typesofchemicalrxn.html Naphthalene is know as the traditional, primary ingredient in moth balls. http://en.wikipedia.org/wiki/Naphthalene http://www1.istockphoto.com/file_thumbview_ approve/2986938/2/istockphoto_2986938- mountain-of-fire.jpg Naphthalene http://www.fishingmegastore.com/acata log/Naphthalene-Crystals.jpg

18. A single replacement reaction also known as a single displacement reaction occurs when one uncombined element and one compound are the reactants in a chemical reaction. In this type of reaction the one single element takes the place of one of the elements in the compound. In this example zinc and a combination of hydrogen and chlorine, called hydrochloric acid, are the reactants. But, as you can see, in the product, zinc took the place of hydrogen in the compound and now hydrogen is the single element. So, in a chemical formula if a lone element takes the place of an element in a compound you know it is a single replacement reaction. http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm Zn H Cl H Zn Cl H H ReactionReaction General Form A + BC ---> AC + B http://misterguch.brinkster.net/6typesofchemicalrxn.html

19. A double replacement reaction occurs when there are two compounds in the reactants and the product. The reaction takes place when part of one of the compounds is switched with a part of the other compound which gives you the product. In this example silver, nitrogen, and oxygen (a.k.a. silver nitrate) is reacting with sodium and chlorine (a.k.a. sodium chloride). When they react two new compounds are formed, silver and chlorine (a.k.a. silver chloride) and sodium, nitrogen, and oxygen (a.k.a. sodium nitrate). In a chemical formula if there is two compounds in both eh reactants and product and the parts of the compounds are switched, the reaction is a double replacement reaction. General Form AB + CD ---> AD + CB http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm http://misterguch.brinkster.net/6typesofchemicalrxn.html O ReactionReaction Ag O O N Cl Na Cl Ag O O O Na N

20. http://misterguch.brinkster.net/6typesofchemicalrxn.html

21.  “ Chemical Reaction” http://en.wikipedia.org/wiki/Chemical_reaction  “ Photosynthesis Investigation Study Guide” http://www.marietta.edu/~spilatrs/biol103/photolab/reaction.html  “Law of Conservation of Mass” http://en.wikipedia.org/wiki/Law_of_Conservation_of_Mass  “ To React or Not to React? That is the Question!” http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm  “ Potential Energy” http://en.wikipedia.org/wiki/Potential_energy  “ Signs of a Reaction” http://www.harpercollege.edu/tm- ps/chm/100/dgodambe/thedisk/chemrxn/signs.htm  “Reactions of Iron with Sulfur, Zinc with Sulfur” http://jchemed.chem.wisc.edu/jcesoft/CCA/CCA3/MAIN/FEZNSUL/PAGE1.HTM  “Endothermic Reactions of Barium Hydroxide and Ammonium Salts” http://genchem.chem.wisc.edu/demonstrations/Gen_Chem_Pages/06thermopage/endothermic_reactions_of_b.htm  “ Activation Energy” http://www.thefreedictionary.com/activation+energy  “ Combustion” http://en.wikipedia.org/wiki/Combustion  “The Six Types of Chemical Reactions” http://misterguch.brinkster.net/6typesofchemicalrxn.html

22.  “Atom with Electrons” http://facstaff.gpc.edu/~pgore/PhysicalScience/atom-with-electrons.gif  “Water Drop” http://www.liquidsculpture.com/images/water/water-drop-a.jpg  “Chemical Formula” http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm  “Endothermic and Exothermic Reaction Examples” http://www.geocities.com/newideasfromtelewise/endo_exothermic.gif  “Chemical Reaction Signs” http://www.harpercollege.edu/tm-ps/chm/100/dgodambe/thedisk/chemrxn/signs.htm  Exothermic Reaction” http://jchemed.chem.wisc.edu/jcesoft/CCA/CCA3/MAIN/FEZNSUL/PAGE1.HTM  “Endothermic Reaction” http://genchem.chem.wisc.edu/demonstrations/Gen_Chem_Pages/06thermopage/endothermic_reactions_of_b.htm  “ Fire” http://upload.wikimedia.org/wikipedia/commons/thumb/c/c1/Streichholz.jpg/250px-Streichholz.jpg  “ Hindenburg” http://web1.caryacademy.org/chemistry/rushin/StudentProjects/ElementWebSites/hydrogen/Hindenberg.jpg  “Liquid Oxygen” http://periodictable.com/Samples/008.10/s13.JPG  “Water” http://www.idswater.com/Common/header/Img-water.jpg  “Glass of Water” http://www.backactive.ca/Portals/backactive/water_glass.jpg  “Hydrogen” http://www.uncp.edu/home/mcclurem/ptable/ca_2.jpg  “ Compressed Oxygen Gas” http://www-personal.umich.edu/~lpt/oxlabel_files/oxlabel.gif  “Naphthalene” http://www.fishingmegastore.com/acatalog/Naphthalene-Crystals.jpg  “ Mountain of Fire” http://www1.istockphoto.com/file_thumbview_approve/2986938/2/istockphoto_2986938-mountain-of-fire.jpg