1. By Ollie Auerbach

2. A chemical Reaction  A process in which atoms of the same or different elements rearrange themselves to form a new substance. While they do so, they either absorb heat or give it off http://www.weldonryan.com/images/chemical_reaction_final.png http://dictionary.reference.com/browse/chemical%20reaction

3. Chemical Reaction Basics  What is happening during a chemical reaction?  Reactants react to form products.  Reactants- the materials that exist before the chemical reaction  Products- substances that are created by the chemical reaction  Atoms are only rearranged.  No new atoms are created.  What part of atoms are affected by chemical reactions?  A chemical reaction involves the motion of electrons in the forming and breaking of chemical bonds.  http://en.wikipedia.org/wiki/Chemical_reaction http://en.wikipedia.org/wiki/Chemical_reaction

4. Signs of a chemical reaction  Bubbling  Change in temperature  Light is emitted  Change in color  Energy is produced  A gas is produced  A precipitate forms ( chemical reaction that forms a solid powder from two liquid substances)  http://images.encarta.msn.com/xrefmedia/sharemed/targets/images/pho/t046/T046403A.jpg http://images.encarta.msn.com/xrefmedia/sharemed/targets/images/pho/t046/T046403A.jpg  http://antoine.frostburg.edu/chem/senese/101/reactions/symptoms.shtml http://antoine.frostburg.edu/chem/senese/101/reactions/symptoms.shtml

5. Law of Conservation Mass  In a chemical reaction, matter is neither gained or lost  Or more simply put, the mass of substances produced (products) by a chemical reaction is always equal to the mass of the reacting substances (reactants).  http://www.mi.mun.ca/users/edurnfor/1100/atomic%20structure/tsld004.htm http://www.mi.mun.ca/users/edurnfor/1100/atomic%20structure/tsld004.htm http://www.biochem.northwestern.edu/holmgren/Glossary/Definitions/Def-L/law_conservation_of_mass.html  http://www.tea.state.tx.us/student.assessment/resources/online/2006/grade10/science/images/40graphicaa.gif http://www.tea.state.tx.us/student.assessment/resources/online/2006/grade10/science/images/40graphicaa.gif

6. Energy in Chemical Reactions  Chemical reactions always involve a change in energy. Energy is neither created or destroyed. Energy is absorbed or released in chemical reactions. Chemical reactions can be described as endothermic or exothermic reactions. http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm http://www.beaconhurst.stirling.sch.uk/departments/science/chem7.jpg

7. Exothermic/ Endothermic Reactions ExothermicEndothermic  Energy is released  The energy released was originally stored in the chemical bonds of the reactants.  Any reaction that involves combustion (burning) is an exothermic chemical reaction.  Often the heat given off causes the product(s) to feel hot  Ex. – Dissolving ammonia chloride into water,  Ex. - 2H 2 +O 2 changes to 2H 2 O  http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chem type.htm http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chem type.htm  Energy is absorbed  Energy is required for reaction to happen  Energy absorbed is usually electrical energy or heat energy  Ex. –Photosynthesis,  sunlight + 6CO 2 (g) + H 2 O(l) = C 6 H 12 O 6 (aq) + 6O 2 (g)

8. Activation Energy  Energy that must be overcome for a chemical reaction to occur  The energy often needed to initiate a certain process  http://chemistry.twu.edu/tutorial/activation-energy.gif http://chemistry.twu.edu/tutorial/activation-energy.gif  http://www.bio-medicine.org/biology-definition/Activation_energy/ http://www.bio-medicine.org/biology-definition/Activation_energy/  http://en.wikipedia.org/wiki/Activation_energy http://en.wikipedia.org/wiki/Activation_energy

9. Chemical Potential Energy  Energy that is stored and can be transformed into other forms of energy  Sound  Heat  Electricity  Light http://www.chemistryland.com/CHM107/Energy/HydrogenElectronNoSpring.jpg

10. Combustion  The act or process of burning  O 2 will always be a reactant in a combustion reaction  When something burns it is almost always a combustion reaction  Combustion reactions are almost always exothermic (Give off heat)  An example- the combustion of hydrogen and oxygen, which is a commonly used reaction in rocket engines:  2H 2 + O 2 → 2H 2 O(g) + heat. The result is water vapor.  http://en.wikipedia.org/wiki/Combustion http://en.wikipedia.org/wiki/Combustion  http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactions/combustion.html http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactions/combustion.html  http://www.ueberbill.com/images/ROCKET.jpg http://www.ueberbill.com/images/ROCKET.jpg

11. Decomposition  The state of being reduced into original elements. (breaking down, disintegration)  Opposite of combination reactions  Compound decomposes (splits up)  Basic formula- AB ---> A + B  An example- Water broken down into hydrogen and oxygen  2H 2 O → 2H 2 + O 2  http://en.wikipedia.org/wiki/Chemical_decomposition http://en.wikipedia.org/wiki/Chemical_decomposition

12. Synthesis  The combining of separate elements or substances to form a whole.  Basic Formula- A + B ---> AB  Examples-  2Na + Cl 2 → 2 NaCl (formation of table salt)  4 Fe + 3 O 2 → 2 Fe 2 O 3 (iron rusting)  http://en.wikipedia.org/wiki/Chemical_synthesis http://en.wikipedia.org/wiki/Chemical_synthesis  http://www.dearbornschools.org/schools/dcmst/staff/whittaker/NaCl123.gif http://www.dearbornschools.org/schools/dcmst/staff/whittaker/NaCl123.gif

13. Single Displacement  An element trades places with another element in a compound.  Basic Formula- A + BC ---> AC + B  An example- magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas  Mg + 2 H 2 O ---> Mg(OH) 2 + H 2  http://misterguch.brinkster.net/6typesofchemicalrxn.html http://misterguch.brinkster.net/6typesofchemicalrxn.html  http://www.hempfieldarea.k12.pa.us/webdir/MILLERS/sd%20reaction.pnghttp://www.hempfieldarea.k12.pa.us/webdir/MILLERS/sd%20reaction.png

14. Double Displacement  Cations and Anions of two different molecules switch places two form to totally different compounds.  Basic Formula- AB + CD ---> AD + CB  An example- The reaction of lead nitrate with potassium iodide to form lead iodide and potassium nitrate  Pb(NO 3 ) 2 + 2 KI ---> PbI 2 + 2 KNO 3  http://www.hempfieldarea.k12.pa.us/webdir/MILLERS/dd%20reaction.png http://www.hempfieldarea.k12.pa.us/webdir/MILLERS/dd%20reaction.png  http://misterguch.brinkster.net/6typesofchemicalrxn.html http://misterguch.brinkster.net/6typesofchemicalrxn.html

15. Bibliography  “Chemical Reaction Definition-”  http://dictionary.reference.com/browse/chemical%20reaction http://dictionary.reference.com/browse/chemical%20reaction  “Chemical Reactions”  http://en.wikipedia.org/wiki/Chemical_reaction http://en.wikipedia.org/wiki/Chemical_reaction  “Ten Signs of a Chemical Change”  http://antoine.frostburg.edu/chem/senese/101/reactions/symptoms.shtml http://antoine.frostburg.edu/chem/senese/101/reactions/symptoms.shtml  “The Law of Conservation Mass”  http://www.mi.mun.ca/users/edurnfor/1100/atomic%20structure/tsld004.htm http://www.mi.mun.ca/users/edurnfor/1100/atomic%20structure/tsld004.htm  “Law of Conservation Mass- Definition”  http://www.biochem.northwestern.edu/holmgren/Glossary/Definitions/Def-L/law_conservation_of_mass.html http://www.biochem.northwestern.edu/holmgren/Glossary/Definitions/Def-L/law_conservation_of_mass.html  “Types of Chemical Reactions”  http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm  “Activation Energy”  http://www.bio-medicine.org/biology-definition/Activation_energy/ http://www.bio-medicine.org/biology-definition/Activation_energy/  http://en.wikipedia.org/wiki/Activation_energy http://en.wikipedia.org/wiki/Activation_energy  “Combustion”  http://en.wikipedia.org/wiki/Combustion http://en.wikipedia.org/wiki/Combustion  “Combustion Reactions”  http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactions/combustion.html http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactions/combustion.html

16. Bibliography Continued  “Chemical Decomposition”  http://en.wikipedia.org/wiki/Chemical_decomposition http://en.wikipedia.org/wiki/Chemical_decomposition  “Chemical Synthesis”  http://en.wikipedia.org/wiki/Chemical_synthesis http://en.wikipedia.org/wiki/Chemical_synthesis  “The Six Types of Chemical Reactions”  http://misterguch.brinkster.net/6typesofchemicalrxn.html http://misterguch.brinkster.net/6typesofchemicalrxn.html

17. Chemical Reaction Power Point By Ollie Auerbach http://www.chemistryland.com/CHM130/IconChemicalReactions.jpg