1. By: Seamus O’Brien

2.  In a chemical reaction the elements bond to each other through the taking or sharing of valence electrons.  During chemical reactions energy changes one form of matter into another. http://www.brownreference.com/php/PDFS/AN_Title_Information/552---Sample_Spreads.pdf http://www.brownreference.com/php/PDFS/AN_Title_Information/552---Sample_Spreads.pdf  The elements going into the chemical reactions are called reactants. After the elements have reacted they create a product. http://en.wikipedia.org/wiki/Chemical_reaction http://en.wikipedia.org/wiki/Chemical_reaction  Signs of a chemical reaction are bubbling, change in color, or a change in temperature. Http://www.harpercollege.edu/tm- ps/chm/100/dgodambe/thedisk/chemrxn/signs2.htm Http://www.harpercollege.edu/tm- ps/chm/100/dgodambe/thedisk/chemrxn/signs2.htm  The law of conservation of matter states that matter cannot be created nor destroyed. During chemical reactions matter seems to be created or destroyed, but really the atoms or molecules are just being rearranged. http://www.cartage.org.lb/en/themes/Sciences/Chemistry/Generalchemistry/Energy/LawofConservation/LawofConservation.htm http://www.cartage.org.lb/en/themes/Sciences/Chemistry/Generalchemistry/Energy/LawofConservation/LawofConservation.htm  Pictures http://twilit.files.wordpress.com/2007/12/thermometer.jpg http://www.fotosearch.com/bthumb/IMZ/IMZ004/vmo0479.jpg

3.  Every substance has energy from its electrons. Most things have potential energy as well.  Potential energy is the energy stored in something, this energy has the potential to be turned into other types of energy, hence the name “potential energy”.  To start a chemical reaction you will need some form of energy. This is called activation energy. This type of energy is needed because sometimes the elements need a little push to collide.  Reactions that release heat, light or sound are exothermic reactions, they can occur spontaneously. Ex) the mixing or sodium and chlorine combine to make table salt.  Endothermic reactions absorb energy instead of producing it. These decrease in temperature. Ex) Photosynthesis  http://chemistry.about.com/cs/generalchemistry/a/aa051903a.htm http://chemistry.about.com/cs/generalchemistry/a/aa051903a.htm  http://en.wikipedia.org/wiki/Potential_energy http://en.wikipedia.org/wiki/Potential_energy

4. Synthesis, Decomposition, Combustion, Single Replacement, and Double replacement.

5.  Synthesis is when two reactants are put together to form one product.  The basic form is: A + B  AB A and B are elements or compounds, and AB is the products that the elements or compounds create. A and B are known as reactants.  2Na + Cl 2  2 NaCl is the formula to form of table salt.  4 Fe + 3 O 2  2 Fe 2 O 3 is the formula of iron rusting. o http://en.wikipedia.org/wiki/Chemical_synthesis http://en.wikipedia.org/wiki/Chemical_synthesis

6. o Decomposition is the splitting of a compound into two different elements. o The basic form of decomposition is: AB  A + B  AB is a chemical compound.  A and B are the elements that are forms after decomposition has occurred.  2H 2 O 2  2H 2 O + O 2 is and example of hydrogen peroxide, which will decompose into water and oxygen. o H 2 CO 3  H 2 O + CO 2 is carbonic acid it will decompose over time into carbon dioxide and water. o http://en.wikipedia.org/wiki/Chemical_decomposition http://en.wikipedia.org/wiki/Chemical_decomposition

7.  Combustion is a series of exothermic chemical reactions involving a type fuel and an oxidant.  These reactions give off heat, light, or both usually in flames or a glow.  There is no basic formula for combustion, however it will always contain oxygen in it.  2H 2 + O 2  2H 2 O(g) + heat, is an example of combustion. This is the combustion of hydrogen and oxygen. The result is water vapor.  http://en.wikipedia.org/wiki/Combustion http://en.wikipedia.org/wiki/Combustion

8.  Single replacement is when an ion or an element switch from one compound to another.  The basic form is A + BX  AX + B. Single replacement will occur if A is more reactive than B. A and B must either be metals, this makes X an anion, or A and B can be halogens, this will make X a cation.  Mg(s) + 2HCl(aq)  MgCl 2 (aq) + H 2 (g) is an example of single replacement. In this reaction magnesium, and hydrochloric acid, form magnesium chloride, and hydrogen.  http://en.wikipedia.org/wiki/Single_replacement_reaction http://en.wikipedia.org/wiki/Single_replacement_reaction The guy in the orange shirt steals the date of the other guy. So, a part of one of the reactants trades places and is in a different place among the products. http://www.usoe.k12.ut.us/CURR/Science/sciber00/8th/matter/sciber/chemtype.htm

9.  Double replacement involves the exchange of bonds between the two reacting chemical species.  It creates products with similar or identical bonding affiliations.  The formula for double replacement is AB + CD  AD + CB These chemical species can either be ionic or covalent.  HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l) is an example of double replacement. This reaction creates a solution of salt and water.  http://en.wikipedia.org/wiki/Double_replacement_reaction http://en.wikipedia.org/wiki/Double_replacement_reaction

10.  Chemical Reactions http://en.wikipedia.org/wiki/Chemical_reactionhttp://en.wikipedia.org/wiki/Chemical_reaction  Signs of a Chemical Reaction Http://www.harpercollege.edu/tm- ps/chm/100/dgodambe/thedisk/chemrxn/signs2.htm Http://www.harpercollege.edu/tm- ps/chm/100/dgodambe/thedisk/chemrxn/signs2.htm  Law of Conservation of Matter http://www.cartage.org.lb/en/themes/Sciences/Chemistry/Generalchemistry/Energy/LawofC onservation/LawofConservation.htm http://www.cartage.org.lb/en/themes/Sciences/Chemistry/Generalchemistry/Energy/LawofC onservation/LawofConservation.htm  Endothermic and Exothermic Reactions http://chemistry.about.com/cs/generalchemistry/a/aa051903a.htm http://chemistry.about.com/cs/generalchemistry/a/aa051903a.htm  Chemical Synthesis http://en.wikipedia.org/wiki/Chemical_synthesishttp://en.wikipedia.org/wiki/Chemical_synthesis  Chemical decomposition http://en.wikipedia.org/wiki/Chemical_decomposition http://en.wikipedia.org/wiki/Chemical_decomposition  Combustion http://en.wikipedia.org/wiki/Combustion http://en.wikipedia.org/wiki/Combustion  Single Displacement Reaction http://en.wikipedia.org/wiki/Single_replacement_reactionhttp://en.wikipedia.org/wiki/Single_replacement_reaction  Metathesis Reaction http://en.wikipedia.org/wiki/Double_replacement_reactionhttp://en.wikipedia.org/wiki/Double_replacement_reaction