Post on 06-Jan-2016
description
By Ollie Auerbach
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
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
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://antoine.frostburg.edu/chem/senese/101/reactions/symptoms.shtml
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.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
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
Exothermic/ Endothermic Reactions Exothermic Endothermic 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. - 2H2+O2 changes to 2H2O
http://www.usoe.k12.ut.us/curr/science/sciber00/8th/matter/sciber/chemtype.htm
Energy is absorbed Energy is required for
reaction to happen Energy absorbed is
usually electrical energy or heat energy
Ex. –Photosynthesis, sunlight + 6CO2(g) + H2O(l) =
C6H12O6(aq) + 6O2(g)
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://www.bio-medicine.org/biology-definition/Activation_energy/
http://en.wikipedia.org/wiki/Activation_energy
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
Combustion
The act or process of burning O2 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:
2H2 + O2 → 2H2O(g) + heat. The result is water vapor.
http://en.wikipedia.org/wiki/Combustion
http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactions/combustion.html
http://www.ueberbill.com/images/ROCKET.jpg
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 2H2O → 2H2 + O2
http://en.wikipedia.org/wiki/Chemical_decomposition
Synthesis
The combining of separate elements or substances to form a whole.
Basic Formula- A + B ---> AB Examples-
2Na + Cl2 → 2 NaCl (formation of table salt) 4 Fe + 3 O2 → 2 Fe2O3 (iron rusting)
http://en.wikipedia.org/wiki/Chemical_synthesis
http://www.dearbornschools.org/schools/dcmst/staff/whittaker/NaCl123.gif
Single Displacement
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(NO3)2 + 2 KI ---> PbI2 + 2 KNO3
http://www.hempfieldarea.k12.pa.us/webdir/MILLERS/dd%20reaction.png
http://misterguch.brinkster.net/6typesofchemicalrxn.html
Bibliography
“Chemical Reaction Definition-” http://dictionary.reference.com/browse/chemical%20reaction
“Chemical Reactions” http://en.wikipedia.org/wiki/Chemical_reaction
“Ten Signs of a Chemical Change” 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
“Law of Conservation Mass- Definition”
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
“Activation Energy” http://www.bio-medicine.org/biology-definition/Activation_energy/
http://en.wikipedia.org/wiki/Activation_energy
“Combustion” http://en.wikipedia.org/wiki/Combustion
“Combustion Reactions” http://www.iun.edu/~cpanhd/C101webnotes/chemical%20reactions/combustion.html
Bibliography Continued
“Chemical Decomposition” http://en.wikipedia.org/wiki/Chemical_decomposition
“Chemical Synthesis” http://en.wikipedia.org/wiki/Chemical_synthesis
“The Six Types of Chemical Reactions” http://misterguch.brinkster.net/6typesofchemicalrxn.html
Chemical Reaction Power Point
By Ollie Auerbach
http://www.chemistryland.com/CHM130/IconChemicalReactions.jpg