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http://www.chemistryexplained.com/images/chf
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Chemical Reaction- When substances change chemically to form a new substance.
1. Forms new bonds between atoms.
2. Make new substances
3. Example2 hydrogen atoms (gas) +1 oxygen atom (gas) react to form 1 water molecule
(h20)
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How do you know a reaction occurred?
1. A gas is produced and the chemical starts to bubble.
2. The chemical changes color.
3. The temperature of the chemical changes from before.
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What happens in a reaction?
1. Reactants react to create a product.
Reactants- the materials that exist before the chemical reaction
Products- Substances that are created by the chemical reaction
2. In a reaction atoms are arranged and no new atoms are created.
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Energy is needed to break chemical
bonds so they can start a chemical
reaction. Energy is released when
bonds form.
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Chemical Energy- energy that is
stored in atoms and molecules.
Chemical energy can be released
during a reaction.
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Potential Energy can be thought of as
energy stored within a physical
system. It is called potential energy
because it has the potential to be
converted into other forms of energy,
such as kinetic energy.
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Activation Energy- the energy needed
by a system to initiate a particular
process. Often used to denote the
minimum energy needed for a
specific chemical reaction to occur.
www.biomedicine.org/biologydefintion/
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Endothermic- Photosynthesis is
an example of an endothermic
reaction. Plants use the energy
to form the sun to convert
carbon dioxide and water into
the glucose and oxygen.
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Exothermic- Mixture of sodium
and chlorine to yield table salt.
This reaction produces 411 (kj)
of energy for each mole of salt
that is produced.
www.chemistry.about.com/cs/gen
ralchemistry
Exothermic processes
Endothermic processes
Making ice cubes
Formation of snow in clouds
Condensation of rain from water vapor
A candle flame
Melting ice cubes
Conversion of frost to water vapor
Evaporation of water
Forming a cation from an atom in the gas
phase
Baking bread
Cooking an egg
Producing sugar by photosynthesis
Separating ion pairs
Splitting a gas molecule apart
Mixing water and ammonium nitrate
Making an anrous salt from a hydrate
Melting solid salts
Reaction of barium hydroxide crystals with
dry ammonium chloride
Reaction of thionyl chloride (SOCl2) with
cobalt(II) sulfate heptahydrate
Mixing sodium sulfite and bleach
Rusting iron
Burning sugar
Forming ion pairs
Combining atoms to make a gas phase
Mixing water and strong acids
Mixing water with an anhydrous salt
Crystallizing liquid salts
Nuclear fission
Mixing water with calcium chloride
Exothermic Reactions- Reactions that releases energy and
the temperature gets hotter.
Endothermic Reactions- Reactions that absorbs energy
and the temperature gets colder.
Synthesis Reaction- two or more
simple substances combine to
form a more complex substance.
Decomposition Reaction- a more
complex substance breaks down
into its more simple parts 1
reactant yields or more products.
Reactions are opposite.
Single Replacement- a single
uncombined element replaces
another in a compound.
Double Replacement- parts of two
compounds that switches places to
forms two new compounds.
www.usoe.k12ut.us/curr/science
Combustion Reaction- always
involves molecular oxygen.
Anytime anything burns it is a
combustion reaction.
www.iun.edu/
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Synthesis Reaction
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Single Replacement
A + B AB
2 AgNO3 + Cu Cu(NO3)2 + 2 Ag
Two materials, elements or
compounds, come together to
make a single product. Some
examples of synthesis reactions
are: Hydrogen gas and oxygen
gas burn to produce water.
The element replaces one of
the ions in the solution and a
new element appears from the
ion in solution.
Decomposition Reaction
XZ = X + Z
Some examples of
decomposition reactions are:
potassium chlorate when
heated comes apart into
oxygen gas and potassium
chloride
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Double Replacement
AgNO3 + KCl AgCl(s) + KNO3
Dissolved silver nitrate
becomes a solution of silver ions
and nitrate ions. Potassium
chloride ionizes the same way.
When the two solutions are
added together, the silver ions
and chloride ions find each
other and become a solid
precipitate.
http://www.chemtutor.com/react.htm
WRITE THE FORMUAL FOR EACH MATERIAL
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1. sulfur trioxide and water combine to make sulfuric acid.
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2. lead II nitrate and sodium iodide react to make lead iodide and sodium nitrate.
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3. calcium fluoride and sulfuric acid make calcium sulfate and hydrogen fluoride (Hydrofluoric acid)
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4. calcium carbonate will come apart when you heat it to leave calcium oxide and carbon dioxide.
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5. ammonia gas when it is pressed into water will make ammonium hydroxide.
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6. sodium hydroxide neutralizes carbonic acid
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7. zinc sulfide and oxygen become zinc oxide and sulfur.
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8. lithium oxide and water make lithium hydroxide
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9. aluminum hydroxide and sulfuric acid neutralize to make water and aluminum sulfate.
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10. sulfur burns in oxygen to make sulfur dioxide.
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11. barium hydroxide and sulfuric acid make water and barium sulfate.
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12. aluminum sulfate and calcium hydroxide become aluminum hydroxide and calcium sulfate.
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13. copper metal and silver nitrate react to form silver metal and copper II nitrate.
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14. sodium metal and chlorine react to make sodium chloride.
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15. calcium phosphate and sulfuric acid make calcium sulfate and phosphoric acid.
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16. phosphoric acid plus sodium hydroxide.
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17. propane burns (with oxygen)
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18. zinc and copper II sulfate yield zinc sulfate and copper metal
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19. sulfuric acid reacts with zinc
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20. acetic acid ionizes.
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21. steam methane to get hydrogen and carbon dioxide
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22. calcium oxide and aluminum make aluminum oxide and calcium
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23. chlorine gas and sodium bromide yield sodium chloride and bromine
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