Section 2 - Types of Chemical Reaction
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| a reaction in which two or more substances combine to form a new compound | Synthesis Reaction
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| a reaction in which a single compound breaks down to form two or more simpler substances | decomposition reaction
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| the process in which an electric current is used to produce a chemical reaction, such as the decomposition of water | Electrolysis
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| a reaction in which one element or radical takes the place of another element or radical in a compound | single-displacement reaction
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| the oxidation reaction of an organic compound, in which energy as heat is released | combustion Reaction
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| five basic types of reactions | synthesis,decomposition, single-displacement, double-displacement, and combustion reactions
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| One simple type of synthesis reaction is the combination of an element with oxygen to produce an | oxide of the element
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| Most metals react with the Group 17 elements, the halogens, to form | ionic or covalent compounds
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| Group 1 metals react with halogens to form | ionic compounds with the formula MX, where M
is the metal and X is the halogen
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| Group 2 metals react with the halogens to form ionic compounds with | formula MX2.
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| is so reactive that it combines with almost all metals | Fluorine
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| can be used to neutralize hydrochloric acid in your stomach | Calcium hydroxide
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| Oxides of active metals react with water to produce | metal hydroxides
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| highly reactive metals | Active metals
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| known as lime or quicklime | Calcium oxide, CaO
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| The addition of water to lime produce | Ca(OH)2,which is also known as slaked lime
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| one of the main ingredients in acid rain | sulfurous acid further reacts with oxygen to
form sulfuric acid
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| metal oxides and nonmetal oxides react with each other in synthesis reactions to form | salts
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| Decomposition reactions are the opposite of | synthesis reactions
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| Decomposition reactions are represented by this equation | AX --> A + X
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| Most decomposition reactions take place only when energy is in what form | electricity or heat is added
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| The simplest kind of decomposition reaction is | the decomposition of a binary compound into its elements
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| Who discovered oxygen through such a decomposition reaction in 1774, when he heated mercury(II) oxide to produce mercury and oxygen | Joseph Priestley
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| When mercury(II) oxide (the red-orange substance in the bottom of the test tube) is heated, it decomposes into | oxygen and metallic mercury
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| When a metal carbonate is heated, it breaks down to produce | metal chloride and oxygen
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| All metal hydroxides except those containing Group 1 metals decompose when heated to yield | metal oxides and water
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| When a metal chlorate is heated, it decomposes to produce | a metal chloride and oxygen
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| Certain acids decompose into | nonmetal oxides and water
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| Carbonic acid is unstable and decomposes readily at room temperature to produce | carbon dioxide and water
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| heated, sulfuric acid decomposes into | sulfur trioxide and water
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| Single-displacement reactions can be represented by the following general equations. | A + BX --> AX + B
or Y + BX --> BY + X
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| When solid aluminum is placed in aqueous lead(II) nitrate, Pb(NO3)2(aq), the aluminum replaces the lead and forms | Solid lead and aqueous aluminum nitrate
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| The most-active metals, such as those in Group 1, react vigorously with water to produce | metal hydroxides and hydrogen
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| Less-active metals, such as iron, react with steam to form a | metal oxide and hydrogen gas.
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| The most combine active halogen | Fluorine
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| in Group 17 each element can replace any element below it,but not | any element above it
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| One of the compounds formed by a double displacement reactions is | usually a precipitate, an insoluble gas that bubbles out of the solution, or a molecular compound, usually water
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| The formation of a precipitate occurs when | the cations of one reactant combine with the anions of another reactant to form an insoluble or slightly soluble compound.
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| examples of combustion reactions | The burning of natural gas, propane, gasoline, and wood
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