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CHEMICAL REACTIONS UNIT 5
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Evidence of Chemical Reactions
Heat or light Color change Odor change Release of gas (bubbles) Formation of a solid (precipitate)
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Law of Conservation of Matter
Matter is neither created nor destroyed in ordinary chemical reactions Must have equal numbers of atoms on both sides of the equation to obey this Law.
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Chemical Equations X + Y XY Coefficients
Statements using words or formulas that describes a chemical change. Consists of two parts Reactants Starting substances in a chemical change Always written on the left side of an equation Products Substances formed in a chemical reaction Always written on the right side of the equation Coefficients Numbers in front of formulas used to balance the numbers of atoms in an equation X + Y XY reactants products
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Diatomic Elements 7 elements that are formed by bonding two atoms of that element. Are written as diatomic molecules in the elemental form Br, I, N, Cl, H, O, & F Ex: Bromine = Br2 Mr. “BrINClHOF
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Examples H2 + Br2 HBr Mg + NaOH Mg(OH)2 + Na
hydrogen + nitrogen ammonia Sulfur + oxygen sulfur trioxide
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Types of Reactions
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Types of Reaction X + Y XY XY X + Y
Synthesis: 2 or more substances combine into 1 Decomposition: 1 substance breaks down into2 or more simpler ones X + Y XY XY X + Y
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Types of Reaction XY + Z XZ + Y XY + AB XB + AY
Single replacement: one element replaces another in a compound Double replacement: two compounds form 2 new ones XY + Z XZ + Y XY + AB XB + AY
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Types of Reaction CH4 + 2O2 CO2 + 2H2O HCl + NaOH NaCl + H2O
Combustion: carbon compound burns in oxygen to form carbon dioxide and water. Acid-Base: an acid & base react to form a salt & water. CH4 + 2O2 CO2 + 2H2O HCl + NaOH NaCl + H2O
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Practice ammonia hydrogen & nitrogen
magnesium + oxygen magnesium oxide hydrochloric acid + calcium hydroxide calcium chloride + water zinc + hydrobromic acid zinc bromide + hydrogen magnesium oxide + calcium fluoride magnesium fluoride + calcium oxide methane (CH4) + oxygen carbon dioxide + water
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