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Chemical Equations & Reactions
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Indications of a Chemical Reaction
Evolution of heat/light Exothermic and Endothermic Production of a gas Formation of a precipitate Solid that is produced and separates Color change Fireworks video (6 min) Overview of chemical reactions (2 min)
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Factors Influencing Rate of Reaction
Nature of reactants Surface area Temperature Concentration Catalyst Increased surface area
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Chemical Equations Chemical Equation = represents, with symbols and formulas, the identities and relative amounts of reactants and products Reactants (R) – left of arrow Products (P) – right of arrow
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Symbols used in Equations
- yields - reversible reaction - gaseous product – solid product (g) – gaseous reactant or product (s) – solid reactant or product (l) – liquid reactant or product (aq) – aqueous (dissolved in water)
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Writing Chemical Equations
Must have correct formulas for each R and P Don’t forget diatomic elements Br2, I2, N2, Cl2, H2, O2, F2 Law of Conservation of Mass must be satisfied Balance the equation with coefficients
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Translating Equations
Write the balanced chemical equations: 1. Calcium phosphate and iron(II) oxide are produced from the reaction of calcium oxide and iron(II) phosphate. 2. The reaction of zinc with aqueous hydrochloric acid produces a solution of zinc chloride and hydrogen gas.
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Types of Chemical Reactions
Synthesis Decomposition Single Replacement Double Replacement Combustion
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Synthesis Reaction Two or more substances combine to form one product
EX: Calcium + oxygen → ?? EX: Barium + chlorine → ??
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Decomposition Reaction
Single compound breaks down into several simpler substances There are 4 types of decomposition reactions
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Binary Decomposition Metal oxide → metal + oxygen gas
EX: Zinc oxide → ?? Decomposition of nitrogen triiodide
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Metal Carbonate Decomposition
Metal carbonate → metal oxide + carbon dioxide EX: Strontium carbonate → ??
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Metal Chlorate Decomposition
Metal chlorate → metal chloride and oxygen gas EX: Iron (III) chlorate → ?? EX: Potassium hypochlorite → ??
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Metal Hydroxide Decomposition
Metal hydroxide → metal oxide + water EX: Calcium hydroxide → ??
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Single Replacement One metal replaces a metal in another compound OR
One nonmetal replaces a nonmetal in another compound EX: Copper + silver nitrate ?? EX: Calcium chloride + fluorine gas ?? Thermite
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Will a SR reaction always occur??
Check the Activity Series The more reactive element will make a bond. If the more reactive element is already bonded, write NR for no reaction. EX: Silver + copper (I) nitrate ?? Reactivity of Alkali Metals
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Double Replacement Ions of 2 reactants exchange places in an aqueous solution to form new products EX: Zinc oxalate + ammonium phosphate → ??
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More on Double Replacement
Some of the products may exist as ions in an aqueous solution, while others may exist as a solid Soluble Cmpd (aq) = Exists as ions in solution Insoluble Cmpd (s) = Exists as a solid in solution
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Soluble or Insoluble?? Check the solubility chart or rules on reference sheet Be sure to indicate which product is soluble and which is insoluble!!!!! Double Replacement - Production of Precipitate
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Examples of Solubility
Are these compounds soluble or insoluble? K2SO4 AgCl BaSO4 CaS K3PO4 MgCO3
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Net Ionic Equations Includes only the compounds and ions that are chemically changed Step 1: Write the products in words. Translate into a balanced equation – including states (use solubility rules) Step 2: Write the overall ionic equation – cancel spectator ions. Step 3: Write the net ionic equation – including states
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Example Zinc nitrate + ammonium sulfide → ??
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Combustion A substance reacts with oxygen to produce lots of energy, usually in the form of heat and light
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Complete Combustion C_H_ + O2 H2O + CO2 + energy
EX: Propane + oxygen gas → ?? Combustion Video (5 min) Origin of Combustion Engine Part 1(2 min) Origin of Combustion Engine Part 2 (3 min) Hindenburg Disaster (4 min)
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Incomplete Combustion
C_H_ + O2 H2O + CO2 + C + CO + E Dangerous product = CO
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