Reactions and Equations. Chemical Reaction - One or more substances change into one or more new...
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Transcript of Reactions and Equations. Chemical Reaction - One or more substances change into one or more new...
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Reactions and Equations
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Chemical Reaction - One or more substances change into one or more new substances
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Represents with symbols and formulas
The identities and relative amounts of the reactants and products in a chemical reaction
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Reactants-Left side of an equation- what starts the reaction
Products- right side of an equation- what a rxn ends with
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1. Production of heat/light
2. Production of gas3. Formation of a
precipitate Precipitate: a
solid produced- separates from a solution
4. Color Change
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Word equation- uses words Formula equation- formulas and
symbols Complete Ionic Formula- shows soluble
substances in their dissociate form Net Ionic equation- removes the
spectator ions which are present on both sides of the equation.spectator ions = IONS that are exactly the same on both sides
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- yields- solidg - gasaq- aqueous- solid producedheat as a catalyst
l - liquid - gas produced reversible reaction
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Reversible reaction- products can reform reactants
Catalyst- “speeds” up a reaction- lowers the activation energy
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1. Write the correct formulas2. Use coefficients to balance (big # in
front)3. Check each individual element4. Reduce coefficients if needed
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1. Synthesis- (combination) two or more substances combine to produce a more complex substance.
x + y xy 2. Decomposition- A substance breaks down into two or
more simpler substances.xy x + y
3. Single Replacement (displacement)- a single element replaces a similar element in a compound
metal will replace metal nonmetal will replace nonmetal
x + ay xy + a4. Double Replacement (double displacement)- positive
ion exchange xy + ab ay + xb
5. Combustion- rapid reaction that involves O2
Organic + O2 CO2 + H2O
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Solute- small part- is dissolved
Solvent- large part- does dissolving
Spectator ions- present in solution on both sides of the yield
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% Composition – Element x100Compound
Empirical Formula – Lowest whole number ration of elements in a compound.
Empirical Formula From % Composition- % → grams → moles→ divide my lowest number of moles = Ratio! :D
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Molecular Formula : From empirical Molecular Mass x Empirical Formula
Empirical Mass
Hydrates: Crystals that contain water in crystal.