chemical reactions
DESCRIPTION
Chemical Reactions. Ch.21 Sec.1. Chemical Reactions. Occurs with chemical changes Make new substances Change in which one or more substances are converted into new substances. Signs of Chemical Reactions. Change in color Release of light, heat, gas, sound, or smell. - PowerPoint PPT PresentationTRANSCRIPT
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Chemical ReactionsChemical ReactionsCh.21 Sec.1Ch.21 Sec.1
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Chemical ReactionsChemical Reactions
•Occurs with chemical changesOccurs with chemical changes
•Make new substancesMake new substances
•Change in which one or more Change in which one or more substances are converted into substances are converted into new substancesnew substances
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Signs of Chemical Signs of Chemical ReactionsReactions
•Change in Change in colorcolor
•Release of Release of light, heat, light, heat, gas, sound, or gas, sound, or smellsmell
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Examples of Chemical Examples of Chemical ReactionsReactions
• GrowingGrowing
• RipeningRipening
• DecayingDecaying
• BurningBurning
• RustingRusting
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Law of Conservation of Law of Conservation of MassMass
•Mass cannot be created or Mass cannot be created or destroyeddestroyed
•Chemical reactions rearrange Chemical reactions rearrange atoms atoms
•Break bonds, rearrange, and make Break bonds, rearrange, and make new bondsnew bonds
•Energy breaks bondsEnergy breaks bonds
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Chemical EquationChemical Equation
•A way to describe a chemical A way to describe a chemical reaction using chemical reaction using chemical formulas and other symbolsformulas and other symbols
•Pg. 635; Table 1 and equationPg. 635; Table 1 and equation
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Products & ReactantsProducts & Reactants
•Reactants = Reactants = left side of left side of equation equation (ALWAYS)(ALWAYS)
•Products = Products = right side of right side of equation equation (ALWAYS)(ALWAYS)
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Chemical EquationsChemical Equations
•Balanced chemical equation Balanced chemical equation – has – has same number of atoms of each same number of atoms of each element on both sides of the element on both sides of the equationequation
•Satisfies the Law of Conservation Satisfies the Law of Conservation of mass.of mass.
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Reaction TypesReaction Types
1.1. SynthesisSynthesis
2.2. DecompositionDecomposition
3.3. Single DisplacementSingle Displacement
4.4. Double DisplacementDouble Displacement
5.5. CombustionCombustion
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SynthesisSynthesis
Combines 2 substances to make 1 Combines 2 substances to make 1 compoundcompound
A + B --> ABA + B --> AB
Blue + Red --> PurpleBlue + Red --> Purple
Na + Cl --> NaClNa + Cl --> NaCl
1 Product1 Product
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SynthesisSynthesis
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DecompositionDecomposition
Takes 1 compound and breaks it Takes 1 compound and breaks it apart into 2 or more substancesapart into 2 or more substances
AB --> A + BAB --> A + B
HH22O --> HO --> H22 + O + O22
Opposite of synthesisOpposite of synthesis
1 Reactant1 Reactant
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DecompositionDecomposition
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Single-DisplacementSingle-Displacement
1 element swaps places with another 1 element swaps places with another element that is in a compoundelement that is in a compound
XA + B --> XB + AXA + B --> XB + AB and A swapped placesB and A swapped places
** Has 1 compound and 1 element on ** Has 1 compound and 1 element on both sidesboth sides
Ex: CuClEx: CuCl22 + Al --> AlCl + Al --> AlCl33 + Cu + Cu
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Single-DisplacementSingle-Displacement
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Double - DisplacementDouble - Displacement
2 compounds exchange elements 2 compounds exchange elements with each otherwith each other
AX + BY --> AY + BXAX + BY --> AY + BX
** 2 Compounds on both sides** 2 Compounds on both sides
Ex: NaCl + AgF Ex: NaCl + AgF NaF + AgCl NaF + AgCl
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Double - DisplacementDouble - Displacement
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CombustionCombustion
Oxygen and another compound Oxygen and another compound BURN to make new productsBURN to make new products
OxygenOxygen is ALWAYS a reactant is ALWAYS a reactant
COCO22 + H + H22O O is ALWAYS a productis ALWAYS a product
Ex: CHEx: CH44 + + OO22 --> --> COCO22 + H + H22OO
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What Type of Reaction? What Type of Reaction?
Double Double DisplacementDisplacement
DecompositionDecomposition
Single Single DisplacementDisplacement
SynthesisSynthesis
1.1. HCl + NaOH --> HCl + NaOH --> HH22O + NaClO + NaCl
2.2. NaCl --> Na + NaCl --> Na + ClCl22
3.3. Al + FeAl + Fe22OO33 --> --> AlAl22OO33 + Fe + Fe
4.4. PP44 + O + O22 --> P --> P44OO1010
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2 Types Energy 2 Types Energy ReactionsReactions
1.1. EndothermicEndothermic
2.2. ExothermicExothermic
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EndothermicEndothermic
• Endo = inEndo = in
• Energy is taken in Energy is taken in (absorbed) with (absorbed) with reactantsreactants
• Drops surrounding Drops surrounding environment temp.environment temp.
• Ex: Photosynthesis Ex: Photosynthesis - takes in sunlight- takes in sunlight
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ExothermicExothermic
• Exo = outExo = out
• Energy is released Energy is released or given out with or given out with productsproducts
• Raises surrounding Raises surrounding environmentenvironment’’s s temperaturetemperature
• Ex: hand warmersEx: hand warmers
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Exo or Endo?Exo or Endo?
1.1. ExoExo
2.2. ExoExo
3.3. EndoEndo
4.4. ExoExo
1.1. Paper burningPaper burning
2.2. Firecracker Firecracker ExplodingExploding
3.3. Plant making Plant making its own foodits own food
4.4. Electric Electric blanketblanket
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Reaction RateReaction Rate
• How fast a reaction is goingHow fast a reaction is going
• Factors on rate:Factors on rate:
1.1. TemperatureTemperature
2.2. Surface AreaSurface Area
3.3. ConcentrationConcentration
4.4. StirringStirring
5.5. CatalystsCatalysts
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CatalystsCatalysts• Substance that Substance that
speeds up reaction speeds up reaction without being without being permanently permanently changedchanged
• Ex: Enzymes in Ex: Enzymes in our stomach speed our stomach speed up digestion up digestion (lactose)(lactose)
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InhibitorsInhibitors
• Substance used to slow down a Substance used to slow down a chemical reactionchemical reaction
• Ex: Food preservatives (prevent Ex: Food preservatives (prevent spoilage)spoilage)
• Product is not changed just how fast Product is not changed just how fast or slow the rate of production occursor slow the rate of production occurs