types of reactions. law of conservation of mass matter cannot be created nor destroyed just...
DESCRIPTION
INDICATIONS OF A CHEMICAL REACTION Production of heat, light, or temperature change Production of a gas Formation of a precipitate Color change Odor changeTRANSCRIPT
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TYPES OF REACTIONS
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LAW OF CONSERVATION OF MASS Matter cannot be created nor destroyed just rearranged Chemical Equation- Represents, with symbols and formulas, the identities and relative amounts of the reactants and products in a chemical reaction
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INDICATIONS OF A CHEMICAL REACTION Production of heat, light, or temperature change
Production of a gas Formation of a precipitate Color change Odor change
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SYMBOLS USED IN CHEMICAL EQUATIONS
NH4OH(aq) → NH3(g) + H2O(l)
→→ Yields- indicates result of reaction
→→
←←
Indicates reversible reaction
(s)(s) solid
(l)(l) Liquid
(g)(g) Gas
(aq)(aq) Aqueous solution- dissolved in water
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SYMBOLS USED IN CHEMICAL EQUATIONS
ºCºC
→→
Temperature at which reaction is carried out
PressurePressure
→→
Pressure exceeds normal atmospheric pressure
↑↑ (g) gaseous product
∆ ∆ heatheat
→→
→→
Reactants are heated
MnOMnO22
→→
Catalyst, alters rate of reaction
2H2O2 (l) 2H2O (l) + O2 (g) MnO2
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7 DIATOMIC COVALENT MOLECULES The 7 elements are never alone in nature and are always a molecule. All of the following are Nonpolar Covalent Br2- liquid Bring =Bromine H2- gas Home =Hydrogen I2- solid Important =Iodine Cl2- gas Class =Chlorine N2- gas Notes =Nitrogen O2- gas Or =Oxygen F2- gas Fail =Fluorine
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SYNTHESISA + B ABExamples:
2Mg + O2 2MgO
Sr + Br2 SrBr2
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DECOMPOSITION AB A + BExamples:
2H2O 2H2 + O2
2H2O2 2H2O + O2 Blood
Electrolysis of water- Decomposition of water using an electric current
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DECOMPOSITION
+
+
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SINGLE-REPLACEMENTA + BC AC + B
Examples: 2Na + 2H2O 2NaOH + H2
Zn + 2HCl ZnCl2 + H2
Fe + CuCl2 Cu + FeCl2
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SINGLE-REPLACEMENT
+ +
+ +
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DOUBLE-REPLACEMENTAB + CD AD + CB
Examples:KI + Pb(NO3)2 KNO3 + PbI2
AgNO3 + NaCl AgCl + NaNO3
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DOUBLE-REPLACEMENTThey generally take place in an aqueous solution and they often produce a precipitate, gas, or a molecular compound.
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COMBUSTIONA combustion reaction is where a substance reacts with
oxygen with the release of heat and usually the production of a flame.
A hydrocarbons will react with oxygen and combust into carbon dioxide and water.
C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g) A nonmetal will react with oxygen and combust into its nonmetal oxide and water SiH4 + 2O2 SiO2 + 2H2O
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EXAMPLE PRACTICE AlBr3 + K KBr + Al
Single replacement
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PRACTICE FeO + PdF2 FeF2 + PdO
Double replacement
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P4 + Br2 PBr3
Synthesis
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LiCl + Br2 LiBr + Cl2
Single replacement
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PbBr2 + HCl HBr + PbCl2
Double replacement
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C3H8 + 5O2 3CO2 + 4H2O
Combustion
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CoBr3 + CaSO4 CaBr2 + Co2(SO4)3
Double replacement
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Na3P + CaF2 NaF + Ca3P2
Single replacement
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•SrBr2 Sr + Br2
Decomposition
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Mn + HI H2 + MnI3
Single replacement
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•SrBr2 Sr + Br2
Synthesis
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Li3PO4 + NaBr Na3PO4 + LiBr
Double replacement
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CaF2 + Li2SO4 CaSO4 + LiF
Single replacement