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Transcript of Chemical Reactions Chapter 11. Describing Chemical Reactions Essential Question: How does one write...
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Chemical Reactions
Chapter 11
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Describing Chemical Reactions
Essential Question:
How does one write a proper word, skeleton or chemical equation?
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Writing Chemical Equations
• How do you describe what has happened in a chemical reaction?
• Recall from Chapter 2 the shorthand method of describing a chemical reaction:
Reactants Products
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Word Equations
iron + oxygen Iron(III) oxide
hydrogen peroxide water + oxygen
methane + oxygen carbon dioxide + water
What does the arrow in these word equations indicate?
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Skeleton Equations
Fe + O2 Fe2O3
H2O2 H2 + O2
CH4 + O2 CO2 + H2O
A skeleton equation is an equation that does not indicate the relative amounts of the substance involved.
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Balancing Chemical Equations
• How would you write a word equation for the production of a tricycle?
frame + wheel + handlebar + pedal
tricycle
This doesn’t tell about the relative amounts involved
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Skeleton Equations
• How would you write a skeleton equation for the production of a tricycle?
F + W + H + P FW3H2P2
Notice:This still doesn’t tell about the relative
amounts involved
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Bicycle Equation
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Balanced Equations
• How would you write a balance chemical equation for the production of a tricycle?
F + 3W + 2H + 2P FW3H2P2
Notice:You must use coefficients to indicate the
relative amounts involved.
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Balancing Chemical Reactions
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Combustion of Methane
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Production of Hydrogen Chloride
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Rules for Writing Balanced Chemical Equations
See the table at the top of page 327.
Balancing Chemical Equations –
Computer lab activity
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Balance These Equations
AgNO3 + H2S Ag2S + HNO3
Zn(OH)2 + H3PO4 Zn3(PO4)2 + H20
FeCl3 + Ca(OH)2 Fe(OH)3 + CaCl2
Ag2S(s) + Al(s) Ag(s) + Al2S3(g)
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Types of Chemical Reactions
Essential Question:
What are the five general types of chemical reactions, and how can you predict the products of these
reactions?
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Classifying Reactions
Reactions fall into five general categories:
• Combination Reactions
• Decomposition Reactions
• Single Replacement Reactions
• Double Replacement Reactions
• Combustion Reactions
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Combination Reactions
• Two or more substances forming a single new substance.
• Our analogy: like a marriage
• What distinguishes combination reactions is the presence of only one product.
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Combination Reactions
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Combination Reactions• Also known as Synthesis reactions.
Examples:
2Mg(s) + O2(g) 2MgO
2K(s) + Cl2(g) 2KCl(s)
Fe(s) + S(s) FeS(s)
2Fe (s) + 3S(s) Fe2S3(s)
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Decomposition Reactions
• A single compound breaks down into two or more simpler products.
• Our analogy: a divorce
• What distinguishes a decomposition reaction is a single reactant.
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Decomposition Reactions
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Decomposition Reactions
Examples:
2HgO(s) 2Hg(l) + O2(g)
2H2O (l) 2H2 (g) + O2(g)
2HI H2(g) + I2(s)
electricity
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Single-Replacement Reactions
• One element replaces another element in a compound.
• Our analogy: Date-stealing
• What distinguishes a S-R reaction is an uncombined element in the reactants with a different uncombined element in the products.
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Single-Replacement Reactions
Examples:
Fe(s) + Pb(NO3)2(aq)
Fe(NO3)2(aq) + Pb(s)
Cl2(g) + 2NaI(aq)
2NaCl(aq) + I2(aq)
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Single-Replacement
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Will S-R Reactions Occur?
• Whether one metal will replace another in a compound depends their respective reactivities.
• A reactive metal will replace any metal below it in the reactivity series.
• See Table 11.2 on page 333.
• What about the reactivity of the halogens?
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Activity Series of the Metals
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The Activity Series of the
Metals
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Double-Replacement Reactions
• A chemical change involving an exchange of positive ions between two compounds.
• Our analogy: Date-Swapping
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Double-Replacement
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Double-Replacement Reactions
Examples:
Na2S(aq) + Cd(NO3)2(aq)
CdS(s) + 2NaNO3(aq)
2NaCN(aq) + H2SO4(aq)
2HCN(g) + Na2SO4(aq)
Ca(OH)2(aq) + 2HCl(aq)
CaCl2(aq) + 2H2O(l)
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Double-Replacement Reactions
• For a D-R reaction to occur, one of the following is usually true:
– One of the products is a solid that precipitates out
– One of the products is a gas
– One of the products is a molecular compound, such as water
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Combustion Reactions
• An element or a compound reacts with oxygen, often producing light and heat.
• Complete combustion = a hydrocarbon reacting with oxygen to produce ONLY carbon dioxide and water as the products.
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Combustion Reactions
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CombustionExamples:
2C8H18(l) + 25O2(g)16CO2(g) + 18H2O(l)
2C6H6(l) + 15O2 12CO2(g) + 6H2O(g)
2Mg(s) + O2(g) 2MgO(s)
Which of these are complete combustion?
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Reactions in Aqueous Solution
Essential Question:
What does a net ionic equation show, and how can one predict the formation of a precipitate in a double-replacement reaction?
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Net Ionic Equations
• A net ionic equation shows only those particles involved in the reaction and is balanced with respect to both mass and charge.
• All ions that are unchanged from the reactants side to the products side of the equation are eliminated.
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Net Ionic Equations
• Begin with a double-replacement reaction:
AgNO3(aq) + NaCl(aq)
AgCl(s) + NaNO3(aq)
Write the complete ionic equation:
Ag+(aq) + NO3–(aq) + Na+ (aq) + Cl– (aq)
AgCl(s) + Na+(aq) + NO3– (aq)
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Net Ionic Equations, cont.
• Eliminate the ions that are “spectators”
Ag+(aq) + NO3–(aq) + Na+ (aq) + Cl– (aq)
AgCl(s) + Na+(aq) + NO3– (aq)
Ag+(aq) + NO3–(aq) + Na+ (aq) + Cl– (aq)
AgCl(s) + Na+(aq) + NO3– (aq)
• What remains is the Net Ionic EquationAg+(aq) + Cl– (aq) AgCl(s)
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Formation of Precipitates
• One can predict the formation of a precipitate by using the general rules for solubility for ionic compounds.
• See Table 11.3 on page 344, or see the Reference Tables.
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Solubility Rules for Ionic Compounds
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Predicting the Formation of a Precipitate
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Formation of PrecipitatesWill a precipitate form when the following
aqueous solutions are mixed?
AgNO3 and Na2SO4
NH4Cl and Ba(NO3)2
CaCl2 and K2SO4
Hg(NO3)2 and HClYes, No, Yes, No