Dstreib:Stoichiometry,adapted with permission from Dr. Cotton. Types of Chemical Reactions...
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Transcript of Dstreib:Stoichiometry,adapted with permission from Dr. Cotton. Types of Chemical Reactions...
![Page 1: Dstreib:Stoichiometry,adapted with permission from Dr. Cotton. Types of Chemical Reactions OBJECTIVES: –Identify a reaction as combination, decomposition,](https://reader031.fdocuments.net/reader031/viewer/2022013004/56649eb55503460f94bbdb6a/html5/thumbnails/1.jpg)
dstreib:Stoichiometry,adapted with permission from Dr. Cotton.
Types of Chemical Reactions
• OBJECTIVES:
–Identify a reaction as combination, decomposition, single-replacement, double-replacement, or combustion
![Page 2: Dstreib:Stoichiometry,adapted with permission from Dr. Cotton. Types of Chemical Reactions OBJECTIVES: –Identify a reaction as combination, decomposition,](https://reader031.fdocuments.net/reader031/viewer/2022013004/56649eb55503460f94bbdb6a/html5/thumbnails/2.jpg)
Types of Chemical Reactions
• OBJECTIVES:– Predict the products of
combination, decomposition, single-replacement, double-replacement, and combustion reactions.
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Types of Reactions• There are millions of reactions.
• Fall into several categories.
• We will learn 5 major types.
• Will be able to predict the products.
• For some, we will be able to predict whether they will happen at all.
• Will recognize them by the reactants
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#1 - Combination Reactions• Combine - put together• 2 substances combine to make one
compound.• Ca +O2 CaO• SO3 + H2O H2SO4
• We can predict the products if they are two elements.
• Mg + N2
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Write and balance
• Ca + Cl2 • Fe + O2 iron (II) oxide• Al + O2 • Remember that the first step is to
write the correct formulas• Then balance by using coefficients
only
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#2 - Decomposition Reactions• decompose = fall apart• one reactant falls apart into two
or more elements or compounds.
• NaCl Na + Cl2 • CaCO3 CaO + CO2
• Note that energy is usually required to decompose
electricity
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#2 - Decomposition Reactions
• Can predict the products if it is a binary compound
• Made up of only two elements• Falls apart into its elements• H2O• HgO
electricity
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#2 - Decomposition Reactions
• If the compound has more than two elements you must be given one of the products
• The other product will be from the missing pieces
• NiCO3 CO2 + ? • H2CO3(aq) CO2 + ?
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#3 - Single Replacement
• One element replaces another• Reactants must be an element and a
compound.• Products will be a different element
and a different compound.• Na + KCl K + NaCl• F2 + LiCl LiF + Cl2
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#3 Single Replacement• Metals replace other metals (and
hydrogen)• K + AlN • Zn + HCl • Think of water as HOH• Metals replace one of the H, combine
with hydroxide.• Na + HOH
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#3 Single Replacement
• We can tell whether a reaction will happen• Some chemicals are more “active” than
others• More active replaces less active • There is a list on page 294(and Table J) -
called the Activity Series of Metals• Higher on the list replaces lower.
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#3 Single Replacement• Note the ** concerning Hydrogen • H can be replaced in acids by everything
higher• Li, K, Ba, Ca, & Na replace H from acids
and water• Fe + CuSO4 • Pb + KCl • Al + HCl
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#3 - Single Replacement• What does it mean that Hg and Ag are
on the bottom of the list?• Nonmetals can replace other nonmetals• Limited to F2 , Cl2 , Br2 , I2 (halogens) • Higher replaces lower.• F2 + HCl • Br2 + KCl
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#4 - Double Replacement• Two things replace each other.• Reactants must be two ionic
compounds or acids.• Usually in aqueous solution• NaOH + FeCl3 • The positive ions change place.• NaOH + FeCl3 Fe+3 OH- + Na+1 Cl-1
• NaOH + FeCl3 Fe(OH)3 + NaCl
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#4 - Double Replacement• Has certain “driving forces”
– Will only happen if one of the products:
– doesn’t dissolve in water and forms a solid (a “precipitate”), or
– is a gas that bubbles out, or– is a covalent compound (usually
water).
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Complete and balance
• assume all of the following reactions take place:
CaCl2 + NaOH
CuCl2 + K2S
KOH + Fe(NO3)3
(NH4)2SO4 + BaF2
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How to recognize which type
• Look at the reactants:
E + E = Combination
C = Decomposition
E + C = Single replacement
C + C = Double replacement
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Examples
• H2 + O2 • H2O • Zn + H2SO4 • HgO • KBr +Cl2 • AgNO3 + NaCl • Mg(OH)2 + H2SO3
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#5 - Combustion• Means “add oxygen”• A compound composed of only C, H,
and maybe O is reacted with oxygen• If the combustion is complete, the
products will be CO2 and H2O.• If the combustion is incomplete, the
products will be CO (possibly just C) and H2O.
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Examples
• C4H10 + O2 (assume complete)
• C4H10 + O2 (incomplete)
• C6H12O6 + O2 (complete)
• C8H8 +O2 (incomplete)
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An equation...• Describes a reaction• Must be balanced in order to follow
the Law of Conservation of Mass• Can only be balanced by changing the
coefficients.• Has special symbols to indicate
physical state, and if a catalyst or energy is required.
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Reactions
• Come in 5 major types.• Can tell what type they are by the
reactants.• Single Replacement happens based
on the activity series• Double Replacement happens if the
product is a solid, water, or a gas.