chemical reactions
DESCRIPTION
Chemical Reactions. with Ionic Equation Writing. 2 Classifications. 1 . Redox Reaction There is a change in oxidation number between reactant side and product side Ca + Fe 3 (PO 4 ) 2 Ca 3 (PO 4 ) 2 + Fe. Oxidation # Ca = 0 Fe 2+ PO 4 3-. Ca 2+ PO 4 3- Fe = 0. - PowerPoint PPT PresentationTRANSCRIPT
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with Ionic Equation Writing
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1. Redox Reaction There is a change in oxidation number
between reactant side and product side
Ca + Fe3(PO4)2 Ca3(PO4)2 + FeOxidation #Ca = 0Fe2+ PO4
3-Ca2+ PO4
3-
Fe = 0Diatomics have an oxidation # of zero
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2. Non-Redox Reaction No change in oxidation number between
reactant side and product side
NaCl + K2SO4 Na2SO4 + KClOxidation #Na+ Cl-K+ SO4
2-Na+ SO4
2-
K+ Cl-Typically 2 ionic compounds reacting together
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If a compound is soluble in water,
it exists as ions in water.
If a compound is insoluble in water,
It exists as a precipitate (solid) in water
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We are going to assume all reactant compounds are soluble in water as we practice making ions…..
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If soluble in water: NH4F will exist as
◦NH4+
◦F-
NH4+
F-
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If soluble in water: H2CO3 will exist as
◦H+ ◦CO3
2-
H+
H+
CO32-
But really 2H+
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If soluble in water: Al(NO3)3 will exist as
◦Al3+ ◦NO3
-
NO3-
Al3+
NO3-
But really 3NO3-
NO3-
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1. Both reactants are soluble in water Mark with (aq)
2. Must determine if products are soluble or insoluble using solubility rules
If soluble – mark with (aq) If insoluble – mark with (s)
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Two elements in reactants take the place of each other
AB + CD AD + CBAgNO3(aq)+ NaCl(aq) AgCl(s) + NaNO3(aq)
Zn(OH)2(aq) + 2HCl(aq) ZnCl2(aq) + 2H2O(l)
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Reactants must be two ionic compounds or acids.
Usually in aqueous solution Na2SO4(aq) + CaCl2(aq) The positive ions change place. Na2SO4(aq)+ CaCl2(aq)Ca+2 SO4
2- + Na+1Cl-1
Na2SO4(aq) + CaCl2(aq) CaSO4(s) + 2NaCl(aq)
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Will only happen if one of the products:
◦doesn’t dissolve in water and forms an insoluble solid (s) (precipitate).
◦is a gas that bubbles out.◦is water (H2O) (neutralization reaction).
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Insoluble salt = a precipitate◦Solubility rules (see handout for explanation)
CASH N GiAm
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KCl Na2SO4 CaSO4 AgSO4 Na2CO3 MgS
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KCl(aq) Na2SO4(aq) CaSO4(s) AgSO4(s) Na2CO3(aq) MgS(s)
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Many reactions occur in water- that is, in aqueous solution
Many ionic compounds “dissociate”, or separate, into cations and anions when dissolved in water
Now we can write a complete ionic equation & net ionic equation.
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Example:AgNO3(aq) + NaCl (aq) AgCl (s) + NaNO3(aq)
1.this is the full equation (molecular equation)
2. now write it as an complete ionic equation Anything (aq) will dissociate (separate into ions)
Ag+ + NO3- + Na+ + Cl- AgCl(s) + Na+ + NO3
-
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Complete ionic equation:Ag+ + NO3
- + Na+ + Cl- AgCl(s) + Na+ + NO3-
3. can be simplified by eliminating ions not directly involved in making the reaction happen (spectator ions) = net ionic equation
Ag+ + Cl- AgCl(s)Na+ and NO3
- are spectator ions and are removed in the net ionic equation.