warm-up
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Warm-up. Determine the type of reaction and predict the products: NaOH Li + Br 2 C 2 H 4 + O 2 . Activity Series . How to use the activity series. Find the element in the compound on the table. Find the Solo element - PowerPoint PPT PresentationTRANSCRIPT
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Warm-up Determine the type of reaction and
predict the products:
NaOH
Li + Br2
C2H4 + O2
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Activity Series How to use the activity series. 1. Find the element in the compound
on the table. 2. Find the Solo element3. If the solo element is above the
element in the compound then the reaction will take place.
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2Al(s) + 3ZnCl2(aq) To replace the Zinc, Aluminum must be
higher on the series
Cu(s) + 2NaCl(aq) Can copper replace sodium in the
compound?
3Zn(s) + 2AlCl3(aq)
NO REACTION
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Activity Series for Halogens Above the activity series for metals,
there is an activity series for Halogens. If your solo element is a halogen, it will
replace the bonded halogen as long as it is above it on the activity series.
Remember, every halogen on the series is a diatomic molecule, so when it’s by itself, there will be two of them (F2, Br2, …)
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Practice!•Cr(s) + Pb(NO3)2(aq)
• Pt(s) + CaCl2(aq)
• Ca(s) + FeO (aq)
Cr(NO3)2(aq) + Pb(s)
NO REACTION
CaO (aq) + Fe(s)
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Warm-up Determine the type of reaction and
predict the products:
NaOH
Li + Br2
C2H4 + O2
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Predicting Products:Double Displacement
Unit 6, Day 5Kimrey
1 November
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Remember Double Displacement
Anions switch places and are each bonded to a different cation
AB + CD AD + CB
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Predicting the Products of Double Displacement
Involves determining charges, criss-crossing, and the solubility rules
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Why do solubility rules matter?
All double displacement reactions (in this unit) will produce a precipitate
A precipitate is a solid that’s produced during a chemical reaction in a solution
So, if a precipitate is not formed, then the reaction will not take place!!
We can determine if a precipitate is formed by looking at our solubility rules
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Solubility If something is soluble, then it can be
dissolved by what it’s bonded to If something is insoluble, then it cannot
be dissolved
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What does it mean for us? If one of your products is insoluble,
then its state of matter is solid and a precipitate has formed.
If one of your products is soluble, then its state of matter is aqueous and no precipitate has formed.
You must have at least one solid product for a reaction to occur.
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Solubility Rules: Soluble Soluble
› All Nitrates, Acetates, Ammoniums, and Group 1 salts.
› All Chlorides, Bromides, and Iodides, except Silver, Lead, and Mercury (I)
› All Fluorides except Group 2, Lead (II), and Iron (III)
› All Sulfates except Calcium, Strontium, Barium, Mercury, Lead(II), and Silver
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Solubility: Insoluble
Insoluble › All Carbonates and Phosphates except
Group 1 and Ammonium › All Hydroxides except Group 1, Strontium,
Barium , and Ammonium › All Sulfides except Group 1, Group 2, and
Ammonium › All Oxides except Group 1
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Steps1. First break the reactants into their ions
(find the charges!).2. Next, swap partners for both (OI with a
twist)3. Check solubility rules to see if a solid
(precipitate) has formed. 4. Write complete balanced equation with
states of matter.
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Example
Sodium Hydroxide + Copper (II) Sulfate What are the Ions? What are the reactants? What are the potential products? Are any potential products insoluble? What is the complete equation
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PracticePredict the products and determine if a precipitate forms.
Sodium phosphate + Nickel (II) chloride › NaCl and Ni3(PO4)2.
Lead (II) Nitrate + Potassium Iodide › PbI2 and KNO3
Sodium Hydroxide + Potassium Chloride› NaCl and KOH
Sodium phosphate + Lead (IV) nitrate› Pb3(PO4)4 and NaNO3
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Writing molecular equations You already know how to do this! This is the chemical equation with the
states of matter in it. Make sure it’s balanced!
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Writing the Net Ionic equation
You almost know how to do this!1. Start with the completely balanced
equation. 2. Look at the solid product and make it
the product of your Net Ionic equation. 3. For the reactants, put the ions that
lead to the product
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Example
Na2SO4 + CaCl2 2NaCl + CaSO4
› SO42-
(aq)+ Ca2+(aq)CaSO4 (s)
3NaOH + FeCl3 3NaCl + Fe(OH)3
› 3OH-(aq) + Fe3+
(aq) Fe(OH)3 (s)
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Net Ionic equation
Take the complete ionic equation and remove the spectator ions.
Spectator ions are the ions not involved in the reaction.
Ex. Na2SO4 + CaCl2 2NaCl + CaSO4
› CaSO4 (s) + 2NaCl(aq) › SO4
2-(aq)+ Ca2+
(aq) CaSO4 (s)
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Practice
NaCl + AgNO3 AgCl +NaNO3› Na+
(aq) + Cl-(aq) + Ag+(aq) + NO3
-(aq) AgCl (s) + Na+
(aq) + NO3-(aq)
› Ag+(aq) + Cl-(aq) AgCl (s)
2NaOH + CuSO4 Cu(OH)2 + Na2SO4› 2Na+
(aq) + 2OH-(aq) + Cu2+
(aq)+ SO42-
(aq) Cu(OH)2(s) + 2Na+(aq) +
SO42-
(aq) › Cu2+
(aq) + 2OH-(aq) Cu(OH)2 (s)