Determine the type of reaction and predict the products: NaOH Li + Br 2 C 2 H 4 + O 2

Warm-up Determine the type of reaction and

predict the products:

NaOH

Li + Br2

C2H4 + O2

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.

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

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, …)

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)

Warm-up Determine the type of reaction and

predict the products:

NaOH

Li + Br2

C2H4 + O2

Predicting Products:Double Displacement

Unit 6, Day 5Kimrey

1 November

Remember Double Displacement

Anions switch places and are each bonded to a different cation

AB + CD AD + CB

Predicting the Products of Double Displacement

Involves determining charges, criss-crossing, and the solubility rules

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

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

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.

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

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

Steps

1. 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.

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

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

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!

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

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)

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)

› SO42-

(aq)+ Ca2+(aq) CaSO4 (s)

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)+ SO4

2-(aq) Cu(OH)2(s) + 2Na+

(aq)

+ SO42-

(aq)

› Cu2+(aq) + 2OH-

(aq) Cu(OH)2 (s)