Measurements and Calculations Review (Foldable)



Precipitation Double Replacement (occur in a solution)

AB + CD ( AD(s) + CB

Use solubility chart to determine if reaction will occur. Predict the products of the reaction. Look up the solubility of each predicted PRODUCT on the solubility chart. If one product is INSOLUBLE reaction will occur. If both products are soluble NO REACTION will occur (it would be a mixture/solution).

When you use the solubility chart:

Insoluble = solid precipitate = (s)

Soluble = aqueous solution = (aq)

Examples: NaCl + LiOH (

Na2CO3 + CoCl2 (

Oxidation – Reduction or Redox

Any reaction in which electrons are transferred. Look up the oxidation number for all elements in the reaction on the Rules for Assigning Oxidation Numbers chart. If the oxidation numbers for all of the elements in the reaction stay the same it is NOT a redox reaction. If the oxidation number of an element changes (look at reactant then product side to see if it changed) then it is a redox reaction. All single replacement reactions will be redox.

Example: 2NaCl + F2 ( 2NaF + Cl2

Oxidation Half Reaction: OIL

Reduction Half Reaction: RIG

Determine if the following are redox reactions or not:

Li2CO3 ( Li2O + CO2 3Ca + N2 ( Ca3N2

Reactions Foldable

Physical Property: a substances ability to physically change, describes a characteristic (boiling point, melting point)

Physical Change: chemical composition remains the same (evaporation, condensation, ripping, dissolving)

Chemical Property: a substances ability to change into a new/different substance (iron has the ability to rust)

Chemical Change/Reactions: chemical composition changes, a NEW substance forms (wood burning, iron rusting)

Types of Chemical Reactions

Synthesis A + B ( AB

Decomposition AB ( A + B

Combustion CxHy + O2 ( CO2 + H2O

Single Replacement A + BC ( B + AC

Precipitation (Double Replacement) AB + CD ( AD(s) + CB

Acid-Base (Double Replacement) AB + CD ( H2O + CB

Oxidation-reduction

Synthesis

A + B ( AB

Special Trends:

When Cu, Fe, Sn, Pb bond with F, O, N use higher charge

(Cu2+, Fe3+, Sn4+, Pb4+) Ask yourself are they having FON?

If bonded to any other nonmetal use lower charge

(Cu1+, Fe2+, Sn2+, Pb2+)

Examples: Ca + N2 (

Cu + F2 (

Decomposition

AB ( A + B

Special Trends:

(ClO3)1- Cl1-

Metal Chlorate ( Metal Chloride + O2

Mg(ClO3)2 ( MgCl2 + 3O2

(CO3)2- O2-

Metal Carbonate ( Metal Oxide + CO2

Li2CO3 ( Li2O + CO2

(OH)1- O2-

Metal Hydroxide ( Metal Oxide + H2O

2NaOH ( Na2O + H2O

Metal Oxide ( will decompose when heated if metal is “heavy”

“heavy”” metals = silver and greater

CaO + heat ( no reaction because calcium is not a heavy metal

2BaO + heat ( 2Ba + O2

Examples: NaClO3 (

MgCO3 (

Ca(OH)2 (

MgO + heat (

RaO + heat (

Combustion (any reaction with O2 as a reactant)

CxHy + O2 ( CO2 + H2O

Examples: C2H2 + O2 (

C4H10 + O2 (

Single Replacement (occur in a solution)

A + BC ( B + AC

Use activity series to determine if reaction will occur. In order for reaction to occur the single element (on reactant side) must be HIGHER on the activity series then the element in the compound it is trying to replace.

Examples: K + MgO (

Ag + CaSO4 (

F2 + NaCl (

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ACTIVITY SERIES:

Nonmetals

F2

Cl2

Br2

I2

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