CHEMICAL REACTIONS

How can we determine if a reaction will occur? What are the different types of reactions?

How can we predict the products of a reaction?

What are solubility rules?

Will a reaction occur? If a solid is formed (a precipitate) If water is formed If a gas is formed If electrons are transferred

Then it is likely that a chemical reaction took place. Also, if a new odor is produced, a new color is

produced, or a change in energy (temperature, light, sound) occurs it is likely that a reaction occurred.

Types of Chemical Reactions Double Displacement (Precipitation Rxn) Combustion Single Replacement Synthesis Decomposition Redox ( reactions involving electron transfer) Acid-Base Reactions

Your Book Classifies as: Precipitation (Double Replacement) Oxidation Reduction or Redox (Combustion,

Synthesis, Single Replacement, & Decomposition

Acid-Base

Predicting products of Double Replacement Reactions If a solid forms from the combining of two

aqueous solutions, a reaction has occurred. To determine what the solid is, we must know

solubility rules. These are rules that indicate which ionic

compounds are soluble in water and which ones are not.

Solubility Rules for Ionic Compounds Compounds containing the following ions are

generally soluble in water: Alkali metal ions and ammonium ions Acetate ions Nitrate ions Halide ions F-, Cl-, Br-, and I- (EXCEPT those

containing Ag+, Hg22+,, and Pb2+ )

Solubility Continued Sulfate ions (EXCEPT Ca2+, Sr2+ , Ba2+, Ag+,

Hg2+, and Pb2+) The following are also soluble in water Strong acids (HCl, HBr, HNO3, H2SO4,

HClO3)

Strong bases (LiOH, NaOH, KOH, Ba(OH)2, Ca(OH)2 )

Some Insoluble Compounds Sulfide, carbonate, and phosphate salts,

EXCEPT the ones previously mentioned Hydroxide compounds EXCEPT the ones

previously mentioned

An Example Sodium carbonate solution is poured into a

calcium nitrate solution. Does a reaction occur? What is the equation if it does?

Does it occur? Look at the two possible products (the

rearranged ions). These are sodium nitrate and calcium carbonate.

Are either of these NOT soluble in water? Calcium carbonate is not soluble in water, so

yes this reaction produces a precipitate (turns cloudy and then settles out).

The Equation Na2CO3 + Ca(NO3)2 2NaNO3 + CaCO3

You Try This One Ammonium hydroxide solution is mixed with

lead (II) phosphate solution. Does a reaction occur? If it does, what is the equation for it?

Six More…(4 of these react) Barium nitrate solution in potassium sulfate solution Silver nitrate solution in sodium bromide solution Sodium nitrate solution is iron (II) acetate solution Iron (III) chloride solution in potassium hydroxide

solution Sodium fluoride solution in sodium sulfate solution Lead (II) nitrate solution in potassium sulfate

solution

Predicting Products of Combustion Always water and carbon dioxide Is a type of redox

Single Replacement ( a type of Redox)

Use a metal activity series to determine if a reaction will occur.

If it will, cations trade places on the product side of the equation.

Ex. Mg + FeCl2 MgCl2 + Fe Magnesium is more reactive than iron, so it

replaces it and forms magnesium chloride

Synthesis ( a type of Redox)

Balance the charges of the reactants to form the product

Example: Mg + Cl2 MgCl2

Decomposition ( a type of Redox)

One reactant breaks into 2 or more products Sometimes the component elements, but not

always. Examples: 2H2O 2H2 + O2

CuCO3 CuO + CO2