1.Group IA and ammonium compounds are_____.

2.All nitrate, chlorate, perchlorate & acetate salts are___.

3.All chloride, bromide, & iodide salts are soluble except___.

4.All sulfate compunds are soluble except____.

5.All hydroxide compounds are insoluble except____.

6.All sulfide compounds are insoluble except____.

7.All sulfites, carbonates, chromates, & phosphates are insoluble except____.

1.soluble

2.soluble

3.Ag+,Pb+2,Hg2+2

4.Ba+2, Sr+2, Ca+2, Pb+2, Hg2+2

5.Group IA, Ba+2, Sr+2, Ca+2,

6.Group IA & IIA

7.NH4+, Group IA

Molecular Formula & Empirical Formula

ex: A combustion ananlysis gives the following mass%

H=9.15  C=54.53  O=36.32. Molecular mass=132.16

Empirical formula=C2H4O

Steps

Convert percent>grams>moles

Divide each amount of moles by the lowest,and multiply to receive whole numbers.

ex:(9.15 g H)/(1mol/1 g) = 9.15 mol

(54.53 g C)/(1 mol/12 g) = 4.54 mol

(36.32 g O)/(1 mol/16 g) = 2.27 mol

then,

2.27/2.27=1  9.15/2.27=4   4.54/2.27=2

2*12.0 + 4*1.0 + 1*16.0 = 44

1.Combustion

2.Synthesis

3.Decomposition

4.Single Displacement

5.Double Displacement

6.Acid-Base

1.Oxygen and another compound to form H20 and CO2.

C₁₀H₈ + 12 O₂ ---> 10 CO₂ + 4 H₂O

2. Two or more simple compounds combine to form a more complex one.

A + B ---> AB      

8 Fe + S₈ ---> 8 FeS

3.A complex molecule breaks down to simpler ones.

AB ---> A + B

2 H₂O ---> 2 H₂ + O₂

4.One element trades place with another in a compound.

A + BC ---> AC + B

Mg + 2 H₂O ---> Mg(OH)₂ + H₂

5. One element trades place with another element in a compound.

AB + CD ---> AD + CB

Pb(NO₃)₂ + 2 KI ---> PbI₂ + 2 KNO₃

6.Acid reacts with a base forming water.

HA + BOH ---> H₂O + BA

HBr + NaOH ---> NaBr + H₂O

Measure of each individual element within the compound.

ex:The percent composition of carbon in CO2.

find molar mass of carbon dioxide>divide the mass of carbon by molar mass of carbon dioxide>multiply by 100

12.01+2(16)=44.01g/mol

(12.01/44.01)=.2729*100=27.29%

Stoichiometry Calculations

1.Limiting Reactants

2.Percent Composition

3.Empirical and Molecular Formula

4.Density

5.Concentrations of solutions(molarity)

1. Used to determine how much reactant you need to react with the other.

2.Used to determine the how much of each element is within the compound.

3.Used to determine the number of atoms in a compound.

4.d=(m/v)

5.M=(moles of solute/Liters of solution)

1.Limiting Reactant

2.Percent Yield

3.Avogadro’s Hypothesis

1.First write a balanced equation for the reaction.

Next, calculate how much product is produced by each reactant.Then, to find the amount of excess reactant.The reactant that produces the lesser amount of product is the "limiting reactant."To find the amount of excess reactant remaining, subtract the amount that reacted from the amount in the original sample.

2.(Actual yield/predicted yield)*100

3.The Volume of a gas is directly proportional to the moles of the gas, n at constant P and T.