2nd Semester Chem
FINAL EXAM GUIDELINE & REVIEW
THE FOLLOWING SERVES AS ONLY A GUIDE
CHEMICAL FORMULAS
1.
What is the overall charge on a chemical formula? __0___
2.
ionic bonds form between:___metals and non-metals____
covalent bonds form between: ____two or more non-metals
3-5 Write the formula for each of the following:
a. sulfur trioxide ____SO3___
 How are chemical equations balanced?
_________Using coefficients________________
c. hydrofluoric acid: __HF__
3. BALANCE CHEMICAL EQUATIONS & TYPES OF RXN
e. nitrous acid: __HNO2_____
f. nickel III carbonate ___Ni2(CO3)3____
g. silver hydroxide __AgOH_____
h. aluminum chromate __Al2(CrO4)3_____
i. iron III oxide ___Fe2O3____
j. barium phosphate __Ba3(PO4)2_____
Write the name for each of the following compounds:
a. N2H4 Dinitrogen tetrahydride____
7.
2. COEFFICIENTS & SUBSCRIPTS
b. tetranitrogen decasulfide ___N4S10____
d. Phosphoric acid: ___H3PO4____
6.
 ___yeilds____________
(l) ______liquid_________
(s) ______solid__________
(g) ________gas_________
(aq) _____aqueous solution_______
∆ _______heat__________
b.
S2F6____Disulfur hexafluoride______
c.
H2SO4___Sulfuric acid________________
d.
HF ___Hydrofluoric acid___________________
e.
HClO2____Chlorous acid___________________
f.
Mn(OH)3__Manganese (III) hydroxide_______
g.
Na2S____Sodium sulfide_________
h.
CaO ___Calcium oxide___________
i.
Sr(NO3)2__Strontium nitrate__________________
j.
Cu3N___Copper(I) nitride________________
Write the ion for nitrate, nitrite, and nitride
___NO3-1 __NO2-1 _N-3
When are parentheses used in formula writing? When you
have a polyatomic ion in the formula and the oxidation
numbers are not the same and when there are more than one
polyatomic ion necessary for stability in the formula.
 What are the 5 types of reactions? (Briefly describe each one.)
a.______Synthesis
b. _____Decompostion______________________
c. ______Single replacement_________________
d. ______Double replacement__________________
e. _______Combustion (complete and incomplete______
 Balance the following reactions and identify the type.
___BaCl2 + __2_NaOH  __2_NaCl + ___Ba(OH)2
Type: ____DR________________________________
__4_Al + __3_O2  _2__Al2O3
Type: ___Synthesis_________________________
__2_KI + ___Br2  __2_KBr + ____ I2
Type: ______SR_____________________________
___CaCO3  ___CaO + ___CO2
Type: ________Decompostion_________________
__2_C2H6 + __7_O2  __4_CO2 + __6_H2O
Type: ____Complete combustion_______________
4. PREDICTING PRODUCTS IN A CHEMICAL EQUATION
 Predict the products of the following reactions, then balance:
a) FeCl2 + K2S  __FeS + 2KCl______________
b) ZnSO4 + SrCl2  ZnCl2 + SrSO4_____________
c) 2AlCl3 + 3 Na2CO3  Al2(CO3)3 + 6NaCl______
d) A combustion rxn involves the rxn of a hydrocarbon and __O2
e) What are the two products of a complete combustion rxn?
____CO2 and H2O___________________________________
f) What are the two products of an incomplete combustion rxn?
_______CO and H2O__________________________________
5. LAW OF CONSERVATION OF MASS
8.
What is the purpose for using Roman numerals? In other
words, why must they by used with certain transition metals?
Certain transition metals form more than one ion and to
separate them from each other Roman numerals are used to
indicate the charge of each form of the metal. Ex. Iron(II) and
Iron(III)
 In a chemical rxn what is true about the mass of the reactants
compared to the mass of the products? __They must be equal.
STOICHIOMETRY
 What is the first thing you must do to an equation before you
begin a stoichiometric calculation? Balance it.
6. FINDING MOLAR MASS
CHEMICAL EQUATION
1. SYMBOLS IN A CHEMICAL REACTION
 What do these symbols mean in a reaction?
 What is the molar mass of Ba3(PO4)2?
_____600.9g________________
 What is the molar mass of O2? _______32.0g______________
7. MOLE RATIOS
 Given: 4Al + 3O2  2Al2O3
a) What is the mole ratio of aluminum to aluminum oxide?
_________2:1_________________________
b) What is the mole ratio of oxygen to aluminum?
________3:4_______________________
8. CONVERT: moles  moles; moles  mass; mass  moles; mass  mass
 Given a chemical rxn: __3_Fe + __4_H2O  __Fe3O4 + 4_H2
a) How many moles of Fe3O4 are produced from 4.1 moles of Fe?
EMPIRICAL & MOLECULAR FORMULA
 What is the empirical formula mass for CH2O?__30.0g_
 Find the empirical formula of a compound contains 40.68 g
carbon, 5.08 g hydrogen, and 54.24 g oxygen.
C2H3O2
1.37 moles
b) If 7.0 mol of H2O is used how many grams if Fe would be
required to react completely with the water?
 If the mass of a molecule with an empirical formula of CH2O is
180.0 g, what is its molecular formula?
294g Fe
Gfm = 180 = 6
Efm
30
MF= C6H12O6
c) If 100 g of water is used in the rxn then how many moles of
Fe3O4 would be produced?
GAS LAWS
1.39 mol
10. CONVERT TEMPERERATURE BETWEEN 0C & KELVIN (K)
d) How many grams of Fe3O4 are produced from the rxn of 400 g
of solid iron?
 What are the values of STP (standard temperature & pressure?
o __273K_________________
o __101.3kPa_____________
 Convert 700C to Kelvin:_343K_________________
554g
11. STATES THREE GAS LAWS
9. LIMITING REACTANTS/THEORETICAL & PERCENT YIELD
b) Charles’s Law: Volume of a gas and its Kelvin temp. are
directly proportional given constant pressure
 Define limiting reactant: _a reactant that limits the amount of
product produced in a chemical reaction.____
_____________________________________________________
 Define theoretical yield: ___maximum amount of product that is
theoretically possible to produce in a chemical reaction_(only
found through calculation
 Given: __2_Al + __6_HCl  __2_AlCl3 + __3_H2
a) If 14.6 g of aluminum reacts with 25.0 g of hydrochloric acid,
how much hydrogen is produced? (SHOW WORK)
59.1 g of HCl is required if you begin with the 14.6g
b) Which one is the limiting reactant: Al or HCl? ____HCl_____
c) Suppose the experiment is run and the actual mass of hydrogen
is found to be 0.593 g. What is the percent yield? 86.4%
PERCENT COMPOSITION
 What is the percent by mass that Hydrogen makes up in water?
11.1%
 What is the percent by mass that Calcium makes up in Calcium
chloride? 36.1%
a) Boyle’s Law: pressure and volume of a fixed mass of gas are
inversely proportional given constant temperature
c) Gay-Lussac’s Law: Pressure and the Kelvin temp of a gas are
directly proportional given a constant volume.
d) According to Charles’s law, what happens to the volume of a
gas if temperature increases? Decreases? Goes up, goes down .
e) According to Boyle’s Law what would happen to the volume of
a gas as pressure decreases? It increases_
f) What would happen to the pressure of a gas in a container when
additional amounts of the same gas are added to the container? It
increases
g) What happens to the pressure of a gas if the container is made
larger? _it decreases_____
h) What happens to the particles of a gas in a container as the
temperature increases? They move faster and collide with more
force
i) At constant temperature, double the volume will __half___ the
pressure.
j) What happens to the air pressure inside the tires of a car when
the car is driven? ____it increases.
k) Define molar volume at STP: _The molar volume of any gas at
standard temperature and pressure is equal to 22.4L_
 Define colloids: __borderline homogenous mixture, will scatter
light, ex. Fog and jello_____
l) Suppose a person sprays perfume in a room. What can the odor
be detected across the room? _diffusion_______________
 Define suspensions:heterogeneous mixture, particles
temporarily suspended, 2 distinct states of matter, scatters light
 If a mixture will settle out, it is a __suspension_____________
 If a mixture will scatter light, it is a colloid or suspension_
 What is the substance dissolved called? _solute___________
APPLYING GAS LAWS & IDEAL GAS LAW
 Define miscible & give one example: two liquids that will
dissolve in each other,ex. Water and alcohol
REMEMBER ALL TEMP. MUST BE IN KELVINS
K = 0C + 273
 Define immiscible & give one example _liquids that do not mix
in one another, ex. Oil and water
12. USE COMBINED GAS LAW FORMULA TO SOLVE THE
FOLLOWING PROBLEMS (show work)
 Explain the terms “Like Dissolves Like” & what is it used to
predict? _polar liquids dissolve other polar liquids, and nonpolar liquids dissolve other non-polar liquids__, used to
determine miscibility.________
a) A 24 L sample of a gas exerts a pressure of 3.0 atm. What
pressure will the gas exert if the volume is changed to 16 L?
4.5 Atm
 A substance who water solution conducts electricity is called:
__An electrolyte_________________________
b) Helium gas in a balloon occupies 2.40 L at 400K. What volume
will it occupy at 300K?
 A substance who water solution does not conduct electricity is
called: a non-electrolyte_____
1.8L
15. MOLARITY (CONCENTRATION) & SOLUBILITY
c) A gas has a pressure of 3.5 atm at 250C. What will the pressure
be at 350C?
 If a solution has a lot of solute and very little solvent, it can be
described as: ___concentrated________________________
3.62 atm
 If a solution has a lot of solvent and very little solute, it can be
describe as: ___diluted_____________________
 Salt & water is an example of which solute-solvent
combination? ______solid in liquid solution_______________
13. USE IDEAL GAS LAW FORMULA TO SOLVE THE FOLLOWING
PROBLEMS (show work)
 Club soda is an example of which solute-solvent combination?
_______gas in a liquid solution_________________
a) A 45.0 L tank contains 7.0 mol of compressed air. If the
pressure inside the tank is 600kPa, what is the temperature of the
compressed air?
 State Henry’s Law: __see below_________________
_____________________________________________________
464K
 At a given temperature, the solubility of a gas in a liquid is
_______________ (directly or inversely) proportional to the
pressure of a gas above the liquid.
b) A large cylinder of He gas has a volume of 25.0 L at 220C and
567kPa. How many moles of He are in such a cylinder?
 What happens to the solubility of a gas in a liquid when you:
o increase temperature? _decreases_____________
o decrease temperature?_increases_________________
5.78 moles
 List three factors that affect the solubility:
________temperature, pressure, and nature of the solute/solvent
_____________________________________________________
c) What volume is occupied by 56.0 g of N2 at STP?
44.8L
SOLUTIONS
14. TERMS & CONCEPTS
 Define solution: a homogeneous mixture with a solute and
solvent with particles too small to be seen and does not scatter
light in the gaseous or liquid form
 A solution of metal is called ___an alloy________

The solubility of a substance is 15 g per 100 g of water.
How many grams of the substance will dissolve in 350 g of
water?
52.5g
MOLARITY & MOLARITY BY DILUTION &
SOLUBILITY CALCULATIONS
16. USING FORMULA FOR MOLARITY TO SOLVE THE FOLLOWING
PROBLEMS. (Show work)
a) What is the molarity of 5.6 moles of NaCl in 525 L of solution?
.01M
b) Calculate the molarity of a solution containing 117 g of NaCl
dissolved in 2500 mL of solution.
.8M
17. USE THE MOLARITY BY DILUTION FORMULA TO ANSWER THE
FOLLOWING QUESTION S (Show work)
a) How much concentrated 12 M HCl is needed to prepare 120
mL of a 2.0 M solution?
V1= 20mL
b) To what volume should 25 mL of 15 M nitric acid to be diluted
to prepare 3.0 M solution?
V2= 125mL
18. USE HENRY’S LAW TO SOLVE THE FOLLOWING QUESTIONS.
a) The solubility of CO in water at 3.5 atm of pressure is 1.25 g/L.
What is the solubility of carbon monoxide at 8.5 atm?(constant T)
S2= 3.04g/L
b) The solubility of a gas in water is 2.6 g/L of 1.0 atm of
pressure. What is the solubility of the same gas at 4.5 atm?
S2= 11.7g/L
SOLUBILITY CURVES
COLLIGATIVE PROPERTIES
 Define colligative properties: _properties of solutions that
depend on particle number and not the substance dissolved in
the solution.
 Name the three colligative properties of solutions: _vapor
pressure lowering, freezing point depression, boiling point
elevation
_____________________________________________________
 How does adding antifreeze to your radiator effect the freezing
point of the solution? __it lowers the freezing
point___________
 ACIDS & BASES
19. PROPERTIES OF ACIDS & BASES
 Describe three characteristics of acids that bases do not have:
___taste sour, pH <7, proton donors, turn litmus red, react with
metals to produce hydrogen gas_______________
 Describe three characteristics of bases that acids do not have:
taste bitter, pH >7, proton acceptors, feel slippery, litmus
blue_______
 What kinds of ions are associated with acids? _H+, H3O+____
 What kinds of ions are associated with bases? __OH-________
 What is the range of acids on the pH scale? __0 - <7________
 What is the range of bases on the pH scale? __>7 -14________
 Identify as an acid, a base, or neutral using the pH scale:
2.5 __A_
7.0 __N___
12.5 __B__
5.0 __A__
 An acid that can donate only one hydrogen ion is called:
______monoprotic______________
 An acid that can donate two hydrogen ions is called:
______diprotic_____________
 What type of acid is found in all citrus fruits? Citric acid____
 What type of acid is found in milk? Lactic acid___________
 What type of acid is found in stomach?_ hydrochloric acid___
 Define binary acid: _contains H+ and a monatomic anion__
 Name the following acids:
o H3PO4 _phosphoric acid_______________
o HBr ___hydrobromic acid___________________
o HNO3 __nitric acid___________________
o H2SO3 _sulfurous acid_______________________
 Write the formula for the following acids:
o Nitrous acid ________HNO2_____________________
o Hydrochloric acid ___HCl___________________
o Sulfuric acid ______H2SO4____________________
20. ACID-BASE INDICATORS
a) Which salt has the greatest solubility at 100C?
_______KI_________
b) Which salt has the least solubility at 100C?
________KClO3__________
c) Which salt shows the least change in solubility from 00C –
1000C? NaCl
d) If 90 g of KNO3 is dissolved in 100 g of water at 600C, the
resulting solution is said to be _____unsaturated____ (saturated,
unsaturated, or supersaturated)
 Define acid-base indicator: _chemical substance that changes
color in the presence of an acid or base. ______
_____________________________________________________
 Complete the following table:
Indicator
Color in Acid
Color in Base
Litmus paper
Red
blue
Phenolphthalein
Colorless/clear
pink
Bromthymol blue
yellow
blue
 Label the following as either (A) acid, (B) base, or (S) salt
__A_ H2SO4
__B_NaOH
__A_H2CO3
__B_KOH
__B_Ca(OH)2
__S_CaS
__A_H2C2H3O2
__S_K2CO3
21. ACID-BASE REACTIONS
 The reaction between an acid and a base is called:
____a neutralization reaction__________________
 What are the two products of acid & base reaction?
____a salt and water____________________
 Complete and balance the following neutralization reactions:
a) Phosphorus acid + Aluminum hydroxide 
H3PO3 + Al(OH)3 → AlPO3 + 3 H2O
b) Carbonic acid + calcium hydroxide 
H2CO3 + Ca(OH)2 → CaCO3 + 2H2O