Download Pre-AP Chemistry Final Exam Review 1. Write the name for

Pre-AP Chemistry Final Exam Review
1. Write the name for the following compounds.
a) Fe2O3
h) H2S
i) FeCrO4
b) HCl
c)Mg(NO3)2
j) K2S
d) NaOH
k) PCl3
e) H3PO5
l) H2SO3
f) As2O5
m)
KClO4
g) N2O3
2. Write the formula from the following names.
a) Ammonium hydroxide
g) Lithium nitrate
b) Chlorous acid
h) Calcium nitrite
c) Potassium chlorate
i) Chromous acid
d) Acetic acid
j) Copper (II) sulfate
e) Sodium iodide
k) Dinitrogen pentoxide
f) Hydrophosphic acid
l) Hyposulfurous acid
NAMES & FORMULAS
□Be able to name and write formulas for ionic
and covalent compounds.
□Know how to determine an ion’s charge from
the periodic table.
Group 1 = 1+
Group 2 = 2+
Group 16 (Oxygen group) = 2Group 17 (Halogens) = 1Aluminum = 3+
Zinc = 2+
Silver = 1+
□Remember to use roman numbers in ionic
compound names when necessary. The
roman number is the cation’s charge – it is
NOT the number of cations.
□Be able to write the names of formulas of
acids
Binary: hydro – nonmetal root –ic acid
Polys ending in –ate: -ic acid
Polys ending in –ite: -ous acid
m)Nitrogen monoxide
n) Copper (I) bromide
o) Nitric acid
-------------------------------------------------------------------------------------------------------------------------------------------------1. Find the molar mass for calcium acetate.
2. For sodium sulfate, calculate the percent composition of each element.
3. How many moles are in 30g of NaCl?
4. How many formula units are in 3.00 moles of KCl?
THE MOLE
□ Define a mole and describe what it tells about
a substance.
□Be able to determine the molar mass of a
substance
□Be able to determine the percent composition
by mass of elements in compound or hydrate.
5. How many grams are there in 3.4 x 1024 molecules
of NH3?
□Be able to convert between units using the
following conversion factors:
1 mole = molar mass in grams = 6.022 x 1023
particles = 22.4 L of a gas at STP
□Be able to define and calculate empirical and
molecular formulas.
6. What is the empirical formula for a compound which
contains 67.1% zinc and the rest is oxygen?
□Be able to define and calculate the formula for
a hydrate.
7. If the empirical formula of a compound is CH and the molecular mass is 78.12g/mol, what is the molecular
formula?
8. How much would 100 L of water vapor weigh in grams at STP?
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CHEMICAL REACTIONS
□Know how to identify the five types of chemical reactions.
a. Synthesis or Combination: A + B  AB (element + element = compound)
b. Decomposition: AB  A + B (compound = element + element)
c. Single Replacement (element + compound = element + compound)
A + BC  AC + B
(if A is a cation) or
A + BC  BA + C
(if A is a anion)
d. Double Replacement: AB + CD  AD + CB (compound + compound = compound + compound)
e. Combustion: CxHy + O2  CO2 + H2O (Looks like a single replacement but the reactants are a hydrocarbon and
O2 and the products are CO2 and H2O.)
Balance the following equations and identify the
type of reaction.
Ca 
1.
NaCl +
2.
Sn(CO3)2 +
3.
NaOH + AlPO4  Na3PO4 + Al(OH)3
4.
FeO +
5.
Al2O3 +
6.
C2H4 +
7.
Na +
CaCl2 +
K
Al 
Na
K2(CO3) + Sn
MgO +
Al
O2  CO2 + H2O
Cl2 
NaCl
Predict the products for the following reactants
(include states of matter) then balance the
equation.
8.
□Know what indicates that a chemical reaction has taken
place: temperature change, color change, formation of a
gas (bubbles), and formation of a precipitant (solid is
formed when two liquids react)
□Know that the reactants are on the left and the products
are on the right.
Al2O3 + Fe
Mg 
CHEMICAL REACTIONS (cont.)
□Know how to predict the products if you’re given the
reactants.
K (s) + F2 (g) 
□Know that single replacement reactions will use either the
metals activity series or the halogen activity series to
predict if the reaction will take place.
□Know how to balance the equation by adding coefficients
until the numbers of atoms are equal on each side.
□Know how to properly use subscripts to count elements.
For example, Al2(SO4)3 means there are 2 Al’s, 3 S’s and 12
O’s.
□Know how to properly use coefficients to count elements.
For example, 3Al2(SO4)3 means there are 6 Al’s, 9 S’s and 36
O’s.
9.
PbCl2 (aq) + Na2CrO4 (aq) 
10.
ZnO (s) + HCl (aq) 
□Know that the following elements are diatomic: H.
Bronclif or Mr. & Mrs. BrINClHOF
11.
C4H10 (l) + O2 (g) 
□Know that a balanced equation is a confirmation of the
law of conservation of mass
12.
C8H18 (l) + O2 (g) 
□Know how to determine the state of matter of room
temperature from the color coding on the periodic table
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STOICHIOMETRY
□Know the steps for solving all stoichiometry
problems.
a. Write a balanced equation. Know that the
coefficients for each compound represent
the ratio of moles in the equation.
b. Convert to moles
c. Set up your mole-mole ratio.
d. Convert to wanted units.
□Know how to calculate the molar mass of a
compound. (Add up the molar mass for each
element. Do not multiply by a coefficient.)
Given the following reaction: H2O2  H2 +
O2 , how many moles of H2 will you make if you
1.
begin with 2.51 moles of H2O2 ?
2. Given the following reaction: 2 ZnS + 3 O2 
2 ZnO + 2 SO2 , how many moles of ZnO will you
make if you begin with 6.82 grams of O2 and
9.23g of zinc sulfide? Identify the limiting and
excess reactants. Determine how much of the
excess reactant remains.
□Know what the Law of Conservation of Mass states:
Matter can be neither created nor destroyed in a
chemical reaction. Therefore, the mass of the
reactants equals the mass of the products. This is
why we can do Stoichiometry.
□Know how to calculate a reaction’s percent yield.
% yield = actual yield/theoretical yield
□Be able to define limiting reactant, excess reactant,
actual yield, theoretical yield
□Be able to solve limiting reactant problems and
determine how much excess remains.
3.
In the following reaction: H2CO3 (aq) + 2 Na
(s)  Na2CO3 (aq) + H2 (g), how many grams of
Na are need to make 5.0 grams of H2 ?
4. Given the following reaction: 2 ZnS + 3 O2 2 ZnO + 2 SO2 , how many moles of ZnO will you make if
you begin with 55.75 grams of O2 ?
5. A 5.95 g sample of silver nitrate is reacted with an excess of barium chloride to form 4.00 grams of silver
chloride and another product. What is the percent yield of silver chloride?
--------------------------------------------------------------------------------------------------------------------------------------------------------------------------------
1. If the pressure of a gas changes from 4.5
atm to 3.75 atm, what was the original
volume if the final volume was 7.55 L?
2. A gas at 30 oC and 3.4 atm pressure is put
under a pressure of 3.0 atm. What is the
new temperature?
3. Two gases with the pressure of 1.5 atm
each are placed into a gas tank. What is
the total pressure in the tank?
4. A gas at STP occupies 2.5 L. What volume
will it occupy if the temperature is
changed to 300 K and the pressure
changes to 1.25 atm?
GAS LAWS
□Know how to use the Gas Laws. The Gas Laws will be
given to you.
□Know how inverse relationships work. (If one part is
increased 5 times, the other part will decrease to 1/5.)
Ex. Pressure vs. volume
□Know how direct relationships work. (If one part is
increased 5 times, the other part will increase 5 times.)
Ex. Pressure vs. Temp and Volume vs. Temp
□Know that STP is standard temperature and pressure.
Standard temperature is 0 C and standard pressure is 1
atmosphere.
□Know Avogadro’s principle – conceptually and
mathematically.
□Know how to convert moles of a gas to liters or liters to
moles using 22.4 L/1 mole.
□Be able to solve gas stoichiometry problems at STP and
non-STP conditions.
□Know that pressure is caused by the number of particles
hitting the sides of a container. Know what can change
the pressure within a container.
5. Given the following reaction: 2 ZnS + 3
O2  2 ZnO + 2 SO2 , how many liters of
O2 are produced at 315 K and 735 torr if
you begin with 55.75 grams of ZnS?
□Know how to convert oC to K or K to oC.
□Know that all gas law problems are solved using the
Kelvin temperature scale.
□Be able to define diffusion vs. effusion
□Know the postulates of the kinetic molecular theory
6. In the following reaction: H2CO3 (aq) + 2
Na (s)  Na2CO3 (aq) + H2 (g), how many
liters of hyrdrogen gas are produced at
STP if you make 12.45 moles of Na2CO3?
□Be able to compare the properties and particle
behaviors of solids, liquids, and gases.
□Know the difference between real and ideal gases.
□Know the variations of the ideal gas law.
□Know the relationship between molar mass and rate of
diffusion/effusion.
7. Calculate the density of hydrogen gas at
STP.
8. Which of the following gases would have the greatest rate of effusion? Justify your answer. H2, O2,
NH3, CH4
SOLUTIONS
□Know that solutions are made up of two parts – the solvent and the solute.
□The solvent is usually water and it makes up the majority of the solution.
□The solute is what is being dissolved and it makes up the smaller portion of the solution.
□Be able to describe the trends in solubility as temperature increases for a solid in water and a gas in water.
□Know how to interpret a Solubility Graph and determine if a solution is supersaturated, unsaturated, or
saturated.
□Define and describe the differences between a saturated, unsaturated, and supersaturated solution.
□Know how to speed up the dissolving of a solute.
□Know what it means to dilute a solution and how to calculate it.
Grams of Solute Dissolved
Solubility (grams of solute/100 g of water)
300
250
KNO3
200
NaNO3
150
LiCl
100
KCl
50
0
0
20
40
60
80
100
o
Temperature ( C)
1. How many grams are needed to make a saturated
solution of KNO3 at 50oC?
2. If 100 grams of LiCl is dissolved at 90oC, how many
additional grams must be added to make a
saturated solution?
3. At 60oC, what type of solution will you have if 70
grams of KCl are dissolved in 100 g of water?
SOLUTIONS (cont.)
□Know that “like dissolves like” which means polar
substances will dissolve polar substances and nonpolar substances will dissolve non-polar substances.
They will not dissolve each other.
□Know that we measure a solution’s concentration by
measuring the number of moles dissolved in 1 L.
(molarity)
□Know how to determine molarity when given moles
and volume or when given grams and volume
□Know how to determine volume when given moles
and molarity.
□Know how to determine moles when given volume
and molarity.
□Be able to define an electrolyte
□Be able to use your solubility rules and determine
precipitates
□Be able to write net ionic equations
4. If 100 grams of NaNO3 are dissolved in 100 grams of water, what must the temperature be to make it a
saturated solution?
5. Which compound is more soluble at 80oC – LiCl or NaNO3 ?
6. Write the molecular and net ionic equations for the following reactions between aqueous solutions:
a. barium chloride and silver nitrate
b. calcium acetate and sodium carbonate
c. potassium chloride and lead(II) acetate
7. Calculate the molarity of a solution of sodium carbonate if 2.35g are dissolved in enough water to
make 1.2L of solution.
8. How many grams are needed to prepare 25.2mL of a 0.3M solution of aluminum oxide?
9. Which of the following would most likely dissolve in water? Justify your answer. Carbon tetrafluoride,
hydrofluoric acid, ammonia (NH3).
10. Which of the following would most likely conduct electricity in solution? Justify your answer. Carbon
tetrafluoride or sodium bicarbonate.
-------------------------------------------------------------------------------------------------------------------------------------------------1. Determine the Lewis structure, polarity, and the
dominant IMF of the following:
IMFs & REDOX
a) CO2
□Be able to determine the polarity of a
substance based on its Lewis Dot Structure
b) H2O
□Be able to determine the dominant
intermolecular force present in a substance
based on its Lewis Dot Structure
c) HCN
□Be able to assign oxidation numbers and
determine if a substance is oxidized or reduced
in a reaction
2. Rank the following by from lowest to highest anticipated boiling point and tell why you put them in that
order: PCl3, CH4, Ne, NH3.
3. Assign oxidation numbers to each atom in the following compounds:
a) NaCl
b) HNO3
c) CaCO3
d) PO43-
4. In the following reactions, assign oxidation numbers to each atom and determine which ones are oxidized
and reduced:
Sn(CO3)2 + K → K2(CO3) + Sn
Al2O3 + Mg → MgO + Al
Na + Cl → NaCl
-------------------------------------------------------------------------------------------------------------------------------------------------1. Determine the pH of a 0.2M solution of hydrochloric
Acids and Bases
acid?
□Be able to list and define the six strong acids.
□Know how to calculate the pH, hydronium ion
concentration, hydroxide concentration, and
pOH.
□Be able to determine if a substance is acidic or
basic based on ion concentrations and pH.
2. Determine the hydroxide concentration in a:
0.5M solution of hydrochloric acid?
□Be able to describe the properties how they
affect litmus paper, their taste, pH range.
□Define a neutralization reaction and determine
the products in these reactions
0.5M solution of potassium hydroxide?
□Describe a titration experiment and be able to
solve for unknown molarities.
□Define and Arrhenius and Bronsted-Lowry acid
and base.
3. What makes an acid/base strong versus weak?
□Be able to determine the conjugate acid and
conjugate base of a reaction.
4. What is the hydroxide ion concentration of a solution if the pH is 5.36?
5. What is the concentration of a hydrochloric acid solution if 3.5mL are needed to neutralize 7.6mL of 0.25M
sodium hydroxide?
6. Write the Bronsted-Lowry reaction between ammonia and sulfuric acid. Label the acid, base, and their
conjugates.
Identify the conjugate base of:
7.
H2O ____________________
9.
HClO4 ___________________
8.
HNO2 ___________________
10.
NH4+1 ____________________
Identify the conjugate acid of:
11.
HCO3-1 _____________________
13.
HPO4-2 _____________________
12.
HS-1 ______________________
14.
H2BO3-1 ____________________
--------------------------------------------------------------------------------------------------------------------------------------1. What is the specific heat of a substance that absorbs
Thermochemistry
25J of heat and has a change in temperature from 20C
□Be able to describe the difference between
to 26C?
an exothermic and endothermic process by
definition and through a potential energy
diagram.
2. Sketch a potential energy diagram for an endothermic
reaction. Label the activation energy, reactants, and
products
□Be able to label the following on a potential
energy diagram: reactants, activation energy,
and products
□Be able to calculate specific heat of
substances
□Be able to define specific heat of a substance
□Be able to use calorimetry to calculate for
the specific heat of a substance involved in a
heat transfer
□Be able to sketch and label a heating curve.
3. Sketch and label the states of matter and phase changes in the heating curve of converting ice to
steam.
4. What is the final temperature of iron if 3.2g of it is heated to 100.0C and dropped into 22.3g of water
at 21.2C. (Ciron=0.448J/g C) (CH2O=4.184J/g C)
Formulas and Constants for the Exam

Purple periodic table (some polys, activity series, solubility rules)

Blue Formula Sheet

1 mole = 22.4 L of a gas at STP = 6.022 x 1023 particles = molar mass in grams

% yield = actual yield/theoretical yield

Gases
o
o
o
o
o
PV = nRT
P1V1/T1 = P2V2/T2
Ptotal = P1 + P2 + P3 + …
Standard Pressure = 1 atm = 760 torr = 760 mmHg = 101.3 kPa
Standard Temperature = 0°C = 273 K

Solutions
o Molarity = moles solute/liters of solution
o M 1V 1 = M 2V 2

Acids/Bases
o pH = -log [H+]
o pOH = -log [OH-]
o pH + pOH = 14
o [H+] = antilog –pH
o [OH-] = antilog –pOH
o Kw = [H+][OH-]
o Kw = 1.0 x 10-14 M2
o MAVA#H = MBVB#OH

Thermochemistry
o Q = mcΔT
o Q = mLv
o Q = mLf
o Any specific heat will be given unless you’re solving for it.