Mrs. Simpson’s CP/GHP Final Exam
Review
Chapters on final:
 Ch. 10 (mole conversions)
 Ch. 12 (stoichiometry)
 Ch. 14 (gas laws)
 Ch. 5 (electrons in atoms)
Resources for you:
 Ch. 10, 12, 14, and 5 in your textbook
 Tutorials on my website
 Packets for each chapter!
 Chapter tests
Format of final: 100 multiple choice questions. Some will require calculations, so you
will need a calculator. NONE WILL BE LOANED FOR YOUR FINAL. You will receive a
periodic table.
Ch. 10 To-do:
 Recreate a Mole Map, showing conversion factors for mole conversions.
 Know how to calculate the molar mass of any compound.
 Know the values of STP, and the molar volume of any gas at STP.
 Know how to write the correct conversion factor: (units converting TO go in the
numerator)!
Ch. 10 practice:
1.
2.
How many particles are in a mole of a substance?



What is the representative particle of:
An atom?
A molecular compound?
An ionic compound?
3.
Convert 5.3 moles of Fe into atoms of Fe:
4.
Convert 5.60 x 10 24 molecules water into moles water:
5.
Convert 2.5 moles Ca into grams Ca:
6.
Convert 254.5 g NaCl into moles NaCl:
7.
Convert 14.5 mol H2 gas into Liters H2 gas at STP:
8.
Convert 45.0 g CO2 into Liters CO2 at STP:
CH. 12 to-do:
 Know how to write mole ratios for any chemical equation.
 Make sure you can balance chemical equations.
 Review how to set up a stoichiometry problem.
 Review and KNOW the 5 types of chemical reactions (from Ch. 11)
 Know when the activity series of the metals is needed.
Ch. 12 practice:
9.
In the reaction: 2Al + 3CuSO4  3Cu + Al2(SO4)3,
if 5.7 mol Al react with copper(II) sulfate, how many moles of Al2(SO4)3 are formed?
10.
In the reaction: 2Al + 3CuSO4  3Cu + Al2(SO4)3,
if 57.0 g Al2(SO4)3 is produced, how many grams of CuSO4 reacted?
11.
In the reaction: 2Al + 3CuSO4  3Cu + Al2(SO4)3
if 10 g Al and 10 g CuSO4 react, which is the limiting reagent?
12.
If you calculate, using stoichiometry, that 15.0 g of a compound can be produced,
but 12.3 g are actually produced in the lab, what is your percent yield?
Ch. 14 Gas Laws
Ch. 14 To-do:
 Know ALL gas laws, their equations, and how to solve for any variable.
 Know the value of R if P is in kPa
 Be able to convert any unit of pressure into kPa using conversion factors.
Ch. 14 practice:
13.
If 3.2 liters of air at a pressure of 102.0 kPa is pressurized to 204.0kPa, what is
the new volume?
14.
If 34.0 L of gas is heated from 200 K to 400 K, what is the new volume?
15.
2.3 L of gas at STP conditions is compressed to 300.0 kPa and heated to 456 K.
What is the new volume of the gas?
16.
How many moles of gas are found in a 2.50 L container, at STP?
17.
gas?
If the molar mass of the gas in question 16 is 71.0 g/mol, what is the mass of the
18.
How much faster would He gas effuse compared to CO2?
19.
If air is 78% nitrogen, what is the partial pressure of nitrogen in a container of
air that has been pressurized to 250 kPa?
Ch. 5 To-do list:
 Summarize the difference between the quantum mechanical model and the Bohr
model of the atom.
 Know the following equations: c=, E = h, h= 6.63 x 10-34 Js, 1 nm = 10-9 m
 Know the wavelengths of red and violet light.
 Know how to complete orbital filling diagrams and how to write electron
configurations.
 Know Aufbau principle, Hund’s Rule, Pauli Exclusion principle.
 Know principle quantum number, sublevel, orbital.
 Know the accomplishments of : Bohr, Schroedinger, deBroglie, Heisenberg.
Ch. 5 Practice:
20.
Calculate the frequencies of light of 400 nm and 700 nm:
21.
Calculate the energies of both colors of light in the above problem.
22.
Which color of light above is produced by an electron dropping down from the
highest energy level to the lowest energy level?
23.
Write orbital filling diagrams AND electron configurations for:
a)
N
b)
V
c)
As
d)
Mg