This document provides a review for a chemistry final exam. It lists 27 topics that will be covered on the exam, with 70% of the exam focusing on material after the third partial. It also includes 7 practice problems covering various chemistry concepts like electron configurations, chemical reactions, stoichiometry, concentrations, and redox reactions. Students are advised to study their notes and practice problems in preparation for the comprehensive final exam.

1. November 23rd, 2011
Final Exam Review
This is the review for the final exam. It by no means intends to depict
the exam’s format, and it is NOT everything you need to know for the
final exam. This review is intended to help you have more chemistry
practice. Below I have written the topics we have covered this
semester (I may have missed some, but you SHOULD have all of
them in your notes!The old reviews should help you study as well.
Make sure you go over your notes and homework. Do not wait until
the day before the exam to study, begin now!
70 percent of the exam will be based on the material covered after
third partial.
10 percent will come from first partial.
10 percent will come from second partial.
10 percent will come from third partial.
For a total of 100 percent
1. Introduction to chemistry: definition of chemistry
2. Matter
3. Substance
4. Mass vs. Weight
5. Conversions (SI Units and English Units)
6. Properties and changes of matter (physical and chemical…
include states of matter)
7. Elements name and symbol of common elements
8. Methods of separating mixtures
9. Types of mixtures
10. The atom and the atomic model
11. Atomic structure (composition, atomic mass, atomic number,
average atomic mass)
12. Ions
13. Isotopes
14. Atomic models
15. Ground vs. Excited State
16. Quantum numbers
17. Electron configurations
18. Periodic Table and periodic trends
19. Types of bonds
20. Types of inorganic compounds

2. November 23rd, 2011
Final Exam Review
21. Types of reactions
22. Nomenclature
23. Oxidation Numbers
24. Balancing (This will include Redox)
25. Stoichiometry
26. Ideal Gas Law
27. Solutions
28. Concentrations
29. pH
Solve the following problems:
1. Draw the orbital diagram, the electron configuration, electron dot notation, and
the noble notation of the following elements. Then find the four quantum numbers
for the given electron.
a. Re (hint this element goes through the f-orbitals): 30th electron
b. Cd: 14th electron
c. Ra: 83rd electron
d. In: 36th electron
2. Differentiate between chemical and physical property and change, give
examples of each.
3.Give the names of the following compounds and find the oxidation numbers.
a. Ca(C2H3O2)2
b. NO2
c. SiF4
d. VCl5
4. Complete the following reactions, state the type of reaction and balance where
necessary, identify the type of inorganic compound:
a. K(s) + Cl2(g)
b. H2CO3
c. MCO3
d. Fe(s) + CuSO4(aq) 
e. AgNO3(aq) + KCl(aq)
f. HCl (aq) + NaOH (aq) 
g. HBr (aq) + Ba(OH)2 (aq)

3. November 23rd, 2011
Final Exam Review
5. Stoichiometry
a. Ethanol, also known as grain, can be made from the
fermentation of sugar (C6H12O6). The unbalanced chemical equation for the
reaction is shown below.
C6H12O6 C2H5OH + CO2
Balance the chemical equation and determine the mass of C2H5OH produced
from 750 g of C6H12O6.
b. Hydrofluoric acid solutions cannot be stored in glass containers
because HF reacts readily with silica dioxide in glass to produce hexafluorosilicic
acid (H2SiF6). 40.0g SiO2 and 40.0g HF react to yield 45.8 g H2SiF6.
SiO2 (s) + 6HF (aq)  H2SiF6 (aq) + 2H2O (l)
I. What is the limiting reactant?
II. What is the mass of the excess reactant?
III. What is the theoretical yield of H2SiF6?
IV. What is the percent yield?
c. This problem is a challenge problem, harder than the ones we
have done before… but not so hard as to where you cannot answer it. Read the
problem carefully!
Phosphorus (P4) is commercially prepared by heating a mixture of calcium
phosphate (Ca3(PO4)2), sand (SiO2), and coke (C) in an electric furnace. The
process involves two reactions.
2Ca3(PO4)2 (s) + 6SiO2 (s) 6CaSiO3 (l) + P4O10 (g)
P4O10 (g) + 10C (s)  P4 + 10CO (g)
The P4O10 produced in the first reaction reacts with an excess of coke (C) in the
second reaction. Determine the theoretical yield P4if 250.0 g of Ca3(PO4)2and
400.0 g of SiO2are heated. If the actual yield of P4 is 45.0g, determine the
percent yield of P4.

4. November 23rd, 2011
Final Exam Review
6. Concentrations
a. What mass of NaOH is in 250 mL of a 3.OM NaOH solution?
b. How many milliliters of a 5.0 M H2SO4 stock solution would you
need to prepare 100.0mL of 0.15M H2SO4?
c. What is the molality of a solution that contains 75.3 g of KCl
dissolved in 95.0 g of water?
d. How many grams of Na2CO3 must be dissolved into 155 g of
water to create a solution with a molality of 8.20 mol/kg?
e. This is also a challenge problem. Hint fin the moles and then
use stoichiometry to solve for the rest of it… What volume of
ethanol (C2H3OH) is in a 100.0 mL of 0.15 M solution? The
density of ethanol is 0.7893 g/mL.
7. Balance the following equations using redox
a. Identify each of the following as either oxidation or reduction.
1. I2 + e- 2I- 2. Fe2+Fe3+ + e-
3. K  K+ + e- 4. Ag+ +e- Ag
b. Identify what is being oxidized and what is being reduced
i. 2Br- + Cl2  Br2 + Cl-
ii. 2Zn + O2 2ZnO
iii. 2Na + 2H+ 2Na+ + H2
c. Balance the following reactions using Redox:
i. Fe + CuSO4 FeSO4 + Cu
ii. Fe + HBr H2 + FeBr3