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Final Exam Study Guide
CP Chemistry
Math:
1. Know significant figure rules.
2. How many sig figs are in the following
a. 6005
b. 8.7300
c. 14.000
d. 0.00038098
3. Convert the following into scientific notation
a. 1,500,000
b. .000336
4. Round these numbers to 4 significant digits
a. 48.275687
b. 123.456
c. 0.00637893
d. 12.56157
5. What are the rules for using significant digits while adding/subtracting? While
multiplying/dividing?
6. Convert 675mL into L.
The Atom
1. What are the 3 subatomic particles, their charge and location within the atom?
2. Given the mass # and protons, explain how to find the element, atomic #, neutrons
and electrons.
3. What is an isotope?
4. What is an ion? What are the 2 different types of ions and how do they form?
5. What is Dalton’s atomic theory? Explain what 2 things are wrong with it.
Average Atomic Mass
1. What is the difference between average atomic mass and mass #
2. What is the avg. atomic mass for the following
a. C-14 at 1.36%
b. C-13 at 2.62%
c. C-12 at 96.02%
Nuclear Chemistry
1. What causes radioactivity?
2. What are the 3 types of radiation? What is the charge of each type?
3. What changes during Beta radiation?
4. What does a radioactive elements half-life refer to?
5. What is this half-life utilized in?
6. What is the main difference between fission and fusion?
7. Where is fission utilized?
8. Where is fusion utilized?
9. Write the nuclear equation for the alpha decay of polonium-218.
10. Write the nuclear equation for the beta decay of Carbon-14.
Electrons
1. Write the complete electron configuration and orbital diagram for Chlorine.
2. 2p² Tell what each part of this configuration represents.
3. How does energy level relate to distance?
4. Write the Noble gas configuration for Selenium.
5. Give 2 examples of atoms which will gain 2 electrons to become stable.
6. Give 2 examples of atoms which will lose 2 electrons to become stable.
7. What element is this (Kr)5s²4d³
8. What are valence electrons?
9. What are the different electron orbitals and their shape?
10. How many electrons can occupy each orbital?
Periodicity
Development of the Modern Periodic Table
1. Who is the father of the periodic table? How did this scientist arrange his table?
2. What characteristic about his periodic table made it so widely accepted?
3. Which scientist corrected the original periodic table and how did he change it?
4. What is periodic trend?
5. Explain how the periodic table is arranged in groups, families, and periods.
6. What are the 3 families of metals?
7. What are the last 2 families of nonmetals? Explain how reactive each family is
and why.
8. Which elements have characteristics of both metals and nonmetals? Give 2
examples.
9. Which group of metals and nonmetals are the most reactive? Explain your
answer.
Classification of elements
1. How do periods correspond to valence electrons for representative elements?
2. How does an elements group correspond to the number of valence electrons?
3. What are the 4 blocks of elements? Where can they be located on the periodic
table?
4. Why do atoms in the same group have similar chemical properties?
5. Alkali Metals and Alkaline Earth Metals represent which block?
6. Why does the s block only span 2 groups?
7. What are the properties of metals?
Periodic Trends
1. Give the definition of Atomic Radius (how is it found), Ionization Energy and
Electronegativity.
2. Draw an outline of the periodic table and label it with arrows representing the
trends for each of the above.
3. Explain Ionic radii.
4.
5.
6.
7.
What element on the periodic table has the highest electronegativity?
What is the shielding effect?
How does the shielding effect relate to periodicity?
What is the octet rule? How does it apply to periodicity?
Bonding, Naming, VSEPR
1. What makes a covalent bond? What makes an ionic bond?
2. What happens with the electrons in an ionic and covalent bond?
3. Why do atoms bond?
4. In a chemical formula what do the symbols and numbers represent?
5. What is a molecule? Is CO2 a molecule? Is NaCl a molecule?
6. What is an elements oxidation number(s)?
7. What rule does bonding (typically) fulfill to create stability?
8. Ionic compounds form what type of structure?
9. Metallic, Covalent, and Ionic bonds have what properties?
10. What are the 3 types of intermolecular forces from strongest to weakest?
11. Give an example of a molecule for each of the above.
12. What is polarity? How does it create surface tension in water?
13. What is a hydrogen bond?
Naming
14. Naming ionic and covalent compounds. Be able to name from formula to
compound and compound to formula.
a. P2O5
b. Ti(SO4)2
c. manganese (II) phosphate
d. Tetraphosphorus decoxide
15. Naming of acids. Be able to name from formula to compound and compound to
formula.
16. Write out the rules for naming an ionic compound? How do you know its ionic?
17. Write out the rules for naming a covalent compound? How do you know its
covalent?
18. Write out the rules for naming acids? What makes something an acid?
VSEPR (molecular shape)
19. What does VSEPR stand for?
20. Be able to draw Lewis structures to determine molecular shape?
a. CCl4
b. Sulfur Dioxide
c. COCl2
21. What are the 5 basic molecular shapes (made of all bonds no lone pairs)?
22. What are the shapes and bond angles according to VSEPR through the
tetrahedrons?
23. What two things are considered areas of high electron density in VSEPR?
24. What takes up more space a lone pair or a bond? Explain how we know? (think
bond angles)
Reaction Chemistry
Reaction Basics
1. Write a reaction labeling the reactant side and product side.
2. What are the 4 signs to a chemical reaction having occurred?
3. What are the 4 physical states with which your reactants and products can be in?
4. What does aqueous mean?
5. What is a precipitate?
6. Write a chemical equation showing heat was added to the reactants.
7. What are the 7 diatomic molecules?
8. What does it mean to be diatomic? Write out Oxygen gas.
Writing Equations
1. Individual atom is called?
2. Covalent compound is called?
3. Ionic compound is called?
4. What do coefficients represent?
5. Write out the equation for the sentence below.
a. Two atoms of aluminum react with three units of aqueous copper(II)
chloride to produce three atoms of copper and two units of aqueous
aluminum chloride.
6. Write out the sentence for the equation below.
a. Zn(s) + 2HCl(aq)  ZnCl2(aq) + H2(g)
7. How many atoms of each element are there in the following? (CH4)3
Balancing Equations
1. Why must we balance chemical equations?
2. By balancing an equation what are you making equal on each side?
3. Write out the steps to balancing an equation.
4. Balance the following: KOH + Co3(PO4)2  K3PO4 + Co(OH)2
6 Types of Reactions
1. What are the 6 types of chemical reactions studied?
2. Give a brief explanation as to what happens in each type of reaction.
3. Give a brief explanation how to recognize each type by its reactants.
4. What makes an acid an acid? What makes a base a base?
5. Identify chemical reaction types and balance.
a. ____ NaBr + ____ Ca(OH)2  ___ CaBr2 + ____ NaOH
b. ____ C5H9O + ____ O2  ____ CO2 + ____ H2O
c. ____ Pb + ____ H3PO4  ____ H2 + ____ Pb3(PO4)2
6. Predict Products, Identify Reaction, Balance
a. ____ Na + ____ FeBr3 
b. ____ C2H4O2 + ____ O2 
c. ____MnO2 + ____ Sn(OH)4 
The Mole and Stoichiometry
1. What is the molar mass of H2SO4?
2. Be able to do molar conversions.
a.
Convert 4g CH4 into moles.
b.
Convert 0.25 moles of Silver to particles.
c.
Convert 16g of NaCl into particles.
3. What is the % composition by mass of FeCl3?
4. Determine the empirical formula of Ibuprofen given that the percentages of its
components by mass are:
C = 75.7%
H = 8.8%
O = 15.5%
5. What is the molecular formula for Ibuprofen (from above) if it has a molar mass
of 412.62 g/mol?
6. What is an empirical and molecular formula?
7. What is molarity?
8. 4Au(s) + 8NaCN(aq) + O2(g) +H2O(l)  4NaAu(CN)2(aq) + 4NaOH(aq)
Determine the mass of gold if 17.0g Sodium cyanide is used.
9. An Alkaline battery produces electrical energy according to this equation.
Zn(s) + 2MnO2(s) + H2O(l)  Zn(OH)2(s) + Mn2O3(s)
Determine the limiting and excess reactants if 25.0g Zn and 30.0 g MnO2 are used
to produce Zn(OH)2.
10. Calculate % yield from the above problem.
Gas Laws
1. How many liters of a gas are in one mole?
2. Write out Boyle’s Law, Charles’ Law, and Gay-Lussac’s Law.
3. Some students believe that teachers are full of hot air. If Mr. C inhales 2.2 liters
of gas at a temperature of 180 C and it heats to a temperature of 380 C in his lungs,
what is the new volume of the gas?
4. What is the combined gas law?
5. A gas has a volume of 400.0 mL at 3.00 °C and 120.0 torr. What would the
volume of the gas be at 117.0 °C and 3350.0 torr of pressure?
6. What is Henry’s Law?
7. What is the ideal gas law?
8. If I have an unknown quantity of gas held at a temperature of 1195 K in a
container with a volume of 25 liters and a pressure of 560 atm, how many moles
of gas do I have?