Name: ______________________________________________________________Hour:______
Chemistry 2 Final Exam Review
The Mole
1. What is the molar mass of fluorine gas?
2. What is the molar mass of Silicon? What is the mass of one Silicon atom?
3. What is the molar mass of aluminum sulfite?
4. If you had one mole samples of zinc, iron, and copper, what would be the same in each
sample? Different?
5. Using the mole concept, you could find the number of _________ in a given mass of gold
or any element.
Atomic Structure
15
1. Using the symbol 7 N ; how many protons, neutrons, and electrons are in this isotope of
nitrogen?
2. Write the symbol for the isotope of nitrogen which contains one less neutron.
3. Which is a more common isotope of nitrogen? How do you know?
15
4. Could this be an isotope of nitrogen? 8 N Why or why not?
5. a. How many valence electrons do groups 1, 2, 13, 14, 15, 16, 17, and 18 have?
b. What are the oxidation numbers of the elements in these same groups?
c. Draw Lewis dot models of three non-metals in different groups. Do the same for
three metals.
6. How many orbitals does sublevel “s” have? What is the shape?
Name: ______________________________________________________________Hour:______
Chemistry 2 Final Exam Review
7. How many orbitals does sublevel “p” have? How are they oriented around the nucleus?
8. How many neutrons does a chlorine atom have? (In the most common isotope?)
9. How many electrons fit in one orbital?
10. If an orbital is full, describe the spin of each electron. What would these “spin” quantum
numbers be?
11. What is an ion? Give the number of protons, neutrons, and electrons in these:
Mn 3 , N 3 , S2  , Al 3
12. Which elements have no “d” sublevels? Where in the periodic table to “d” sublevels
begin to fill?
13. If an element if found to have a mass of 51 amu and 22 protons, which element would it
be?
14. If an element has an atomic number of 38, what is the formula of the compound formed
when it reacts with nitrogen ions?
15. If you averaged the atomic mass of all of the isotopes of nitrogen in any nitrogen sample,
what would be the value? By the way, what is an isotope?
16. Write the electron configuration for a sodium atom. Where would be a likely place for
the 3s electron to go if the atom was in an “excited” state (like in the flame test lab).
(Give any example of a probable location.)
17. True or false and why? “Atoms of the same element can have different masses.”
Name: ______________________________________________________________Hour:______
Chemistry 2 Final Exam Review
The Periodic Table
1. Point out the metals, non-metals on the periodic table. Point out the metalloids.
2. Are there any non-metals in the metal area of the periodic table? Point any out.
3. List at least three properties of metals? Three of non metals?
4. Name groups 1, 2, 17, and 18.
5. List the symbols of all halogens.
6. Do metals like to gain or lose electrons? Why?
7. Do non-metals like to gain or lose electrons? Why?
8. Which elements exist as diatomic molecules? What does diatomic mean?
9. What is nitrogen’s atomic number? What is nitrogen’s mass? What is nitrogen’s molar
mass?
10. What happens to the atomic radius across a period? Why? Down a group? Why?
Bonding
1. a. How many electrons do elements in these groups gain or lose to make octets?
1, 2, 13, 14, 15, 16, & 17?
b. The electron configuration for Sulfur is 1s22s22p63s23p4. How many electrons does
sulfur need to be a stable octet?
c. Which group in the P. Table already has an octet in place (except for one member of
the group)?
2. What does the Roman numeral 3 stand for in iron(III) oxide?
3. What’s the difference between ionic and covalent bonds, as far as electrons go?
Name: ______________________________________________________________Hour:______
Chemistry 2 Final Exam Review
Matter
Identify the following types of matter as substances or homogenous mixtures: Clearly
explain the difference.
1. brass
2. copper
3. tap water 4. salt 5. air
6. carbon dioxide
Reactions
___C3H8 + ___O2  ___CO2 + ___H2O
1. a. Balance the combustion of propane reaction above.
b. Given 3 moles of propane and 5 moles of oxygen, how many moles of water could be
made, maximum?
c. How many moles of propane would be needed to make 9 moles of carbon dioxide?
2. What are the reactants and products in a combustion reaction?
3. Complete this reaction and state the reaction type:
NaOH + H2SO4  __________ + ___________
Molar Mass
1. How much would 6.02 x 1023 molecules of water weigh?
2. 1 mole of salt, NaCl, would weigh how many grams?
3. How many grams would 6.02 x 1023 formula units of aluminum sulfate weigh?
4. How many molecules would be in 75 milliliters of water?
Name: ______________________________________________________________Hour:______
Chemistry 2 Final Exam Review
Nomenclature and Writing Reactions
Write the formula or name of the following:
________________ lead(II) nitrate
________________ diphosphorus triiodide
________________ K2S
________________ (NH4)3PO4
________________ N2O3
________________ aluminum carbonate
________________ sodium phosphate
Write, finish, and balance these reactions. Write the type.
1. Ethene, C2H4, burns.
2. Magnesium sulfide reacts with calcium phosphate.
3. Iron(III) sulfate reacts with calcium metal.
4. Hydrogen and oxygen gas burn together, making steam.
Lewis Structures.
1. Draw the Lewis Structure of a water molecule.
2. Draw the Lewis Structure of the carbonate ion.
3. Draw the Lewis Structure of the chlorite ion, ClO2-
Name: ______________________________________________________________Hour:______
Chemistry 2 Final Exam Review
Stoichiometry and Theoretical Yield
Iron (Fe) reacts with steam (H2O) to make magnetite, or Fe3O4 (231.6 g/mole), and hydrogen
gas (H2).
1. Write and balance the reaction.
2. If 25.0 grams of iron is reacted with excess water, how many moles of magnetite could be
made? How many grams of magnetite could be made?
3. If you had 15.0 grams of each reactant, how much magnetite (in grams) could you make?
What is the limiting reactant?
4. If you do the above (#3) experiment and 15.4 grams of magnetite is made, what is the
percent yield?