Chemistry Final Review
Chapters 9 – 13
Chapter 9:
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What is a monatomic ion? Give three examples
What is a cation? Give three examples
What is an anion? Give three examples?
How are anions named?
What is unique about transition metals?
How are transition metals named?
Write the charge for the elements K, Pb, and S. Determine whether they are anions or cations.
What type of element (metals or nonmetals) tends to form cations?
What type of element tends to form anions?
What is a polyatomic ion? How do they differ from monatomic ions?
Give three examples of a polyatomic ion.
What is a binary compound?
How do you write binary compounds?
Give three examples of a binary compound. (crisscross method)
Write the formulas for the following binary ionic compouds: copper (II) sulfide and potassium
nitride
How are binary ionic compounds named?
Name the following binary ionic compounds: Li₂Se and CoI₂
How are binary molecular compounds named?
Give three examples of a binary molecular compound.
Name the following binary molecular compounds: N₂O and PCl₃
What is an acid? How are acids named?
Name the following acids: HClO and HCN
What is a base? How are bases named?
Name the following bases: KOH and Fe(OH)₂
Chapter 10:
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How do chemists count the number of atoms, molecules, or formula units in a substance?
What is a mole?
What is Avogadro’s number?
What is a representative particle?
Converting representative particles to moles: How many moles of magnesium is 1.25 × 1023
atoms of magnesium?
6. Converting moles to representative particles: How many atoms are in 2.12 mol of propane
(C3H8)?
7. What is molar mass?
8. How is molar mass calculated?
9. Find the molar mass of a compound: What is the molar mass of hydrogen peroxide? (H₂O₂)
10. How do you convert the mass of substance into moles of a substance?
11. Converting moles to mass: What is the mass, in grams, of 9.45 mol of aluminum oxide?
12. Converting mass to moles: How many moles of iron(III) oxide are contained in 92.2 g of pure
Fe₂O₃?
13. How do you convert the volume of a gas at STP to the number of moles of the gas?
14. What is STP?
15. Converting moles to volume: Determine the volume, in liters, of 0.60 mol SO2 gas at STP.
16. Converting volume to moles: The density of a gaseous compound containing carbon and oxygen
is found to be 1.964 g/L at STP. What is the molar mass of the compound?
Chapter 11:
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What is a skeleton equation? How do you write a skeleton equation? (Give example)
What is a word equation? How do you write a word equation? (Give example)
What is a catalyst? How are catalysts written in an equation?
Write a skeleton equation for the following example: Hydrochloric acid reacts with solid sodium
hydrogen carbonate. The products formed are aqueous sodium chloride, water, and carbon
dioxide gas. Write a skeleton equation for this chemical reaction.
What is a balanced equation? How do you write a balanced equation?
Balance the following equation: AgNO3(aq) + Cu(s) → Cu(NO3)2(aq) + Ag(s)
Balance the following equation: C3H8(g) + O2(g) → CO2(g) + H2O(l)
What are the five general types of reactions?
What is a combination reaction? Give an example.
What is a decomposition reaction? Give an example.
What is a single replacement reaction? Give an example.
What is a double replacement reaction? Give an example.
What is a combustion reaction? Give an example.
What is a net ionic equation? What does it show?
What is a complete ionic equation?
How do you write a complete ionic equation?
How do you write a net ionic equation?
What is a spectator ion?
Write the complete ionic equation and the net ionic equation for the following example: Pb(s) +
AgNO3(aq) → Ag(s) + Pb(NO3)2(aq)
20. Write and balance the net ionic equation: Aqueous solutions of iron(III) chloride and potassium
hydroxide are mixed. A precipitate of iron(III) hydroxide forms. Identify the spectator ions and
write a balanced net ionic equation for the reaction
21. How can you predict the formation of a precipitate in a double-replacement reaction? (Solubility
Chart)
22. Will a precipitate form when aqueous solutions of Na2CO3(aq) and Ba(NO3)2(aq) are mixed?
Chapter 12:
1. What is stoichiometry?
2. Interpret the following equation in terms of volumes of gas at STP: 2H2(g) + 2NO(g)  N2(g) +
2H2O(g)
3. Interpret the following equation in terms of molecules: N2(g) + 3H2(g)  2NH3(g
4. Interpret the following equation in terms of moles: N2(g) + 3H2(g)  2NH3(g
5. Interpret the following equation in terms of mass: N2(g) + 3H2(g)  2NH3(g)
6. What is a mole ratio?
7. How are mole ratios calculated?
8. Mole-Mole calculation: How many moles of NH3 are produced when 0.60 mol of nitrogen reacts
with hydrogen?
9. Mass- Mass calculation: Calculate the number of grams of NH3 produced by the reaction of 5.40
g of hydrogen with an excess of nitrogen. N2(g) + 3H2(g)  2NH3(g)
10. Mass-Molecules calculation: How many molecules of oxygen are produced when 29.2 g of water
is decomposed by electrolysis according to this balanced equation: 2H2O(l) → 2H2(g) + O2(g)
11. Volume-Volume Calculation: How many liters of nitrogen dioxide are produced when 34 L of
oxygen react with an excess of nitrogen monoxide? Assume conditions are at STP.
2NO(g) + O2(g)  2NO2(g)
Chapter 13:
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What are the three assumptions of the kinetic theory as it applies to gases?
What is kinetic energy?
What is kinetic theory?
What is gas pressure?
How does the kinetic theory explain gas pressure?
What is atmospheric pressure?
What is a barometer?
What is the SI unit of pressure?
What is standard atmosphere (atm)?
10. What is a pascal?
11. What is 760 mm Hg?
12. A pressure gauge records a pressure of 450 kPa. Convert this measurement to atmospheres and
millimeters of mercury
13. What is vaporization?
14. What is evaporation?
15. Explain why heating a liquid causes evaporation to occur faster?
16. When can dynamic equilibrium exist?
17. What is vapor pressure?
18. How does an increase in the temperature of a contained liquid affect the vapor pressure?
19. Under what conditions does boiling occur?
20. What is the normal boiling point?
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