Semester II Final Review Guide
Study Tips:
1. Do the practice problems in the book for each section.
2. Do the multiple choice practice test at the end of the chapter.
3. Review your homework problems and Reading Notes
Chapter 9 – Chemical Reactions
Know the following terms
Chemical reaction
Reactant
Product
Coefficient
Chemical equation
Word equation
Skeleton equation
Complete Ionic Equation
Net Ionic Equation
Spectator Ion
Precipitate
Balancing Equations
1. Make sure all the chemical formulas are written correctly
2. Count all the metals and balance them using coefficients (number place before the chemical formula)
3. Balance all the polyatomic ions (count them as a single unit if they repeat on both sides of the rxn)
4. Balance the oxygen and hydrogens
Evidence of chemical rxn
1. Color change
2. Change of temperature (burn, coldness)
3. Production of gas (odor, bubbles, explosion)
4. Production of light, heat (fire, explosion)
5. Production of a precipitate
Notes to Remember:
· Words such as: reacts with, mix with, added to, in addition to; indicate (+)
· Produce, yield, react to produce, producing, decompose, indicate (à) for products
· Always H2, N2, O2, F2, Br2, I2, when they are by themselves (elemental form)
· Aqueous (aq), gas (g), solid (s), liquid (l), precipitate (s)
REACTANTS à PRODUCTS
A + B à C + D
TYPES OF REACTIONS (Be able to identify/write each type)
1. Synthesis
2. Decomposition
3. Single Replacement
4. Double Replacement
5. Combustion
Chapter 10 – The Mole
Know the following terms
Avogadro’s number
Molar mass
Representative particles (types?)
Percent composition
Empirical formula
Molecular formula
Hydrate
Anhydrous
What is the relationship between a molecular and empirical formula
Practice Problems
1. A colorless liquid composed of 46.68% nitrogen and 53.32% oxygen has a molar mass of 60.01 g/mol.
(a) Determine the empirical formula of the compound.
(b) Calculate the molar mass of the empirical formula.
2. What is the empirical formula for a compound that contains 10.89% magnesium, 31.77% chlorine, and 57.34% oxygen?
3. The pain reliever morphine contains 17.900 g C, 1.680 g H, 4.225 g O, and 1.228 g N. Determine the empirical formula.
Percent composition
1. What’s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen?
2. If the molar mass of the compound in problem 1 is 110 grams/mole, what’s the molecular formula?
3. What’s the empirical formula of a molecule containing 18.7% lithium, 16.3% carbon, and 65.0% oxygen?
Hydrates
1. A chemist heats a sample of hydrated lithium nitrate, which weighs 170 grams and finds, after heating, that it weighs 95.3 grams. Find the correct formula of the hydrate and name it. Determine the percent composition of anhydrous and water
Chapter 11 – Stoichiometry
Know the following terms
Stoichiometry
Mole Ratio
Limiting Reactant
Excess Reactant
Theoretical Yield
Actual Yield
Percent Yield
Know and be able to identify all the “tools” in your tool box, write them in the space below:
Molar Mass Mole Ratio Avogadro’s Number
Practice Problems
Butane burns in the following reaction: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)
a. Interpret the equation in terms of moles.
b. How many moles of CO2 can be produced from 2.5 mol C4H10?
c. How many moles of O2 are needed to react with 3.75 mol C4H10?
2. Using the balanced equation: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)
a. If 15 g of O2 react, what is the mass of H2O that can be produced?
b. If 17 mol of C4H10 react, what is the mass of CO2 that can be produced?
c. If 10.0 g of C4H10 react with 10.0 g O2, What is the limiting reactant? What is the excess reactant?
d. How much excess reactant is remaining after the reaction is complete?
3. Nickel carbonyl (Ni(CO)4) decomposes into nickel and carbon monoxide. In a laboratory reaction, 25.0 g nickel carbonyl produced 5.34 g nickel.
a. Balance the following equation for the reaction.
b. Determine the theoretical yield of nickel.
c. Determine the percent yield.
Chapter 12 - States of Matter
Know the following terms
Kinetic molecular theory
Particle Size
Elastic collision
Kinetic energy
Pressure
Dalton’s Law of Partial Pressures
Melting
Vaporization
Evaporation
Vapor Pressure
Boiling Point
Freezing Point
Condensation
Deposition
Phase diagram
Triple Point
Chapter 13 – Gases
Know the following terms
Molar Volume
STP
Boyle’s Law
Charles’ Law
Gay-Lussac’s Law
Combined Gas Law
Ideal Gas Law
List the units of pressure
1 atm = mm Hg = 760 torr = kPa
Explain how pressure and volume are related
Be able to identify and define the variables of Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, the Combined Gas Law, and the Ideal Gas Law
Chapter 14 – Solutions
Know the following terms
Solution (know some examples)
Solute
Solvent
Soluble
Insoluble
Solvation
Heat of solution
High solubility
Low solubility
Saturated solution
Supersaturated solution
Unsaturated solution
Concentration
Dilution
Percent by mass
Percent by volume
Molarity
Molality
Dilution Equation
What affects a solute’s solubility in a solvent? Why can some substances dissolve while others can’t?
What are some factors that affect the rate of solvation?
Concentration Ratios:
Practice Problems
What is the percent by mass of NaHCO3 in a solution containing 20 g NaHCO3 dissolved in 600 mL H2O?
What is the percent by volume of ethanol in a solution that contains 35 mL of ethanol dissolved in 115 mL water?
Calculate the molarity of 100.0 mL of an aqueous solution containing 0.85 mol potassium chloride.
What is the molarity of a solution that contains 5.10-g glucose in 100.5 mL solution. The molar mass of glucose is 180.16 g/mol.
How many grams of CaCl2 should be dissolved in 1.75 L of a 0.10 M solution of CaCl2?
Determine the molarity of 1.60 L of a solution containing 1.55 g of dissolved KBr.
How many moles of NaOH are needed to make 100 mL of a 2 M solution of NaOH?
What volume of 2.00 M calcium chloride stock is needed to make 0.50 L of 0.300 M calcium chloride?
If you dilute 20.0 mL of a 3.5 M solution to make 100.0 mL of solution, what is the molarity of the dilute solution?
In lab, a student adds 4.5 g of NaCl to 100.0 g of water. Calculate the molality of the solution.