Study Guide for 2^nd Semester Final Exam

Topics to be covered include:

Gas Laws (Chapter 5)

Thermochemistry (Chapter 6)

Atomic Structure (Chapter 7)

Bonding (Chapter 8)

Equilibrium (Chapter 13)

Acid Base Chemistry (Chapter 14)

Organic Chemistry (Chapter 22)

Test will be an 80 question, multiple choice test that will focus primarily on problems. There will be between 14 and 17 questions from each chapter. This study guide is meant to offer suggestions for areas to focus upon but should not be construed as the only topics that will be covered on the final exam.

GasLaws

Boyles Law (Pressure and Volume)

Charles Law (Pressure and Temperature)

Ideal Gas Law (Pressure, Temperature, Volume and Moles)

Dalton's Law of Partial Pressure

Reaction stoichiometry with gases

1. How many moles of helium are needed to fill a balloon that has a volume of 6.45 L and a pressure of 800 mm of Hg at a temperature of 24°C?

2. Oxygen can be prepared in small quantities in the laboratory using the thermal decomposition of potassium chlorate according to the equation:

2 KClO₃ (s) à 2 KCl (s) + 3 O₂ (g)

3. Consider that 2.0 g of potassium chlorate is heated and the oxygen is collected over water at 27°C and 770 torr. The vapor pressure of the water vapor at 27°C is 26.7 torr. What is the partial pressure of the oxygen produced in the reaction? What is mass of oxygen produced in the reaction? What is the volume of oxygen collected?

4. The carbon dioxide from the combustion of 1.5 g of C₂H₆ is collected over water at 25°C. The pressure of the carbon dioxide is 746 torr and the volume is 2.0 L. How much carbon dioxide dissolved in the water?

Thermochemistry

Specific Heat and Calorimetry

Enthalpy

Hess's Law

Standard Heat's or Enthalpy's of Formation (ΔH^rxn = ∑ ΔH°_prod - ∑ ΔH°_react)

1. A 250.0-g sample of water at 25.0°C is mixed with 100.0 g of a certain metal at 100.0°C. After thermal equilibrium is established, the (final) temperature of the mixture is 27.6°C. What is the heat capacity of the metal, assuming it is constant over the temperature range concerned?

2. Given the following reactions and their respective enthalpies:

2N₂O (g) à O₂ (g) + 2N₂ (g) ΔH = -164 kJ

2NH₃ (g) + 3N₂O à 4N₂ (g) + 3H₂O (l) ΔH = -1012 kJ

Calculate ΔH for:

4NH₃ (g) + 3O₂ (g) à 2N₂ (g) + 6H₂O (l)

3. Consider the reaction: C₂H₅OH (l) + 3O₂ (g) à 2CO₂ (g) +3H₂O(l) ∆H = -1.37 x 10³ kJ

When a 30-g sample of ethyl alcohol (molar mass = 46.1 g/mol) is burned, how much energy is released as heat?

What is the enthalpy for the reaction:

2C₂H₆ (g) + 9O₂ (g) à 6CO₂ (g) + 6H₂O (l)

given that the ΔH° for C₂H₆, CO₂, and H₂O are -20.9 kJ/mol, -393.5 kJ/mol and 286 kJ/mol, respectively.

Atomic Structure, Periodicity, Bonding

Electromagnetic Radiation

Hydrogen Spectrum and Bohr Model of Atom

Quantum numbers and atomic orbitals

Atomic structure and periodic table

Lewis Structures, electronegativity, atomic radii

1. Which of the following principal quantum numbers is not allowed? 0, 1, 2, 3, 4

2. How many unpaired electrons are there in aluminum, in barium, in carbon?

3. Write the expected electron configuration for lithium, sodium, nitrogen, calcium, zinc, bromine, argon.

4. What is the outer shell electron configuration for alkali metals, alkaline earth metals, halogens and inert gases?

5. What wavelength of light has the greatest energy? the least?

6. What color of light has the greatest energy

7. Which element is the most electronegative? which would be the least? From a collection of molecules which would be the most polar? the least?

Equilibrium

The Equilibrium State

Predict Changes in Equilibrium

Equilibrium Constant and Equilibrium Expressions

Le Chatelier's Principle

1. At equilibrium, carbon monoxide gas and water vapor have reacted to produce concentrations of 0.127M CO₂ (g), 0.127 M H₂ (g). The molarity of the reactants is 0.061 M CO and 0.0262 M H₂O. What is the balance equation, the equilibrium expression and the equilibrium constant for the reaction.

2. When N₂O₄ initially at 1.0 M is placed in a flask at 298 K and allowed to come to equilibrium, according to the following equation:

N₂O₄(g) D 2NO₂(g)

the equilibrium concentration of N₂O₄ is 0.82 M. What is the equilibrium concentration of the NO₂ and what is the change in the concentration of NO₂ between the start of the reaction and equilibrium in terms of “x”?

3. Given the reaction:

CoCl₂ (aq) + Ca(OH)₂ (aq) à Co(OH)₂ + CaCl₂

suppose KOH were added to the system. How would to additional OH- ions affect the equilibrium. What would happen if solid CaCl₂ were added?

Acid-Base Chemistry

Strong Acids and Bases, Weak acids

Molarity, salts and solutions of salts

pH scale, calculating pH, water equilibrium

Acid Base reactions or neutralization reactions, titrations

1. Distinguish a strong acid from a weak acid.

2. Calculate the pH of a 0.1 M HCl solution, 0.2 M H2SO4 solution and 0.25 M NaOH solution.

3. What is the NaOH concentration of a pH 12.65 solution?

4. Consider the preparation of a solution of 0.1 M lactic acid (HLa) which has an equilibrium constant (K_a) of 1.38 x 10^-4. What is the pH of this solution? Lactic acid would best form a buffer at what pH?

5. What volume of 0.100 M NaOH is required to neutralize 347 mL of 0.125 M HCl.

Organic Chemistry

Alkanes, Alkenes and Alkynes

Naming Compounds

Functional Groups (Alcohols, Aldehydes, Carboxylic Acids, Amines, Halogens, Esters, Ethers)

Polymers and polymerization reactions

1. Draw all the possible isomers of hexane and name them.

2. An alkyne would have at least two carbon atoms with what?

3. Given the following structure (without hydrogens):

C-C-C

|

C-C-C-C-C-C

what is the correct name?

4. Draw all the possible single alcohols with one through 5 carbons.

5. Draw butadiene, benzene, cyclohexane and benzoic acid.

6. What is a benzene ring? Draw 1,4-dichlorobenzene. What is the empirical formula for benzene?

7. Common plastics are formed from monomers with what type of bond?

8. Cellulose and starch are composed of what monomer?