Make sure you can do all the homework problems as well as the list of study questions and learning goals below.

CHAPTER 5
1. Describe how the balance between the strength of the attractions between particles in a sample of matter and the kinetic energy of the sample determine the physical state (solid, liquid, or gas) of the sample.
2. What is the relationship between the melting point or boiling point of a sample of matter and the strength of the  attractions between particles in the sample?
2. Be able to describe these four types of attractions between particles by name, types of particles involved, how the particles attract each other, the relative strength of the attractions, and examples: ionic, dipole, hydrogen bonding, dispersion.
3. Given the chemical formula of a substance and its shape if it is molecular, be able to determine which type of attractions are present between the particles.
4. Why do temporary or induced dipoles have weaker attractions than permanent dipoles?
5. What are "hydrogen bonds"?  Which type of attraction are they and why are they special?
6. How is the strength of dispersion forces between molecules related to the size or mass of the molecules?
7. Be able to predict relative melting point and boiling point of a several substances based on the strength of the attractions between particles given the formulas and/or electron dot structures of the substances.
8. What is the definition of a solution?  Review - how is a mixture different from a pure substance?
9. Define solute and solvent.
10. What does "like" mean in the rule, "like dissolves like"? Predict what substances are soluble in other substances using this rule.

CHAPTER 6
1. Review! Describe the difference between physical and chemical changes. How do you know if a chemical change has occurred - in other words, what is the identifying feature of a chemical rather than physical change?  Remember - chemical changes are chemical reactions.
2. Identify all the features of a chemical equation - formulas of substances, reactants, products, reaction arrow, indicators of physical state of each substance.  Be able to write a chemical equation from a word description of the chemical change given the formulas and physical states of the substances involved.
3. What important law is used in balancing chemical equations?  Which of the following cannot be created or destroyed - mass, number of atoms, number of molecules? In other words, what must be the same on the two sides of the equation?
4. What are the "coefficients" in a chemical equation?
5. Review!  What do the numerical subscripts in chemical formulas indicate?  
6. Be able to balance a chemical equation by adding appropriate coefficients.  Remember - you cannot change the subscripts in formulas when balancing equations - why not?  
7.  What is a "mole" in chemistry? You do not need to memorize Avogadro's number but you do need to know that it is the number of things in one mole.  Remember - the word "mole" is used the same way as the word "dozen"; the difference is that the mole is a much bigger number than the dozen.
8. Be able to calculate the formula mass or molecular mass of a substance given its formula.  What are the units used for formula mass or molecular mass?  Review - Where do you find the atomic masses on the periodic table and what are the units for atomic masses?
9. What is the molar mass of a substance?  Be able to calculate the molar mass of a substance given its chemical formula.  What are the units for molar mass?  Remember - the molar mass is an amount of the substance that is big enough to see and weigh.
10. Be able to "read" a chemical equation in terms of molecules or moles of molecules. Be able to read a chemical equation in terms of relative masses.
11. Know the relationship between the pressure and the volume of a given amount of gas at constant temperature. Predict how volume changes when the pressure changes.
12. Know the relationship between the temperature (in Kelvins) and the volume of a given amount of gas at constant pressure. Predict how volume changes when the temperature changes.
13. Know the relationship between the number of moles of a gas and the volume of the gas at constant temperature and pressure. Predict how volume changes when the quantity (number of moles) of gas changes.
14. Be able to "read" a chemical equation for gaseous reaction in terms of the relative volumes of the gases. 
15. Use the kinetic molecular theory of gases to explain why gases always take the shape and volume of their containers, and why gases have low density values.
16. Know the relationship between the temperature of a gas and the kinetic energy of the gas particles. What is the physical significance of absolute zero on a the Kelvin temperature scale?
17. Using the description of gas pressure as the force of collisions per area on the container walls, explain the P/V relationship and the T/V relationship on the molecular level.
18. What is the definition of a solution?  Review - how is a mixture different from a pure substance?
19. Define solute and solvent.  What is the solvent in an aqueous solution?
20. Identify the solute and solvent in the following notation:  NaCl(aq).
21. "Concentration" is used to specify the composition of a solution.  Describe the relative amounts of solute and solvent in a "concentrated" solution versus a "dilute" solution.
22. Define molarity. What happens to the molarity value as the concentration of the solution increases?

CHAPTER 7
1. Be able to list four properties of acidic solutions and four properties of basic solutions.
2. What ions must be present in excess in an aqueous solution in order for a solution to be acidic? to be basic? Be able to write the name and formula of the ions.
3. Be able to give both the Arrhenius and Bronsted-Lowry definitions for acids and bases. Be able to identify acids and bases in chemical reactions.
4. What is the formula of the hydronium ion? How is it formed in water?
5. Be able to write the chemical equation for the ionization of an acid as an Arrhenius acid and as a Bronsted-Lowry acid.
6. How do you recognize the formula of most acids? most bases?
7. What are the two reactants and the two products in neutralization reactions? (not specific formulas but kinds of substances)
8. What does the word "salt" mean in chemistry?  Review - how do you recognize the formula of an ionic compound?
9. What does the pH scale measure?
10. What do the brackets indicate in the notation, [H⁺]?
11. Define neutral, acidic, and basic solutions in terms of the relative amounts of hydrogen ion and hydroxide ion.
12. Define neutral, acidic, and basic solutions in terms of pH values.
13. What happens to the pH value as the amount of hydrogen ion in the solution increases? Does the solution become more acidic or more basic? 
14. What happens to the pH value as the amount of hydrogen ion in the solution decreases? Does the solution become more acidic or more basic?
15. If the pH increases by 1 unit on the pH scale, by how much will the hydrogen ion concentration change and will it increase or decrease?
16. Why is the pH of "normal" rainwater 5.6 rather than 7.0? What reaction occurs that causes the pH to be less than 7.0? What is the name of the acid that is produced by this reaction?
17. What it the definition of "acid rain" in terms of pH value?
18. What in the major gas that produces acid rain and where does it come from?  What is the name of the acid produced by this reaction?
19. What is the name of the acid in your stomach? What kind of reaction is used to relieve excess stomach acid (heartburn), and what kind of substances do antacids contain?   

CHAPTER 8
1. Give three definitions of oxidation and reduction in terms of gain or loss of (1) electrons, (2) oxygen, (3) hydrogen.
2. Define an oxidizing agent and a reducing agent.
3. Be able to identify substances being oxidized, substances being reduced, and the oxidizing agents and reducing agents, given chemical equations for a reaction.
4. Define electrochemistry.
5. Why are redox reactions necessary for making electrochemical cells?
6. Describe the transfer of electrons that takes place in redox reactions in terms of substances being oxidized/reduced.
7. Be able to identify the half reactions for oxidation and reduction that occur in an electrochemical cell. On which side of the equation are the electrons in each type of half reaction?
8. Identify the features of a voltaic cell - the anode, cathode, flow of electrons, salt bridge (porous partition).
9. Distinguish between the anode and cathode in a voltaic cell in terms of where oxidation and reduction occur.
10. What is the difference between a cell and a battery?
11. Describe how a rechargeable battery such as the lead storage battery gets recharged.
12. What specific type of redox reaction is used in a fuel cell?