Comprehensive Study Notes for General Chemistry 115 Exam 2 (Midterm)

Arrival: Students should arrive by 10:55 AM.
Seating Arrangement: After the previous class exits, students should be seated every other seat, with no additional space between seats except in the first two rows.
Duration: Students have 50 minutes to complete the exam (11 AM - 11:50 AM).
Materials to Bring:
- UIC student ID
- A working calculator with batteries
- Pencils and erasers
- No additional outside materials are allowed.
Restrictions: Cell phones and smart watches are prohibited; they cannot replace calculators.
Exam Content: A periodic table and Reference Packet will be provided as part of the exam.
Question Types: The exam will consist of multiple choice, fill-in-the-blank, and numeric problem-solving questions.
Partial Credit: Students are required to show their work for problem-solving to receive partial credit on certain exam questions.
Scratch Paper Policy: No outside scratch paper is permitted; exam provides extra room for problem-solving.
Academic Honesty: The Academic Honesty Statement from the syllabus will be enforced.

Chapters covered: 4 (4-9), 5 (1-5, 7-8), 6 (1-8), 7 (1-7), and 8 (1-8)
- Reference: Bettelheim et al., Introduction to General, Organic, and Biochemistry, 12th ed.

Assigning Oxidation Numbers:
- Determine oxidation states in ionic and covalent compounds.
- Identify redox reactions based on changes in oxidation state; figure out what is oxidized/reduced and the electrons transferred.
- Identify oxidizing and reducing agents in redox reactions.
Stoichiometry, Heat, Heat of Reaction:
- Differentiate between formula weight, molecular weight, and molar mass; calculate these for a chemical formula.
- Relate amounts of substance (moles), mass (grams), and chemical entities (molecules, atoms, etc.) using formulas, molar masses, and Avogadro's number as conversion factors.
- Apply principles of mass and element conservation in chemical equations.
- Use balanced equations for stoichiometric calculations.
- Identify limiting and excess reactant(s); perform calculations to find theoretical yield and percent yield.
- Understand heat transfer and perform calculations involving specific heat, mass, and temperature changes.
- Define and distinguish among endothermic and exothermic reactions, specifically referencing heat of combustion.
- Calculate heat absorbed/released during reactions from given amounts.

Outline essential properties and measurements of gases.
PVT Properties:
- How properties of gases differ from solids and liquids.
- Convert between pressure units.
- Use barometers and manometers for pressure measurement.
- Qualitatively relate changes in pressure, volume, temperature, and moles of gas.
- Understand Boyle's, Charles's, and Avogadro's Laws.
Ideal Gas Law:
- Use the formula: $\frac{P1V1}{n1T1} = \frac{P2V2}{n2T2}$ for calculations involving pressure, volume, temperature, and moles.
- Calculate moles of gas for given values.
- Relate partial pressures to total pressure and mole fractions.
Intermolecular Forces:
- Recognize differences between bonding forces and intermolecular forces, describing types and their energies.
- Analyze vapor pressure and boiling point behaviors at the molecular level.

Homogeneous Mixtures: Identify solutes, solvents, and solutions.
Types of Solutions:
- Distinguish between saturated, unsaturated, and supersaturated solutions.
- Define solubility and apply "like dissolves like" rule.
- Describe how temperature affects solubility of solids, liquids, and gases per Henry's law.
Concentration Units:
- Percent composition, Molarity, and people/counterpart measures like ppm and ppb.
- Use molarity to interconvert between moles and solution volume, and solve dilution problems using the dilution equation.
Electrolytes and Intermolecular Forces:
- Identify strong, weak electrolytes, and nonelectrolytes.
- Compare how water dissolves ionic versus molecular compounds.
- Explore colligative properties and osmotic pressure.

Reaction Rate Definition: Change in concentration over time.
Calculate rates and rate constants; understand coefficients in balanced reactions.
Identify factors affecting reaction rates:
- Nature of reactants, concentration, temperature, presence of a catalyst.
Define and explain activation energy and transition state.
Construct energy diagrams to show reaction progress.
Equilibrium Reactions:
- Reversible reactions and equilibrium constant expressions; calculate K based on concentrations.
Understand Le Chatelier's Principle and predict shifts in equilibrium due to disturbances.

Definitions:
- Identify Arrhenius acids/bases, define acid-base strength.
Bronsted-Lowry Theory: Apply definitions of acids as proton donors and bases as proton acceptors, and identify conjugate pairs.
Strength Relationships:
- Stronger acids yield weaker conjugate bases and vice versa.
Autoionization of Water: Understand and calculate pH from hydronium and hydroxide ion concentrations.
Acid Reactions: Identify reactions producing salts from acids, examine reactions with carbonates, hydroxides, and amines.
pH Measurement: Use pH meters and pH paper; understand ion products.

Review each exam learning objective systematically.
Use provided periodic table and Reference Packet for problem-solving.
Assign problems to each objective from various resources (worksheets, textbooks).
Redo discussion worksheet problems without looking for mastery.
Review lecture notes and redo related problems.
Work on assigned OWL homework problems by their due dates.
Engage with multiple-choice review problems for practice.
Read End of Chapter Summaries for key concepts.
Attend instructor and TA/Peer Leading Office Hours for support.
Participate in the MSLC (Mathematics and Science Learning Center) for further assistance with chemistry concepts and problems.

Dr. Hatfield: Regular drop-in hours on Mon./Wed. 12:00-1:00 pm, Fri 10:15-10:45 am in MSLC.
Additional Office Hour: Zoom session on the Sunday before the exam from 6:00-7:15 pm.
TA Office Hours: Available in MSLC, with updates available on Blackboard.

Work on odd-numbered problems from Chapters 4 (4-9), 5 (1-5, 7-8), 6 (1-8), 7 (1-7), and 8 (1-8) as they have answers provided in the appendix of the textbook. These problems may have been included in OWL assignments for review.