CHEM 162: Exam 1 Review Overview

Exam Logistics & Allowed Materials
- Required: Pencil/eraser (or pen), scientific calculator.
- Identification: Picture ID (UH ID preferred) required for exam submission.
- Seating: Assigned seats in SPAL 155 or ART 132 (posted on Lamakū).
- Calculator Rules:
  - For calculations only; no stored notes.
  - Graphing calculators are *not* allowed.
  - Covers/cases must be removed; memory cleared.
  - Subject to random checks; no sharing.
- Prohibited: All other electronic devices (phones, tablets, laptops, smartwatches, headphones).
- Format: Closed-book, closed-notes.
- Provided: Periodic Table, gas constant (R = 0.08206 \frac{l \cdot atm}{K \cdot mol}), and selected equations:
  - P_{soln} = X_{solvent} P^0_{solvent}
  - \Delta T = K \cdot m
  - \Pi = M \cdot R \cdot T
- Other Constants: Specific heat, molar heat of phase changes, freezing/boiling point constants will be given.
- Water Properties: Normal melting and boiling points of H₂O must be known (not provided).
- Absence Policy: If sick or emergency, contact instructor (check syllabus for full instructions).
Chapter 12 & 13: Liquids, Solids, & Intermolecular Forces (IMFs)
- States of Matter: Understand differences among gas, liquid, and solid states.
- Interactions: Compare relative strengths of intermolecular (between molecules) and intramolecular (within molecules) interactions.
- Types of IMFs:
  - Ion-ion, ion-dipole (discussed in class).
  - Other IMFs: London Dispersion Forces, Dipole-Dipole Forces, Hydrogen Bonding.
  - Identify compounds where each IMF is found and provide examples.
- IMF Strength & Properties: Stronger IMFs correlate with:
  - Higher boiling point (b.p.)
  - Higher melting point (m.p. or f.p.)
  - Lower vapor pressure
- London Dispersion Forces: Factors influencing their strength (e.g., molecular size, shape).
- Solids:
  - Classifications: Two general types of solids.
  - Crystal Types: Five types of crystals (e.g., ionic, metallic, network, molecular).
  - For each crystal type, describe lattice species, bonding/forces, and physical properties.
- Heating Curves
  - Sketch & Label: Understand and label a typical heating curve (1-5 regions).
  - Dimensions: Label horizontal (heat added) and vertical (temperature) axes.
  - Regions:
    - (1), (3), (5) (Sloped): Represent heating a single phase (solid, liquid, gas). Calculations involve q = mc\Delta T. Units typically J or kJ.
    - (2), (4) (Plateaus): Represent phase changes (melting/freezing, boiling/condensation). Calculations involve q = n\Delta H (where n is moles and \Delta H is molar enthalpy of fusion/vaporization). Units typically J or kJ.
- Phase Diagrams
  - Interpretation: Identify and describe key points and regions (e.g., gas only, solid-liquid equilibria, normal boiling point, triple point, critical point).
- Chapter 14: Solutions
  - Factors Affecting Solubility:
    - Molecular structure (polarity,