General Chemistry I Review Notes

Chem. 1311: General Chemistry I Review Guidelines

Exam Coverage

• Exam #1: Chapters 1 and 2
• Exam #2: Chapters 3 and 4
• Exam #3: Chapters 5, 6, and ½ of 7
• Exam #4: Chapter ½ of 7, 8, and 9
• Final Exam: Comprehensive

Chapter 1: Study of Change

• Classification of Matter:

  • Pure substances: elements and compounds
  • Mixtures: homogeneous and heterogeneous

• Conversion:

  • How to convert a mixture to a pure substance.
  • How to convert elements into compounds.

• States of Matter:

  • Properties of solid, liquid, and gas (see slide #9).

• Changes and Properties:

  • Physical change (or physical properties).
  • Chemical change (or chemical properties) (see slide #10).

• Separation Techniques:

  • Filtration.
  • Distillation process (see slide #11).

• Scientific Notation:

  • How to convert a number to scientific notation and vice versa.

• Significant Figures:

  • Determine significant figures.
  • Apply significant figure rules to calculations.

• Calculations:

  • Density.
  • Temperature.

• Unit Conversion:

  • Using “dimensional analysis” (see slide #49).

Chapter 2: Electronic Structure of Atom

• Dalton’s Atomic Theory:

  • (See slide #2 & 3)

• Discovery of Sub-Atomic Particles:

  • The cathode rays.
  • Millikan oil drop experiment.
  • Radioactivity.
  • Plum pudding model.
  • Gold foil experiment.
  • Note: Know the group leader of each experiment and what the experiments were about.

• Atomic Number and Mass Number:

  • Determine atomic number (Z).
  • Determine mass number (A).

• Subatomic Particle Calculation:

  • Calculate # of protons.
  • Calculate # of electrons.
  • Calculate # of neutrons.

• Isotopes:

  • What is an isotope?
  • How to write isotope symbol notation (see slide #16, 17).

• Average Atomic Mass:

  • How to calculate the average atomic mass using isotopes and their natural percent abundances (see Example 2, 3).

• Periodic Table:

  • Study the periodic table: main group elements and transition elements.

• Group Names:

  • Name group 1A, 2A, 5A, 6A, 7A, 8A, and the two bottom rows (see slide #21).

• Diatomic Molecules:

  • There are 7 diatomic molecules. What are they? (see slide #22).

• Ions and Oxidation States:

  • Which ion loses (gains) electrons?
  • Determine the oxidation state for elements from group 1A, 2A, 4A, 5A, 6A, and 7A (see slide #23).

• Empirical Formula:

  • How to calculate the empirical formula (see slides #25 & Example #4).

• Nomenclature:

  • Naming ionic compounds, molecular compounds, acids, and hydrates.

Chapter 2 (cont.): Naming Compounds

• Naming & Writing ionic compounds.
• Naming molecular compounds.
• Naming binary acids & ternary acids.
• Naming hydrates compounds.

Chapter 3: Mass Relationships in Chemical Reactions

• Balancing Equations:

  • How to balance chemical equations.

• Types of Reactions:

  • Identify three different types of chemical reactions:
    • Combination reactions
    • Decomposition reactions
    • Combustion reactions

• Atomic vs. Molar Mass:

  • What is the difference between “atomic mass” and “molar mass”? (see slide # 16).

• Molar Mass Calculation:

  • Calculate molar mass for chemical molecules.

• Percent Composition:

  • Practice calculating “percent composition” or “percent by mass” (see slides #20-21).

• Conversion Factors:

  • Calculations involve the following conversion factors:
    • $1 \text{ mol } = \text{Molar mass (g)}$
    • $1 \text{ mol } = 6.022 \times 10^{23} \text{ atoms/molecules/formula units}$
    • Molar ratios (using the coefficients from the balanced chemical reactions).

• Stoichiometric Calculations:

  • Stoichiometric calculations (gram of A → gram of B) (see slides #25).

• Empirical & Molecular Formula:

  • Determine (and calculate) the “Empirical Formula” & “Molecular Formula”.

• Limiting Reactants & Percent Yield:

  • Determine “limiting reactants” and calculate “percent yield”.

Chapter 4: Reactions in Aqueous Solution

• Evidence of Chemical Reactions:

  • What are five evidences that indicate chemical reactions have occurred? (see slide #3).

• Solutions:

  • Definition of solution?
  • What are two components in a solution (see slide #4).

• Aqueous Solution:

  • What is an aqueous solution? (see slide #4).

• Electrolyte Solutions:

  • What is an electrolyte solution? (see slides #5-7).
    • Strong electrolyte
    • Weak electrolyte
    • Non-electrolyte

• Electrolyte Strength Prediction:

  • Which compounds will be strong/weak/Non-electrolyte?

• Solubility:

  • What is solubility? (see slide #9).

• Solubility Table:

  • How to use the “solubility table”?

• Describing Reactions in Aqueous Solution:

  • Molecular equation (ME)
  • Complete ionic equation (CIE)
  • Net ionic equation (NIE)

• Spectator Ions:

  • What are “spectator ions”? (see slide #14).

• Single Displacement Reactions:

  • Determine the products for single displacement using the “Activity Series”.

• Acids and Bases:

  • What are acids (and Bases)?
  • Which acid (or base) is strong (or weak)?

• Indicators:

  • What is “indicator”? (see slide #23).

• Neutralization Reactions:

  • Acids & Bases Reactions (Neutralization Reactions).

• Redox Reactions:

  • What are Oxidation – Reduction Reactions (Redox reactions)?
    • Oxidation reaction
    • Reduction reaction

• Solution Concentration:

  • Calculate concentration (Molarity) of a solution (see slide #33).
  • Calculate concentration for a dilution (see slide #35).
  • Calculate concentration for a titration (acid & base reaction).

Chapter 5: Thermodynamics (all formulas will be provided)

• Energy, Heat, Work, Temperature:

  • What is energy?
  • What is heat (q), work (w), and temperature (T)?

• State Function:

  • Is energy a state function?
  • What is the state function?

• First Law of Thermodynamics:

  • What is “The First Law of Thermodynamics”?

• Exothermic/Endothermic Processes:

  • Identify exothermic / endothermic process (reactions)
    • $q \text{ (positive) = energy flow into the system via heat (endothermic process)}$
    • $q \text{ (negative) = energy flow out of the system via heat (exothermic process)}$

• Heat Capacity/Specific Heat Capacity:

  • What is Heat Capacity / Specific Heat Capacity?
    • $C_s = \frac{q}{m \times \Delta T}$
    • $q = C_s \times m \times \Delta T$
    • Unit of $C_s$ is $\left(\frac{J}{g \times ^\circ C}\right)$ or $\left(\frac{J}{g \times K}\right)$

• Hess’s Law:

  • $\Delta H = \text{the sum of enthalpy from all the steps}$

• Enthalpy of Formation:

  • $\Delta H = \Sigma n \Delta H<em>{\text{products}} – \Sigma m \Delta H</em>{\text{reactants}}$, where n and m are the stoichiometric coefficients.

Chapter 6: Electronic Structure of Atom

• Electromagnetic Radiation:

  • Study the electromagnetic Radiation: How energy travels through space

• Wave Properties:

  • What are three properties of a wave (wavelength, amplitude, and frequency)

• Electromagnetic Spectrum:

  • Study the Electromagnetic Spectrum (slide #5)

• Spectrum Types:

  • What is the different between the continuous spectrum vs. Line Spectrum?

• Quantum Numbers:

  • Study Quantum Number (n, l, ml, and ms)

• Orbital Shapes:

  • Orbital shapes (s and p orbitals)

• Electron Configuration:

  • Students will be asked to draw orbital diagram and electron configuration for certain element. (both “full electron configuration” and “short cut” using the Noble gas to replace core electrons)

• Principles/Rules:

  • What is “Aufbau Principle”, “Pauli Exclusion Principle”, and “Hund’ Rule” about?

• Valence vs. Core Electrons:

  • Locate valence electrons and core electrons

• Electron Dot Symbols:

  • Draw “Electron Dot Symbols” for elements. (slide #30)

• Trends:

  • Compare “atomic radius”, “ionization energy”, and “metallic character”.

Chapter 7: Bonding

• Compound Types:

  • Identify ionic compounds and molecular compound

• Bond Types:

  • Study ionic bond and covalent bond

• Electron Behavior:

  • Which type of bond is formed by transferring of electrons / sharing of electrons?

• Octet Rule:

  • What is “the Octet Rule”?

• Electron Transfer Maps:

  • Use “Electron Transferring Maps” to determine the ionic compounds.

• Why Atoms Bond:

  • Why atoms bond?

• Lewis Structures:

  • Drawing Lewis Structures (following 5 steps) (slide #14)

• Resonance Structures:

  • Drawing Resonance Structures. (slide #15)

Chapter 8: Molecular Geometry

• Electron Domains:

  • What is Electron Domains?
  • How to determine electron domain around a particular atom

• Molecular Geometry:

  • Determine the Molecular Geometry for compounds that have:
    • 2 electron domains
      • Linear
    • 3 electron domains
      • Trigonal planar
      • V-shape or Bent
    • 4 electron domains
      • Tetrahedral
      • Trigonal pyramid or pyramidal
    • 5 electron domains
      • Trigonal bipyramid
      • Seesaw
      • T-shape
      • Linear
    • 6 electron domains
      • Octahedral
      • Square pyramid
      • Square planar

• Bond Angles:

  • Bond angle for:
    • Linear ($180^o$)
    • Trigonal ($120^o$)
    • Tetrahedral ($109.5^o$)
    • Trigonal pyramid ($> 109.5^o$)

• Electronegativity:

  • What is Electronegativity?

• Bond Polarity:

  • Determine Bond Polarity by calculate $\Delta EN$
    • Non polar bond ($\Delta EN \le 0.4$)
    • Polar covalent ($\Delta EN > 0.4$)
    • Polar Ionic ($\Delta EN \ge 2.0$)

• Molecular Polarity:

  • Determine Molecular Polarity by adding up “dipole moment vectors”
    • All vectors are adding up → polar compound
    • All vectors are canceled → Non polar compound

• Orbital Shapes:

  • Shape of s, p, and d orbitals

• Steric Number:

  • How to calculate “Steric Number”

• Hybrid Orbitals:

  • Determine hybrid orbitals for an atom (sp, sp2, sp3) using steric number (SN)

• Sigma and Pi Bonds:

  • The differences between sigma and pi bond

• Bond Order:

  • Compare single, double, and triple bond.

Chapter 9: Gases

• Gas Behavior:

  • The behavior of gases

• Boyle’s Law:

  • What is Boyle’s law?

• Charles’s Law:

  • What is Charles’s law?

• Avogadro’s Law:

  • What is Avogadro’s law?

• Combined Gas Law:

  • What is Combined gas law?

• Ideal Gas Law:

  • What is the Ideal Gas Law?