Final Exam Coverage: General, Organic, and Biological Chemistry

Overview

This study guide summarizes the key topics and skills required for the final exam in a GOB (General, Organic, and Biological) Chemistry course. The exam includes multiple choice, free response, and laboratory components, covering foundational concepts, calculations, and laboratory techniques.

Chemistry Fundamentals

Scientific Notation and Significant Figures

• Scientific Notation: A method to express very large or small numbers using powers of ten. For example, 0.00045 = .

• Significant Figures (Sig Figs): Digits in a measurement that are known with certainty plus one estimated digit. Rules for determining sig figs must be followed in calculations.

• Reporting Measurements: Always report measurements to the correct number of significant figures based on the instrument's precision.

Temperature Conversions

• Common temperature scales: Celsius (°C), Kelvin (K), Fahrenheit (°F).

• Conversion formulas:

  • Celsius to Kelvin:

  • Celsius to Fahrenheit:

  • Fahrenheit to Celsius:

Matter and Its Classification

Physical vs. Chemical Changes

• Physical Change: Alters the form or appearance of matter but does not change its composition (e.g., melting, boiling).

• Chemical Change: Produces new substances with different properties (e.g., rusting, combustion).

Classification of Matter

• By Composition: Elements, compounds, mixtures.

• By State: Solid, liquid, gas.

• Mixtures: Can be homogeneous (solutions) or heterogeneous (suspensions, colloids).

Atomic Structure and Nuclear Chemistry

Anatomy of the Atom

• Atoms consist of protons, neutrons, and electrons.

• Isotopes: Atoms of the same element with different numbers of neutrons.

• Atomic number = number of protons; Mass number = protons + neutrons.

• Charge = protons - electrons.

Radioactivity and Radiation

• Types of Radiation: Alpha (α), Beta (β), Gamma (γ).

• Radioactive Decay: Spontaneous emission of particles or energy from an unstable nucleus.

• Half-life: Time required for half of a radioactive sample to decay.

  • Half-life formula:

• Safety: Different types of radiation require different safety precautions (e.g., alpha blocked by paper, gamma requires lead shielding).

Chemical Nomenclature and Structure

Nomenclature

• Inorganic Compounds: Naming based on cation and anion names.

• Organic Compounds: Alkanes, alkenes, alkynes, benzene derivatives. Use IUPAC rules for naming.

Functional Groups

• Recognize and name: alkane, alkene, alkyne, alcohol, aldehyde, ketone, carboxylic acid, amine, amide, thiol.

Lewis Structures and Molecular Geometry

• Draw Lewis structures to represent valence electrons.

• Use VSEPR theory to predict molecular geometry (e.g., linear, trigonal planar, tetrahedral).

• Determine molecular polarity based on symmetry and vector addition of bond dipoles.

Chemical Reactions and Stoichiometry

Types of Chemical Reactions

• Single displacement, double displacement, neutralization, redox, combination, decomposition, combustion, gas-evolution.

Balancing Chemical Equations

• Ensure the same number of each atom on both sides of the equation.

Stoichiometry

• Relate quantities of reactants and products using balanced equations.

• Use dimensional analysis for mass-mole, mole-mole, and mole-number (particles) conversions.

• Avogadro's number: particles/mol.

Redox Chemistry

• Identify oxidizing and reducing agents, species oxidized and reduced.

• Assign oxidation numbers to elements in compounds.

Gases and Gas Laws

Gas Laws

• Boyle's Law: (at constant T, n)

• Charles' Law: (at constant P, n)

• Gay-Lussac's Law: (at constant V, n)

• Avogadro's Law: (at constant P, T)

• Combined Gas Law:

• Dalton's Law of Partial Pressures:

Solutions and Concentrations

Types of Mixtures

• Solution: Homogeneous mixture with small particles (e.g., salt water).

• Colloid: Medium-sized particles, scatter light (e.g., milk).

• Suspension: Large particles, settle out (e.g., muddy water).

Concentration Calculations

• Percent (m/v):

• Molarity (M):

• Use concentrations as conversion factors in calculations.

• Dilution:

Acids, Bases, and Equilibrium

pH and pOH Calculations

• Calculate and from pH or pOH.

Acid-Base Reactions and Buffers

• Identify acids, bases, conjugate acids, and conjugate bases in reactions.

• Buffer: A solution that resists changes in pH upon addition of small amounts of acid or base.

• Effect of adding acid or base to a buffer: pH changes only slightly.

Chemical Equilibrium

• Le Chatelier's Principle: A system at equilibrium will shift to counteract a disturbance (adding/removing reactants or products).

Thermochemistry

Calorimetry and Specific Heat

• Calorimetry: Measurement of heat flow in a chemical or physical process.

• Specific Heat (c): Amount of heat required to raise the temperature of 1 g of a substance by 1°C.

• Formula:

Laboratory Skills and Safety

Laboratory Safety and Conduct

• Know procedures for fire, chemical spills, and handling broken glassware.

• Proper disposal of chemical waste.

• Use of Bunsen burner and other common laboratory equipment.

Measurement and Precision

• Make accurate measurements of volume, mass, length, etc., using appropriate equipment.

• Report measurements with correct significant figures.

Data Analysis and Graphing

• Use dimensional analysis to solve problems.

• Interpret graphs to determine relationships between variables.

• Draw conclusions from observed data and chemical reactions.

Summary Table: Types of Radiation

Additional info:

• For all calculations, always include units and use dimensional analysis where appropriate.

• Practice drawing and interpreting Lewis structures for both organic and inorganic molecules.

• Be familiar with laboratory equipment and their uses, as well as standard safety protocols.