MCAT Review Sheets Overview

Main Sections

  • Atomic Structure: 1
  • The Periodic Table: 2
  • Bonding and Chemical Interactions: 3
  • Compounds and Stoichiometry: 4
  • Chemical Kinetics: 5
  • Equilibrium: 6
  • Thermochemistry: 7
  • The Gas Phase: 8
  • Solutions: 9
  • Acids and Bases: 10
  • Oxidation-Reduction Reactions: 11
  • Electrochemistry: 12
  • Biology: 49
  • Human Structure & Functions: 49
  • Psychological & Social Issues: 49

General Chemistry

Atomic Structure

  • Rutherford Model (1911): Electrons orbit a nucleus.
  • Bohr Model (1913): Describes detailed orbits of electrons; energy changes when an electron moves between shells.
    • Photon Emission: Energy is emitted when an electron moves down to a lower orbit. Absorbed during upward transitions.
  • Uncertainty Principle: Cannot know both position and momentum of a particle simultaneously.
  • Hund’s Rule: Electrons fill degenerate orbitals singly before pairing.
  • Pauli Exclusion Principle: Two electrons in an orbital must have opposite spins.

Quantum Numbers

  • n: Principal quantum number (energy level), integer values (1, 2, 3, …).
  • l: Azimuthal quantum number (shape of orbital), ranges from 0 to n-1.
  • m_l: Magnetic quantum number (orbital orientation), integers from -l to +l.
  • m_s: Spin quantum number, either +1/2 or -1/2.

Electron Configuration

  • Diamond vs. Paramagnetic:
    • Diamagnetic: All electrons are paired; repelled by a magnetic field. e.g., He.
    • Paramagnetic: One or more unpaired electrons; attracted to a magnetic field. e.g., C.

The Periodic Table

  • Trends:
    • Atomic Radius: Decreases across a period; increases down a group.
    • Ionization Energy (IE): Energy required to remove an electron; increases across a period and decreases down a group.
    • Electronegativity (EN): Ability of an atom to attract electrons in a bond; increases across a period. e.g., values for H, C, N, O, F.

Classification of Elements

  • Metals: Good conductors, malleable, ductile, lose electrons easily.
  • Nonmetals: Poor conductors, brittle, gain electrons.
  • Metalloids: Intermediate properties.

Bonding and Chemical Interactions

  • Hybridization: Atomic orbitals mix to form new hybrid orbitals for bonding.
    • Types: sp, sp2, sp3, sp3d, sp3d2.

Molecular Geometry

  • Determined by VSEPR theory, considers bonded and lone pairs.
  • Common Geometries:
    • Linear: 180°
    • Trigonal planar: 120°
    • Tetrahedral: 109.5°

Bond Types

  • Ionic Bonds: Transfer of electrons; usually between metals and nonmetals.
  • Covalent Bonds: Sharing electrons; usually between nonmetals.

Reaction Types

  • Combination, Decomposition, Combustion, Single-Displacement, Double-Displacement, Neutralization.
    • Example Reactions:
    • Combustion: Hydrocarbon + O2 → CO2 + H2O
    • Neutralization: Acid + Base → Salt + H2O

Chemical Kinetics

  • Rate of reaction determined by concentration, temperature, catalysts:
    • Rate = k[A]^m[B]^n
    • Catalyst lowers activation energy (Ea).

Equilibrium

  • Le Châtelier’s Principle: If a dynamic equilibrium is disturbed, the system shifts to counteract the change.

Thermochemistry

  • Enthalpy (H): Heat content; reflects energy stored in chemical bonds.
  • Endothermic vs. Exothermic: Energy absorption vs. release during reactions.
  • Hess's Law: Total enthalpy change is the sum of enthalpy changes for individual steps in a reaction.

The Gas Phase

  • Ideal Gas Law: PV = nRT

Biology

The Cell

  • Cell Components: Nucleus, cytoplasm, organelles (mitochondria, Golgi apparatus, etc.).
  • Mitosis: Division of somatic cells. Phases include Prophase, Metaphase, Anaphase, Telophase.
  • Meiosis: Produces gametes through two rounds of division.
    • Prophase I: Homologous chromosomes pair.

Human Anatomy and Physiology

  • Nervous System: CNS and PNS comprised of neurons and glial cells.
  • Circulatory System: Heart, blood vessels. Blood types (A, B, AB, O) determined by antigens.

Muscular System

  • Types of muscles: skeletal, smooth, cardiac. Each has distinct properties regarding control and function.

Endocrine System

  • Hormones: Chemical messengers regulating physiological processes. Examples: insuline, glucagon.
    • Negative Feedback: Hormonal regulation mechanism to maintain homeostasis.

Genetics and Evolution

  • Mendelian Genetics: Law of Segregation, Law of Independent Assortment.
  • Natural Selection: Mechanism driving evolution.

Biochemistry

Amino Acids and Proteins

  • Structure: Composed of amino group, carboxyl group, and R group; 20 standard amino acids.
  • Protein Structure: 1° (sequence), 2° (folding patterns), 3° (3D shape), 4° (subunit interaction).

Enzyme Function

  • Roles: Catalysts facilitating biochemical reactions; lower activation energy (Ea).
  • Inhibition: Competitive, non-competitive, uncompetitive inhibition mechanisms.

Metabolism Overview

  • Pathways: Catabolism and Anabolism of biomolecules (carbohydrates, fats, proteins).
    • Glycolysis: Conversion of glucose to pyruvate producing ATP and NADH.
    • Krebs Cycle: Central metabolic pathway further oxidizing acetyl-CoA.

DNA Structure and Function

  • Structure: Double helix composed of nucleotides (A, G, C, T)
  • Replication: Synthesis of new DNA strands; requires helicase, DNA polymerase.

RNA and the Genetic Code

  • Types of RNA: mRNA, tRNA, rRNA.
  • Protein Synthesis: Transcription (DNA to mRNA) and Translation (mRNA to protein).

Conclusion

  • Prepare using this exhaustive guide, ensuring to grasp the connections between concepts for full understanding. Ensure familiarity with diagrams and terminology, and practice problems to strengthen retention.

This format represents a comprehensive encapsulation of the information from the metabolites and organ systems covered in the study notes, serving as a useful resource for exam preparation.