Full AAMC Science Content Outline
Here is a list of all the content the AAMC has listed that could be tested on the MCAT:
The AAMC classifies each subject with abbreviations like "PHY" (physics), "GC" (general chemistry), "OC" (organic chemistry), "BC" (biochemistry), "BIO" (biology).
Some content falls under multiple subjects, so I've classified them under one particular category, for the sake of simplicity.
Translational Motion (PHY)
Units and dimensions
Vectors, components
Vector addition
Speed, velocity (average and instantaneous)
Acceleration
Force (PHY)
Newton’s First Law, inertia
Newton’s Second Law (F = ma)
Newton’s Third Law, forces equal and opposite
Friction, static and kinetic
Center of mass
Equilibrium (PHY)
Vector analysis of forces acting on a point object
Torques, lever arms
Work (PHY)
Work done by a constant force: W = Fd cosθ
Mechanical advantage
Work Kinetic Energy Theorem
Conservative forces
Energy of Point Object Systems (PHY)
Kinetic Energy: KE = ½ mv2; units
Potential Energy
PE = mgh (gravitational, local)
PE = ½ kx2 (spring)
Conservation of energy
Power, units
Periodic Motion (PHY)
Amplitude, frequency, phase
Transverse and longitudinal waves: wavelength and propagation speed
Fluids (PHY)
Density, specific gravity
Buoyancy, Archimedes’ Principle
Hydrostatic pressure
Pascal’s Law
Hydrostatic pressure; P = ρgh (pressure vs. depth)
Viscosity: Poiseuille Flow
Continuity equation (A⋅v = constant)
Concept of turbulence at high velocities
Surface tension
Bernoulli’s equation
Venturi effect, pitot tube
Electrostatics (PHY)
Charge, conductors, charge conservation
Insulators
Coulomb’s Law
Electric field E
Field lines
Field due to charge distribution
Electrostatic energy, electric potential at a point in space
Circuit Elements (PHY)
Current I = ΔQ/Δt, sign conventions, units
Electromotive force, voltage
Resistance
Ohm’s Law: I = V/R
Resistors in series
Resistors in parallel
Resistivity: ρ = R⋅A / L
Capacitance
Parallel plate capacitor
Energy of charged capacitor
Capacitors in series
Capacitors in parallel
Dielectrics
Conductivity
Metallic
Electrolytic
Meters
Magnetism (PHY)
Definition of magnetic field B
Motion of charged particles in magnetic fields; Lorentz force
Sound (PHY)
Production of sound
Relative speed of sound in solids, liquids, and gases
Intensity of sound, decibel units, log scale
Attenuation (Damping)
Doppler Effect: moving sound source or observer, reflection of sound from a moving object
Pitch
Resonance in pipes and strings
Ultrasound
Shock waves
Light, Electromagnetic Radiation (PHY)
Concept of Interference; Young Double-slit Experiment
Thin films, diffraction grating, single-slit diffraction
Other diffraction phenomena, X-ray diffraction
Polarization of light: linear and circular
Properties of electromagnetic radiation
Velocity equals constant c, in vacuo
Electromagnetic radiation consists of perpendicularly oscillating electric and magnetic fields; direction of propagation is perpendicular to both
Classification of electromagnetic spectrum, photon energy E = hf
Visual spectrum, color
Geometrical Optics (PHY)
Reflection from plane surface: angle of incidence equals angle of reflection
Refraction, refractive index n; Snell’s law: n1 sin θ1 = n2 sin θ2
Dispersion, change of index of refraction with wavelength
Conditions for total internal reflection
Spherical mirrors
Center of curvature
Focal length
Real and virtual images
Thin lenses
Converging and diverging lenses
Use of formula 1/p + 1/q = 1/f, with sign conventions
Lens strength, diopters
Combination of lenses
Lens aberration
Optical Instruments, including the human eye
Atomic Nucleus (PHY, GC)
Atomic number, atomic weight
Neutrons, protons, isotopes
Nuclear forces, binding energy
Radioactive decay
α, β, γ decay
Half-life, exponential decay, semi-log plots
The Periodic Table - Classification of Elements into Groups by Electronic Structure (GC)
Alkali metals
Alkaline earth metals: their chemical characteristics
Halogens: their chemical characteristics
Noble gases: their physical and chemical characteristics
Transition metals
Representative elements
Metals and non-metals
Oxygen group
The Periodic Table - Variations of Chemical Properties with Group and Row (GC)
Valence electrons
First and second ionization energy
Definition
Prediction from electronic structure for elements in different groups or rows
Electron affinity
Definition
Variation with group and row
Electronegativity
Definition
Comparative values for some representative elements and important groups
Electron shells and the sizes of atoms
Electron shells and the sizes of ions
Electronic Structure (PHY, GC)
Orbital structure of hydrogen atom, principal quantum number n, number of electrons per orbital (GC)
Ground state, excited states
Absorption and emission line spectra
Use of Pauli Exclusion Principle
Paramagnetism and diamagnetism
Conventional notation for electronic structure (GC)
Bohr atom
Heisenberg Uncertainty Principle
Effective nuclear charge (GC)
Photoelectric effect
Covalent Bond (GC)
Lewis Electron Dot formulas
Resonance structures
Formal charge
Lewis acids and bases
Partial ionic character
Role of electronegativity in determining charge distribution
Dipole Moment
σ and π bonds
Hybrid orbitals: sp3, sp2, sp and respective geometries
Valence shell electron pair repulsion and the prediction of shapes of molecules (e.g., NH3, H2O, CO2)
Structural formulas for molecules involving H, C, N, O, F, S, P, Si, Cl
Delocalized electrons and resonance in ions and molecules
Multiple bonding
Effect on bond length and bond energies
Rigidity in molecular structure
Stoichiometry (GC)
Molecular weight
Empirical versus molecular formula
Metric units commonly used in the context of chemistry
Description of composition by percent mass
Mole concept, Avogadro’s number NA
Definition of density
Oxidation number
Common oxidizing and reducing agents
Disproportionation reactions
Description of reactions by chemical equations
Conventions for writing chemical equations
Balancing equations, including redox equations
Limiting reactants
Theoretical yields
Solubility (GC)
Units of concentration (e.g., molarity)
Solubility product constant; the equilibrium expression Ksp
Common-ion effect, its use in laboratory separations
Complex ion formation
Complex ions and solubility
Solubility and pH
Electrochemistry (GC)
Concentration cell: direction of electron flow, Nernst equation
Electrolytic cell
Electrolysis
Anode, cathode
Electrolyte
Faraday’s Law relating amount of elements deposited (or gas liberated) at an electrode to current
Electron flow; oxidation, and reduction at the electrodes
Galvanic or Voltaic cells
Half-reactions
Reduction potentials; cell potential
Direction of electron flow
Concentration cell
Batteries
Electromotive force, Voltage
Lead-storage batteries
Nickel-cadmium batteries
Gas Phase (GC, PHY)
Absolute temperature, (K) Kelvin Scale
Pressure, simple mercury barometer
Molar volume at 0°C and 1 atm = 22.4 L/mol
Ideal gas
Definition
Ideal Gas Law: PV = nRT
Boyle’s Law: PV = constant
Charles’ Law: V/T = constant
Avogadro’s Law: V/n = constant
Kinetic Molecular Theory of Gases
Heat capacity at constant volume and at constant pressure (PHY)
Boltzmann’s Constant (PHY)
Deviation of real gas behavior from Ideal Gas Law
Qualitative
Quantitative (Van der Waals’ Equation)
Partial pressure, mole fraction
Dalton’s Law relating partial pressure to composition
Energy Changes in Chemical Reactions – Thermochemistry, Thermodynamics (GC, PHYC)
Thermodynamic system – state function
Zeroth Law – concept of temperature
First Law - conservation of energy in thermodynamic processes
PV diagram: work done = area under or enclosed by curve (PHY)
Second Law – concept of entropy
Entropy as a measure of “disorder”
Relative entropy for gas, liquid, and crystal states
Measurement of heat changes (calorimetry), heat capacity, specific heat
Heat transfer – conduction, convection, radiation (PHY)
Endothermic/exothermic reactions (GC)
Enthalpy, H, and standard heats of reaction and formation
Hess’ Law of Heat Summation
Bond dissociation energy as related to heats of formation (GC)
Free energy: G (GC)
Spontaneous reactions and ΔG° (GC)
Coefficient of expansion (PHY)
Heat of fusion, heat of vaporization
Phase diagram: pressure and temperature
Rate Processes in Chemical Reactions - Kinetics and Equilibrium (GC)
Reaction rate
Dependence of reaction rate on concentration of reactants
Rate law, rate constant
Reaction order
Rate-determining step
Dependence of reaction rate upon temperature
Activation energy
Activated complex or transition state
Interpretation of energy profiles showing energies of reactants, products, activation energy, and ΔH for the reaction
Use of the Arrhenius Equation
Kinetic control versus thermodynamic control of a reaction
Catalysts
Equilibrium in reversible chemical reactions
Law of Mass Action
Equilibrium Constant
Application of Le Châtelier’s Principle
Relationship of the equilibrium constant and ΔG°
Principles of Bioenergetics (BC, GC)
Bioenergetics/thermodynamics
Free energy/Keq
Equilibrium constant
Relationship of the equilibrium constant and ΔG°
Concentration
Le Châtelier’s Principle
Endothermic/exothermic reactions
Free energy: G
Spontaneous reactions and ΔG°
Acid/Base Equilibria (GC, BC)
Brønsted–Lowry definition of acid, base
Ionization of water
Kw, its approximate value (Kw = [H+][OH−] = 10−14 at 25°C, 1 atm)
Definition of pH: pH of pure water
Conjugate acids and bases (e.g., NH4+ and NH3)
Strong acids and bases (e.g., nitric, sulfuric)
Weak acids and bases (e.g., acetic, benzoic)
Dissociation of weak acids and bases with or without added salt
Hydrolysis of salts of weak acids or bases
Calculation of pH of solutions of salts of weak acids or bases
Equilibrium constants Ka and Kb: pKa, pKb
Buffers
Definition and concepts (common buffer systems)
Influence on titration curves
Ions in Solutions (GC, BC)
Anion, cation: common names, formulas and charges for familiar ions (e.g., NH4+ ammonium, PO43− phosphate, SO42− sulfate)
Hydration, the hydronium ion
Liquid Phase - Intermolecular Forces (GC)
Hydrogen bonding
Dipole Interactions
Van der Waals’ Forces (London dispersion forces)
Aldehydes and Ketones (OC)
Description
Nomenclature
Physical properties
Important reactions
Nucleophilic addition reactions at C=O bond
Acetal, hemiacetal
Imine, enamine
Hydride reagents
Cyanohydrin
Oxidation of aldehydes
Reactions at adjacent positions: enolate chemistry
Keto-enol tautomerism (α-racemization)
Aldol condensation, retro-aldol
Kinetic versus thermodynamic enolate
General principles
Effect of substituents on reactivity of C=O; steric hindrance
Acidity of α-H; carbanions
Alcohols (OC)
Description
Nomenclature
Physical properties (acidity, hydrogen bonding)
Important reactions
Oxidation
Substitution reactions: SN1 or SN2
Protection of alcohols
Preparation of mesylates and tosylates
Carboxylic Acids (OC)
Description
Nomenclature
Physical properties
Important reactions
Carboxyl group reactions
Amides (and lactam), esters (and lactone), anhydride formation
Reduction
Decarboxylation
Reactions at 2-position, substitution
Acid Derivatives (Anhydrides, Amides, Esters) (OC)
Orbital structure of hydrogen atom, principal quantum number n, number of electrons per orbital (GC)
Ground state, excited states
Absorption and emission line spectra
Use of Pauli Exclusion Principle
Paramagnetism and diamagnetism
Conventional notation for electronic structure (GC)
Bohr atom
Heisenberg Uncertainty Principle
Effective nuclear charge (GC)
Photoelectric effect
Covalent Bond (GC)
Lewis Electron Dot formulas
Resonance structures
Formal charge
Lewis acids and bases
Partial ionic character
Role of electronegativity in determining charge distribution
Dipole Moment
σ and π bonds
Hybrid orbitals: sp3, sp2, sp and respective geometries
Valence shell electron pair repulsion and the prediction of shapes of molecules (e.g., NH3, H2O, CO2)
Structural formulas for molecules involving H, C, N, O, F, S, P, Si, Cl
Delocalized electrons and resonance in ions and molecules
Multiple bonding
Effect on bond length and bond energies
Rigidity in molecular structure
Acid Derivatives (Anhydrides, Amides, Esters) (OC)
Description
Nomenclature
Physical properties
Important reactions
Nucleophilic substitution
Transesterification
Hydrolysis of amides
General principles
Relative reactivity of acid derivatives
Steric effects
Electronic effects
Strain (e.g., β-lactams)
Phenols (OC, BC)
Oxidation and reduction (e.g., hydroquinones, ubiquinones): biological 2e− redox centers
Polycyclic and Heterocyclic Aromatic Compounds (OC, BC)
Biological aromatic heterocycles
Molecular Structure and Absorption Spectra (OC)
Infrared region
Intramolecular vibrations and rotations
Recognizing common characteristic group absorptions, fingerprint region
Visible region (GC)
Absorption in visible region gives complementary color (e.g., carotene)
Effect of structural changes on absorption (e.g., indicators)
Ultraviolet region
π-Electron and non-bonding electron transitions
Conjugated systems
NMR spectroscopy
Protons in a magnetic field; equivalent protons
Spin-spin splitting
Mass spectrometer
Separations and Purifications (OC, BC)
Extraction: distribution of solute between two immiscible solvents
Distillation
Chromatography: Basic principles involved in separation process
Column chromatography
Gas-liquid chromatography
High pressure liquid chromatography
Paper chromatography
Thin-layer chromatography
Separation and purification of peptides and proteins (BC)
Electrophoresis
Quantitative analysis
Chromatography
Size-exclusion
Ion-exchange
Affinity
Stereochemistry of covalently bonded molecules (OC)
Isomers
Structural isomers
Stereoisomers (e.g., diastereomers, enantiomers, cis/trans isomers)
Conformational isomers
Polarization of light, specific rotation
Racemic mixtures, separation of enantiomers (OC)
Absolute and relative configuration
Conventions for writing R and S forms
Conventions for writing E and Z forms