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MCAT (Medical College Admission Test) Chemical and Physical Foundations of Biological Systems Syllabus

The Chemical and Physical Foundations of Biological Systems syllabus for MCAT (Medical College Admission Test) in full: 5 chapters, 17 topics and 45 sub-topics, every one listed below, plus 52 Chemical and Physical Foundations of Biological Systems flashcards with answers.

5Chapters
17Topics
45Sub-topics
52Flashcards

Chemical and Physical Foundations of Biological Systems syllabus: all 5 chapters

Expand any chapter to see its topics and sub-topics.

  1. Mechanics, Energy, and Fluids in Living Systems

     4 topics
    • Translational and Rotational Motion
      • Vectors, displacement, velocity, and acceleration
      • Kinematics and projectile motion
      • Torque, center of mass, and equilibrium
    • Force, Work, and Energy
      • Newton's laws and free-body diagrams
      • Work-energy theorem and conservation of energy
      • Kinetic, potential, and mechanical energy
    • Fluids and Gases
      • Density, pressure, and Pascal's principle
      • Buoyancy and Archimedes' principle
      • Continuity equation and Bernoulli's principle
      • Viscosity, Poiseuille flow, and blood circulation
    • Thermodynamics of Biological Systems
      • Heat, temperature, and specific heat
      • First and second laws of thermodynamics
      • Entropy and energy transfer

  2. Electrostatics, Circuits, and Magnetism

     3 topics
    • Electrostatics
      • Coulomb's law and electric fields
      • Electric potential and potential energy
      • Dipoles in biological membranes
    • Circuit Elements
      • Current, voltage, and resistance (Ohm's law)
      • Capacitance and dielectrics
      • Series and parallel circuits
    • Magnetism and Bioelectricity
      • Magnetic fields and forces on charges
      • Nerve conduction and membrane potentials

  3. Waves, Sound, Light, and Optics

     3 topics
    • Periodic Motion and Sound
      • Simple harmonic motion and resonance
      • Sound intensity, the decibel scale, and the Doppler effect
      • Ultrasound and hearing physiology
    • Electromagnetic Radiation and Light
      • The electromagnetic spectrum
      • Reflection, refraction, and total internal reflection
    • Geometrical and Physical Optics
      • Thin lenses, mirrors, and image formation
      • Optics of the human eye and corrective lenses
      • Diffraction, interference, and polarization

  4. General Chemistry of Biological Systems

     4 topics
    • Atomic Structure and Periodicity
      • Quantum numbers and electron configuration
      • Periodic trends in reactivity
    • Bonding and Stoichiometry
      • Ionic, covalent, and intermolecular forces
      • Mole concept, balancing equations, and limiting reagents
    • Solutions and Phases
      • Solubility, concentration units, and colligative properties
      • Phase diagrams and phase changes
    • Kinetics and Equilibrium
      • Rate laws and reaction order
      • Le Chatelier's principle and equilibrium constants

  5. Thermodynamics, Electrochemistry, and Acid-Base Chemistry

     3 topics
    • Chemical Thermodynamics
      • Enthalpy, entropy, and Gibbs free energy
      • Spontaneity and coupled reactions
    • Acids, Bases, and Buffers
      • pH, pKa, and the Henderson-Hasselbalch equation
      • Titration curves and buffer systems
      • Physiological buffering (bicarbonate system)
    • Electrochemistry
      • Oxidation states and redox reactions
      • Galvanic and electrolytic cells
      • Nernst equation and cell potentials

MCAT (Medical College Admission Test) Chemical and Physical Foundations of Biological Systems flashcards — 52 questions with answers

  1. What is the equation for displacement of an object under constant acceleration, starting from initial velocity v0?

    x = v0·t + ½at². Final velocity: v = v0 + at, and v² = v0² + 2a·x.

  2. For projectile motion, how do the horizontal and vertical components of velocity behave?

    Horizontal velocity is constant (no horizontal acceleration); vertical velocity changes at g = 9.8 m/s² due to gravity. The two components are independent.

  3. Define torque and give its formula.

    Torque (τ) is the rotational effect of a force: τ = r·F·sin(θ), where r is the lever arm, F the force, and θ the angle between them. Units: N·m.

  4. What is the relationship between linear and angular quantities for an object moving in a circle of radius r?

    v = rω (velocity), a_t = rα (tangential acceleration). Centripetal acceleration a_c = v²/r = ω²r, directed toward the center.

  5. State the condition for static equilibrium of a rigid body.

    Net force equals zero (ΣF = 0) AND net torque equals zero (Στ = 0). Both translational and rotational equilibrium must hold.

  6. State Newton's three laws of motion.

    1) An object stays at rest or in uniform motion unless acted on by a net force (inertia). 2) F = ma. 3) For every action there is an equal and opposite reaction.

  7. Define work and give the conditions under which a force does zero work.

    Work W = F·d·cos(θ). Work is zero when force is perpendicular to displacement (θ = 90°) or when there is no displacement.

  8. What is the work-energy theorem?

    The net work done on an object equals its change in kinetic energy: W_net = ΔKE = ½mv_f² − ½mv_i².

  9. Give the formulas for kinetic energy and gravitational potential energy.

    Kinetic energy KE = ½mv². Gravitational potential energy PE = mgh (near Earth's surface).

  10. Define power and give two equivalent formulas.

    Power is the rate of doing work: P = W/t = F·v (for constant force along velocity). Units: watts (W = J/s).

  11. What distinguishes conservative from non-conservative forces?

    Conservative forces (gravity, spring, electrostatic) do path-independent work and have an associated potential energy. Non-conservative forces (friction, drag) dissipate mechanical energy and are path-dependent.

  12. State the principle of conservation of mechanical energy and when it applies.

    KE + PE = constant when only conservative forces do work. If non-conservative forces (e.g., friction) act, mechanical energy is not conserved.

  13. State Pascal's principle.

    A pressure change applied to an enclosed incompressible fluid is transmitted undiminished to every part of the fluid and the container walls. Basis of hydraulic systems: F1/A1 = F2/A2.

  14. State Archimedes' principle and the buoyant force formula.

    A submerged object experiences an upward buoyant force equal to the weight of the displaced fluid: F_b = ρ_fluid·V_displaced·g.

  15. What is the continuity equation for fluid flow?

    For incompressible fluid, A1·v1 = A2·v2 (volume flow rate Q = Av is constant). Narrower cross-section means faster flow.

  16. State Bernoulli's equation.

    P + ½ρv² + ρgh = constant along a streamline. Higher fluid speed corresponds to lower pressure (for constant height).

  17. Define absolute (gauge vs. absolute) pressure in a static fluid at depth h.

    Absolute pressure P = P0 + ρgh, where P0 is surface (atmospheric) pressure. Gauge pressure is the part ρgh above atmospheric.

  18. What is the ideal gas law and the value/units of R?

    PV = nRT. R = 8.314 J/(mol·K) = 0.0821 L·atm/(mol·K). T must be in kelvin.

  19. State the first law of thermodynamics.

    ΔU = Q − W, where ΔU is change in internal energy, Q is heat added to the system, and W is work done by the system. Energy is conserved.

  20. State the second law of thermodynamics in terms of entropy.

    The total entropy of an isolated system never decreases; spontaneous processes increase the entropy of the universe (ΔS_universe ≥ 0).

Show the other 32 Chemical and Physical Foundations of Biological Systems flashcards

  1. Define specific heat and the heat equation for temperature change.

    Specific heat c is the heat needed to raise 1 kg (or 1 g) of substance by 1°C. Heat: Q = mcΔT (no phase change).

  2. What equation governs heat exchange during a phase change?

    Q = mL, where L is the latent heat (of fusion for solid↔liquid, of vaporization for liquid↔gas). Temperature stays constant during the phase change.

  3. State Coulomb's law for the force between two point charges.

    F = k·q1·q2/r², where k ≈ 8.99×10⁹ N·m²/C². Like charges repel, opposite charges attract.

  4. Define electric field and give its formula for a point charge.

    Electric field E = F/q (force per unit positive test charge). For a point charge: E = kQ/r², pointing away from positive charge. Units: N/C or V/m.

  5. Define electric potential and potential difference (voltage).

    Electric potential V = kQ/r (potential energy per unit charge). Potential difference (voltage) is the work per charge to move a charge between two points: V = W/q.

  6. What is the relationship between energy, charge, and voltage; and capacitance?

    Energy U = qV. Capacitance C = Q/V (farads). Energy stored in a capacitor: U = ½CV² = ½QV.

  7. State Ohm's law and the formula for electrical power.

    V = IR. Power dissipated: P = IV = I²R = V²/R.

  8. How do resistors combine in series and in parallel?

    Series: R_total = R1 + R2 + ... (resistances add). Parallel: 1/R_total = 1/R1 + 1/R2 + ... (total is less than the smallest).

  9. How do capacitors combine in series and in parallel?

    Parallel: C_total = C1 + C2 + ... (capacitances add). Series: 1/C_total = 1/C1 + 1/C2 + ... (total is less than the smallest). Opposite of resistors.

  10. What is the magnetic force on a moving charge?

    F = qvB·sin(θ), where θ is the angle between velocity and the magnetic field B. The force is perpendicular to both v and B (direction by right-hand rule).

  11. What is the resting membrane potential of a typical neuron, and what maintains it?

    About −70 mV (inside negative). Maintained by the Na⁺/K⁺ ATPase pump and selective ion permeability (mainly K⁺ leak channels).

  12. Give the formula for the period of a simple pendulum and a mass-spring oscillator.

    Pendulum: T = 2π√(L/g). Mass-spring: T = 2π√(m/k). Note the pendulum period is independent of mass.

  13. What is the relationship between frequency, period, and wave speed?

    f = 1/T, and v = fλ (wave speed equals frequency times wavelength).

  14. What is the speed of sound in air and how does it depend on the medium?

    About 343 m/s in air at room temperature. Sound travels faster in liquids and fastest in solids; speed increases with medium stiffness and with temperature in gases.

  15. State the Doppler effect qualitatively for sound.

    Observed frequency increases when source and observer approach each other and decreases when they move apart, because of compression/stretching of the wave fronts.

  16. What is the relationship between intensity and the decibel sound level?

    β (dB) = 10·log10(I/I0), where I0 = 1×10⁻¹² W/m². Every 10 dB corresponds to a 10× change in intensity.

  17. Order the electromagnetic spectrum from longest to shortest wavelength.

    Radio → microwave → infrared → visible → ultraviolet → X-ray → gamma. Shorter wavelength means higher frequency and higher energy.

  18. Give the equation relating photon energy to frequency and wavelength.

    E = hf = hc/λ, where h = 6.626×10⁻³⁴ J·s (Planck's constant) and c = 3×10⁸ m/s.

  19. State Snell's law of refraction.

    n1·sin(θ1) = n2·sin(θ2). Light bends toward the normal when entering a denser (higher n) medium, and the index of refraction n = c/v.

  20. What is total internal reflection and when does it occur?

    All light reflects back into the denser medium when it strikes the boundary at an angle greater than the critical angle θ_c, where sin(θ_c) = n2/n1 (n1 > n2).

  21. State the thin-lens / mirror equation and the sign conventions for image distance.

    1/f = 1/o + 1/i. Positive image distance (i) = real image; negative i = virtual image. Magnification m = −i/o.

  22. Compare converging and diverging lenses by focal length and image type.

    Converging (convex) lens: positive focal length, can form real or virtual images. Diverging (concave) lens: negative focal length, always forms a virtual, upright, reduced image.

  23. What are the four quantum numbers and what does each specify?

    n (principal, energy/shell), l (azimuthal, subshell shape s/p/d/f), m_l (magnetic, orbital orientation), m_s (spin, +½ or −½). No two electrons share all four (Pauli exclusion).

  24. State Hund's rule and the Aufbau principle.

    Aufbau: electrons fill lowest-energy orbitals first. Hund's rule: within a subshell, electrons singly occupy each orbital with parallel spins before pairing.

  25. How do atomic radius, ionization energy, and electronegativity trend across the periodic table?

    Across a period (left→right): radius decreases; ionization energy and electronegativity increase. Down a group: radius increases; ionization energy and electronegativity decrease.

  26. Compare ionic, covalent, and metallic bonds.

    Ionic: electron transfer between metal and nonmetal (electrostatic attraction). Covalent: electron sharing between nonmetals. Metallic: delocalized 'sea' of electrons among metal cations.

  27. How do you find the limiting reagent in a reaction?

    Convert each reactant to moles, divide by its stoichiometric coefficient; the reactant giving the smallest result is limiting and determines the maximum product yield.

  28. Define molarity, molality, and how to calculate percent yield.

    Molarity = moles solute / L solution. Molality = moles solute / kg solvent. Percent yield = (actual yield / theoretical yield) × 100%.

  29. What are the four colligative properties and what do they depend on?

    Vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. They depend on the number (concentration) of solute particles, not their identity.

  30. Write the rate law form and the Arrhenius relationship for reaction kinetics.

    Rate = k[A]^m[B]^n (orders from experiment). Arrhenius: k = A·e^(−Ea/RT); rate constant rises with temperature and falls with higher activation energy.

  31. State Le Chatelier's principle and write the relationship between ΔG° and K.

    A system at equilibrium shifts to counteract an applied stress (change in concentration, pressure, or temperature). ΔG° = −RT·ln(K); negative ΔG° means K > 1 (products favored).

  32. Define a buffer, give the Henderson-Hasselbalch equation, and state the Nernst-related cell potential sign for spontaneity.

    A buffer resists pH change; it contains a weak acid and its conjugate base. Henderson-Hasselbalch: pH = pKa + log([A⁻]/[HA]). For electrochemistry, a positive cell potential (E°cell > 0) indicates a spontaneous (galvanic) reaction; ΔG = −nFE.

MCAT (Medical College Admission Test) Chemical and Physical Foundations of Biological Systems FAQ

What is in the MCAT (Medical College Admission Test) Chemical and Physical Foundations of Biological Systems syllabus?

MCAT (Medical College Admission Test) Chemical and Physical Foundations of Biological Systems is split into 5 chapters: Mechanics, Energy, and Fluids in Living Systems, Electrostatics, Circuits, and Magnetism, Waves, Sound, Light, and Optics, General Chemistry of Biological Systems and Thermodynamics, Electrochemistry, and Acid-Base Chemistry. Together they contain 17 topics and 45 sub-topics.

How many chapters are in MCAT (Medical College Admission Test) Chemical and Physical Foundations of Biological Systems?

5 chapters, containing 17 topics and 45 sub-topics. The largest chapter is Mechanics, Energy, and Fluids in Living Systems, with 4 topics.

Are there flashcards for MCAT (Medical College Admission Test) Chemical and Physical Foundations of Biological Systems?

Yes — a 52-card Chemical and Physical Foundations of Biological Systems deck, printed in full in the flashcards section of this page and available in the Examius app with spaced repetition. The free plan covers one exam of your choice, including its flashcards; Examius Pro, a one-time purchase, unlocks every other exam and deck.