Fundamentals of Engineering Exam (FE) Chemistry, Biology and Environmental Engineering Syllabus

Chemistry, Biology and Environmental Engineering syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry, Biology and Environmental Engineering in Fundamentals of Engineering Exam (FE), not a summary of it.

1. 1

   General Chemistry

   4 topics

   • Atomic and Molecular Structure
     • Periodic table trends
     • Chemical bonding and nomenclature
   • Stoichiometry and Reactions
     • Balancing equations and mole concept
     • Limiting reagents and yield
     • Oxidation-reduction reactions
   • Solutions and Equilibrium
     • Concentration units and molarity
     • Acids, bases and pH
     • Chemical and ionic equilibrium
   • Thermochemistry and Kinetics
     • Enthalpy and Hess's law
     • Reaction rates and rate laws
2. 2

   Biology and Biochemistry

   3 topics

   • Cell and Molecular Biology
     • Cell structure and function
     • Biomolecules: carbohydrates, lipids, proteins, nucleic acids
   • Microbiology Fundamentals
     • Bacteria, viruses and growth kinetics
     • Metabolism and energy
   • Toxicology and Health
     • Dose-response relationships
     • Exposure pathways and risk
3. 3

   Environmental Engineering

   4 topics

   • Water Quality and Treatment
     • Water quality parameters (BOD, DO, TSS)
     • Coagulation, sedimentation and filtration
     • Disinfection processes
   • Wastewater and Solid Waste
     • Activated sludge and biological treatment
     • Solid and hazardous waste management
   • Air Quality
     • Air pollutants and sources
     • Emission control technologies
   • Mass Balances and Fate
     • Conservation of mass in reactors
     • Contaminant transport and dispersion

Chemistry, Biology and Environmental Engineering flashcards for Fundamentals of Engineering Exam (FE)

22 of 51 cards from the Chemistry, Biology and Environmental Engineering deck — real questions with worked answers.

1. What are the four quantum numbers and what does each specify for an electron in an atom?

   Principal $n$ (energy level/shell size), Azimuthal $l$ (subshell shape, $0$ to $n-1$), Magnetic $m_l$ (orbital orientation, $-l$ to $+l$), and Spin $m_s$ ($\pm\tfrac{1}{2}$). No two electrons in an atom share all four (Pauli exclusion principle).

2. State the formula relating wavelength and energy of a photon, and define each term.

   $$E = h\nu = \frac{hc}{\lambda}$$ where $h$ is Planck's constant ($6.626\times10^{-34}\ \text{J·s}$), $\nu$ is frequency, $c$ is the speed of light, and $\lambda$ is wavelength. Energy is inversely proportional to wavelength.

3. Distinguish ionic, covalent, and metallic bonding.

   Ionic: electrostatic attraction between cations and anions (electron transfer, e.g. $\ce{NaCl}$). Covalent: shared electron pairs between nonmetals (e.g. $\ce{H2O}$). Metallic: positive ion cores in a delocalized 'sea' of electrons, giving conductivity and malleability.

4. What does electronegativity measure, and which element is most electronegative?

   Electronegativity is an atom's tendency to attract bonding electrons. It increases across a period and up a group; fluorine ($\chi \approx 4.0$ on the Pauling scale) is the most electronegative element.

5. Define Avogadro's number and a mole.

   A mole is the amount of substance containing Avogadro's number of entities, $N_A = 6.022\times10^{23}\ \text{mol}^{-1}$. One mole of a substance has a mass in grams equal to its molar mass.

6. How do you balance the combustion of propane $\ce{C3H8}$ in oxygen?

   $$\ce{C3H8 + 5O2 -> 3CO2 + 4H2O}$$ Balance carbon first (3 $\ce{CO2}$), then hydrogen (4 $\ce{H2O}$), then oxygen (10 O atoms on the right require 5 $\ce{O2}$).

7. What is a limiting reactant and how is theoretical yield determined?

   The limiting reactant is the reactant fully consumed first, capping how much product can form. Theoretical yield is computed from the moles of the limiting reactant via the balanced stoichiometric ratios. Percent yield $= \frac{\text{actual}}{\text{theoretical}}\times 100\%$.

8. Classify these reaction types: synthesis, decomposition, single replacement, double replacement, combustion.

   Synthesis: $\ce{A + B -> AB}$. Decomposition: $\ce{AB -> A + B}$. Single replacement: $\ce{A + BC -> AC + B}$. Double replacement: $\ce{AB + CD -> AD + CB}$. Combustion: fuel $+\ \ce{O2} \to \ce{CO2} + \ce{H2O}$ (+ heat).

9. State the ideal gas law and the value of R in SI units.

   $$PV = nRT$$ with $R = 8.314\ \text{J·mol}^{-1}\text{·K}^{-1}$ (or $0.08206\ \text{L·atm·mol}^{-1}\text{·K}^{-1}$). $P$ = pressure, $V$ = volume, $n$ = moles, $T$ = absolute temperature.

10. Define molarity, molality, and normality.

    Molarity $M = \frac{\text{mol solute}}{\text{L solution}}$. Molality $m = \frac{\text{mol solute}}{\text{kg solvent}}$. Normality $N = \frac{\text{equivalents of solute}}{\text{L solution}}$ (equivalents depend on reactive units, e.g. $\ce{H+}$ or electrons).

11. What is the pH formula and the relationship between pH and pOH at 25°C?

    $$\text{pH} = -\log_{10}[\ce{H+}]$$ and $\text{pH} + \text{pOH} = 14$ at 25°C, since $K_w = [\ce{H+}][\ce{OH-}] = 1.0\times10^{-14}$.

12. State Le Chatelier's principle.

    If a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the equilibrium shifts in the direction that partially counteracts the disturbance to re-establish equilibrium.

13. Write the equilibrium constant expression for $\ce{aA + bB <=> cC + dD}$.

    $$K = \frac{[\ce{C}]^{c}[\ce{D}]^{d}}{[\ce{A}]^{a}[\ce{B}]^{b}}$$ Pure solids and liquids are omitted. $K>1$ favors products; $K<1$ favors reactants.

14. What is the solubility product $K_{sp}$ for $\ce{Ca(OH)2}$ dissolving in water?

    For $\ce{Ca(OH)2 -> Ca^2+ + 2OH-}$: $$K_{sp} = [\ce{Ca^2+}][\ce{OH-}]^{2}$$ If solubility is $s$, then $K_{sp} = (s)(2s)^2 = 4s^3$.

15. How does a buffer work, and what is the Henderson–Hasselbalch equation?

    A buffer resists pH change using a weak acid and its conjugate base, which neutralize added acid or base. $$\text{pH} = \text{p}K_a + \log\frac{[\text{A}^-]}{[\text{HA}]}$$

16. Differentiate enthalpy, entropy, and Gibbs free energy.

    Enthalpy $H$: heat content at constant pressure. Entropy $S$: measure of disorder/dispersal of energy. Gibbs free energy $G$: $G = H - TS$; $\Delta G < 0$ indicates a spontaneous process.

17. State the Gibbs free energy equation and the spontaneity criteria.

    $$\Delta G = \Delta H - T\Delta S$$ $\Delta G < 0$: spontaneous; $\Delta G = 0$: equilibrium; $\Delta G > 0$: nonspontaneous. Also $\Delta G = -RT\ln K$.

18. State Hess's law.

    The total enthalpy change of a reaction is independent of the pathway taken and equals the sum of the enthalpy changes of the individual steps: $$\Delta H_{rxn} = \sum \Delta H_{steps}$$ Reactions can be added/reversed/scaled with their $\Delta H$.

19. What is the Arrhenius equation and what does it describe?

    $$k = A\,e^{-E_a/RT}$$ It relates the rate constant $k$ to activation energy $E_a$, temperature $T$, and pre-exponential factor $A$. Higher temperature or lower $E_a$ increases the rate.

20. Define reaction order and give the integrated rate law for a first-order reaction.

    Reaction order is the exponent on a reactant's concentration in the rate law. First-order: rate $= k[\text{A}]$, integrated form $$\ln[\text{A}] = \ln[\text{A}]_0 - kt$$ with half-life $t_{1/2} = \frac{0.693}{k}$ (independent of concentration).

21. How does a catalyst affect a reaction?

    A catalyst lowers the activation energy $E_a$ by providing an alternative pathway, speeding both forward and reverse rates equally. It is not consumed and does not change $\Delta G$, $\Delta H$, or the equilibrium position.

22. Contrast prokaryotic and eukaryotic cells.

    Prokaryotes (bacteria, archaea): no membrane-bound nucleus or organelles, circular DNA, smaller. Eukaryotes (plants, animals, fungi, protists): true nucleus, membrane-bound organelles (mitochondria, ER), linear chromosomes, generally larger.

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