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TU B.Sc. First Year Syllabus: Chemistry
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TU B.Sc. First Year Chemistry (Chem. 101) — Complete Syllabus Overview

Chemistry is one of the major subjects offered under the Four-Year Bachelor of Science (B.Sc.) programme of Tribhuvan University’s Institute of Science and Technology (IoST), Kirtipur, Kathmandu. The First Year Chemistry course, officially titled Basic Chemistry I (Course No. Chem. 101), is a 100-mark theory paper accompanied by a 50-mark practical paper (Chem. 102), making the combined First Year Chemistry assessment worth 150 marks. The syllabus was last revised in 2073 BS (2016) and has been in effect since the 2073 admission batch.

The course is organized into three major branches of chemistry — Inorganic Chemistry, Organic Chemistry, and Physical Chemistry — with equal emphasis on theory and laboratory work. It is a foundational course for students planning to major in Chemistry, and also serves as a minor subject for students of Physics, Microbiology, Environmental Science, and other science disciplines.

Subject Information at a Glance

  • Course Title: Basic Chemistry I
  • Course No.: Chem. 101 (Theory) | Chem. 102 (Practical)
  • Year: First Year — Four Year B.Sc. Programme
  • Full Marks: 100 (Theory) + 50 (Practical) = 150 total
  • Pass Marks: 35 (Theory) | 20 (Practical) — both must be passed separately
  • Theory Structure: Three equal sections — Inorganic Chemistry, Organic Chemistry, Physical Chemistry
  • Examination: Annual (end-of-year exam conducted by IoST, TU)
  • Conducting Institution: Institute of Science and Technology (IoST), Tribhuvan University
  • Curriculum Version: Revised Course of Study 2073 BS (2016)

Why Chemistry at TU B.Sc. Level?

Chemistry has been taught at the bachelor’s level in Nepal since 1947, when Tri-Chandra College upgraded the subject from the Intermediate of Science (I.Sc.) level — making it one of the oldest science disciplines in Nepali higher education. At TU B.Sc. level, Chemistry provides the rigorous theoretical and experimental foundation required for advanced studies in pure chemistry, pharmaceutical sciences, environmental chemistry, materials science, biotechnology, forensic science, and chemical engineering. The four-year TU B.Sc. Chemistry programme progresses systematically from foundational principles in First Year through advanced inorganic, organic, physical, analytical, and applied chemistry in later years, culminating in a final-year research project.

The First Year course is specifically designed to bridge the gap between NEB Grade 12 Chemistry and university-level chemical science. Students encounter quantum mechanical treatments of atomic structure, stereochemical analysis of organic molecules, mechanistic approaches to organic reactions, and rigorous thermodynamic and kinetic treatments of physical chemistry — all at a depth and mathematical sophistication significantly beyond the +2 curriculum. Laboratory work in Chem. 102 develops practical skills in quantitative analysis, organic synthesis, and identification that are directly relevant to careers in analytical chemistry, quality control, research, and teaching.

Chem. 101 Theory Syllabus — Topic-wise Detail

SECTION A: INORGANIC CHEMISTRY

Topic 1: Atomic Structure

  • Review of Bohr’s atomic model: successes and limitations
  • Wave-particle duality: de Broglie’s equation, Heisenberg’s uncertainty principle
  • Schrödinger’s wave equation (time-independent): derivation concept, physical significance of wave function (ψ), probability density (ψ²)
  • Probability density patterns for hydrogen atom: radial and angular wave functions, radial distribution curves
  • Shapes of s, p, and d orbitals: charge cloud diagrams, boundary surface diagrams, nodal planes
  • Quantum numbers: principal (n), azimuthal (l), magnetic (mₗ), spin (ms) — physical significance and allowed values
  • Multi-electron atoms: electron-electron repulsion, screening (shielding) effect, effective nuclear charge, Slater’s rules
  • Electronic configuration: Aufbau principle, Pauli’s exclusion principle, Hund’s rule; stability of completely filled, half-filled, and empty orbitals

Topic 2: Nuclear Chemistry

  • Atomic nucleus: composition, nuclear forces, nuclear binding energy, mass defect, Einstein’s mass-energy relation (E = mc²)
  • Nuclear stability: n/p ratio, belt of stability, magic numbers
  • Radioactivity: natural and artificial; types of radioactive decay (alpha, beta, gamma); decay kinetics — rate of decay, decay constant, half-life, mean life
  • Group displacement law (radioactive displacement law): alpha and beta disintegration series
  • Radioactive equilibrium: secular and transient equilibrium
  • Nuclear reactions: nuclear fission and fusion; chain reactions; nuclear reactor design (thermal reactors, moderators, control rods, coolants)
  • Applications of radioactivity: radiocarbon dating, nuclear medicine, radiation therapy, tracer technique

Topic 3: Periodic Classification of Elements and Physical Properties

  • Development of periodic table: Mendeleev’s periodic law, modern periodic law, IUPAC classification
  • Long form of periodic table: blocks (s, p, d, f), periods, groups
  • Periodic trends — atomic and ionic radii, ionization energy (successive ionization energies), electron affinity, electronegativity (Pauling, Mulliken, Allred-Rochow scales), melting and boiling points, oxidation states
  • Detailed discussion of periodicity across periods and down groups for s-, p-, d-, and f-block elements
  • Effective nuclear charge and its role in periodic properties

Topic 4: Chemical Bonding

  • Ionic bonding: formation, lattice energy, Born-Haber cycle, Fajan’s rules and polarizing power
  • Covalent bond: Lewis structure, valence bond theory (VBT) — orbital overlap, hybridization (sp, sp², sp³, sp³d, sp³d², sp³d³)
  • VSEPR theory: prediction of molecular geometry (linear, bent, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral, T-shaped, seesaw, square pyramidal, square planar)
  • Molecular orbital theory (MOT): bonding and antibonding MOs, LCAO method, MO energy level diagrams for homonuclear diatomic molecules (H₂ through Ne₂) and heteronuclear diatomics (NO, CO, HF); bond order calculation, magnetic properties
  • Metallic bonding: electron sea model, band theory concept
  • Intermolecular forces: van der Waals forces (dipole-dipole, dipole-induced dipole, London/dispersion forces), hydrogen bonding — types, conditions, effects on physical properties

Topic 5: Covalent Bond (Advanced)

  • Resonance: concept, resonance structures, resonance energy, conditions for resonance; examples — benzene, carbonate, nitrate, ozone
  • Dipole moment: definition, measurement, bond dipole vs. molecular dipole; use in determining molecular geometry and bond polarity; dipole moments of polyatomic molecules
  • Back bonding (π-bonding involving d-orbitals): conditions, examples (BF₃, SiF₄, PCl₃)
  • Bond parameters: bond length, bond energy (dissociation energy, mean bond energy), bond angle — variation with hybridization, electronegativity, and lone pairs

Topic 6: Acids and Bases

  • Arrhenius theory: limitations
  • Brønsted-Lowry theory: conjugate acid-base pairs, amphoteric species
  • Lewis theory: Lewis acids and bases, hard and soft acid-base (HSAB) principle — classification, applications in predicting reaction products and stability of complexes
  • Lux-Flood concept: oxoacid-base reactions
  • Strength of acids and bases: Ka and Kb, pKa and pKb, relationship between Ka and Kb for conjugate pairs
  • Acid-base equilibria in water: pH calculation for strong acids/bases, weak acids/bases (using approximation and exact methods), buffers (Henderson-Hasselbalch equation), hydrolysis of salts

Topic 7: Principles of Qualitative and Quantitative Analysis

  • Systematic qualitative inorganic analysis: general approach, separation of cation groups (Groups I–VI) by selective precipitation, anion analysis (Group A and Group B anions)
  • Principles behind group separations: solubility products, common ion effect, pH control
  • Introduction to quantitative analysis: volumetric analysis (acid-base, redox, precipitation, complexometric titrations), gravimetric analysis (precipitation gravimetry, volatilization)
  • Concentration expressions: molarity, normality, molality, mole fraction, weight/weight%, weight/volume%
  • Standardization of solutions: primary standards, secondary standards

SECTION B: ORGANIC CHEMISTRY

Topic 8: Structure and Properties

  • Hybridization: sp³, sp², sp carbon; bond lengths and bond angles in organic molecules
  • Electronic effects: inductive effect (I-effect), mesomeric/resonance effect (M-effect or R-effect), electromeric effect, hyperconjugation — definitions, examples, and effect on stability and reactivity
  • Homolytic and heterolytic bond fission: carbocations, carbanions, free radicals, carbenes — structure, stability, and reactivity
  • Reaction intermediates: comparison of stability and reactivity; rearrangements (1,2-hydride shift, 1,2-alkyl shift)
  • Aromaticity: Hückel’s rule (4n+2 π electrons), aromatic, antiaromatic, non-aromatic compounds; examples beyond benzene

Topic 9: Alkanes

  • IUPAC nomenclature: branched and unbranched alkanes, cycloalkanes
  • Conformational analysis: Newman projections for ethane (staggered, eclipsed) and butane (anti, gauche, eclipsed), energy diagrams, conformational stability
  • Sources of alkanes: natural gas, petroleum (fractional distillation, cracking, reforming)
  • Industrial synthesis: Fischer-Tropsch synthesis
  • Reactions of alkanes: combustion (complete and incomplete), halogenation (free radical mechanism — initiation, propagation, termination; reactivity order, selectivity); pyrolysis

Topic 10: Stereochemistry

  • Types of isomerism: constitutional (structural) isomers, stereoisomers — enantiomers and diastereomers
  • Chirality: chiral and achiral molecules, chiral centre (stereocentre), asymmetric carbon
  • Configuration: R/S designation (Cahn-Ingold-Prelog priority rules); D/L designation (Fischer convention)
  • Optical activity: polarimetry, specific rotation, enantiomers, racemic mixture, racemization
  • Meso compounds: definition, properties, superimposability
  • Geometric isomerism: cis-trans (E/Z) in alkenes and cyclic compounds; E/Z designation by CIP rules
  • Diastereomers: erythro/threo designation; multiple stereocentres — maximum number of stereoisomers (2ⁿ rule)
  • Conformational isomers vs. configurational isomers

Topic 11: Alkyl Halides — Nucleophilic Substitution

  • Classification of alkyl halides: primary, secondary, tertiary; vinyl, allyl, benzyl
  • Methods of preparation: from alcohols (SOCl₂, PCl₃, PCl₅, HX), from alkanes (halogenation), from alkenes (HX addition, X₂ addition), Hunsdiecker reaction
  • Physical properties: boiling points, solubility, dipole moments
  • Nucleophilic substitution reactions:
    • SN2 mechanism: bimolecular, transition state, inversion of configuration (Walden inversion), stereochemistry, factors affecting rate (substrate structure, nucleophile strength, leaving group ability, solvent)
    • SN1 mechanism: unimolecular, carbocation intermediate, racemization, stability of carbocations, factors affecting rate (substrate, solvent, leaving group)
    • Comparison of SN1 and SN2: substrate, solvent, and nucleophile effects
  • Elimination reactions: E1 and E2 mechanisms, Saytzeff rule, competition between substitution and elimination

Topic 12: Alcohols and Ethers

  • Classification and nomenclature: primary, secondary, tertiary alcohols; IUPAC names; common names
  • Preparation: hydration of alkenes (acid-catalyzed), from carbonyl compounds (reduction), Grignard reaction, from alkyl halides (SN2)
  • Physical properties: hydrogen bonding, boiling points, solubility
  • Reactions of alcohols: acid-base behavior, with HX (Lucas test, mechanism), with SOCl₂ and PCl₃/PCl₅, with Na/K, oxidation (Jones’ reagent, PCC, KMnO₄, K₂Cr₂O₇ — product control by alcohol class), dehydration (mechanism, Saytzeff rule, carbocation rearrangements)
  • Diols (glycols): preparation, pinacol-pinacolone rearrangement, periodic acid oxidation of vicinal diols
  • Nomenclature and preparation of ethers: Williamson’s synthesis, acid-catalyzed addition of alcohols to alkenes
  • Reactions of ethers: cleavage by HI and HBr, epoxide ring opening (under acidic and basic conditions — regiochemistry and stereochemistry)

Topic 13: Alkenes

  • Structure and nomenclature: double bond geometry, IUPAC and E/Z naming
  • Preparation: dehydration of alcohols, dehydrohalogenation (E2), Wittig reaction (introduction)
  • Physical properties
  • Reactions of alkenes:
    • Electrophilic addition: HX addition (Markovnikov’s rule, anti-Markovnikov — peroxide effect/free radical addition), X₂ addition (anti addition, bromonium ion mechanism, halohydrin formation), H₂O addition (acid-catalyzed), H₂SO₄ addition
    • Carbene additions: Simmons-Smith reaction (introduction)
    • Oxidative reactions: KMnO₄ (cold dilute — syn dihydroxylation; hot concentrated — oxidative cleavage), OsO₄, ozonolysis (reductive and oxidative workup)
    • Epoxidation: mCPBA, ring-opening reactions

Topic 14: Alkynes

  • Structure and nomenclature: sp hybridization, linear geometry, IUPAC names
  • Preparation: dehydrohalogenation of geminal and vicinal dihalides; from calcium carbide
  • Acidity: terminal alkynes as weak acids; sodium acetylide and lithium acetylide as nucleophiles (alkylation of alkynes)
  • Reactions of alkynes:
    • Electrophilic addition: HX addition (Markovnikov, syn and anti), X₂ addition, hydration (Markovnikov — Kucherov reaction giving ketones; anti-Markovnikov — hydroboration-oxidation giving aldehydes)
    • Reduction: catalytic hydrogenation (Lindlar’s catalyst — cis alkene; Na/liq.NH₃ — trans alkene); reduction by dissolving metal
    • Oxidative cleavage: KMnO₄, ozonolysis
    • Cycloaddition: Diels-Alder reaction (introduction)

SECTION C: PHYSICAL CHEMISTRY

Topic 15: Gaseous State

  • Kinetic molecular theory of gases: assumptions, derivation of kinetic gas equation PV = ⅓mnu̅², derivation of gas laws from kinetic theory
  • Molecular speeds: root mean square speed (u_rms), average speed (ū), most probable speed (u_mp) — derivation, comparison, temperature dependence
  • Maxwell-Boltzmann distribution of molecular speeds: graphical representation, effect of temperature
  • Real gases: deviation from ideal behavior, van der Waals equation — significance of constants a and b, derivation, Boyle temperature
  • Compressibility factor (Z): graphical interpretation for different gases; Joule-Thomson effect and inversion temperature; liquefaction of gases

Topic 16: Liquid and Solid States

  • Liquid state: structure, properties — surface tension (measurement by capillary rise, drop weight method), viscosity (Poiseuille’s equation, Stokes’ law), measurement of viscosity (Ostwald viscometer)
  • Vapour pressure: definition, measurement, effect of temperature; Clausius-Clapeyron equation and its applications (calculation of enthalpy of vaporization, boiling point at different pressures)
  • Solid state: types of solids (crystalline and amorphous), unit cells, crystal systems (7 crystal systems, 14 Bravais lattices), coordination number
  • Close packing in crystals: 2D hexagonal close packing, 3D hexagonal close packing (hcp) and cubic close packing (ccp/fcc), body-centred cubic (bcc) — packing efficiency, number of atoms per unit cell
  • Ionic crystal structures: NaCl (rock salt), ZnS (zinc blende), CsCl — coordination numbers and structure derivation
  • Bragg’s law: X-ray diffraction, derivation, applications in determining crystal structure

Topic 17: Chemical and Ionic Equilibrium

  • Law of mass action and equilibrium constant: Kc and Kp, relationship between Kc and Kp (Kp = Kc(RT)^Δn)
  • Le Chatelier’s principle: effect of concentration, pressure, temperature, and catalyst on equilibrium; industrial applications (Haber’s process, Contact process)
  • Degree of dissociation: calculation of Kc from degree of dissociation and vice versa
  • Ionic equilibrium: Ostwald’s dilution law, Arrhenius theory of electrolytic dissociation
  • Acid-base equilibria: Ka and Kb, pKa and pKb, relative strengths of acids and bases; buffer solutions (acidic and basic buffers, Henderson-Hasselbalch equation, buffer capacity)
  • Solubility product (Ksp): definition, calculation of solubility from Ksp and Ksp from solubility; common ion effect on solubility; precipitation reactions and conditions for precipitation

Topic 18: Colligative Properties

  • Definition and characteristics: colligative properties depend on number of solute particles, not nature
  • Relative lowering of vapour pressure: Raoult’s law (ideal solutions), derivation of Raoult’s law for dilute solutions, determination of molar mass
  • Elevation of boiling point: derivation, ebullioscopic constant (Kb), determination of molar mass
  • Depression of freezing point: derivation, cryoscopic constant (Kf), determination of molar mass; applications (antifreeze, road salting)
  • Osmotic pressure: van’t Hoff equation (π = MRT), measurement, applications (osmometry, reverse osmosis)
  • Abnormal molar masses: van’t Hoff factor (i), cases of association (acetic acid in benzene) and dissociation (electrolytes in water); modified colligative property equations using i

Topic 19: Chemical Kinetics

  • Rate of reaction: instantaneous rate, average rate; rate in terms of concentration of reactants and products
  • Rate law and order of reaction: rate constant, molecularity vs. order; zero, first, second, and nth order reactions
  • Integrated rate laws: zero order (derivation, t₁/₂), first order (derivation, t₁/₂, half-life independence of concentration), second order (derivation)
  • Methods of determining order: initial rate method, integrated rate law method, half-life method
  • Temperature dependence of rate constant: Arrhenius equation (k = Ae^(-Ea/RT)), derivation of activation energy from temperature-rate data; Arrhenius plot
  • Theories of reaction rates: collision theory (derivation of rate constant, steric factor, activation energy), transition state theory (activated complex, energy profile diagram, relationship to thermodynamics)
  • Mechanisms: elementary reactions, rate-determining step, consecutive and parallel reactions (introduction)

Topic 20: Thermodynamics and Thermochemistry

  • Review and extension of thermodynamic terms: system, surroundings, state functions, extensive and intensive properties, reversible and irreversible processes
  • First Law of Thermodynamics: internal energy (E), enthalpy (H), relationship ΔH = ΔE + PΔV = ΔE + ΔnRT
  • Heat capacities: Cp and Cv, derivation of Cp − Cv = R for ideal gases; Kirchhoff’s equation (variation of ΔH with temperature)
  • Thermochemistry: standard enthalpy of formation, combustion, neutralization, solution, and atomization; Hess’s law; bond energies and enthalpy calculation
  • Experimental measurement: bomb calorimeter (determination of ΔE for combustion), calorific value of food and fuels
  • Isothermal processes: reversible and irreversible expansion of ideal gas — work done, heat absorbed, ΔE
  • Entropy (S): concept, ΔS for reversible and irreversible processes, ΔS for isothermal expansion, entropy and disorder
  • Second Law of Thermodynamics: statements, Carnot cycle and efficiency, entropy change of universe
  • Gibbs free energy (G): definition ΔG = ΔH − TΔS, standard Gibbs free energy change, criterion for spontaneity; relationship between ΔG° and equilibrium constant K

Chem. 102 Practical Syllabus (50 Marks)

A. Qualitative Inorganic Analysis

  • Systematic identification of cations: Groups I–VI (Pb²⁺, Cu²⁺, Hg²⁺, Al³⁺, Fe³⁺, Cr³⁺, Mn²⁺, Co²⁺, Ni²⁺, Zn²⁺, Ba²⁺, Ca²⁺, Mg²⁺, Na⁺, K⁺, NH₄⁺) using group reagents and confirmatory tests
  • Systematic identification of anions: Group A and Group B anions (CO₃²⁻, S²⁻, SO₃²⁻, NO₂⁻, Cl⁻, Br⁻, I⁻, SO₄²⁻, NO₃⁻, PO₄³⁻) using preliminary tests (dil. H₂SO₄ and conc. H₂SO₄), Group A tests (volatile acid anions), and Group B tests
  • Mixed salt analysis (two cations + two anions) within the same salt mixture

B. Quantitative Inorganic Analysis (Volumetric)

  • Acid-base titrations: standardization of NaOH with oxalic acid; standardization of HCl with Na₂CO₃; determination of acidity/alkalinity of given samples; determination of total alkalinity and phenolphthalein alkalinity
  • Redox titrations: standardization of KMnO₄ with sodium oxalate; determination of Fe²⁺ and Fe³⁺ in a mixture using KMnO₄; determination of hardness of water by EDTA method (complexometric titration)
  • Precipitation titration: determination of Cl⁻ by Mohr’s method (argentometry)

C. Organic Chemistry Practicals

  • Determination of melting point (by capillary tube method) and boiling point of organic compounds
  • Qualitative identification of organic functional groups: unsaturation, alcohols (primary, secondary, tertiary by Lucas test), aldehydes and ketones (Tollens’, Fehling’s, Brady’s 2,4-DNP), carboxylic acids, amines (primary aromatic by diazonium coupling)
  • Recrystallization and determination of melting point of purified compounds
  • Thin layer chromatography (TLC): separation of organic mixtures, calculation of Rf values

Recommended Textbooks and References

Inorganic Chemistry

  • Huheey, J.E., Keiter, E.A. and Keiter, R.L. Inorganic Chemistry: Principles of Structure and Reactivity. Addison Wesley Publishing House
  • Cotton, F.A. and Wilkinson, G. Advanced Inorganic Chemistry. Wiley-Interscience, New York
  • Bhagi, A.K. and Chatwal, G.R. Bioinorganic and Supramolecular Chemistry. Himalaya Publishing House, Mumbai
  • Chaudhary, N. A Textbook of B.Sc. Chemistry (Vol. I & II), 2nd Edition. Ekta Books Nepal (recommended for Nepali students)

Organic Chemistry

  • Morrison, R.T. and Boyd, R.N. Organic Chemistry. Prentice Hall (standard reference for TU B.Sc. Organic Chemistry)
  • Clayden, J., Greeves, N. and Warren, S. Organic Chemistry. Oxford University Press
  • Finar, I.L. Organic Chemistry, Vols I and II. Longman, UK
  • March, J. Advanced Organic Chemistry: Reactions, Mechanisms and Structure. Wiley-Interscience

Physical Chemistry

  • Atkins, P.W. and de Paula, J. Physical Chemistry. Oxford University Press
  • Castellan, G.W. Physical Chemistry. Addison-Wesley
  • Kapoor, K.L. A Textbook of Physical Chemistry, Vols 1–5. Macmillan India
  • Engel, T. and Reid, P. Physical Chemistry. Pearson/Benjamin Cummings

Practical Chemistry

  • Vogel, A.I. A Text Book of Quantitative Inorganic Analysis. ELBS and Longman
  • Vogel, A.I. A Text Book of Qualitative Inorganic Analysis. ELBS and Longman
  • Shriner, R.L., Fusion, R.C. and Curtin, D.Y. The Systematic Identification of Organic Compounds. John Wiley and Sons

Difference Between NEB Grade 12 and TU B.Sc. First Year Chemistry

Students entering TU B.Sc. First Year from NEB Grade 12 Chemistry will notice an immediate step-up in both depth and mathematical treatment. While Grade 12 Chemistry covered atomic structure through the Bohr model, TU First Year introduces the Schrödinger wave equation, quantum numbers, radial and angular wave functions, and orbital shapes derived from wave mechanics. Organic Chemistry at Grade 12 covered reactions and functional groups descriptively; TU First Year introduces formal mechanistic reasoning — SN1, SN2, E1, E2 mechanisms with stereochemical outcomes, carbocation rearrangements, and reaction selectivity explained through electronic effects. Physical Chemistry at Grade 12 introduced gas laws and thermodynamics qualitatively; TU First Year derives Maxwell-Boltzmann distribution, derives van der Waals equation, proves Clausius-Clapeyron equation, and derives Gibbs free energy relationships from first principles.

Tips to Succeed in TU B.Sc. First Year Chemistry

  • Build mechanistic reasoning from the start: TU B.Sc. Organic Chemistry is fundamentally mechanistic — every reaction must be understood through electron movement (curved arrow notation), intermediate stability, and transition state arguments. Students who memorize reactions without understanding the mechanism struggle in Second Year and beyond. Invest time early in mastering electronic effects (inductive, mesomeric, hyperconjugation) and reaction intermediates before attempting each reaction class.
  • Master the integration between the three branches: Many examination questions require synthesis of ideas from multiple branches — for example, thermodynamic stability of ionic vs. covalent bonds (Inorganic + Physical), rate constants and their temperature dependence in the context of reaction mechanism (Organic + Physical), or solubility product and common ion effect applied to qualitative analysis (Inorganic + Physical). Practice connecting concepts across branches during revision.
  • Physical Chemistry requires daily mathematical practice: The Thermodynamics, Kinetics, and Colligative Properties units involve multi-step derivations and numerical calculations. Work through at least 3–5 numerical problems per unit per day. Focus especially on: Kirchhoff’s equation, van’t Hoff equation for osmotic pressure, integrated rate laws, Arrhenius equation calculations, and Clausius-Clapeyron equation applications.
  • For Inorganic Chemistry, understand the ‘why’ behind periodic trends: Rote memorization of trends is insufficient at university level. Understand why ionization energy has exceptions (B < Be, O < N), why Fajan’s rules determine ionic/covalent character, why HSAB principle predicts soft-soft and hard-hard interactions, and why the band theory explains conductivity differences between metals, semiconductors, and insulators.
  • Attend all practical sessions and maintain a clean lab notebook: The 50-mark practical exam directly tests your ability to perform systematic qualitative analysis (cation and anion identification), titrations (standardization and unknown determination), and organic functional group tests. These skills can only be developed through repeated hands-on practice — not from reading descriptions.
  • Use Morrison and Boyd as your primary Organic Chemistry reference: This standard text is the most widely used Organic Chemistry resource in TU B.Sc. programmes across Nepal and aligns closely with the TU First Year syllabus. For Nepali-specific supplementary material, Chaudhary’s Textbook of B.Sc. Chemistry (Ekta Books Nepal) is widely available and useful.
  • Review NEB Grade 12 Chemistry thoroughly before the first semester begins: TU B.Sc. Chemistry assumes complete fluency with the NEB curriculum. Areas such as organic nomenclature, basic organic reactions, gas laws, ionic equilibrium, acid-base concepts, and electrochemistry should be confidently revisited before university classes begin, since TU lectures build immediately on this foundation without review.

Frequently Asked Questions (FAQs)

What is the course code for TU B.Sc. First Year Chemistry?

The theory paper is Chem. 101 (Basic Chemistry I), carrying 100 marks with a pass mark of 35. The practical paper is Chem. 102, carrying 50 marks with a pass mark of 20. Both must be passed independently — failing one while passing the other does not result in an overall pass.

How is TU B.Sc. First Year Chemistry structured?

The theory paper (Chem. 101) is divided into three equal sections: Inorganic Chemistry, Organic Chemistry, and Physical Chemistry. Each section carries approximately equal weightage. The practical paper (Chem. 102) covers qualitative and quantitative inorganic analysis and organic functional group identification and is assessed in a separate practical examination.

How many topics are covered in Inorganic, Organic, and Physical Chemistry?

Inorganic Chemistry covers 7 major topics: Atomic Structure, Nuclear Chemistry, Periodic Classification, Chemical Bonding, Covalent Bond (Advanced), Acids and Bases, and Principles of Qualitative and Quantitative Analysis. Organic Chemistry covers 7 topics: Structure and Properties, Alkanes, Stereochemistry, Alkyl Halides (Nucleophilic Substitution), Alcohols and Ethers, Alkenes, and Alkynes. Physical Chemistry covers 6 topics: Gaseous State, Liquid and Solid States, Chemical and Ionic Equilibrium, Colligative Properties, Chemical Kinetics, and Thermodynamics and Thermochemistry.

What is the examination pattern for TU B.Sc. First Year Chemistry?

TU B.Sc. uses an annual examination system — both theory (Chem. 101, 100 marks) and practical (Chem. 102, 50 marks) exams are held at the end of the academic year by the IoST Examination Control Office. Both must be passed separately (theory pass mark: 35; practical pass mark: 20). The theory exam is 3 hours and the practical exam is a full-day (6-hour) session.

When was the current TU B.Sc. First Year Chemistry syllabus introduced?

The current syllabus is the Revised Course of Study 2073 BS (2016), developed by the Institute of Science and Technology (IoST), Tribhuvan University. It has been in effect since the 2073 BS admission batch. Chemistry has been taught at TU since 1947, making it one of the oldest university-level science subjects in Nepal.

Which textbook is most recommended for TU B.Sc. First Year Organic Chemistry?

Morrison and Boyd’s Organic Chemistry (Prentice Hall) is the most widely recommended and used text for TU B.Sc. Organic Chemistry. For supplementary Nepali-context material, Chaudhary’s A Textbook of B.Sc. Chemistry (Ekta Books Nepal) is widely available across Nepal.

Where can I find Chemistry notes and past papers for TU B.Sc. First Year?

You can find study resources on nneducation.com. The official Chem. 101 syllabus PDF is also embedded at the top of this page. For past papers, the IoST TU official website (tuiost.edu.np) publishes previous year question papers; Bidhya Mandir and EducateNepal also maintain collections of past TU B.Sc. First Year Chemistry question papers.

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