CTEVT diploma in Engineering chemistry syllabus(course) :

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CTEVT diploma in engineering  first year (first and second semester) chemistry syllabus(course):  Complete note of diploma in engineering  is also available in this website.

 CTEVT diploma in engineering syllabus

First Semester : 45 teaching hours

Unit-1: Language of chemistry:  4 hrs

  1.1 Symbol:

  • Definition
  • Significance (qualitative and quantitative).

 1.2 Formula:

  • Definition
  • Significance (qualitative and quantitative)
  • Concept of valency in terms of combining capacity with H2, O2, and Cl2
  • Variable valency (ref. Fe, Sn, Pb, Cu, Hg, S and N)
  • Radicals (electro- positive and electro – negative)
  • Writing a formula.

 1.3 Chemical equation:

  • Definition
  • Types requisites
  • Significance and limitation
  • Balancing of chemical equation by hit and trial method and Partial equation method.
Unit: 2: General chemistry: 8 hrs

2.1 Atom and molecule:

  • Definition
  • Dalton’s atomic theory and modern position of the theory.

2.2 Atomic weight:

  • Definition
  • Determination of atomic weight by Dulong and Petit’s method and Related numerical problems.

2.3 Molecular Weight:

  • Definition
  • Avogadro’s hypothesis
  • Application of Avogadro’s hypotheses ( Mol. Wt=2×V.D., in the deduction of atomicity of elementary gases H2 , Cl2, O2, and N2)
  • Molecular weight determination by Victor Meyer’s method and Related numerical problems.

2.4 Equivalent weight:

  • Definition
  • Equivalent weight of element, acid, base and salt
  • Equivalent weight determination by hydrogen displacement method and oxide method.
  • Numerical relation between equivalent weight, atomic weight and valency
  • Some related problems of equivalent wt. (From Hydrogen displacement method and oxide method).

2.5 Simple mole concept:

  • Mole of an atom
  • Mole of a molecule
  • Molar volume and
  • Simple calculation on mole concept.
Unit – 3: System of classification: 33 hrs.

3.1 Acid, Base and Salt:

  • Arrhenius concept of acid and base
  • Lowry and Bronsted concept of acid and base
  • Conjugate acid and base
  • Amphoteric nature of water
  • Lewis concept of acid and base
  • Properties of acid and base.
  • Definition of Salt
  • Types of salt (normal, acidic and basic)
  • Concept of hydrogen ion concentration, pH value and pH Scale
  • Buffer solution.

3.2 Volumetric analysis:

  • Definition of titration (acidimetry and alkalimetry),
  • Indicator
  • End-point (neutralization point)
  • Standard solution (primary and secondary standard solution), Normal, Decinormal, Molar, Molal solution
  • Requisites of primary standard substance
  • Volumetric equation,
  • Express the strength of solution Normality, Molarity, Molality, gram per litre and percentage and related numerical problems.

3.3 Periodic table:

  • Mendeleev’s periodic law
  • Mendeleev’s periodic table
  • Characteristics of groups and periods in the table
  • Advantages and anomalies of the periodic table
  • Modern periodic law.

3.4 Electronic theory valency:

  • Assumptions
  • Types
  • Electrovalency eg. NaCl, MgO, CaS
  • Covalency eg. H2, O2, N2, CH4, H2O, NH3, C2H2
  • Coordinate co-valency eg.H2O2, SO2, O3, SO3)
  • Electronic dot structure of some compounds eg.H2SO4, CaCO3, K2SO3

3.5 Electrolysis:

  • Definition of electrolyte, non-electrolyte and electrolysis
  • Faraday laws of electrolysis,
  • Application of electrolysis (electroplating and electro refining)
  • Electrolysis of acidulated water.

3.6 Oxidation and reduction:

  • Classical definition
  • Electronic interpretation
  • Oxidizing agent: Definition and eg O2, O3, oxyacids, halogens, K2Cr2O7, KMnO4
  • Reducing agent: Definition and eg. H2, H2S with some examples,
  • auto-oxidation eg.H2O2, HNO2, SO2
  • Idea of oxidation number
  • Balancing chemical equation by oxidation number method.

3.7 Atomic structure :

  • Subatomic particles (electron, proton and neutron)
  • Classical α – rays scattering experiment
  • Rutherford’s atomic model and its drawbacks
  • Bohr’s atomic model (postulates only)
  • Composition of nucleus
  • Mass number and atomic number
  • Isotopes and isobar
  • Arrangement of electron (Bohr – Bury Scheme)
  • Concept of shell and sub shell,
  • Electronic Configuration and atomic structure of Some elements (Atomic no. 1 to 30)
  • Hund’s rule
  • General idea of quantum number and Pauli’s exclusion principle.

3.8 Corrosion:

  • Definition
  • Types
  • Direct and indirect method and prevention against corrosion.

3.9 Activity and electrochemical series:

  • Definition
  • Action of water, acid and oxygen on metals.

Second Semester : 45 teaching hours

Unit- 1: Non-metals and their compounds: 20 hrs.

 1. Water:

  • Source of water
  • Hard and soft water
  • Removal of temporary and permanent hardness of water
  • Water treatment of domestic and industrial purpose

 2. Ammonia:

  • Lab preparation
  • Manufacture by Haber’s process
  • Properties and uses

 3. Nitric acid:

  • Manufacture by Ostwald’s process
  • Properties and uses.
  • Nitrogen cycle
  • Fixation of Nitrogen
  • Chemical fertilizers
  • Oxides of nitrogen as pollutant (general concept)
  • Acid rain (due to oxides of nitrogen and oxide of Sulphur “Sulphur dioxide”)

 4. Halogens (Chlorine): Lab preparation, Properties and uses.

 5. Hydrochloric acid: Lab preparation, Properties and uses.

 6. Hydrogen Sulphide: Lab preparation, Properties and uses.

 7. Sulphuric acid: Manufacture by contact process, Properties and uses.

 8. Carbon and its compounds:

  • Allotropes of carbon (reference of diamond & graphite & their structure).
  • Oxides of carbon (Ref. carbon dioxide & carbon mono oxide as pollutants)- general idea only.
Unit: 2: Metals and their compounds: 15 hrs.

2.1 General study of metals and their components:

  • Difference between metal and non metal
  • Combined & free state of metals
  • Chemistry of Metallic Carbonates, Sulphates, Chlorides and Nitrates.

2.2 Alkali metals:

  • General characteristics of Alkali metals
  • Properties & uses of sodium.

2.3 Alkaline earth metals:

  • General characteristics of the Alkaline earth metals
  • Properties & uses of calcium.

 2.4 Aluminum: Properties and uses

2.5 Coinage metals:

  • General properties of coinage metals
  • Properties and uses of cupper

2.6 Zinc: Properties & uses

2.7 Iron: Properties & uses

2.8 Lead: Properties & uses

2.9 Alloys:

  • Definition
  • Purpose of making alloys
  • Types of alloys
Unit: 3: Organic compounds and synthetic materials: 10hrs

3.1. Organic compounds

  • Historical background, classification, and nomenclature
  • Functional groups and homologous series
  • Saturated hydrocarbon: Properties of Methane
  • Unsaturated hydrocarbon: Properties of Ethylene and Acetylene
  • Aromatic compounds: Definition , Comparison of aliphatic and aromatic compounds
  • Properties of Benzene.

3.2. Synthetic materials:

  • Polymer and polymerization – Definition , Types of polymer
  • Rubber: Types (Natural and Synthetic ) ,Preparation and uses.
  • Polyvinyl chloride (PVC): Preparation and uses
  • Polythene: Preparation and uses.

REFERENCE :

http://www.ctevt.org.np/