Aims: 1. To foster acquisition of knowledge and understanding of terms, concepts, facts, processes, techniques and principles relating to the subject of Chemistry. 2. To develop the ability to apply the knowledge of contents and principles of Chemistry in new or unfamiliar situations. 3. To develop skills in proper handling of apparatus and chemicals. 4. To develop an ability to appreciate achievements in the field of Chemistry and its role in nature and society. 5. To develop an interest in activities involving usage of the knowledge of Chemistry. 6. To develop a scientific attitude through the study of Physical Sciences. 7. To acquaint students with the emerging frontiers and interdisciplinary aspects of the subject. 8. To develop skills relevant to the discipline. 9. To apprise students with interface of Chemistry with other disciplines of Science, such as, Physics, Biology, Geology, Engineering, etc.
There will be two papers in the subject. Paper I: Theory- 3 hours Paper II: Practical - 3 hours Project Work Practical File ... 70 marks ...20 marks … 7 marks … 3 marks Main postulates of the theory. Its limitations. Modern atomic theory. Laws of chemical combinations: Law of conservation of mass. Law of definite proportion. Law of multiple proportion. Law of reciprocal proportion. Gay-Lussac’s law of gaseous volumes. Statement, explanation and simple problems based on these laws. (ii) Atomic and isotopic masses. The atomic mass unit is one of the experimentally determined unit. It is equal to 1/12 of the mass of the carbon 12 isotope. (iii) Chemical equivalents, volumetric calculations in terms of normality. C = 12.00 should be taken as a standard for expressing atomic masses. Equivalent weight expresses the combining capacity of the elements with the standard elements such as H, Cl, O, Ag, etc. Variable equivalent weight. Gram equivalent weights, relationship between gram equivalent weight, gram molecular weight and valency. Determination of equivalent weight of acids, alkalis, salts, oxidising and reducing agents. (experimental details not required). 128
PAPER I –THEORY – 70 Marks There will be one paper of 3 hours duration divided into 2 parts. Part I (20 marks) will consist of compulsory short answer questions, testing knowledge, application and skills relating to elementary/fundamental aspects of the entire syllabus. Part II (50 marks) will be divided into 3 Sections, A, B and C. Candidates are required to answer two out of three questions from Section A (each carrying 10 marks), two out of three questions from Section B (each carrying 5 marks) and two out of three questions from Section C (each carrying 10 marks). Therefore, a total of six questions are to be answered in Part II. SECTION A 1. Atoms and Molecules (i) The concept of atoms having fixed properties in explaining the laws of chemical combination. The study about the atoms. Dalton’s atomic theory:
Terms used in volumetric calculations such as percentage (w/w and w/v), normality, molarity, molality, mole fraction, etc. should be discussed. Students are required to know the formulae. Simple calculations on the above topics. (iv) Relative molecular mass and mole. The following methods may be considered for the determination of relative molecular masses for the gases: the molar volume method; Victor Meyer’s method (experimental details not required). Numerical problems based on the above method and Victor Meyer’s method. Mole concept, Avogadro’s number and numerical problems on mole concept. Gram molecular volume. (v) Chemical Reaction calculations based mass-volume and relationships. Self explanatory. 2. Atomic Structure (i) Electrons, Protons and Neutrons as fundamental particles, their charges and masses. Concept of indivisibility of atom as proposed by Dalton does not exist. The atom consists of subatomic fundamental particles. Production of cathode rays and their properties. Production of anode rays and their...
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