Acquisition of knowledge Essay

Aims 1. To foster acquisition of friendship and understanding of monetary value, concepts, facts, processes, techniques and principles relating to the subject of alchemy. 2. To let out the strength to apply the realizeledge of meats and principles of Chemistry in new or unfamiliar with(predicate) situations. 3. To develop skills in proper use of apparatus and chemics. 4. To develop an ability to give nonice achievements in the field of Chemistry and its fiber in nature and society. 5. To develop an amour in activities involving usage of the knowledge of Chemistry. 6. To develop a scientific attitude with the study of Physical Sciences. 7. To acquaint students with the acclivitous frontiers and interdisciplinary aspects of the subject. 8. To develop skills relevant to the discipline. 9. To advise students with interface of Chemistry with other disciplines of Science, such(prenominal) as, Physics, Biology, Geology, Engineering, etceteraCLASS XI in that location lea ve be dickens written document in the subject. Paper I Theory- 3 hours Paper II Practical 3 hours Project figure out Practical data file 70 mark 20 tag 7 marks 3 marks Main postulates of the opening. Its limitations. Modern nuclear theory. Laws of chemic substance substance combinations Law of conservation of mass. Law of explicit proportion. Law of multiple proportion. Law of reciprocatory proportion. Gay-Lussacs law of shove alongeous vividnesss. Statement, translation and wide problems base on these laws. (ii) nuclear and isotopic masses. The atomic mass unit of measurement is one of the observationally determined unit. It is jibe to 1/12 of the mass of the degree Celsius 12 isotope. (iii) chemic substance comparables, volumetric enumerations in terms of normality. C = 12.00 should be interpreted as a standard for expressing atomic masses. Equivalent weight expresses the combining might of the elements with the standard elements such as H, Cl, O, Ag, et c. varying same weight. Gram equivalent weights, relationship amidst gram equivalent weight, gram molecular weight and valency. object of equivalent weight of acids, alkalis, salts, oxidising and reducing agents. (experimental flesh out not necessitate). 128PAPER I hypothesis 70 Marks There will be one paper of 3 hours duration divided into 2 parts. branch I (20 marks) will consist of supreme shortanswer questions, testing knowledge, employment and skills relating to elementary/ natural aspects of the entire syllabus. kick downstairs II (50 marks) will be divided into 3 Sections, A, B and C. Candidates are required to answer two out of trine questions from Section A (each carrying 10 marks), two out of lead 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 prope rties in explaining the laws of chemical combination. The study about the atoms. Daltons atomic theoryTerms used in volumetric calculations such as piece (w/w and w/v), normality, molarity, molality, mole fraction, etc. should be discussed. Students are required to know the influenceulae. unbiased calculations on the preceding(prenominal) topics. (iv) proportional molecular mass and mole. The side by side(p) order actings may be considered for the determination of comparative molecular masses for the gases the molar volume mode Victor Meyers method (experimental inside tuition not required). Numerical problems based on the in a higher place method and Victor Meyers method. Mole concept, Avogadros bite and numeric problems on mole concept. Gram molecular volume. (v) chemic Reaction calculations based mass-volume and relationships. ego explanatory. 2. Atomic Structure (i) negatrons, Protons and Neutrons as underlying particles, their charges and masses.Concept of indi visibility 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 properties. Chadwicks experiment for the discovery of neutron and properties of neutron. (ii) Rutherfords nuclear molding based on the divide experiment. Rutherfords nuclear model of atom. Rutherfords scattering experiment. Discovery of nucleus. Defects of Rutherford model. (iii) Bohrs atomic model. 1. Postulates of Bohrs theory based on Plancks quantum theory. 2. Numericals on Bohrs atomic radii, upper and vital force of orbits (derivation not required). 129 Stoichiometric on mass-mass, volume-volume3. Defects in the Bohrs Model. (iv) Atomic building wave mechanical model-a simple mathematical treatment. Quantum human actions shape, size and preference of s and p orbitals totally. Hunds principle of maximum multiplicity. Paulis exclusion principle, Aufbau principle, negatronic manakin of elements in terms of s, p, d, f subshells. Wave mechanical model experimental verification of wave nature of negatron. de de Broglies equation. Numericals. Heisenbergs Numericals. uncertainity principle. Quantum numbers types of quantum numbers, in organic law obtained in terms of distance of electron from the nucleus, zippo of electron, number of electrons present in an orbit and an orbital. Paulis exclusion principle. Shape, size and orientation of the s and p subshells. Hunds rule of maximum multiplicity. Aufbau principle, (n+l) rule. Electronic configuration of elements in terms of s, p, d, f subshells. 3. cyclic Table (i) Atomic number (Proton number) as the primer coat for classification of the elements in the occasional(a) Table.IUPAC nomenclature for elements with Z 100. Mendeleevs semiannual law, defects in the Mendeleevs periodic slacken. Advantages and disadvantages. Modern periodic law (atomic number taken as the can of classification of th e elements). Extended and unyielding form of periodic circumvent. General characteristics of groups and periods. variability of periodic table as s, p, d and f blocks. (ii) Extra nuclear organize as the basis of periodicity. Some supposition of the fol lower-rankinging ionisation enthalpy, electron come enthalpy, atomic radius, atomic volume, electronegativity, etc moldiness be given. The periodicity of electronic structure wind tothe periodicity of elements e.g the relative ease of ionisation of elements. Periodic properties such as valence electrons, atomic volume, atomic and loft radii and their variability in groups and periods. The idea of ionisation enthalpy, electron come enthalpy and electronegativity must be given and their variation in groups and periods may be discussed. The factors (atomic number, atomic volume and shielding effect, the number of electrons in the outermost orbit) which affect these periodic properties and their variation in groups and peri ods. (iii) Periodicity of elements with reference to s, p, d and f block elements. Classification of elements on the basis of s, p, d, f block elements and likewise on the basis of their complete and incomplete electron shells.Study of the periodicity of propertiesmentioned in power point (ii) in terms of s, p, d, f blocks and the brass factors in terms of the block characteristics. 4. Chemical stinging Electrovalent Bond (i) Electrovalent or bean bond e.g formation of NaCl, Li2O, MgO, CaO, MgF2, and Na2 S. Cause of chemical combination, eight-spot rule, types of chemical bonds. Electrovalent formation of NaCl, Li2O, MgO, CaO, MgF2, and Na2S. Properties of bonce compounds. Electron dot structure of the following ionic compounds NaCl, Li2O, MgO, CaO, MgF2, and Na2S must be taught in detail. (ii) Factors influencing the formation of ionic bond, e.g electron gain enthalpy, ionisation enthalpy, lattice zip and electronegativity. The conditions prerequisite for the formation of ionic bonds such as low ionisation enthalpy of metals. luxuriously electron gain enthalpy of non-metals. full(prenominal) lattice capacity.All these points must be discussed in detail. (iii) The relation between the ionic stick to and Periodic Table. The relationship between the formation of cations and anions of the atoms and their positions in the periodic table should be discussed. Correlate the periodic property and the position of the elements in the periodic table to show the ease of formation of anions and cations and electrovalent and covalent compounds. (iv) Variable electrovalency and its causes. Variable electrovalency reasons for variable electrovalency i.e, referable to inert electron pair effect, by using suitable examples. Covalent Bond (i) Covalent bond, sigma and pi bonds e.g. formation of ammonia, nitrogen, ethene, ethyne, and ascorbic acid dioxide. ring. Definition of covalent bonding, conditions for formation of covalent bonds, types of covalent bonds i.e single, geminate and triple bonds. Sigma and pi bonds. H2, O2, N2. Classification of covalent bonds based on electronegativity of atoms glacial and non polar covalent bond, dipole moment, formation of CH4, H2O, NH3, ethane, ethene, ethyne and CO2, etc. and their electron dot structure or Lewis structure.Characteristics of covalent compounds. Comparison in electrovalency and covalence. Resonance in simple inorganic molecules like ozone, carbon dioxide, carbonate ion and nitrateion. (ii) Variable valency chlorine exhibits the valency of 1,3,5 & 7 respectively. Variable valency, cause of variable covalence e.g. chlorine exhibits the valency 1, 3, 5 and 7 respectively. Discuss in terms of atomic structure. Variable covalency of phosphorus and randomness may be discussed. Discuss in terms of atomic structure.(iii) Deviation from octet rule and Fajans rules. Definition of Octet rule. Failure of Octet rule, due to both(prenominal) incomplete octet or olympian of Octet with suitabl e examples. Fajans rules Statements. patterns for electrovalency and covalency must be discussed. Polar and non polar bonds should be correlated with Fajans rules.(viii) molecular orbital theory, Qualitative treatment of homonuclear diatomic molecules of first two periods. Energy aim diagrams, bonding, antibonding molecular orbitals, bond order, paramagnetism of O2 molecule. Relative stabilities of O2, O2-, O2- , O2+, O2++ Self-explanatory. 5. The gassy State (i) The gas laws, qualitatively. kinetic theory treated(iv) Co-ordinate or dative covalent bond, e.g.formation of oxy-acids of chlorine. Co-ordinate or dative covalent bonding definition, formation of hypochlorous acid, chloric acid, perchloric acid, ammonium ion, hydronium ion, nitric acid, ozone structural formulae of the above molecules based on co-ordinate bonding. (v) atomic number 1 bonding its essential requirements, the examples of enthalpy fluoride, water carcass supply (ice), alcohol, etc may be considered. H -bonding definition, types, condition for altering content bond formation, examples of inter-molecular hydrogen bonding in detail winning hydrogen fluoride, water and ice and ethanol into account. Intramolecular hydrogen bonding.(vi) Metallic bonding, cutting edge der Waals forces. Metallic bonding Electron sea model and bar model. Explanation of metallic properties in terms of metallic bonding. Van der Waals forces and its types. (vii)Valence Shell Electron Pair Repulsion Theory hybridisation and shapes of molecules hybridisation involving s, p and d orbitals only sigma and pi bonds. Concept of electron-pair repulsion and shapes ofmolecules taking methane, ammonia and water as examples. crossroad and molecular shapes definition, hybridization of orbitals involving s, p and d orbitals (examples ethane, ethene, ethyne, PCl5 and SF6).Characteristics of gases, comparison between sohid, liquid and gas. Properties of gases on the basis of kinetic theory of gases. Laws of gases Boyles Law, Charles Law, Absolute Temperature, Pressure Temperature Law, Avogadros Law. Simple numeral problems based on the above laws. Postulates of Kinetic Theory must be discussed to explain gas laws. (ii) PV = nRT or PV= (w/M)RT and the coating of this equation of state. bringing close togetherl gas equation PV = nRT its application in calculation of relative molecular mass and in the calculation of the value of R.(iii) Non ideal behaviour of gases and Van der Waals equation. Non ideal behaviour of gases i.e. deviation from gas laws may be discussed at low and at high temperature and pressure. Van der Waals equation (P + a/V2) (V-b) = RT for one mole of a gas. The pressure chastening and volume correction may be explained. (iv) Daltons law, the Avogadro constant, the mole, whole meal flours law of diffusion, simple numerical problems on the above. Daltons Law of overtone pressure. Application of Daltons Law. Numerical problems based on the above law. Avogadros cons tant. kindred between the mole and Avogadro number. Grahams Law of diffusion and its application. Simple numerical problems on the above.6. Colloidal Solutions cookery and properties of colloids, both lyophilic and lyophobic colloids. Precipitation as evidence that the colloidal particles are charged. Idea of gold number is required, but application of gold number is not required. The importance of large bob up area in adsorption should also be appreciated. Thomas Graham classified advertisement the substances as crystalloid and colloid. Classification of substances on the basis of the particle size i.e. true solution, sol and suspension. Colloidal strategy is heterogeneous. Lyophilic and lyophobic colloids. Classification of colloidal solutions as micro, macro and associated colloids. Preparation of lyophilic colloids.Preparation oflyophobic colloids by colloid mill, peptisation, Bredigs arc method (procedural details not required) by oxidation, reduction, double decomp osition and ex transmute of solvent method should be discussed. Purification of colloids (dialysis, ultra filtration, and ultracentrifugation). Properties of colloidal solutions such as Brownian movement, Tyndall effect, coagulation and protection (protective colloids), should be discussed. Gold number and tough Schulze rule. Application of colloids in life. Electrophoresis (movement of dispersed phase). Emulsions, surfactants, micelles (only definition and examples).8. Chemical Energetics (i) Introduction. (a) Scope of thermodynamicals- characteristics of thermodynamics. (b) Types of scheme ideal system, real system, discriminate system, disagreeable system, open system. (c) import of environ. (d) Properties of the system macroscopic, intensifier and extensive properties of the system. (e) State of the system. (f) Main processes the system undergoes two-sided, irreversible, adiabatic, isothermal, isobaric, isochoric, cyclic. (g) mean of thermodynamic equilibrium. (h) Mea ning of thermodynamic process. (ii) First law of Thermodynamics mathematical statement. and its(a) Idea of conservation of push total muscle of the system and the surrounding. (b) Meaning of knowledgeable energy of the system and change in national energy of the system. (c) Meaning of operate through with(p) by the system and by the surrounding at constant temperature. (d) Meaning of heat absent-minded by the system and by the surrounding at constant temperature. (e) The undertake convention for change in internal energy, heat given out or gained, work done by the system or by the surrounding. (f) State melt down and path function- inwardness with examples. (g) sexual energy change, work done and heat absorbed in a cyclic process. (h) Internal energy change in an isolated system and in non isolated system.7. Chemical Kinetics Rate of a chemical reaction, basic idea of order and molecularity of a reaction. Rate of a chemical reaction Relation between order and the stoich iometric coefficients in the balanced equation Meaning of molecularity. Differences between the order and molecularity of the reaction.Physical moment of sulphur State function and not path function. Relationship between adiabatic change and entropy. sec change of the founding and a reversible isothermal process. Entropy change of the universe and irreversible process. Meaning of thermal death. Meaning of energy content and work content ( let loose energy) of the system thermodynamic quantity state function. Types of work and meaning of the two types of work. Meaning of Helmholtzs rationalise energy and Gibbs surplus energy and the change in Gibbs and Helmholtzs free energy.Relationship between Gibbs free energy and Helmholtzs free energy. Simple calculation on the change in Gibbs free energy and Helmholtzs free energy. Relationship between change in Gibbs free energy and equilibrium constant of a chemical reaction. Change in Gibbs free energy in reversible, irreversible, is obaric and isochoric processes. found on change in Gibbs free energy, defining the criteria for the spontaneity of a change in terms of entropy and enthalpy defining the limits for reversible chemical reactions.(k) Chemical change and internal energy. (l) contain for enthalpy constant pressure or open vessel processes. (m) Enthalpy a thermodynamic property state function. (n) mathematical form constant pressure.(iii) Ideas about Heat, Work and Energy. Heat the energy in transit.Condition for the transfer of heat. Limitation in spiritual rebirth of heat into work. Condition at which heat transfer ceases. Unit of heat. Meaning of energy capacity to do work. Meaning of work intensity factor and capacity factor. Types of work. numeral form of reversible work. Mathematical form of irreversible work. Difference between the reversible and irreversible work done graphically. adiabatic reversible expansion. Relationship between Cv and internal energy change.