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Organisation : Department of Pre University Education
Subject : Chemistry
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Chemistry Syllabus :

Unit  I : Some Basic Concepts of Chemistry
General introduction : Importance and scope of chemistry, nature of matter-classification, homogeneous and heterogeneous mixtures – examples, concept of elements, atoms, molecules and compounds.

Related : Psychology Syllabus Department of Pre University Education :

Properties of matter and their measurement: seven basic physical quantities, their SI units and scientific notation (exponential notation). Laws of chemical combination, with suitable examples. Dalton’s atomic theory – postulates.

Atomic and molecular masses: Atomic mass, amu (value of 1amu), average atomic mass with an example, molecular mass, examples, formula mass – NaCl as example. Mole concept and molar mass: Avogadro constant, mole and molar mass – examples.

Percentage composition, empirical formula and molecular formula- numerical problems. Stoichiometry relations –numerical problems to calculate amount of reactants/ products formed (in terms of mole and mass in grams) by giving balanced equations, limiting reagent –numerical problems.

Reactions in solutions: concentration terms – mass %, mole fraction, molality, molarity. Numerical problems.

Unit II : Structure of Atom
Discovery of electron – name of the discoverer, characteristics of cathode rays, values of charge and mass. Discovery of proton – characteristic of canal rays, values of charge and mass. Discovery of neuron – name of the discoverer, value of charge and mass.

Atomic number, mass number, isotopes, isobars, problems. Atomic models: Thomson atomic model and its limitations. Mention the observations and conclusions of – ray scattering experiment. Rutherford atomic model and its limitations(based on Maxwell electromagnetic theory).

Electromagnetic radiations – c, , , , their relationships, electromagnetic spectrum, particle nature of EMR(E = h ), line spectrum of hydrogen, formula to calculate of spectral lines in hydrogen – numerical problems.

Bohr’s model-postulates and its limitations, concept of shells and subshells, dual nature of matter and light, de-Broglie relationship – numerical problems. Heisenberg uncertainity principle and its mathematical form. Concept of orbitals ,meaning of and 2, nodal surfaces or nodes.

Quantum numbers, shapes of s, p, d orbitals, rules for filling electrons in orbitals- (n + l) rule, Aufbau principle, Pauli exclusion principle, Hund’s rule. Electronic configuration of atoms (1 to 36). Stability of half filled and completely filled orbitals.

Unit III : Classification of Elements and Periodicity in Properties
Significance of classification, brief history of development of periodic table – law of triads with an example, law of octaves, Mendeleev periodic law – statement, Henry moseley observation based on X- ray spectra of elements, modern periodic law, long form of periodic table.

Brief account of groups, periods, s, p, d and f blocks, Nomenclature of elements with atomic number greater than 100. Periodic trends in properties of elements with reason: atomic radii, inert gas radii, ionic radii.

compare radius of cation and anion with parent atom ,with reason, variation of radii of isoelectronic species, ionisation enthalpy, exception in first ionization enthalpy of N and O, with reason, electron gain enthalpy, compare egH of F and Cl with reason. Electronegativity. valence – periodicity of valence or oxidation states (s and p block elements).

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