The course consists of 22 lectures with 18.5 hours of video contents along with the lecture notes of each lecture as PDF files. Each lecture is supported with assignments for the students for home-work. The solutions to the assignments are also given at the end.
This course is designed very meticulously by the instructor using his more than 40 years of teaching experience to equip beginners in class XI to pursue Chemistry as major course. The primary objective behind preparing this course is to infuse a high level confidence at the initial stage to study Inorganic chemistry and its multitudinous reactions with utmost ease and confidence. The instructor has put all efforts to dispel the notion that inorganic chemistry does have a strong logic like physical and organic chemistry and never a subject to be crammed mechanically. This course is precisely meant for hard working students with higher IQ levels who intend to acquire higher level thinking and application skills in Inorganic Chemistry. It will give tremendous confidence for national and international level competition in Chemistry.
The course has the following main parts.
(1) Writing formula of ionic compounds with large number of uncommon polyatomic ions
(2) Solubility Rules and writing Ionic Equations
(3) Oxidation Number(ON)/Oxidation State(OS) concept including large number of paradoxical cases resolved from their bond structures.
(4) Balancing Redox reaction equations by Oxidation Number Method, Electron Balance Diagram Method, Ion-Electron Method, Algebraic Method and Partial Equation Method.
(5) Broad Classification of Inorganic Reactions: Redox and Non-Redox(Metathesis) : Determining Oxidation and Reduction processes along with Oxidant and Reductants with the assignment of ON in Redox Reactions
(6) Eleven types of Non-Redox Reactions: Double Displacement(Precipitation and Neutralization), Reaction of metallic and nonmetallic oxides with water, Reaction of carbonate, bicarbonate, sulfite, thiosulfate, sulfide and nitrite salts with dilute non-oxidizing acids like HCl and sulfuric acid; Reaction of nitride, phosphide, sulfide and carbide salts with water; Reaction of ammonium salts with a base; Amphoterism; Thermal decomposition of carbonates and bicarbonates; thermal decomposition of hydroxides; Displacement of more volatile acids by a less volatile acid; Complexation reactions.
(7)Redox Reactions explained in the light of Standard Electrode Potentials: Electrochemical Series(Metal Activiety Series); Displacement Reactions : The anomaly of Na and Ca in the Activity series explained, Hydrogen Displacement, Metal Displacement; Halogen Displacement
(8) Redox Reaction studied as Galvanic Cell Reaction with to half cells; Determination of Standard Cell EMF.
(9) Relative Strengths of Oxidants and Reductants and predicting the spontaneity of redox reactions from Standard Electrode Potential data
(10) Some Name Redox Reactions: Combination, Combustion, Thermal Decomposition, Disproportionation, Comproportionation, Auto-redox reaction, Amphoterism, Reaction of metallic hydrides with water.
(11)Some Compounds used only as Oxidants and Reductants and the OS to which they change to during a reaction in acidic and basic medium - explained with large number of reactions with electrochemical logic.
(12) Some common Oxidants and Reductants and the OS to which they change.
(13) Some species which act both as Oxidants and Reductants and the OS to which they change to
(14) Non-spontaneous Reactions by Electrolysis: Preferential Discharge of ions at electrodes; Faraday's Laws of Electrolysis
(15) Fuel Cells