Jd Lee Concise Inorganic Chemistry Pdf Free Download
Kody Coste
Inorganic chemistry is a vast and important field, ranging from the nature and structure of minerals, to the involvement of metals in biological structures, to the design of novel materials with diverse properties. Ionic compounds range from ionic solids that can be described simply with the electrostatic model, to covalent compounds and metals, which are best described using quantum mechanical models. For the rationalisation and interpretation of most inorganic properties, qualitative models based on quantum mechanics, such as the properties of atomic orbitals and their use in the formation of molecular orbitals.
The student must demonstrate knowledge of the basic concepts of general chemistry and know how to apply them in the resolution of exercises (stoichiometry, balance of reactions, calculations of thermodynamic quantities) as well as in the description of the phenomena studied in the teaching module.
It is required to be able to:
1. Be able to use the scientific language of the topics covered in the chemistry course. (knowledge and understanding)
2. demonstrate an adequate knowledge of the basic laws of general chemistry and to know their application in real cases ( applying knowledge and understanding)
3. express in a concise and precise form the basic concepts of general chemistry in the written test. (Communication skills )
4. to create links between the various chapters dealt with and apply the acquired knowledge to the solution of problems of stoichiometric calculation and to demonstrate the understanding of the basics of chemistry by illustrating some of the basic laws and by the formulation of some examples (making judgments)
5. to integrate the didactic material provided with textbooks is required in order to formulate a synthesis in order to construct a base of preparatory knowledge to face the comprehension of successive courses of chemistry. ( learning skills)
Classification of the matter. Elements substances and mixtures. Mass conservation laws
Structure of the atom (neutron proton and electron) atomic number, atomic mass. Elements and Isotopes. Orbitals and rules of electron distribution. Periodic table and correlation with the electronic configuration. Periodic properties.
Chemical bond. Ionic and covalent bond. Oxidation number. Valence bond and octet rule. Lewis structures. Resonance formulas and formal charge. Orbitalic hybridization .Polarity in molecular bonds. Nomenclature of cations, anions and inorganic compounds.
Chemical reaction. Formula weight, molecular weight, size and use in the calculation of mass reactions. Stoichiometry. Balancing different types of chemical reactions. Ox-redox reactions.
Introduction to thermodynamics. First and second principles of thermodynamics. Reaction heat. Exothermic and endothermic reactions. Gibbs free energy, spontaneity of a process.
Chemical equilibrium. K equilibrium constant, Le Chậtelier's law. Factors that influence chemical balance.
States of the matter. Gaseous state: perfect gas state equation. Liquid state: vapor pressure, surface tension, boiling point, intermolecular forces (van der Waals forces, hydrogen bond). Notes on the solid state. Phase changes and phase diagrams, supercritical state.
Solutions. Solvent and solute, solubility. Colloidal solutions, emulsions. Methods to indicate the concentration (molarity, molality, normality, percentages). Henry's law. Colligative properties (cryoscopic lowering, ebullioscopic elevation, osmotic pressure).
Acids and Bases. Definition according to Brønsted. Conjugated acid and base. Ionic product of water, pH, calculation of Ka and Kb and their use in determining the strength of an acid or base. Strong acids and bases, weak acids and bases. Examples of hydrolysis of some salts, buffer solutions, pH of a buffer. Electrochemistry - Convention on redox half-reactions. Electrical work and galvanic cells. Standard hydrogen electrode. Scale of standard reduction potentials. Nernst equation. Concentration cells. Electrolysis. Faraday's laws. electrolytic cells. Electrolysis of water. Basics of kinetics. Reaction rate, effect of concentration and temperature, Arrhenius law, activation energy, catalysts (homogeneous, heterogeneous, enzymatic).
Elements of Inorganic Chemistry. Elements of the first and second group. Fourth, fifth and sixth group chemistry (C, Si, Sn, N, P, As, O, S). Chemistry of halogens.