| Summary, Abstract, Review |
This textbook introduces students to the basic principles of chemistry at the college level. It covers atomic structure, bonding, states of matter, thermodynamics, and chemical reactions, providing a strong foundation for higher studies in chemistry, medicine, engineering, and related fields. Contents Summary 1. Basic Concepts o Importance of chemistry in daily life. o Atomic mass, molecular mass, empirical & molecular formulas. o Mole concept, Avogadro’s number, and chemical calculations. 2. Experimental Techniques in Chemistry o Common laboratory apparatus. o Methods of purification & separation of substances (filtration, crystallization, chromatography, distillation). o Safety measures in chemistry labs. 3. Gases o Properties of gases. o Gas laws (Boyle’s, Charles’, Avogadro’s, Ideal Gas Law). o Kinetic molecular theory. o Diffusion & effusion. 4. Liquids & Solids o Intermolecular forces (hydrogen bonding, Van der Waals forces). o Properties of liquids: viscosity, surface tension. o Crystal systems, unit cells, and types of solids (ionic, covalent, metallic, molecular). 5. Atomic Structure o Discovery of subatomic particles. o Rutherford’s and Bohr’s atomic models. o Quantum numbers, orbitals, and electronic configuration. o Dual nature of electrons, wave-particle concept. 6. Chemical Bonding o Ionic, covalent, coordinate, metallic bonds. o Valence bond theory (VBT). o Hybridization and molecular shapes (VSEPR theory). o Bond energies and polarity. 7. Thermochemistry o Heat of reaction, enthalpy, and calorimetry. o Hess’s Law. o Bond enthalpies. o Enthalpies of combustion, formation, and neutralization. 8. Chemical Equilibrium o Reversible reactions and dynamic equilibrium. o Law of mass action. o Equilibrium constant (Kc, Kp). o Le Chatelier’s principle (factors affecting equilibrium). 9. Solutions o Types of solutions and methods of expressing concentration (molarity, molality, %). o Solubility and factors affecting it. o Colligative properties (osmotic pressure, depression in freezing point, elevation in boiling point). 10. Electrochemistry o Electrolytes and non-electrolytes. o Electrolysis and Faraday’s laws. o Electrochemical cells, redox reactions. o Applications in industry and daily life (batteries, electroplating). 11. Reaction Kinetics o Rate of reaction and rate laws. o Factors affecting reaction rate (concentration, temperature, catalysts). o Activation energy and collision theory. Learning Outcomes By the end of Chemistry Intermediate Part 1, students should be able to: • Apply the mole concept and perform chemical calculations. • Understand atomic structure, bonding, and molecular geometry. • Explain gas laws, solutions, equilibrium, and electrochemistry. • Perform basic laboratory techniques safely. • Connect chemistry principles to industrial and real-life applications. |
