Fundamental Concepts Of Inorganic Chemistry By Dr. C. Viswanatha (informative)
Free download Fundamental Concepts Of Inorganic Chemistry By Dr. C. Viswanatha
Authors of: Fundamental Concepts Of Inorganic Chemistry By Dr. C. Viswanatha
Dr. C. Viswanatha
Dr. N. Radhakrishna
B N. Nagalaxmi
Dr. K. Ramakrishna Reddy
N V. Rajendra Kumar
Table of Contents in Fundamental Concepts Of Inorganic Chemistry By Dr. C. Viswanatha
CHAPTER:1 Fundamental Laws of Chemistry
1.1 The early History of chemistry
1.2 Atomic Theory (Dalton’s Atomic Theory)
1.3 Laws of chemical combination
1.3.1 Law of conservation of mass
1.3.2 Law of Definite Proportions
1.3.3 Law of Multiple Proportions
– Revision Questions
CHAPTER: 2 Solid State
2.0 Introduction
2.1 Classification of solids
2.2 The structures of ionic solids
2.3 The radius ratio rules for ionic compounds
2.4 Close packing
2.5 Classification of ionic structures:
– Revision Questions
CHAPTER: 3 Acids and Bases
3.0 Introduction
3.1 Properties of acids and bases
3.2 pH scale
3.3 Overview of the three theories
3.3.1 Arrhenius Concept of acids and bases
3.3.2 Neutralization
3.3.3 Bronsted – Lowry concept of acids and bases
3.3.4 The Lewis concept of acids and bases
3.4 Solvent –system concept
– Revision Questions
CHAPTER: 4 Atomic Structure
4.0 Introduction
4.1 Bohr’s model of the atom:
4.2 Quantum numbers
4.3 Atomic Spectrum of Hydrogen
Revision Questions
CHAPTER: 5 Chemical Bonding
5.0 Introduction to Bonding
5.1 Types of bonds
5.1.1 Ionic bonds
5.1.2 Covalent bonds (electron sharing)
5.1.3 Coordinate covalent or Dative bond
5.2 Valence shell electron pair repulsion (VSEPR) theory
5.3 Valence Bond Theory
5.4 Molecular Orbital Theory
5.4.1 Linear combination of atomic orbitals (LCAO)
5.4.2 Rules for Linear combination of atomic orbitals (LCAO)
Revision Questions
CHAPTER: 6 Chemistry of Main Group Elements
6.0 Introduction
6.1 Chemistry of Hydrogen
6.2 General properties of the elements
6.2.1 Ionization Energy(IE)
6.2.2 Electron Affinity
6.2.3 Electro negativity
6.2.4 Metallic Character
6.2.5 Polarizing Power and Polarizability-Fajans Rule
6.2.6 Variable Valency
6.3 Diagonal relationships in the periodic table
6.4 The S- block elements
Revision Questions
CHAPTER:7 Chemistry of Transition Elements
7.0 Introduction
7.1 Generallyphysical and chemical properties
7.2.1 Melting point and boiling points
7.2.2 Catalytic properties
7.2.3 Atomic Size
7.2.4 Ionization Energy
7.2.5 Color
7.2.6 Magnetic properties
7.2.7 Oxidation States
7.3.1 Crystal field theory
7.3.2 Octahedral complexes
7.3.3 Tetrahedral complexes
7.3.4 Color of transition metal complexes
7.3.5 Nomenclature of Coordination Compounds
7.4 Isomerism
Revision Questions
CHAPTER 1: Fundamental Laws of Chemistry
1.1 The Origins of Chemistry
The genesis of chemistry traces back to ancient times, where rudimentary forms of experimentation and observation laid the foundation for understanding matter and its transformations.
1.2 The Atomic Theory (Dalton’s Postulations)
Dalton’s Atomic Theory, proposed in the early 19th century, revolutionized chemistry by asserting that elements are composed of indivisible particles called atoms, which combine in fixed ratios to form compounds.
1.3 Laws Governing Chemical Combinations
1.3.1 Law of Conservation of Mass
This law, established by Antoine Lavoisier, stipulates that in a chemical reaction, the total mass of the reactants remains constant, thus affirming the principle of matter conservation.
1.3.2 Law of Definite Proportions
Pioneered by Joseph Proust, this law asserts that a compound always contains the same elements in fixed proportions by mass, regardless of its origin or preparation method.
1.3.3 Law of Multiple Proportions
This law, also credited to Dalton, elucidates that when two elements form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers.
Revision Questions:
1. What pivotal theories shaped the early development of chemistry?
2. Explain Dalton’s Atomic Theory and its significance.
3. Elaborate on the Laws of Chemical Combination and their implications.
CHAPTER 2: The Solid State
2.0 Introduction
The study of solids constitutes a significant domain in chemistry, encompassing various structural arrangements and properties.
2.1 Classification of Solids
Solids are categorized into crystalline and amorphous forms based on their internal structural organization, with crystalline solids exhibiting ordered arrangements of atoms or molecules.
2.2 Structures of Ionic Solids
Ionic solids are characterized by an orderly arrangement of positively and negatively charged ions held together by strong electrostatic forces.
2.3 Radius Ratio Rules for Ionic Compounds
The radius ratio rules elucidate the relationship between the sizes of ions and their coordination numbers in ionic compounds, influencing their crystal structures.
2.4 Close Packing
Close packing refers to the densest arrangement of spheres in a crystal lattice, optimizing the packing efficiency of constituent particles.
2.5 Classification of Ionic Structures
Ionic structures are classified based on the relative sizes of ions and their coordination numbers, which determine the types of crystal lattices formed.
Revision Questions:
1. Distinguish between crystalline and amorphous solids.
2. Explain the structural characteristics of ionic solids.
3. How do the radius ratio rules influence the formation of crystal structures?
CHAPTER 3: Acids and Bases
3.0 Introduction
Acids and bases represent fundamental chemical entities with distinctive properties and behaviors, playing pivotal roles in various chemical processes.
3.1 Properties of Acids and Bases
Acids donate protons, while bases accept protons, exhibiting properties such as sourness (acids) and bitterness (bases) in aqueous solutions.
3.2 pH Scale
The pH scale quantifies the acidity or basicity of a solution based on the concentration of hydrogen ions, ranging from acidic (pH < 7) to basic (pH > 7), with neutral solutions having a pH of 7.
3.3 Overview of Acid-Base Theories
3.3.1 Arrhenius Concept of Acids and Bases
Svante Arrhenius proposed that acids dissociate in water to yield hydrogen ions (H⁺), while bases dissociate to produce hydroxide ions (OH⁻).
3.3.2 Neutralization
Neutralization reactions involve the combination of acids and bases to form water and a salt, effectively neutralizing the acidic or basic properties of the reactants.
3.3.3 Bronsted-Lowry Concept of Acids and Bases
According to this theory, acids donate protons (H⁺), while bases accept protons, emphasizing proton transfer in acid-base reactions.
3.3.4 The Lewis Concept of Acids and Bases
Proposed by Gilbert N. Lewis, this theory defines acids as electron pair acceptors and bases as electron pair donors, focusing on electron transfer in chemical interactions.
3.4 Solvent-System Concept
The solvent-system concept elucidates the behavior of acids and bases in non-aqueous solvents, highlighting the role of solvents in facilitating acid-base reactions.
Revision Questions:
1. Define the properties of acids and bases.
2. Discuss the significance of the pH scale in acid-base chemistry.
3. Compare and contrast the Arrhenius, Bronsted-Lowry, and Lewis concepts of acids and bases.
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