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Basic Concepts of Inorganic Chemistry, 2nd Edition

Book Description

Basic Concepts of Inorganic Chemistry is thoroughly revised and designed as a student text to meet the needs of the students preparing for various competitive examinations. Each concept and principle is unfolded systematically, reflecting the vast experience, command and authority of the author on the subject. The subject has been explained using basic principles that make things easy to understand and absorb both for beginners as well as advanced learners. Each chapter is followed by graded multiple choice questions (the core of the competitive exams) based on concepts, principles and applications, providing the student with necessary recapitulation and ensuring speed and accuracy.

Table of Contents

  1. Cover
  2. Title page
  3. Contents
  4. Dedication
  5. Preface
  6. Chapter 1. Periodic Table and Periodicity of Properties
    1. Mendeleev’s periodic law
    2. Modern Periodic Table
    3. IUPAC table
    4. Periodic table and Aufbau principle
    5. Determination of group and period of an element
    6. Classification of elements
    7. Atomicity and elements of the periodic table
    8. Effective nuclear charge
    9. Atomic and ionic size
    10. Ionization energy
    11. Electron affinity
    12. Electronegativity
    13. Physical properties and the periodic table
    14. Artificial elements
    15. Some records of periodic table
  7. Chapter 2. Chemical Bonding and Molecular Structure
    1. Different types of chemical bonds
    2. Summery of bond types
    3. Ionic bond
    4. Born — Haber cycle
    5. Cations of stable electron configuration
    6. Polarization and its effects
    7. Lattice energy
    8. General properties of ionic compounds
    9. Covalent bonding
    10. σ and π bonds
    11. Comparison of σ and π bond
    12. Electronegativity
    13. Coordinate covalent bond
    14. Electronegativity and Dipole moment
    15. Lewis structure (or Dot structure)
    16. Resonance structure
    17. Hybridization
    18. Resonance
    19. Resonance effect
    20. Resonance energy
    21. Bond length
    22. Bond energy
    23. VSEPR model
    24. Structure and shape
    25. Shape of Molecules
    26. Bond angle
    27. Odd electron molecules
    28. Molecular orbital model
    29. Shape and symmetry of molecular orbitals
    30. Formation of π bonds
    31. Diatomics of the first period elements
    32. Homonuclear Diatomics of Second Period Elements
    33. NO molecule
    34. CO molecule
    35. Hydrogen bond
    36. Van der Waals, forces
    37. Metallic bond
    38. Metal structures
    39. Electron gas model
    40. Band model
    41. Cohesive energy
  8. Chapter 3. Acids and Bases
    1. Bronsted-Lowry theory
    2. Strength of acids and bases
    3. PH
    4. Buffer solution
    5. Henderson equation
    6. Amphoterism
    7. Acid strength
    8. Strength of hydra acids
    9. Strength of Oxy acids
    10. Base strength
    11. Strength of hydra bases
    12. Strength of hydroxide bases
    13. Lewis Acid — Base theory
    14. Hard and soft acids and bases
  9. Chapter 4. Chemical Reaction
    1. Types of chemical reactions
    2. Hydrolysis
    3. Oxidation-reduction reactions
    4. Oxidation number
    5. Oxidizing agents
    6. Reducing agents
    7. Oxidizing and reducing agents
    8. Strength of oxidants and reductants
    9. Equivalent weights of oxidizing and reducing agents
    10. Balancing of redox reactions
    11. Oxidation number method
    12. Ion-electron method
    13. Some important half reactions
  10. Chapter 5. Transition Elements
    1. General properties
    2. Atomic and ionic radii
    3. Bonding in Transition metals and its effect on properties
    4. Electrode potential
    5. Oxidation states
    6. Paramagnetic nature of transition metal compounds
    7. Complex compound formation
    8. Colour of transition metal compounds
    9. The d — d transition
    10. Colour and charge transfer
    11. Hydrolysis of transition metal compounds
    12. Catalytic property
    13. Lanthanides and actinides
  11. Chapter 6. Coordination Chemistry
    1. Coordination number
    2. Types of ligands
    3. Chelates
    4. Conditions for complex formation
    5. Werner’s coordination theory
    6. Nomenclature
    7. Valence bond model for complexes
    8. Crystal field model of bonding
    9. Stability and CF model
    10. Magnetic properties and CF model
    11. Colour and CF model
    12. Isomerism in coordination compounds
    13. Geometrical isomerism
    14. Optical isomerism
    15. Preparations of complex compounds
    16. Stability of complex compound in a solution
    17. Applicability of complex compounds
    18. Organometallic compounds
    19. Preparation of organometallies
    20. Bonding in organometallic compounds
    21. Bonding in alkene complexes
  12. Chapter 7. Abundance and metallurgy
    1. Chemical elements in the Earth’s crust
    2. Cosmic abundance of elements
    3. Abundance in oceans
    4. Occurrence of metals
    5. Metallurgy
    6. Terms used in metallurgical process
    7. Concentration of ore
    8. Leaching
    9. Isolation of metal from concentrated ore
    10. Thermal (or chemical reduction)
    11. Auto reduction
    12. Electrolytic method of reduction
    13. Displacement of one metal by the other
    14. Purification of isolated metals
    15. Sodium
    16. Magnesium
    17. Calcium
    18. Aluminium
    19. Iron
    20. Ashoka Pillar at Delhi
    21. Pig iron
    22. Grey cast iron
    23. White cast iron
    24. Wrought iron
    25. Steel
    26. Special steel
    27. Conversion of iron into steel
    28. Steel from wrought iron
    29. Comparison Pig iron, Wrought and Steel
    30. Heat treatments of steel
    31. Chemically pure iron
    32. Brief chemistry of iron
    33. Corrosion of iron
    34. Important compounds of iron
    35. Copper
    36. Alloys of copper
    37. Brief chemistry of Cu
    38. Important compounds and complexes
    39. Zinc
    40. Brief chemistry of Zn
    41. Important compounds
    42. Mercury
    43. Brief chemistry of Hg
    44. Important compounds
    45. Tin
    46. Allotropic forms
    47. Chemical reaction
    48. Lead
    49. Physical properties
    50. Important compounds
  13. Chapter 8. Important Chemical Compounds
    1. Metal compounds
    2. NaOH
    3. Na2Co3
    4. K2Cr2O7
    5. KMnO4
    6. Non-metal compounds
    7. O3
    8. H2O2
    9. NA2S2O3
    10. H2S
  14. Chapter 9. Hydrogen and Its Chemistry
    1. Position in the periodic table
    2. Isotopes of H
    3. Oxidation states and bonding
    4. Preparation of H2
    5. Uyeno’s reaction
    6. Bosch’s process
    7. Lane’s process
    8. Laboratory Preparation of H2
    9. Nascent Hydrogen
    10. Compounds of protium (H)
    11. Water
    12. Zeolite water
    13. Water clathrates
    14. Hard and soft water
    15. Temporary hardness
    16. Permanent hardness
    17. Inorganic exchangers
    18. Organic exchangers
    19. Bad effects of hard water
    20. Structure of water and ice
    21. Density of water and ice
    22. Density of water at 4°C
    23. Heavy water
  15. Chapter 10. Group — 1(IA) The alkali metals
    1. Chemical reactions
    2. OXO salts
    3. Halides
    4. Flame colour
    5. Alkali metals and liquid NH3
    6. Anomalous behaviour of Li
  16. Chapter 11. Group — 2(IIA) [Be, Mg, Ca, Sr, Ba, Ra]
    1. Properties which decrease down the group
    2. Properties which increase down the gorup
    3. Oxidation states and nature of bond
    4. Hydrides
    5. Halides
    6. Oxides and hydroxides
    7. Oxo salts
    8. Flame colouration
  17. Chapter 12. Group — 11(IIB) Cu, Ag, Au
    1. Metallic bond strength
    2. Sublimation energy
    3. Atomic and ionic radii
    4. Ionization energy
    5. Noble metal nature
    6. Malleability, thermal and electrical conductivities
    7. Oxidation states
    8. Magnetic properties
    9. Colour of compounds
    10. Solubility of Silver-Hlides
    11. Chemistry of photography
  18. Chapter 13. Group — 12(IIB) Zn, Cd, Hg
    1. Ionization energy
    2. Oxidation states
    3. Nature of bonds
    4. Electrode potential
    5. Magnetic properties
    6. Colour of compounds
    7. Some useful compounds
    8. Biochemistry of Zn, Cd and Hg
  19. Chapter 14. Group — 13 (IIIA) B, Al, Ga, In, Td
    1. Oxidation states and nature of bond
    2. Hydrides
    3. Diborane
    4. Structure of B2H6
    5. Borazole
    6. Boric acid
    7. Halides
    8. Lewis acid strength of BX3
    9. Alums
    10. Isolation of B
    11. Crystalline B
  20. Chapter 15. Group — 14(IVA) C, Si, Ge, Sn, Pb
    1. Catenation
    2. Allotropy and structure
    3. Graphite
    4. Diamond
    5. Fullerenes
    6. Semiconductor property of Si and Ge
    7. Physical properties of group — 14 elements
    8. Oxidation states and bonding
    9. Carbides
    10. Oxides
    11. Cyanogens
    12. HCN
    13. Cyanides
    14. Halides
    15. Hydrides
    16. Silicones
    17. Silicates
    18. Isolation of Si
  21. Chapter 16. Group — 15(VA)N, P, As, Sb, Bi
    1. Allotropes of P
    2. Oxidation state and nature of bond
    3. Hydrides
    4. NH3
    5. PH3
    6. Oxides on N and P
    7. N2O
    8. NO
    9. N2O3
    10. NO2
    11. N2O5
    12. P4O6 and P4O10
    13. HNO2
    14. HNO3
    15. Aquaregia
    16. H3PO2
    17. H3PO3
    18. Phosphoric acids
    19. Acid strength of H3PO2, H3PO3 and P3PO4
    20. Halides
    21. Isolation of N and P
    22. Fertilizers
  22. Chapter 17. Group-16(VIA) O, S, Se, Te, Po
    1. Physical state of the elements
    2. Allotropy of O and S
    3. Effect of heat on S
    4. Viscosity of liquid S and temperature
    5. Oxidation state and nature of bond
    6. Hydrides
    7. H2O2
    8. Strength of H2O2
    9. Acid strength of H2O2 and H2O
    10. Structure of H2O2
    11. Halides
    12. SOCl2
    13. Oxides
    14. Oxo acids
  23. Chapter 18. Group — 17 (VIIIA) Halogens F, Cl, Br, I, and At
    1. Physical state
    2. Special properties of F
    3. Oxidation state and bonding
    4. Formation of X2
    5. Manufacture of Cl2
    6. Manufacture of Br2
    7. Manufacture of I2
    8. Reactions of X2
    9. Hydrogen halides
    10. HF
    11. HCl
    12. HBr
    13. Hl
    14. Halides
    15. Preparation of anhydrous halides
    16. Halogen oxides
    17. Oxo acids
    18. Acid Strength
    19. Oxidizing power
    20. CIO-n anions
    21. Halic acids
    22. Perhalic acids
    23. Interhalogen compounds
    24. Pseudohalogens and pseudohalides
  24. Chapter 19. Group — 18 The Noble Gases
    1. Atomicity
    2. Radii
    3. Water solubility
    4. Special properties of He
    5. Uses of noble gas
    6. Clathrate
    7. Xe compounds
    8. Structure of Xe — Compounds
  25. Chapter 20. Analytical Chemistry
    1. Carbonates
    2. Sulphite
    3. Nitrite
    4. Chlorides
    5. Bromides
    6. Iodide
    7. Nitrate
    8. Sulphate
    9. Tests for basic radicals
    10. Flame test
    11. Borax bead test
    12. Solution test for basic radicals
    13. Test of NH+4 ion
  26. Chapter 21. Problems on Inorganic Reactions
  27. Additional Practice Questions
  28. Copyright