- Description :- This book is about fundamental concepts that any chemistry student should not only be aware of but proficient at. This book deals with the states of matter, the mole, the shapes of molecules, the elements and their properties in the periodic table, the electronic structure of the elements and includes many numerical examples to apply the newly-learned concepts. Solutions to the exercises will be provided in the second volume of “Fundamental of Chemistry”.
- Fundamentals of Chemistry
- Aim of this Book
- Scope of this Book
- Substances and Reactions
- Classifying Substances
- Solids, Liquids and Gases
- Changing state
- Element
- Metals & Non-metals
- Chemical symbols
- Compound
- Mixture
- Physical separation
- Physical and chemical change
- Elements, mixtures or compounds?
- Atomic theory
- Chemical formulae
- Ion
- Naming Compounds
- Chemical Equations Subatomic Structure Relative Atomic Mass
- Chemical equations
- Atomic Structure
- Fundamental subatomic particles
- Chemical Masses
- Mass spectrometer
- Th e Mole
- Introduction
- Why is the mole useful?
- Molecules
- Ionic compounds
- Useful relationships involving the mole
- Mass Percentage composition of elements in compounds
- Empirical formulae of compounds
- Th eoretical yield
- Percentage yield
- Limiting reagent
- Solutions and Concentrations
- Introduction
- Dissolving
- Concentration
- Changing volume
- Most useful unit of concentration - Molarity
- Equation to learn
- Ionic Solutions
- Diluting Solutions
- Th e pH scale
- Other units for concentration
- Electromagnetic Radiation and Spectroscopy
- Electromagnetic Spectrum
- Definition of Electromagnetic Radiation (EMR)
- Energy of Light
- Emission Spectra
- Absorption Spectra
- Uses of spectroscopy
- Quantum theory
- Interpreting electronic spectra
- Quantum-Mechanical Model
- Sublevels
- s orbitals
- p orbitals
- d orbitals
- Quantum Numbers
- Th e Pauli Exclusion Principle
- Electronic Confi guration
- Th e Aufb au Principle
- Summary
- Electron Confi guration Bonding Redox equations
- Valence Electrons and Bonding
- Valence electrons
- Bonding
- Lewis diagrams
- Single and multiple covalent bonds
- Redox reactions
- Summary
- Shapes of Molecules
- Exceptions to the octet rule
- Exceptions to the octet rule
- Limitations of Lewis structures
- Shapes of covalent molecules
- Molecules with lone pairs
- Distorted shapes
- Exercise - What shape is an ammonia molecule?
- Non-equivalent positions
- Molecules with lone pairs
- Limitations with Lewis structures
- Metallic bonding
- Ionic and Covalent
- Electronegativity
- Polar bonds
- Intermolecular forces
- Chemical Bonding and Solid Structures
- Introduction
- Giant metallic structures and their properties
- Giant Ionic structures and their properties
- Molecular structures and their properties
- Simple molecular structures and their properties
- Trends in the Periodic Table
- Historical trends
- Mendeleev’s table ()
- Modern Periodic Table
- Metals / non-metals
- Physical Properties
- Electronegativity
- Trends across a Period
- Trends down a Group
- Thermochemistry
- Introduction
- Forms of Energy
- Energy and Chemical Reactions
- Enthalpy, H
- Heat Energy and Chemical Reactions
- Enthalpy and Enthalpy Change
- Endothermic reactions
- Enthalpy and Enthalpy Change
- Th ermochemical equations
- Standard State Enthalpy Changes
- Standard State Enthalpies
- Specifi c heat capacity
- Standard State Enthalpies
- Summary
- Blogger Comment
- Facebook Comment
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