Chemistry Chapter 6 | 1st Year


Chapter 6 Notes | Chemistry 1st Year

 “Chemical Bonding”


  1. Introduction
  2. Atomic Sizes, Atomic Radii, Ionic Radii And Covalent Radii
  3. Ionization Energy, Electron Affinity And Electronegativity
  4. Types of Bonds
  5. Bond Energy, Bond Length And Dipole Moment.
  6. The Effect of Bonding on the Properties of Compounds

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Key Points:

  1. Atoms combine together due to their inherent tendency to attain the nearest noble gas electronic configurations and the formation of a chemical bond always results in a decrease of energy.
  2.  The size of an atom is expressed in terms of atomic radius, ionic radius and covalent radius and van der Waals radius.
  3. It is necessary to understand thermodynamic properties of elements. The minimum amount of energy require to remove an electron from an atom in gaseous state is called ionization energy.
  4. The ionic bonds are formed by transfer of electron from one atom to another. Covalent bonds are formed by mutual sharing of electrons b/w combining atoms. After the formation of a coordinate covalent bond, there s no distinction b/w a covalent bond and a coordinate covalent bond.
  5. A polar covalent bond is formed when atoms having different electronegativity values mutually share their electrons. Due to polarity, bonds become shorter and stronger and dipole moment may develop.
  6. According to valence bond theory, the atomic orbitals overlap to form bonds but the individual character of the atomic orbitals are retained. To greater the overlap, the stronger will be the bond formed.

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