Bonds

There are several types of bonds depending upon how the electrons are shared, gained or lost. The electronegativity of the atom is the force which either holds its valence electrons or attracts other atoms' valence electrons. Values for some of the elements electronegativity are given in the Periodic Table.

• Ionic or Electrovalence Bond -- The valence electron or electrons go from one atom to a another when the difference between the electronegativity of the atoms in the bond is greater than 1.7, thus each of the atoms charge changes. This is because the electron has a charge of -1 and the atoms had a neutral charge before ( an atom has the same number of electrons (-1 charge each) as protons (+1 charge each)). The atoms in this compond are positive or negative ions. The atom that gave up the electron now has a positive charge and the atom that gained the electron has a negative charge.
• Covalent Bond-- The valence electron or electrons are shared.
  • Nonpolar --The difference between the electronegativity of the atoms is vary small (less than about 0.5).
  • Polar -- The difference between the electronegativity of the atoms is between 0.5 and 1.7. In this case ther is a un equal attraction draws the shared electrons closer to the atom with the higher electronegativity.
• Metallic Bond -- As with most metals, one or more of the valence electrons release from the atom (thus making the atom a positive ion, because it lost 1 or more electrons) and float in a sea of free electrons amongst the now positive ions. The difference between these charged particles form a strong bond (opposite charges attract). Because of these free electrons, metals make good conductors of electricity as electricity is the flow of electrons.
• Hydrogen Bond -- to be continued...
• Sigma Bond -- to be continued...
• Pi Bond -- to be continued...