Key Differences Between Ionic, Covalent, and Metallic Bonds

1. Formation and Structure:

   • Ionic Bonds: These bonds happen between metals and non-metals when electrons are transferred from one atom to another.

     • For example, table salt, known as sodium chloride (NaCl), is made this way.

   • Covalent Bonds: These occur between non-metal atoms that share electrons with each other.

     • An example of this is water (H₂O).

   • Metallic Bonds: Metallic bonds occur between metal atoms.

     • In these bonds, the atoms share a "sea" of electrons. This helps metals conduct electricity and be shaped easily.
     • Copper (Cu) is a good example of a metal with metallic bonds.

2. Properties:

   • Ionic Compounds:

     • They have high melting and boiling points. For example, sodium chloride (table salt) melts at 801°C.
     • They dissolve well in water and can conduct electricity when they do.

   • Covalent Compounds:

     • These usually have lower melting and boiling points. Water boils at 100°C.
     • They usually don't conduct electricity and can be either soluble or not in water.

   • Metallic Compounds:

     • They have high melting and boiling points. Copper melts at 1,085°C.
     • Metallic substances are excellent at conducting heat and electricity.

3. Electronegativity Differences:

   • Ionic Bonds: The difference in electronegativity (the ability of an atom to attract electrons) is greater than 1.7 in these bonds.

   • Covalent Bonds: The electronegativity difference is less than 1.7.

   • Metallic Bonds: These involve elements that tend to have low electronegativity, usually found on the left side of the periodic table.