The structure of the methane, CH4, molecule exhibits single covalent bonds. Covalent bonding involves the sharing of electrons. In the methane molecule, the four hydrogen atom share one electron each with the carbon atom.
Some properties of covalent bonds are that they tend to occur between two non-metal atoms, have low boiling and melting points and low polarity. At room temperature, these covalent molecules are either gaseous or liquids. For example, methane is a gas.
In contrast, ionic bonds tend to be present in solid compounds. Ionic bonds occur between a metal and non-metal. Some characteristics of ionic bonds in compounds are that they exhibit high melting and boiling points.