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.Continue Reading
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.Learn more about Atoms & Molecules
The molecule known as CH4, or methane, is affected by van der Waals forces between individual molecules. Van der Waals forces are created when the molecule temporarily becomes electrically charged due to the natural movement of electrons across the shared bonds of the atoms making up the molecule.Full Answer >
Atoms that typically form covalent bonds with each other have similar electronegativity, which expresses the atom's tendency to attract electrons, such as with carbon and hydrogen, which form methane. They stand in contrast to ionic bonds, where electronegativities are vastly different, as with sodium and chlorine, which combine to form table salt. These actually exist on a continuum with significant but lesser differences in electronegativity causing the formation of polar molecules.Full Answer >
Hydrogen bonds hold together the atoms in a water molecule. A single water molecule is made up of two hydrogen atoms and one oxygen atom.Full Answer >
Hydrogen bonds form because of the attraction between a slightly positive hydrogen atom of one molecule and the slightly negative atom of another molecule. Differences in electronegativity between the hydrogen atom and the other atom or atoms of the molecule lead to these partial positive and partial negative charges.Full Answer >