Blog #3; Hannah Boynton

There are three divisions for the types of bonds that occur;

-metallic bonding; Metals tend to have high melting points and boiling points suggesting strong bonds between the atoms. The nature of metals in metallic bonding is that they have loosely held electrons that can be taken away easily. Metallic bonding is usually done when metals naturally bond with other metal atoms. About 80 of the 100 elements, are in fact, metals. They are very malleable and ductile. They are very conductive toward heat and electricity. They easily lose electrons during the bonding process.
*Examples; Silver, Copper, Gold.

-ionic bonding; Electrons are completely transferred from one atom to another. In the process of the atoms losing or gaining negatively charged electrons, the reacting atoms form ions. The opposite charged ions are attracted to each other by electrostatic forces, which are the basis of the ionic bond. Ionic bonds form between metals and nonmetals. In naming ionic compounds, the metal always comes first, the nonmetal second. (Ex. Sodium Chloride.) Very soluble in water and other polar solvents. They, also like metals, conduct electricity very easily. Ionic compounds tend to form crystalline solids.
*Example; Sodium Chloride

-covalent bonding; Occurs because the atoms in the compound have a similar tendency for electrons (generally to gain electrons.) Form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms, and other covalent bonds. Covalent bonds are usually formed between two atoms that are able to share electrons and are usually gases and are both nonmetals. Covalent is usually found in elements and compounds; unlike the others, it has very low boiling point, low polarity, and has definite shape.
*Example; Hydro Chloric Acid, Methane