Ionic, Covalent, and Metallic Bonds
An Ionic Bond is where atoms will either lose or gain an electron. An example would be NaCl. Having seven valence electrons, Cl will try to combine itself with another atom that has only one valence electron to achieve noble gas configuration, and in this case Na has to only one valence electron. Due to the octet rule, the valence electron from Na will move to complete Cl. Ionic Bonds are known to have solubility in water, not melt at a low temperature, and are only able to conduct in either a liquid state or dissolved in water.
A covalent bond is when a nonmetal and a nonmetal share one electron in order for them both to become stable. Covalent bonds form from sharing electrons to obtain the Octet configuration.
The characteristics of a covalent bond are that it doesn't conduct electricity in water, they aren't very soluble (dissolvable) in water, and they have low melting points.
Carbon Diamonds are an example of Covalent Bonds
Metallic bonds are bonds between metals and metals
Characteristics: shiny, does not dissolve, high melting point, conducts all the time
Ex. Fe Iron