Blog Test Question #3

Ionic, Covalent, and Metallic are the three divisions of bonds.

Ionic Bonding

Description: Ionic bonding is when you have a cation (loses an electron to become positively charged) and anion (gains an electron to become negatively charged) combine together due to opposites attracting. This is basically a strong bond between a metal and a non-metal. Also called extrovalent bonding.

Characteristics: Have High melting points. Have Conduct electricity. Dissolve easily in water. Have well-defined crystals. One atom has a high electronegativity value, while the other value is relatively low.

Reasons: The strong bond of metal and non-metal causes a tighter structure and a higher melting point.

Examples: Sodium chloride

Covalent Bonding

Description: A bond formed by the sharing of electrons between atoms and sometimes other covalent bonds. Different types are metal to metal bonding, σ-bonding, and π-bonding. Covalent bonds are affected by the electro negativity of the connected atoms. Two atoms with equal electro negativity will make non-polar covalent bonds such as H-H. An unequal relationship creates a polar covalent bond such as with H-Cl.

Characteristics: Covalent bonds are molecules (neutral). Does not always conduct electricity. Low melting and boiling points. Definite shape.

Reasons: The sturdy “inputs” of the bond can cause the definite shape.

Examples: Hydrogen Chloride

Metallic Bonding

Description: Although the term metallic bond is often used in contrast to the term covalent bond, it is preferable to use the term metallic bonding, because this type of bonding is collective in nature and a single metallic bond does not exist. It is not considered covalent due to some bonds being metal to metal, but not metallic. Based on the sharing of free electrons.

Characteristics: Conductors of heat and electricity. Some of the same characteristics as covalent.

Reasons: The metal on metal causes the heat and electricity conducting.

Examples: Bronze. Brass. Steel.