Ionic, Covelant, and Metallic Bonds

Ionic Bonds: Ionic bonds are chemical bonds that result from the electrical attraction between cations and anions. In purely ionic bonds, atoms completely give up electrons to other atoms.  Atoms in ionic material have a strong attraction to other ions nearby. Ionic solids tend to have the following characteristics:

1. They are crystal-like in structure

2. They have high melting and boiling points

3. They conduct electricity when dissolved in water or as a liquid

4. They are soluble

5. they do not conduct electricity as a solid

Covalent bonds: Covalent bonds are bonds that result from the sharing of electron pairs between two atoms. In purely covalent bonds, the shared electron are owned equally by two bonded atoms.  Atoms of covalent materials are bound closely together in stable molecules but aren't strongly attracted to each other.

1. They are  gases, liquids or solids

2. They have low melting and boiling points

3. They are poor electrical conductors in all forms

4. They are mostly soluble in non polar liquids but not in water

Metallic Bonds: Metallic bonds are the result of attraction between positively charges atomic nuclei of metal atoms and relocalized electrons in the metal. There are strong bonds between the atoms, explaining the tendency to have high melting and boiling points.

1. They are shiny

2.  They aren't soluble

3. They have high melting/boiling points

4. They are conductive as solids and liquids

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