Types of Compounds

Metallic Bonding Metal atoms of the same element bond with each other by sharing valence electrons because they do not have a lot of valence electrons so they disperse valence electrons between each other. This is a lot like an atomic game of “hot potato”, where metal kernals (the atom inside the valence electrons) sit in a crystal lattice (atoms are arranged in a uniformed pattern), passing valence electrons back and forth between each other). Ex: Copper, Calcium, Zinc, Gold, Silver

Since electrons can be forced to travel in a certain direction within the metal, metals are very good at conducting electricity in all phases.

Alloys Calcium solid consists of Ca atoms linked or bonded together. What about different metals? Alloy- metal to metal blending (mixture). In an Alloy, metals are not bonded together, just mixed. Ex: Brass, Bronze

Ionic Compounds made of metal and nonmetal ions. Form an ionic crystal lattice when in the solid phase due to super strong bond (attraction for each other). Ions separate when melted or dissolved in water, allowing electrical conduction. Examples: NaCl, Can dissolve in water due to water’s polarity Very high melting and boiling points. When you melt an ionic solid, you free up the ions . Now they can move around liquid and conduct electricity. Do not conduct electricity as solids because ions are locked into place (crystal lattice). All ionic substances are called salts.

Ionic Compounds

Covalent Compounds Covalent: made of nonmetal atoms bonded together. Have weak + and – attractions so Bonds break easily upon melting or dissolving, also called molecular substances, do not conduct electricity. Low Melting and Boiling points. Many are gases and liquids at room temperature. Do not conduct electricity, no free ions to move around. Pure water does not conduct electricity, tap water does due to ions dissolved into it during filtration process.

Metallic Compounds Do not dissolve in water. They all conduct electricity. Malleable and Ductile.