1. Metallic Bonds Quartz

2. Metal atoms are arranged in very compact and orderly patterns. Although metals do not bond ionically, they often form lattices in the solid state. 8 to 12 other metal atoms surround each metal atom.

3. Crystal Structure of Metals ChromiumGold Zinc

4. In this crowded condition, the outer energy levels of the metal atoms overlap. This overlapping of orbitals allows the outer electrons of the atoms to roam freely throughout the entire metal. The electrons are delocalized, which means that the electrons are not held by any specific atom, instead they can move freely throughout the metal lattice.

5. This mobile electrons form a sea of electrons around the metal atoms.

6. Metallic bonds are the forces of attraction between the metal cations(+) and the delocalized, mobile valence electrons. Sea of electrons model

7. Properties of Metals Metals are good conductors of electrical current and heat because electrons can flow freely throughout the metal lattice.

8. Metals are malleable and ductile because metallic bonding is the same in all directions throughout the solid. Malleable: can be hammered or beaten into thin sheets. Ductile: can be drawn or pulled to produce a wire.

9. Alloys are a mixture of two or more elements, at least one of which is a metal. ALLOYS Brass is an alloy of copper and zinc. Sterling silver: 92.5% silver 7.5% copper Bronze is an alloy of copper and tin.

10. Steel is an alloy composed largely of iron and a lesser amount of carbon, along with other metals. STEEL