Metallic Bonding and Properties of Metals

Flashcards covering the definition, formation, and strength of metallic bonds, as well as explanations for the physical properties of metals.

Between what types of atoms do metallic bonds form?

Metallic bonds are formed between metal atoms in a metal or metal alloy.

What happens to the outer electrons of metal atoms during metallic bonding?

The outer electrons leave the metal atoms, giving metal ions and free electrons around the metal ions.

What creates the attraction that forms a metallic bond?

The attraction between the positive metal ions and the negative free electrons.

How strong are metallic bonds?

Metallic bonds are strong.

Why do metals have high melting and boiling points?

Because they form a giant lattice with strong metallic bonds.

Why do metals conduct electricity when solid and melted?

Because of free electrons which carry electric charge.

What does it mean that metals are malleable?

They can be readily bent, pressed, or hammered into shape.

Why are metals malleable according to their atomic structure?

Because the layers of atoms can slide over each other, while the free electrons can move (not broken and can drawn into wires).

What term is used in the diagram to describe the free electrons surrounding the metal ions ($M^+$)?

Delocalized electron.