Metallic Bonding

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Slide 1

Metallic Bonding

Strong forces of attraction are responsible for the high melting point of most metals.

Slide 2

CA Standards

Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds.

Slide 3

Metallic Bonding

The chemical bonding that results from the attraction between metal cations and the surrounding sea of electrons

Vacant p and d orbitals in metal's outer energy levels overlap, and allow outer electrons to move freely throughout the metal

Valence electrons do not belong to any one atom

Slide 4

Packing in Metals

Model: Packing uniform, hard spheres to best use available space. This is called closest packing. Each atom has 12 nearest neighbors.

Slide 5

Metal Alloys

Substitutional Alloy: some metal atoms replaced by others of similar size.

Slide 6

Metal Alloys

Interstitial Alloy: Interstices (holes) in closest packed metal structure are occupied by small atoms.

Slide 7

Properties of Metals

Metals are good conductors of heat and electricity

Metals are malleable

Metals are ductile

Metals have high tensile strength

Metals have luster