1. Metallic Bonding

2. Metallic Bonding
Metallic Bond – the force that holds metal atoms together
Metals do not form covalent bonds with one another because they do not have enough electrons in their outer shells to form stable octets.
Even though they do not form covalent bonds, they do share electrons.
They release their electrons to a shared pool of electrons.
Imagine a metal as a non-rigid arrangement of metal ions in a sea of free electrons.

3. Sea of electrons
The valence electrons delocalize from the positive atoms.

4. Melting point According to the strength of the bond
Depends on the number of electrons the atom can delocalize to its “sea”
Group 1 metals have the lowest m.p. since they only have one valence electron to contribute; also they have the largest radius so the positive nucleus is further from the sea
Transition metals have particularly high melting points because they can involve the d electrons in their delocalization in addition to the s e’s.

5. Conductivity Electrical Thermal
Metals conduct electricity well because the electrons can flow in the sea.
Thermal
Metals also conduct heat well because the freely moving electrons have kinetic energy.

6. Strength and Workability
Malleable – can be beaten into sheets
Ductile – can be stretched into wires
BECAUSE the atoms are able to roll over each other without breaking bonds
Stress can be put on the metal and released and the atoms will go back to normal because metals are ELASTIC.

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