Final answer:
Ionic bonding involves the transfer of electrons forming ions that attract each other to create a lattice structure, while metallic bonding is characterized by the electrostatic attraction between metal ions and a sea of delocalized electrons allowing for conductivity and malleability in metals.
Step-by-step explanation:
Ionic bonding involves the complete transfer of electrons from one atom to another, leading to the creation of ions. These ions—cations, which are positively charged, and anions, which are negatively charged—then attract each other due to electrostatic forces.
This can be visualized as represented in Figure 7.10, which uses Lewis symbols to show electron transfer, forming ionic compounds as seen in Figure 3.9.3. The ions in ionic crystals optimize the attractive forces between opposite charges to form a stable lattice structure.
On the other hand, metallic bonding is characterized by the electrostatic attraction between the positively charged atomic nuclei of metal atoms and the delocalized electrons that surround them. In Figure 3.9.2, a model illustrates how the valence electrons, or the 'sea of electrons', are not bound to any specific atom but rather move freely, allowing for the positive metal ions to be attracted to this sea of electrons. The atoms form a crystal lattice maintained by this metallic bond, which is among the strongest chemical bonds.
Both ionic and metallic bonds are key in understanding the properties of substances. Ionic crystals often have high melting points and are soluble in water, and their structure is well illustrated in Figure 3.1.6. Metals, with their delocalized electrons and metallic bonds, are typically malleable, ductile, and conductive.
Each type of bond gives the material its distinct properties, like conductivity in metals due to the sea of electrons, and the crystalline structure in ionic compounds which often leads to brittleness.