Final answer:
Ionic and metallic bonds differ in terms of the elements involved, electron behavior, and properties. Ionic bonds form between metals and nonmetals through electron transfer, resulting in oppositely charged ions. Metallic bonds occur between metal atoms, with the outer electrons being delocalized. Ionic compounds are solid, have high melting points, are brittle, and conduct electricity, while metals are solid, malleable, and conductive.
Step-by-step explanation:
Ionic and metallic bonds are both types of chemical bonds that form between atoms, but they differ in several ways.
Ionic Bonds:
Ionic bonds usually form between metal and nonmetal elements. In an ionic bond, electrons are transferred from the metal atom (which becomes a positive ion) to the nonmetal atom (which becomes a negative ion). These oppositely charged ions are then attracted to each other, creating the bond.
For example, in sodium chloride (NaCl), sodium (Na) donates an electron to chlorine (Cl), creating Na+ and Cl- ions, which attract each other.
Typical properties of ionic compounds include being solid at room temperature, having high melting and boiling points, being brittle, and conducting electricity when dissolved in water or molten.
Metallic Bonds:
Metallic bonds occur between metal atoms. In a metallic bond, the outer electrons of the metal atoms are delocalized, meaning they are not associated with any specific atom and can move freely throughout the metal lattice.
For example, in a piece of copper (Cu), the copper atoms share their outer electrons, creating a sea of delocalized electrons that hold the metal together.
Typical properties of metals include being solid, malleable, and ductile, having high thermal and electrical conductivity, and having lustrous appearances.
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