![]() The properties of metallic substances are primarily due to the nature of metallic bonding. This creates a strong, continuous electrostatic attraction between the metal ions and the delocalized electrons, forming a network of metallic bonds. The delocalized electrons are shared between all metal atoms in the lattice, resulting in a “sea” of electrons surrounding a lattice of positively charged metal ions. In metallic bonding, the valence electrons of metal atoms are delocalized, meaning they are free to move throughout the crystal lattice of metal ions. In A-level Chemistry, metallic bonding refers to the chemical bonding that occurs between metal atoms in a metallic substance. →What is metallic bonding in A-level Chemistry? Metals cannot dissolve in solvents because metallic bonds are very strong.
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